Chapter 4 Electrons in Atoms

This chapter is about electrons in the atom- a tricky

subject at best- and the evolution of the atomic model

This chapter covers much material some of it very

difficult and abstract It is essential that you bring your

book to class and do all assigned homework

Chapter 4 Arrangement of Electrons in Atoms

bull Atomic Models

- already discussed atomic structure ndash what was it

- inadequate ndash describes only a few properties of atoms

- need a model that is focused on arrangement of ____ the basis of chemistry

Rutherford Model of the AtomThe Rutherford Model (aka the Planetary Model) was an

improvement over the previous models but it was still incomplete It did not include the distribution of the negatively

charged electrons in the atom

We know that negative and positive particles (that is e- and p+)

attract each other so the big question became

Why donrsquot the electrons crash into the nucleus

If + and ndash charges attract why donrsquot e- collapse into the nucleus

In 1913 a student of Rutherfordrsquos created a new model for the atom he proposed the e-rsquos were arranged in

concentric circles around the nucleus (patterned after the movement of planets around the sun)

The Planetary Model

Along with this he stated that the e-rsquos have fixed energy that allows them to avoid falling into the nucleus

analogous to the rungs of a ladder More on this later

The Planetary Model of the Atom

But first letrsquos talk about

The Properties of LightBefore 1900 scientists thought light behaved solely as a wave

What idiots It was soon discovered that light also has particle

characteristics But letrsquos first review the wavelike properties

The Electromagnetic Spectrum

The electromagnetic spectrum shows all the types of

electromagnetic radiation- a form of energy that exhibits wavelike

behavior as it travels through space

All forms of electromagnetic radiation move at a constant speed

of 300 x 108 ms through a vacuum This is about 186000 miless

Also known as the speed of light

Letrsquos talk about waves and wave motion for a minute

Frequency and wavelength are mathematically related This relationship is

c = λv

c = λvIn the equation c is the speed of light (in ms) λ is the wavelength of

the electromagnetic wave (in m) and v is the frequency of the electromagnetic wave (in s-1 or Hz)

Important λ and v are inversely proportional so as the wavelength of light increases the frequency decreases and vice versa

Practice Problems

1 Determine the frequency of light whose wavelength is 4257 x 10-5 m

2 Determine the wavelength (λ) of a photon whose frequency is 355 x 1017 s-1

Electromagnetic Spectrum

The Photoelectric Effect

The photoelectric effect is a phenomenon that refers to

the emission of electrons from a metal when light shines

on the metal

Yoursquore most likely thinking who cares

Well herersquos the thing- for any given metal no electrons were

emitted if the lightrsquos frequency were below a certain minimum

Metal

Light

Electrons

The Photoelectric Effect (contrsquod)

So obviously light was known to be a form of energy capable of

knocking electrons loose from metal But (important)

the wave theory of light predicted that any frequency of light could

supply enough energy to eject an electron so the fact that there had

to be a minimum frequency for a given metal made no sense

Something about the assumption of light behavior was wrong

Metal

Light

Electrons

The Particle Description of Light

The German physicist Max Planck came up with the idea that light

is emitted in small packets called quanta

A quantum of energy is the minimum quantity of energy that

can be gained or lost by an atom

Here is the relationship between quantum and frequency of radiation

E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the

physical constant called Planckrsquos Constant h = 6626 x 10-34 Js

Srsquoup

The Particle Description of Light

In 1905 Einstein took this idea further by stating that light can

act as both a wave and a stream of particles Each particle of light

carries a quantum of energy and is called a photon

A photon is a particle of electromagnetic radiation having zero

mass and carrying a quantum of energy

Ephoton = hvEinstein was able to explain the photoelectric effect this way

Different metals bind their electrons differently so v changes

The Hydrogen-Atom Line-Emission Spectrum

When an electric current is passed through a gas sample at low

pressure the potential energy of the gas changes

The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron

There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized

When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle

The Hydrogen-Atom Line-Emission Spectrum

So what does this mean

Well when scientists passed an electric current through a vacuum

tube with a pure gas in it (like H or O) each atom would go through

the steps listed above they would gain energy and then reemit it

in the form of a photon or light This light was then passed through

a prism and the wavelengths (colors) in that element could be seen

Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed

The Hydrogen-Atom Line-Emission Spectrum

So letrsquos use the example of helium A tube of helium has a current of electricity

pass through it and the absorbed energy is then released in the form of light thus

the tube glows That light is then passed through a prism which separates all the

colors (wavelengths) in that light Helium has a particular emission-spectra or set

of lines at specific color spectra

Every element has a signature color spectra

The Hydrogen-Atom Line-Emission Spectrum

But why are there only some colors appearing and

not all of them

Because the electrons in these atoms have specific

fixed energy levels and only give off certain colors

when jumping from level to level Whenever an

excited helium atom falls to its ground state or to a

lower-energy excited state it emits a photon of

radiation The energy of this photon (Ephoton = hv) is

equal to the difference in energy between the atomrsquos initial state and

itrsquos final state Because different atoms have different energy levels

different atoms give off different frequencies (colors) of light

The Bohr Model of the Hydrogen Atom

Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the

atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed

paths or orbits Notice this

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Chapter 4 Arrangement of Electrons in Atoms

bull Atomic Models

- already discussed atomic structure ndash what was it

- inadequate ndash describes only a few properties of atoms

- need a model that is focused on arrangement of ____ the basis of chemistry

Rutherford Model of the AtomThe Rutherford Model (aka the Planetary Model) was an

improvement over the previous models but it was still incomplete It did not include the distribution of the negatively

charged electrons in the atom

We know that negative and positive particles (that is e- and p+)

attract each other so the big question became

Why donrsquot the electrons crash into the nucleus

If + and ndash charges attract why donrsquot e- collapse into the nucleus

In 1913 a student of Rutherfordrsquos created a new model for the atom he proposed the e-rsquos were arranged in

concentric circles around the nucleus (patterned after the movement of planets around the sun)

The Planetary Model

Along with this he stated that the e-rsquos have fixed energy that allows them to avoid falling into the nucleus

analogous to the rungs of a ladder More on this later

The Planetary Model of the Atom

But first letrsquos talk about

The Properties of LightBefore 1900 scientists thought light behaved solely as a wave

What idiots It was soon discovered that light also has particle

characteristics But letrsquos first review the wavelike properties

The Electromagnetic Spectrum

The electromagnetic spectrum shows all the types of

electromagnetic radiation- a form of energy that exhibits wavelike

behavior as it travels through space

All forms of electromagnetic radiation move at a constant speed

of 300 x 108 ms through a vacuum This is about 186000 miless

Also known as the speed of light

Letrsquos talk about waves and wave motion for a minute

Frequency and wavelength are mathematically related This relationship is

c = λv

c = λvIn the equation c is the speed of light (in ms) λ is the wavelength of

the electromagnetic wave (in m) and v is the frequency of the electromagnetic wave (in s-1 or Hz)

Important λ and v are inversely proportional so as the wavelength of light increases the frequency decreases and vice versa

Practice Problems

1 Determine the frequency of light whose wavelength is 4257 x 10-5 m

2 Determine the wavelength (λ) of a photon whose frequency is 355 x 1017 s-1

Electromagnetic Spectrum

The Photoelectric Effect

The photoelectric effect is a phenomenon that refers to

the emission of electrons from a metal when light shines

on the metal

Yoursquore most likely thinking who cares

Well herersquos the thing- for any given metal no electrons were

emitted if the lightrsquos frequency were below a certain minimum

Metal

Light

Electrons

The Photoelectric Effect (contrsquod)

So obviously light was known to be a form of energy capable of

knocking electrons loose from metal But (important)

the wave theory of light predicted that any frequency of light could

supply enough energy to eject an electron so the fact that there had

to be a minimum frequency for a given metal made no sense

Something about the assumption of light behavior was wrong

Metal

Light

Electrons

The Particle Description of Light

The German physicist Max Planck came up with the idea that light

is emitted in small packets called quanta

A quantum of energy is the minimum quantity of energy that

can be gained or lost by an atom

Here is the relationship between quantum and frequency of radiation

E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the

physical constant called Planckrsquos Constant h = 6626 x 10-34 Js

Srsquoup

The Particle Description of Light

In 1905 Einstein took this idea further by stating that light can

act as both a wave and a stream of particles Each particle of light

carries a quantum of energy and is called a photon

A photon is a particle of electromagnetic radiation having zero

mass and carrying a quantum of energy

Ephoton = hvEinstein was able to explain the photoelectric effect this way

Different metals bind their electrons differently so v changes

The Hydrogen-Atom Line-Emission Spectrum

When an electric current is passed through a gas sample at low

pressure the potential energy of the gas changes

The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron

There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized

When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle

The Hydrogen-Atom Line-Emission Spectrum

So what does this mean

Well when scientists passed an electric current through a vacuum

tube with a pure gas in it (like H or O) each atom would go through

the steps listed above they would gain energy and then reemit it

in the form of a photon or light This light was then passed through

a prism and the wavelengths (colors) in that element could be seen

Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed

The Hydrogen-Atom Line-Emission Spectrum

So letrsquos use the example of helium A tube of helium has a current of electricity

pass through it and the absorbed energy is then released in the form of light thus

the tube glows That light is then passed through a prism which separates all the

colors (wavelengths) in that light Helium has a particular emission-spectra or set

of lines at specific color spectra

Every element has a signature color spectra

The Hydrogen-Atom Line-Emission Spectrum

But why are there only some colors appearing and

not all of them

Because the electrons in these atoms have specific

fixed energy levels and only give off certain colors

when jumping from level to level Whenever an

excited helium atom falls to its ground state or to a

lower-energy excited state it emits a photon of

radiation The energy of this photon (Ephoton = hv) is

equal to the difference in energy between the atomrsquos initial state and

itrsquos final state Because different atoms have different energy levels

different atoms give off different frequencies (colors) of light

The Bohr Model of the Hydrogen Atom

Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the

atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed

paths or orbits Notice this

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Rutherford Model of the AtomThe Rutherford Model (aka the Planetary Model) was an

improvement over the previous models but it was still incomplete It did not include the distribution of the negatively

charged electrons in the atom

We know that negative and positive particles (that is e- and p+)

attract each other so the big question became

Why donrsquot the electrons crash into the nucleus

If + and ndash charges attract why donrsquot e- collapse into the nucleus

In 1913 a student of Rutherfordrsquos created a new model for the atom he proposed the e-rsquos were arranged in

concentric circles around the nucleus (patterned after the movement of planets around the sun)

The Planetary Model

Along with this he stated that the e-rsquos have fixed energy that allows them to avoid falling into the nucleus

analogous to the rungs of a ladder More on this later

The Planetary Model of the Atom

But first letrsquos talk about

The Properties of LightBefore 1900 scientists thought light behaved solely as a wave

What idiots It was soon discovered that light also has particle

characteristics But letrsquos first review the wavelike properties

The Electromagnetic Spectrum

The electromagnetic spectrum shows all the types of

electromagnetic radiation- a form of energy that exhibits wavelike

behavior as it travels through space

All forms of electromagnetic radiation move at a constant speed

of 300 x 108 ms through a vacuum This is about 186000 miless

Also known as the speed of light

Letrsquos talk about waves and wave motion for a minute

Frequency and wavelength are mathematically related This relationship is

c = λv

c = λvIn the equation c is the speed of light (in ms) λ is the wavelength of

the electromagnetic wave (in m) and v is the frequency of the electromagnetic wave (in s-1 or Hz)

Important λ and v are inversely proportional so as the wavelength of light increases the frequency decreases and vice versa

Practice Problems

1 Determine the frequency of light whose wavelength is 4257 x 10-5 m

2 Determine the wavelength (λ) of a photon whose frequency is 355 x 1017 s-1

Electromagnetic Spectrum

The Photoelectric Effect

The photoelectric effect is a phenomenon that refers to

the emission of electrons from a metal when light shines

on the metal

Yoursquore most likely thinking who cares

Well herersquos the thing- for any given metal no electrons were

emitted if the lightrsquos frequency were below a certain minimum

Metal

Light

Electrons

The Photoelectric Effect (contrsquod)

So obviously light was known to be a form of energy capable of

knocking electrons loose from metal But (important)

the wave theory of light predicted that any frequency of light could

supply enough energy to eject an electron so the fact that there had

to be a minimum frequency for a given metal made no sense

Something about the assumption of light behavior was wrong

Metal

Light

Electrons

The Particle Description of Light

The German physicist Max Planck came up with the idea that light

is emitted in small packets called quanta

A quantum of energy is the minimum quantity of energy that

can be gained or lost by an atom

Here is the relationship between quantum and frequency of radiation

E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the

physical constant called Planckrsquos Constant h = 6626 x 10-34 Js

Srsquoup

The Particle Description of Light

In 1905 Einstein took this idea further by stating that light can

act as both a wave and a stream of particles Each particle of light

carries a quantum of energy and is called a photon

A photon is a particle of electromagnetic radiation having zero

mass and carrying a quantum of energy

Ephoton = hvEinstein was able to explain the photoelectric effect this way

Different metals bind their electrons differently so v changes

The Hydrogen-Atom Line-Emission Spectrum

When an electric current is passed through a gas sample at low

pressure the potential energy of the gas changes

The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron

There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized

When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle

The Hydrogen-Atom Line-Emission Spectrum

So what does this mean

Well when scientists passed an electric current through a vacuum

tube with a pure gas in it (like H or O) each atom would go through

the steps listed above they would gain energy and then reemit it

in the form of a photon or light This light was then passed through

a prism and the wavelengths (colors) in that element could be seen

Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed

The Hydrogen-Atom Line-Emission Spectrum

So letrsquos use the example of helium A tube of helium has a current of electricity

pass through it and the absorbed energy is then released in the form of light thus

the tube glows That light is then passed through a prism which separates all the

colors (wavelengths) in that light Helium has a particular emission-spectra or set

of lines at specific color spectra

Every element has a signature color spectra

The Hydrogen-Atom Line-Emission Spectrum

But why are there only some colors appearing and

not all of them

Because the electrons in these atoms have specific

fixed energy levels and only give off certain colors

when jumping from level to level Whenever an

excited helium atom falls to its ground state or to a

lower-energy excited state it emits a photon of

radiation The energy of this photon (Ephoton = hv) is

equal to the difference in energy between the atomrsquos initial state and

itrsquos final state Because different atoms have different energy levels

different atoms give off different frequencies (colors) of light

The Bohr Model of the Hydrogen Atom

Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the

atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed

paths or orbits Notice this

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

If + and ndash charges attract why donrsquot e- collapse into the nucleus

In 1913 a student of Rutherfordrsquos created a new model for the atom he proposed the e-rsquos were arranged in

concentric circles around the nucleus (patterned after the movement of planets around the sun)

The Planetary Model

Along with this he stated that the e-rsquos have fixed energy that allows them to avoid falling into the nucleus

analogous to the rungs of a ladder More on this later

The Planetary Model of the Atom

But first letrsquos talk about

The Properties of LightBefore 1900 scientists thought light behaved solely as a wave

What idiots It was soon discovered that light also has particle

characteristics But letrsquos first review the wavelike properties

The Electromagnetic Spectrum

The electromagnetic spectrum shows all the types of

electromagnetic radiation- a form of energy that exhibits wavelike

behavior as it travels through space

All forms of electromagnetic radiation move at a constant speed

of 300 x 108 ms through a vacuum This is about 186000 miless

Also known as the speed of light

Letrsquos talk about waves and wave motion for a minute

Frequency and wavelength are mathematically related This relationship is

c = λv

c = λvIn the equation c is the speed of light (in ms) λ is the wavelength of

the electromagnetic wave (in m) and v is the frequency of the electromagnetic wave (in s-1 or Hz)

Important λ and v are inversely proportional so as the wavelength of light increases the frequency decreases and vice versa

Practice Problems

1 Determine the frequency of light whose wavelength is 4257 x 10-5 m

2 Determine the wavelength (λ) of a photon whose frequency is 355 x 1017 s-1

Electromagnetic Spectrum

The Photoelectric Effect

The photoelectric effect is a phenomenon that refers to

the emission of electrons from a metal when light shines

on the metal

Yoursquore most likely thinking who cares

Well herersquos the thing- for any given metal no electrons were

emitted if the lightrsquos frequency were below a certain minimum

Metal

Light

Electrons

The Photoelectric Effect (contrsquod)

So obviously light was known to be a form of energy capable of

knocking electrons loose from metal But (important)

the wave theory of light predicted that any frequency of light could

supply enough energy to eject an electron so the fact that there had

to be a minimum frequency for a given metal made no sense

Something about the assumption of light behavior was wrong

Metal

Light

Electrons

The Particle Description of Light

The German physicist Max Planck came up with the idea that light

is emitted in small packets called quanta

A quantum of energy is the minimum quantity of energy that

can be gained or lost by an atom

Here is the relationship between quantum and frequency of radiation

E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the

physical constant called Planckrsquos Constant h = 6626 x 10-34 Js

Srsquoup

The Particle Description of Light

In 1905 Einstein took this idea further by stating that light can

act as both a wave and a stream of particles Each particle of light

carries a quantum of energy and is called a photon

A photon is a particle of electromagnetic radiation having zero

mass and carrying a quantum of energy

Ephoton = hvEinstein was able to explain the photoelectric effect this way

Different metals bind their electrons differently so v changes

The Hydrogen-Atom Line-Emission Spectrum

When an electric current is passed through a gas sample at low

pressure the potential energy of the gas changes

The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron

There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized

When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle

The Hydrogen-Atom Line-Emission Spectrum

So what does this mean

Well when scientists passed an electric current through a vacuum

tube with a pure gas in it (like H or O) each atom would go through

the steps listed above they would gain energy and then reemit it

in the form of a photon or light This light was then passed through

a prism and the wavelengths (colors) in that element could be seen

Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed

The Hydrogen-Atom Line-Emission Spectrum

So letrsquos use the example of helium A tube of helium has a current of electricity

pass through it and the absorbed energy is then released in the form of light thus

the tube glows That light is then passed through a prism which separates all the

colors (wavelengths) in that light Helium has a particular emission-spectra or set

of lines at specific color spectra

Every element has a signature color spectra

The Hydrogen-Atom Line-Emission Spectrum

But why are there only some colors appearing and

not all of them

Because the electrons in these atoms have specific

fixed energy levels and only give off certain colors

when jumping from level to level Whenever an

excited helium atom falls to its ground state or to a

lower-energy excited state it emits a photon of

radiation The energy of this photon (Ephoton = hv) is

equal to the difference in energy between the atomrsquos initial state and

itrsquos final state Because different atoms have different energy levels

different atoms give off different frequencies (colors) of light

The Bohr Model of the Hydrogen Atom

Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the

atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed

paths or orbits Notice this

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

The Planetary Model of the Atom

But first letrsquos talk about

The Properties of LightBefore 1900 scientists thought light behaved solely as a wave

What idiots It was soon discovered that light also has particle

characteristics But letrsquos first review the wavelike properties

The Electromagnetic Spectrum

The electromagnetic spectrum shows all the types of

electromagnetic radiation- a form of energy that exhibits wavelike

behavior as it travels through space

All forms of electromagnetic radiation move at a constant speed

of 300 x 108 ms through a vacuum This is about 186000 miless

Also known as the speed of light

Letrsquos talk about waves and wave motion for a minute

Frequency and wavelength are mathematically related This relationship is

c = λv

c = λvIn the equation c is the speed of light (in ms) λ is the wavelength of

the electromagnetic wave (in m) and v is the frequency of the electromagnetic wave (in s-1 or Hz)

Important λ and v are inversely proportional so as the wavelength of light increases the frequency decreases and vice versa

Practice Problems

1 Determine the frequency of light whose wavelength is 4257 x 10-5 m

2 Determine the wavelength (λ) of a photon whose frequency is 355 x 1017 s-1

Electromagnetic Spectrum

The Photoelectric Effect

The photoelectric effect is a phenomenon that refers to

the emission of electrons from a metal when light shines

on the metal

Yoursquore most likely thinking who cares

Well herersquos the thing- for any given metal no electrons were

emitted if the lightrsquos frequency were below a certain minimum

Metal

Light

Electrons

The Photoelectric Effect (contrsquod)

So obviously light was known to be a form of energy capable of

knocking electrons loose from metal But (important)

the wave theory of light predicted that any frequency of light could

supply enough energy to eject an electron so the fact that there had

to be a minimum frequency for a given metal made no sense

Something about the assumption of light behavior was wrong

Metal

Light

Electrons

The Particle Description of Light

The German physicist Max Planck came up with the idea that light

is emitted in small packets called quanta

A quantum of energy is the minimum quantity of energy that

can be gained or lost by an atom

Here is the relationship between quantum and frequency of radiation

E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the

physical constant called Planckrsquos Constant h = 6626 x 10-34 Js

Srsquoup

The Particle Description of Light

In 1905 Einstein took this idea further by stating that light can

act as both a wave and a stream of particles Each particle of light

carries a quantum of energy and is called a photon

A photon is a particle of electromagnetic radiation having zero

mass and carrying a quantum of energy

Ephoton = hvEinstein was able to explain the photoelectric effect this way

Different metals bind their electrons differently so v changes

The Hydrogen-Atom Line-Emission Spectrum

When an electric current is passed through a gas sample at low

pressure the potential energy of the gas changes

The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron

There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized

When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle

The Hydrogen-Atom Line-Emission Spectrum

So what does this mean

Well when scientists passed an electric current through a vacuum

tube with a pure gas in it (like H or O) each atom would go through

the steps listed above they would gain energy and then reemit it

in the form of a photon or light This light was then passed through

a prism and the wavelengths (colors) in that element could be seen

Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed

The Hydrogen-Atom Line-Emission Spectrum

So letrsquos use the example of helium A tube of helium has a current of electricity

pass through it and the absorbed energy is then released in the form of light thus

the tube glows That light is then passed through a prism which separates all the

colors (wavelengths) in that light Helium has a particular emission-spectra or set

of lines at specific color spectra

Every element has a signature color spectra

The Hydrogen-Atom Line-Emission Spectrum

But why are there only some colors appearing and

not all of them

Because the electrons in these atoms have specific

fixed energy levels and only give off certain colors

when jumping from level to level Whenever an

excited helium atom falls to its ground state or to a

lower-energy excited state it emits a photon of

radiation The energy of this photon (Ephoton = hv) is

equal to the difference in energy between the atomrsquos initial state and

itrsquos final state Because different atoms have different energy levels

different atoms give off different frequencies (colors) of light

The Bohr Model of the Hydrogen Atom

Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the

atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed

paths or orbits Notice this

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

But first letrsquos talk about

The Properties of LightBefore 1900 scientists thought light behaved solely as a wave

What idiots It was soon discovered that light also has particle

characteristics But letrsquos first review the wavelike properties

The Electromagnetic Spectrum

The electromagnetic spectrum shows all the types of

electromagnetic radiation- a form of energy that exhibits wavelike

behavior as it travels through space

All forms of electromagnetic radiation move at a constant speed

of 300 x 108 ms through a vacuum This is about 186000 miless

Also known as the speed of light

Letrsquos talk about waves and wave motion for a minute

Frequency and wavelength are mathematically related This relationship is

c = λv

c = λvIn the equation c is the speed of light (in ms) λ is the wavelength of

the electromagnetic wave (in m) and v is the frequency of the electromagnetic wave (in s-1 or Hz)

Important λ and v are inversely proportional so as the wavelength of light increases the frequency decreases and vice versa

Practice Problems

1 Determine the frequency of light whose wavelength is 4257 x 10-5 m

2 Determine the wavelength (λ) of a photon whose frequency is 355 x 1017 s-1

Electromagnetic Spectrum

The Photoelectric Effect

The photoelectric effect is a phenomenon that refers to

the emission of electrons from a metal when light shines

on the metal

Yoursquore most likely thinking who cares

Well herersquos the thing- for any given metal no electrons were

emitted if the lightrsquos frequency were below a certain minimum

Metal

Light

Electrons

The Photoelectric Effect (contrsquod)

So obviously light was known to be a form of energy capable of

knocking electrons loose from metal But (important)

the wave theory of light predicted that any frequency of light could

supply enough energy to eject an electron so the fact that there had

to be a minimum frequency for a given metal made no sense

Something about the assumption of light behavior was wrong

Metal

Light

Electrons

The Particle Description of Light

The German physicist Max Planck came up with the idea that light

is emitted in small packets called quanta

A quantum of energy is the minimum quantity of energy that

can be gained or lost by an atom

Here is the relationship between quantum and frequency of radiation

E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the

physical constant called Planckrsquos Constant h = 6626 x 10-34 Js

Srsquoup

The Particle Description of Light

In 1905 Einstein took this idea further by stating that light can

act as both a wave and a stream of particles Each particle of light

carries a quantum of energy and is called a photon

A photon is a particle of electromagnetic radiation having zero

mass and carrying a quantum of energy

Ephoton = hvEinstein was able to explain the photoelectric effect this way

Different metals bind their electrons differently so v changes

The Hydrogen-Atom Line-Emission Spectrum

When an electric current is passed through a gas sample at low

pressure the potential energy of the gas changes

The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron

There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized

When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle

The Hydrogen-Atom Line-Emission Spectrum

So what does this mean

Well when scientists passed an electric current through a vacuum

tube with a pure gas in it (like H or O) each atom would go through

the steps listed above they would gain energy and then reemit it

in the form of a photon or light This light was then passed through

a prism and the wavelengths (colors) in that element could be seen

Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed

The Hydrogen-Atom Line-Emission Spectrum

So letrsquos use the example of helium A tube of helium has a current of electricity

pass through it and the absorbed energy is then released in the form of light thus

the tube glows That light is then passed through a prism which separates all the

colors (wavelengths) in that light Helium has a particular emission-spectra or set

of lines at specific color spectra

Every element has a signature color spectra

The Hydrogen-Atom Line-Emission Spectrum

But why are there only some colors appearing and

not all of them

Because the electrons in these atoms have specific

fixed energy levels and only give off certain colors

when jumping from level to level Whenever an

excited helium atom falls to its ground state or to a

lower-energy excited state it emits a photon of

radiation The energy of this photon (Ephoton = hv) is

equal to the difference in energy between the atomrsquos initial state and

itrsquos final state Because different atoms have different energy levels

different atoms give off different frequencies (colors) of light

The Bohr Model of the Hydrogen Atom

Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the

atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed

paths or orbits Notice this

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

The electromagnetic spectrum shows all the types of

electromagnetic radiation- a form of energy that exhibits wavelike

behavior as it travels through space

All forms of electromagnetic radiation move at a constant speed

of 300 x 108 ms through a vacuum This is about 186000 miless

Also known as the speed of light

Letrsquos talk about waves and wave motion for a minute

Frequency and wavelength are mathematically related This relationship is

c = λv

c = λvIn the equation c is the speed of light (in ms) λ is the wavelength of

the electromagnetic wave (in m) and v is the frequency of the electromagnetic wave (in s-1 or Hz)

Important λ and v are inversely proportional so as the wavelength of light increases the frequency decreases and vice versa

Practice Problems

1 Determine the frequency of light whose wavelength is 4257 x 10-5 m

2 Determine the wavelength (λ) of a photon whose frequency is 355 x 1017 s-1

Electromagnetic Spectrum

The Photoelectric Effect

The photoelectric effect is a phenomenon that refers to

the emission of electrons from a metal when light shines

on the metal

Yoursquore most likely thinking who cares

Well herersquos the thing- for any given metal no electrons were

emitted if the lightrsquos frequency were below a certain minimum

Metal

Light

Electrons

The Photoelectric Effect (contrsquod)

So obviously light was known to be a form of energy capable of

knocking electrons loose from metal But (important)

the wave theory of light predicted that any frequency of light could

supply enough energy to eject an electron so the fact that there had

to be a minimum frequency for a given metal made no sense

Something about the assumption of light behavior was wrong

Metal

Light

Electrons

The Particle Description of Light

The German physicist Max Planck came up with the idea that light

is emitted in small packets called quanta

A quantum of energy is the minimum quantity of energy that

can be gained or lost by an atom

Here is the relationship between quantum and frequency of radiation

E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the

physical constant called Planckrsquos Constant h = 6626 x 10-34 Js

Srsquoup

The Particle Description of Light

In 1905 Einstein took this idea further by stating that light can

act as both a wave and a stream of particles Each particle of light

carries a quantum of energy and is called a photon

A photon is a particle of electromagnetic radiation having zero

mass and carrying a quantum of energy

Ephoton = hvEinstein was able to explain the photoelectric effect this way

Different metals bind their electrons differently so v changes

The Hydrogen-Atom Line-Emission Spectrum

When an electric current is passed through a gas sample at low

pressure the potential energy of the gas changes

The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron

There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized

When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle

The Hydrogen-Atom Line-Emission Spectrum

So what does this mean

Well when scientists passed an electric current through a vacuum

tube with a pure gas in it (like H or O) each atom would go through

the steps listed above they would gain energy and then reemit it

in the form of a photon or light This light was then passed through

a prism and the wavelengths (colors) in that element could be seen

Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed

The Hydrogen-Atom Line-Emission Spectrum

So letrsquos use the example of helium A tube of helium has a current of electricity

pass through it and the absorbed energy is then released in the form of light thus

the tube glows That light is then passed through a prism which separates all the

colors (wavelengths) in that light Helium has a particular emission-spectra or set

of lines at specific color spectra

Every element has a signature color spectra

The Hydrogen-Atom Line-Emission Spectrum

But why are there only some colors appearing and

not all of them

Because the electrons in these atoms have specific

fixed energy levels and only give off certain colors

when jumping from level to level Whenever an

excited helium atom falls to its ground state or to a

lower-energy excited state it emits a photon of

radiation The energy of this photon (Ephoton = hv) is

equal to the difference in energy between the atomrsquos initial state and

itrsquos final state Because different atoms have different energy levels

different atoms give off different frequencies (colors) of light

The Bohr Model of the Hydrogen Atom

Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the

atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed

paths or orbits Notice this

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Letrsquos talk about waves and wave motion for a minute

Frequency and wavelength are mathematically related This relationship is

c = λv

c = λvIn the equation c is the speed of light (in ms) λ is the wavelength of

the electromagnetic wave (in m) and v is the frequency of the electromagnetic wave (in s-1 or Hz)

Important λ and v are inversely proportional so as the wavelength of light increases the frequency decreases and vice versa

Practice Problems

1 Determine the frequency of light whose wavelength is 4257 x 10-5 m

2 Determine the wavelength (λ) of a photon whose frequency is 355 x 1017 s-1

Electromagnetic Spectrum

The Photoelectric Effect

The photoelectric effect is a phenomenon that refers to

the emission of electrons from a metal when light shines

on the metal

Yoursquore most likely thinking who cares

Well herersquos the thing- for any given metal no electrons were

emitted if the lightrsquos frequency were below a certain minimum

Metal

Light

Electrons

The Photoelectric Effect (contrsquod)

So obviously light was known to be a form of energy capable of

knocking electrons loose from metal But (important)

the wave theory of light predicted that any frequency of light could

supply enough energy to eject an electron so the fact that there had

to be a minimum frequency for a given metal made no sense

Something about the assumption of light behavior was wrong

Metal

Light

Electrons

The Particle Description of Light

The German physicist Max Planck came up with the idea that light

is emitted in small packets called quanta

A quantum of energy is the minimum quantity of energy that

can be gained or lost by an atom

Here is the relationship between quantum and frequency of radiation

E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the

physical constant called Planckrsquos Constant h = 6626 x 10-34 Js

Srsquoup

The Particle Description of Light

In 1905 Einstein took this idea further by stating that light can

act as both a wave and a stream of particles Each particle of light

carries a quantum of energy and is called a photon

A photon is a particle of electromagnetic radiation having zero

mass and carrying a quantum of energy

Ephoton = hvEinstein was able to explain the photoelectric effect this way

Different metals bind their electrons differently so v changes

The Hydrogen-Atom Line-Emission Spectrum

When an electric current is passed through a gas sample at low

pressure the potential energy of the gas changes

The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron

There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized

When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle

The Hydrogen-Atom Line-Emission Spectrum

So what does this mean

Well when scientists passed an electric current through a vacuum

tube with a pure gas in it (like H or O) each atom would go through

the steps listed above they would gain energy and then reemit it

in the form of a photon or light This light was then passed through

a prism and the wavelengths (colors) in that element could be seen

Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed

The Hydrogen-Atom Line-Emission Spectrum

So letrsquos use the example of helium A tube of helium has a current of electricity

pass through it and the absorbed energy is then released in the form of light thus

the tube glows That light is then passed through a prism which separates all the

colors (wavelengths) in that light Helium has a particular emission-spectra or set

of lines at specific color spectra

Every element has a signature color spectra

The Hydrogen-Atom Line-Emission Spectrum

But why are there only some colors appearing and

not all of them

Because the electrons in these atoms have specific

fixed energy levels and only give off certain colors

when jumping from level to level Whenever an

excited helium atom falls to its ground state or to a

lower-energy excited state it emits a photon of

radiation The energy of this photon (Ephoton = hv) is

equal to the difference in energy between the atomrsquos initial state and

itrsquos final state Because different atoms have different energy levels

different atoms give off different frequencies (colors) of light

The Bohr Model of the Hydrogen Atom

Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the

atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed

paths or orbits Notice this

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

c = λvIn the equation c is the speed of light (in ms) λ is the wavelength of

the electromagnetic wave (in m) and v is the frequency of the electromagnetic wave (in s-1 or Hz)

Important λ and v are inversely proportional so as the wavelength of light increases the frequency decreases and vice versa

Practice Problems

1 Determine the frequency of light whose wavelength is 4257 x 10-5 m

2 Determine the wavelength (λ) of a photon whose frequency is 355 x 1017 s-1

Electromagnetic Spectrum

The Photoelectric Effect

The photoelectric effect is a phenomenon that refers to

the emission of electrons from a metal when light shines

on the metal

Yoursquore most likely thinking who cares

Well herersquos the thing- for any given metal no electrons were

emitted if the lightrsquos frequency were below a certain minimum

Metal

Light

Electrons

The Photoelectric Effect (contrsquod)

So obviously light was known to be a form of energy capable of

knocking electrons loose from metal But (important)

the wave theory of light predicted that any frequency of light could

supply enough energy to eject an electron so the fact that there had

to be a minimum frequency for a given metal made no sense

Something about the assumption of light behavior was wrong

Metal

Light

Electrons

The Particle Description of Light

The German physicist Max Planck came up with the idea that light

is emitted in small packets called quanta

A quantum of energy is the minimum quantity of energy that

can be gained or lost by an atom

Here is the relationship between quantum and frequency of radiation

E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the

physical constant called Planckrsquos Constant h = 6626 x 10-34 Js

Srsquoup

The Particle Description of Light

In 1905 Einstein took this idea further by stating that light can

act as both a wave and a stream of particles Each particle of light

carries a quantum of energy and is called a photon

A photon is a particle of electromagnetic radiation having zero

mass and carrying a quantum of energy

Ephoton = hvEinstein was able to explain the photoelectric effect this way

Different metals bind their electrons differently so v changes

The Hydrogen-Atom Line-Emission Spectrum

When an electric current is passed through a gas sample at low

pressure the potential energy of the gas changes

The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron

There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized

When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle

The Hydrogen-Atom Line-Emission Spectrum

So what does this mean

Well when scientists passed an electric current through a vacuum

tube with a pure gas in it (like H or O) each atom would go through

the steps listed above they would gain energy and then reemit it

in the form of a photon or light This light was then passed through

a prism and the wavelengths (colors) in that element could be seen

Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed

The Hydrogen-Atom Line-Emission Spectrum

So letrsquos use the example of helium A tube of helium has a current of electricity

pass through it and the absorbed energy is then released in the form of light thus

the tube glows That light is then passed through a prism which separates all the

colors (wavelengths) in that light Helium has a particular emission-spectra or set

of lines at specific color spectra

Every element has a signature color spectra

The Hydrogen-Atom Line-Emission Spectrum

But why are there only some colors appearing and

not all of them

Because the electrons in these atoms have specific

fixed energy levels and only give off certain colors

when jumping from level to level Whenever an

excited helium atom falls to its ground state or to a

lower-energy excited state it emits a photon of

radiation The energy of this photon (Ephoton = hv) is

equal to the difference in energy between the atomrsquos initial state and

itrsquos final state Because different atoms have different energy levels

different atoms give off different frequencies (colors) of light

The Bohr Model of the Hydrogen Atom

Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the

atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed

paths or orbits Notice this

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Electromagnetic Spectrum

The Photoelectric Effect

The photoelectric effect is a phenomenon that refers to

the emission of electrons from a metal when light shines

on the metal

Yoursquore most likely thinking who cares

Well herersquos the thing- for any given metal no electrons were

emitted if the lightrsquos frequency were below a certain minimum

Metal

Light

Electrons

The Photoelectric Effect (contrsquod)

So obviously light was known to be a form of energy capable of

knocking electrons loose from metal But (important)

the wave theory of light predicted that any frequency of light could

supply enough energy to eject an electron so the fact that there had

to be a minimum frequency for a given metal made no sense

Something about the assumption of light behavior was wrong

Metal

Light

Electrons

The Particle Description of Light

The German physicist Max Planck came up with the idea that light

is emitted in small packets called quanta

A quantum of energy is the minimum quantity of energy that

can be gained or lost by an atom

Here is the relationship between quantum and frequency of radiation

E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the

physical constant called Planckrsquos Constant h = 6626 x 10-34 Js

Srsquoup

The Particle Description of Light

In 1905 Einstein took this idea further by stating that light can

act as both a wave and a stream of particles Each particle of light

carries a quantum of energy and is called a photon

A photon is a particle of electromagnetic radiation having zero

mass and carrying a quantum of energy

Ephoton = hvEinstein was able to explain the photoelectric effect this way

Different metals bind their electrons differently so v changes

The Hydrogen-Atom Line-Emission Spectrum

When an electric current is passed through a gas sample at low

pressure the potential energy of the gas changes

The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron

There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized

When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle

The Hydrogen-Atom Line-Emission Spectrum

So what does this mean

Well when scientists passed an electric current through a vacuum

tube with a pure gas in it (like H or O) each atom would go through

the steps listed above they would gain energy and then reemit it

in the form of a photon or light This light was then passed through

a prism and the wavelengths (colors) in that element could be seen

Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed

The Hydrogen-Atom Line-Emission Spectrum

So letrsquos use the example of helium A tube of helium has a current of electricity

pass through it and the absorbed energy is then released in the form of light thus

the tube glows That light is then passed through a prism which separates all the

colors (wavelengths) in that light Helium has a particular emission-spectra or set

of lines at specific color spectra

Every element has a signature color spectra

The Hydrogen-Atom Line-Emission Spectrum

But why are there only some colors appearing and

not all of them

Because the electrons in these atoms have specific

fixed energy levels and only give off certain colors

when jumping from level to level Whenever an

excited helium atom falls to its ground state or to a

lower-energy excited state it emits a photon of

radiation The energy of this photon (Ephoton = hv) is

equal to the difference in energy between the atomrsquos initial state and

itrsquos final state Because different atoms have different energy levels

different atoms give off different frequencies (colors) of light

The Bohr Model of the Hydrogen Atom

Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the

atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed

paths or orbits Notice this

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

The Photoelectric Effect

The photoelectric effect is a phenomenon that refers to

the emission of electrons from a metal when light shines

on the metal

Yoursquore most likely thinking who cares

Well herersquos the thing- for any given metal no electrons were

emitted if the lightrsquos frequency were below a certain minimum

Metal

Light

Electrons

The Photoelectric Effect (contrsquod)

So obviously light was known to be a form of energy capable of

knocking electrons loose from metal But (important)

the wave theory of light predicted that any frequency of light could

supply enough energy to eject an electron so the fact that there had

to be a minimum frequency for a given metal made no sense

Something about the assumption of light behavior was wrong

Metal

Light

Electrons

The Particle Description of Light

The German physicist Max Planck came up with the idea that light

is emitted in small packets called quanta

A quantum of energy is the minimum quantity of energy that

can be gained or lost by an atom

Here is the relationship between quantum and frequency of radiation

E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the

physical constant called Planckrsquos Constant h = 6626 x 10-34 Js

Srsquoup

The Particle Description of Light

In 1905 Einstein took this idea further by stating that light can

act as both a wave and a stream of particles Each particle of light

carries a quantum of energy and is called a photon

A photon is a particle of electromagnetic radiation having zero

mass and carrying a quantum of energy

Ephoton = hvEinstein was able to explain the photoelectric effect this way

Different metals bind their electrons differently so v changes

The Hydrogen-Atom Line-Emission Spectrum

When an electric current is passed through a gas sample at low

pressure the potential energy of the gas changes

The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron

There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized

When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle

The Hydrogen-Atom Line-Emission Spectrum

So what does this mean

Well when scientists passed an electric current through a vacuum

tube with a pure gas in it (like H or O) each atom would go through

the steps listed above they would gain energy and then reemit it

in the form of a photon or light This light was then passed through

a prism and the wavelengths (colors) in that element could be seen

Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed

The Hydrogen-Atom Line-Emission Spectrum

So letrsquos use the example of helium A tube of helium has a current of electricity

pass through it and the absorbed energy is then released in the form of light thus

the tube glows That light is then passed through a prism which separates all the

colors (wavelengths) in that light Helium has a particular emission-spectra or set

of lines at specific color spectra

Every element has a signature color spectra

The Hydrogen-Atom Line-Emission Spectrum

But why are there only some colors appearing and

not all of them

Because the electrons in these atoms have specific

fixed energy levels and only give off certain colors

when jumping from level to level Whenever an

excited helium atom falls to its ground state or to a

lower-energy excited state it emits a photon of

radiation The energy of this photon (Ephoton = hv) is

equal to the difference in energy between the atomrsquos initial state and

itrsquos final state Because different atoms have different energy levels

different atoms give off different frequencies (colors) of light

The Bohr Model of the Hydrogen Atom

Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the

atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed

paths or orbits Notice this

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

The Photoelectric Effect (contrsquod)

So obviously light was known to be a form of energy capable of

knocking electrons loose from metal But (important)

the wave theory of light predicted that any frequency of light could

supply enough energy to eject an electron so the fact that there had

to be a minimum frequency for a given metal made no sense

Something about the assumption of light behavior was wrong

Metal

Light

Electrons

The Particle Description of Light

The German physicist Max Planck came up with the idea that light

is emitted in small packets called quanta

A quantum of energy is the minimum quantity of energy that

can be gained or lost by an atom

Here is the relationship between quantum and frequency of radiation

E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the

physical constant called Planckrsquos Constant h = 6626 x 10-34 Js

Srsquoup

The Particle Description of Light

In 1905 Einstein took this idea further by stating that light can

act as both a wave and a stream of particles Each particle of light

carries a quantum of energy and is called a photon

A photon is a particle of electromagnetic radiation having zero

mass and carrying a quantum of energy

Ephoton = hvEinstein was able to explain the photoelectric effect this way

Different metals bind their electrons differently so v changes

The Hydrogen-Atom Line-Emission Spectrum

When an electric current is passed through a gas sample at low

pressure the potential energy of the gas changes

The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron

There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized

When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle

The Hydrogen-Atom Line-Emission Spectrum

So what does this mean

Well when scientists passed an electric current through a vacuum

tube with a pure gas in it (like H or O) each atom would go through

the steps listed above they would gain energy and then reemit it

in the form of a photon or light This light was then passed through

a prism and the wavelengths (colors) in that element could be seen

Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed

The Hydrogen-Atom Line-Emission Spectrum

So letrsquos use the example of helium A tube of helium has a current of electricity

pass through it and the absorbed energy is then released in the form of light thus

the tube glows That light is then passed through a prism which separates all the

colors (wavelengths) in that light Helium has a particular emission-spectra or set

of lines at specific color spectra

Every element has a signature color spectra

The Hydrogen-Atom Line-Emission Spectrum

But why are there only some colors appearing and

not all of them

Because the electrons in these atoms have specific

fixed energy levels and only give off certain colors

when jumping from level to level Whenever an

excited helium atom falls to its ground state or to a

lower-energy excited state it emits a photon of

radiation The energy of this photon (Ephoton = hv) is

equal to the difference in energy between the atomrsquos initial state and

itrsquos final state Because different atoms have different energy levels

different atoms give off different frequencies (colors) of light

The Bohr Model of the Hydrogen Atom

Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the

atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed

paths or orbits Notice this

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

The Particle Description of Light

The German physicist Max Planck came up with the idea that light

is emitted in small packets called quanta

A quantum of energy is the minimum quantity of energy that

can be gained or lost by an atom

Here is the relationship between quantum and frequency of radiation

E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the

physical constant called Planckrsquos Constant h = 6626 x 10-34 Js

Srsquoup

The Particle Description of Light

In 1905 Einstein took this idea further by stating that light can

act as both a wave and a stream of particles Each particle of light

carries a quantum of energy and is called a photon

A photon is a particle of electromagnetic radiation having zero

mass and carrying a quantum of energy

Ephoton = hvEinstein was able to explain the photoelectric effect this way

Different metals bind their electrons differently so v changes

The Hydrogen-Atom Line-Emission Spectrum

When an electric current is passed through a gas sample at low

pressure the potential energy of the gas changes

The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron

There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized

When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle

The Hydrogen-Atom Line-Emission Spectrum

So what does this mean

Well when scientists passed an electric current through a vacuum

tube with a pure gas in it (like H or O) each atom would go through

the steps listed above they would gain energy and then reemit it

in the form of a photon or light This light was then passed through

a prism and the wavelengths (colors) in that element could be seen

Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed

The Hydrogen-Atom Line-Emission Spectrum

So letrsquos use the example of helium A tube of helium has a current of electricity

pass through it and the absorbed energy is then released in the form of light thus

the tube glows That light is then passed through a prism which separates all the

colors (wavelengths) in that light Helium has a particular emission-spectra or set

of lines at specific color spectra

Every element has a signature color spectra

The Hydrogen-Atom Line-Emission Spectrum

But why are there only some colors appearing and

not all of them

Because the electrons in these atoms have specific

fixed energy levels and only give off certain colors

when jumping from level to level Whenever an

excited helium atom falls to its ground state or to a

lower-energy excited state it emits a photon of

radiation The energy of this photon (Ephoton = hv) is

equal to the difference in energy between the atomrsquos initial state and

itrsquos final state Because different atoms have different energy levels

different atoms give off different frequencies (colors) of light

The Bohr Model of the Hydrogen Atom

Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the

atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed

paths or orbits Notice this

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

The Particle Description of Light

In 1905 Einstein took this idea further by stating that light can

act as both a wave and a stream of particles Each particle of light

carries a quantum of energy and is called a photon

A photon is a particle of electromagnetic radiation having zero

mass and carrying a quantum of energy

Ephoton = hvEinstein was able to explain the photoelectric effect this way

Different metals bind their electrons differently so v changes

The Hydrogen-Atom Line-Emission Spectrum

When an electric current is passed through a gas sample at low

pressure the potential energy of the gas changes

The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron

There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized

When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle

The Hydrogen-Atom Line-Emission Spectrum

So what does this mean

Well when scientists passed an electric current through a vacuum

tube with a pure gas in it (like H or O) each atom would go through

the steps listed above they would gain energy and then reemit it

in the form of a photon or light This light was then passed through

a prism and the wavelengths (colors) in that element could be seen

Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed

The Hydrogen-Atom Line-Emission Spectrum

So letrsquos use the example of helium A tube of helium has a current of electricity

pass through it and the absorbed energy is then released in the form of light thus

the tube glows That light is then passed through a prism which separates all the

colors (wavelengths) in that light Helium has a particular emission-spectra or set

of lines at specific color spectra

Every element has a signature color spectra

The Hydrogen-Atom Line-Emission Spectrum

But why are there only some colors appearing and

not all of them

Because the electrons in these atoms have specific

fixed energy levels and only give off certain colors

when jumping from level to level Whenever an

excited helium atom falls to its ground state or to a

lower-energy excited state it emits a photon of

radiation The energy of this photon (Ephoton = hv) is

equal to the difference in energy between the atomrsquos initial state and

itrsquos final state Because different atoms have different energy levels

different atoms give off different frequencies (colors) of light

The Bohr Model of the Hydrogen Atom

Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the

atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed

paths or orbits Notice this

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

The Hydrogen-Atom Line-Emission Spectrum

When an electric current is passed through a gas sample at low

pressure the potential energy of the gas changes

The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron

There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized

When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle

The Hydrogen-Atom Line-Emission Spectrum

So what does this mean

Well when scientists passed an electric current through a vacuum

tube with a pure gas in it (like H or O) each atom would go through

the steps listed above they would gain energy and then reemit it

in the form of a photon or light This light was then passed through

a prism and the wavelengths (colors) in that element could be seen

Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed

The Hydrogen-Atom Line-Emission Spectrum

So letrsquos use the example of helium A tube of helium has a current of electricity

pass through it and the absorbed energy is then released in the form of light thus

the tube glows That light is then passed through a prism which separates all the

colors (wavelengths) in that light Helium has a particular emission-spectra or set

of lines at specific color spectra

Every element has a signature color spectra

The Hydrogen-Atom Line-Emission Spectrum

But why are there only some colors appearing and

not all of them

Because the electrons in these atoms have specific

fixed energy levels and only give off certain colors

when jumping from level to level Whenever an

excited helium atom falls to its ground state or to a

lower-energy excited state it emits a photon of

radiation The energy of this photon (Ephoton = hv) is

equal to the difference in energy between the atomrsquos initial state and

itrsquos final state Because different atoms have different energy levels

different atoms give off different frequencies (colors) of light

The Bohr Model of the Hydrogen Atom

Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the

atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed

paths or orbits Notice this

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

The Hydrogen-Atom Line-Emission Spectrum

So what does this mean

Well when scientists passed an electric current through a vacuum

tube with a pure gas in it (like H or O) each atom would go through

the steps listed above they would gain energy and then reemit it

in the form of a photon or light This light was then passed through

a prism and the wavelengths (colors) in that element could be seen

Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed

The Hydrogen-Atom Line-Emission Spectrum

So letrsquos use the example of helium A tube of helium has a current of electricity

pass through it and the absorbed energy is then released in the form of light thus

the tube glows That light is then passed through a prism which separates all the

colors (wavelengths) in that light Helium has a particular emission-spectra or set

of lines at specific color spectra

Every element has a signature color spectra

The Hydrogen-Atom Line-Emission Spectrum

But why are there only some colors appearing and

not all of them

Because the electrons in these atoms have specific

fixed energy levels and only give off certain colors

when jumping from level to level Whenever an

excited helium atom falls to its ground state or to a

lower-energy excited state it emits a photon of

radiation The energy of this photon (Ephoton = hv) is

equal to the difference in energy between the atomrsquos initial state and

itrsquos final state Because different atoms have different energy levels

different atoms give off different frequencies (colors) of light

The Bohr Model of the Hydrogen Atom

Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the

atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed

paths or orbits Notice this

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

The Hydrogen-Atom Line-Emission Spectrum

So letrsquos use the example of helium A tube of helium has a current of electricity

pass through it and the absorbed energy is then released in the form of light thus

the tube glows That light is then passed through a prism which separates all the

colors (wavelengths) in that light Helium has a particular emission-spectra or set

of lines at specific color spectra

Every element has a signature color spectra

The Hydrogen-Atom Line-Emission Spectrum

But why are there only some colors appearing and

not all of them

Because the electrons in these atoms have specific

fixed energy levels and only give off certain colors

when jumping from level to level Whenever an

excited helium atom falls to its ground state or to a

lower-energy excited state it emits a photon of

radiation The energy of this photon (Ephoton = hv) is

equal to the difference in energy between the atomrsquos initial state and

itrsquos final state Because different atoms have different energy levels

different atoms give off different frequencies (colors) of light

The Bohr Model of the Hydrogen Atom

Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the

atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed

paths or orbits Notice this

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

The Hydrogen-Atom Line-Emission Spectrum

But why are there only some colors appearing and

not all of them

Because the electrons in these atoms have specific

fixed energy levels and only give off certain colors

when jumping from level to level Whenever an

excited helium atom falls to its ground state or to a

lower-energy excited state it emits a photon of

radiation The energy of this photon (Ephoton = hv) is

equal to the difference in energy between the atomrsquos initial state and

itrsquos final state Because different atoms have different energy levels

different atoms give off different frequencies (colors) of light

The Bohr Model of the Hydrogen Atom

Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the

atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed

paths or orbits Notice this

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

The Bohr Model of the Hydrogen Atom

Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the

atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed

paths or orbits Notice this

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)

Conversely when energy is given off by an atom (in the form of a photon)

the electrons move down one or more energy levels

The principal quantum number is

denoted with the letter n and it

indicates the main energy level

occupied by the electron As n

increases the electronrsquos energy and

itrsquos average distance from the nucleus

increases

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in

the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but

never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture

of where it occupies space 90 of the time This is called an orbital

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus

As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These

are known as sublevels

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow

ball where you can find the electron 95 of the time They are

labeled 1-s 2-s and so on to denote how close they are to the

nucleus

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the

electrons is the s-orbital But at the 2nd energy level- after the 2-s

orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped

to represent where the electron can be found 95 of the time

Notice that near the nucleus the area where they are usually found

is very narrow

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular

direction At any one energy level it is possible to have three

absolutely equivalent p orbitals pointing mutually at right angles to

each other These are arbitrarily given the symbols px py and pz

This is simply for convenience - what you might think of as the x

y or z direction changes constantly as the atom tumbles in space

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals

which becomes available for electrons to inhabit at higher energy

levels At the third level there is a set of five d orbitals (with more

complex shapes names) as well as the 3s and 3p orbitals (3px 3py

3pz) At the third level there are a total of nine orbitals altogether

3dxy 3dxz 3dyz

3dx2

-y2 3dz

2

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

N

ldquoRungs of a ladderrdquo

Energy of e- increases as you travel further away from the nucleus

e- can jump from energy levels when they gainlose energy

Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo

Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

The Quantum Mechanical Model (QMM)

bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-

bull All previous models differed bc they were _______

bull This model doesnrsquot define an exact path of an e- rather the QMM does what

ldquoChancerdquo

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud

The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)

N

The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Atomic Orbitals

bull Designate energy levels that e- are in by using principal quantum numbers (n)

bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus

bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level

n =1

n = 2

n = 3

n = 4

uarr en

erg

y uarr

dis

tan

ce fr

om

nucl

eus

darr s

pac

ing

N

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

bull Within each energy level

there are sublevels the of sublevels equals the principal energy level (n)

bull The sublevels are also arranged from lowest to highest energy

bull These sublevels have orbitals within them each orbital can hold a max of 2 e-

Principal energy level (n)

of sublevels in that level

n = 1 1 sublevel

n = 2 2 sublevels

n = 3 3 sublevels

Sublevels (lowest highest energy)

of orbitals within each sublevel

1st = s 1 orbital

2nd = p 3 orbitals

3rd = d 5 orbitals

4th = f 7 orbitals

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Do Now

1 Discuss points you have learned about the PT

a What does it tell us

b How can we use it to talk about an element and its characteristics

c How and why do we use the Aufbau Diagram

Homework

1 Finish electron configuration sheet QUIZ

2 Bring all lab materials tomorrowhellip

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Basicallyhellip

Principal energy level (n) Energy sublevels Orbitals in sublevels

n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7

(2 e- 6 e- 10 e- 14 e-)

QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY

s orbital

p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)

Fig 134 5 in book

Low to High

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Another representation of the atomic orbitalshellip

Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node

bull Again the and types of atomic orbitals depends on what

bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s

Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

bull The 2nd energy level (n = 2) has 2 sublevels s and p

N PP

P

P

P

Coming you

Going away from you

3) Spaces represent what

P

S2) How many total orbitals are there What are the max of e- that can be held in n= 2

1) P orbitals stick out further therefore they have gt ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

bull As mentioned the principal quantum always

equals the of sublevels in that energy levelbull The max of e- that can occupy a principal

energy level is given by the formulahellip

2n2

What is the max of e- in the 6th principal energy level Sublevels

Still confused Review p 366 for max e- per energy level

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Homework

bull Electron configuration worksheet (work on wkst)

bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do

you create it What does it tell about filling orbitals (use book to help you out)

2 What is the total of e- in n = 9 n = 53 What does the quantum tell you

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Electron Configurations

bull Natural phenomena to work towards stability ndash lowest possible energy

WHY

High energy systems are very unstable

Atom works to attain the most stable e- configuration possible

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

bull There are 3 rules that help you to determine this

1 Aufbau Principle

2 Pauli Exclusion Principle

3 Hundrsquos Rule

1 s 2 s 2 p

Long form vs Short form

Electron ConfigurationsAufbau Diagrams

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital

Aufbau Diagram

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr

3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Some practice

____

5s ___ ___ ___

4p

___ ___ ___

4d

___ ___

Element

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Electron Configuration

This is the order which electrons will fill their energy levels

You MUST learn this

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Electron Configuration (contrsquod)

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or

tests

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Show the electron configuration of the following elements

1) Fe 1s22s22p63s23p64s23d6

2) Ga 1s22s22p63s23p64s23d104p1

3) Ar 1s22s22p63s23p6

4) Sr 1s22s22p63s23p64s23d104p65s2

5) Mg 1s22s22p63s2

6) Ru 1s22s22p63s23p64s23d104p65s24d6

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Homework

bull Have worksheets out to quickly review questions (131 and 2)

bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help

bull Do Now1 Starting form n = 1 (to n = 4) list the order that

electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-

configuration discussed previouslyhellip

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Take Quiz ndash 7 minutes

Do Now1 What is the difference between an atom and its

ion2 What is a node3 Why is it unnatural for systemsatoms to be at

high energy How do atoms fix this problem

Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

Physics and the QMM

bull QMM developed through study of light

bull Through its study found light was energy that contained _____ and moved by ____

bull According to the ldquowave modelrdquo light consists of electromagnetic waves

bull Includeshellip

All waves travel in a vacuum at

30 x 10^10 cms (or 30 x 10^8

ms) =

Irsquom smarter

than he is Howrsquod he measure

that

Anatomy of a Wavelength

origin

amplitude

Λ = ldquolambdardquo

Frequency (ν) = ldquonurdquo

= of wave cycles that that pass through a point in a given time

= Hertz (Hz) or s^-1

Wavelength and frequency are inversely related Which leads us tohellip

Take 3 minutes only for quiz ndash hand in when finished

Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light

Which portion makes up the smallest portion of this ldquospectrumrdquo

3 How are wavelength and frequency related Do they relate to anything else

4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14

create a ldquomaprdquo of how to interpret the periodic trends

ν ldquotimesrdquo λ = speed of light

bull Every time

bull Light bends through prisms to create thehellip

Electromagnetic Spectrum = relative size

Every element bends light in a specific wayhellip

Open book and complete sample 132 and practice problem 11

Another idea that came about through the study of lighthellip

bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo

bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos

constant bull E = bull Problem 13 on page 379

• Chapter 4 Electrons in Atoms
• Chapter 4 Arrangement of Electrons in Atoms
• If + and ndash charges attract why donrsquot e- collapse into the nucleus
• Slide 5
• Slide 6
• Slide 7
• Slide 8
• Slide 9
• Slide 10
• Slide 11
• Slide 12
• Slide 13
• Slide 14
• Slide 15
• Slide 16
• Slide 17
• Slide 18
• Slide 19
• Slide 20
• Slide 21
• Slide 22
• Slide 23
• Slide 24
• Slide 25
• Slide 26
• ldquoRungs of a ladderrdquo
• The Quantum Mechanical Model (QMM)
• Slide 29
• Atomic Orbitals
• Slide 31
• Do Now
• Basicallyhellip
• Slide 34
• Another representation of the atomic orbitalshellip
• Slide 36
• Slide 37
• Slide 38
• Slide 39
• Homework
• Electron Configurations
• Slide 42
• Slide 43
• Slide 44
• Slide 45
• Slide 46
• Slide 47
• Slide 48
• Slide 49
• Slide 50
• Slide 51
• Physics and the QMM
• Slide 53
• Anatomy of a Wavelength
• Take 3 minutes only for quiz ndash hand in when finished
• ν ldquotimesrdquo λ = speed of light
• Every element bends light in a specific wayhellip
• Another idea that came about through the study of lighthellip

Anatomy of a Wavelength

origin

amplitude

Λ = ldquolambdardquo

Frequency (ν) = ldquonurdquo

= of wave cycles that that pass through a point in a given time

= Hertz (Hz) or s^-1

Wavelength and frequency are inversely related Which leads us tohellip

Take 3 minutes only for quiz ndash hand in when finished

Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light

Which portion makes up the smallest portion of this ldquospectrumrdquo

3 How are wavelength and frequency related Do they relate to anything else

4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14

create a ldquomaprdquo of how to interpret the periodic trends

ν ldquotimesrdquo λ = speed of light

bull Every time

bull Light bends through prisms to create thehellip

Electromagnetic Spectrum = relative size

Every element bends light in a specific wayhellip

Open book and complete sample 132 and practice problem 11

Another idea that came about through the study of lighthellip

bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo

bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos

constant bull E = bull Problem 13 on page 379

• Chapter 4 Electrons in Atoms
• Chapter 4 Arrangement of Electrons in Atoms
• If + and ndash charges attract why donrsquot e- collapse into the nucleus
• Slide 5
• Slide 6
• Slide 7
• Slide 8
• Slide 9
• Slide 10
• Slide 11
• Slide 12
• Slide 13
• Slide 14
• Slide 15
• Slide 16
• Slide 17
• Slide 18
• Slide 19
• Slide 20
• Slide 21
• Slide 22
• Slide 23
• Slide 24
• Slide 25
• Slide 26
• ldquoRungs of a ladderrdquo
• The Quantum Mechanical Model (QMM)
• Slide 29
• Atomic Orbitals
• Slide 31
• Do Now
• Basicallyhellip
• Slide 34
• Another representation of the atomic orbitalshellip
• Slide 36
• Slide 37
• Slide 38
• Slide 39
• Homework
• Electron Configurations
• Slide 42
• Slide 43
• Slide 44
• Slide 45
• Slide 46
• Slide 47
• Slide 48
• Slide 49
• Slide 50
• Slide 51
• Physics and the QMM
• Slide 53
• Anatomy of a Wavelength
• Take 3 minutes only for quiz ndash hand in when finished
• ν ldquotimesrdquo λ = speed of light
• Every element bends light in a specific wayhellip
• Another idea that came about through the study of lighthellip

Take 3 minutes only for quiz ndash hand in when finished

Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light

Which portion makes up the smallest portion of this ldquospectrumrdquo

3 How are wavelength and frequency related Do they relate to anything else

4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14

create a ldquomaprdquo of how to interpret the periodic trends

ν ldquotimesrdquo λ = speed of light

bull Every time

bull Light bends through prisms to create thehellip

Electromagnetic Spectrum = relative size

Every element bends light in a specific wayhellip

Open book and complete sample 132 and practice problem 11

Another idea that came about through the study of lighthellip

bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo

bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos

constant bull E = bull Problem 13 on page 379

• Chapter 4 Electrons in Atoms
• Chapter 4 Arrangement of Electrons in Atoms
• If + and ndash charges attract why donrsquot e- collapse into the nucleus
• Slide 5
• Slide 6
• Slide 7
• Slide 8
• Slide 9
• Slide 10
• Slide 11
• Slide 12
• Slide 13
• Slide 14
• Slide 15
• Slide 16
• Slide 17
• Slide 18
• Slide 19
• Slide 20
• Slide 21
• Slide 22
• Slide 23
• Slide 24
• Slide 25
• Slide 26
• ldquoRungs of a ladderrdquo
• The Quantum Mechanical Model (QMM)
• Slide 29
• Atomic Orbitals
• Slide 31
• Do Now
• Basicallyhellip
• Slide 34
• Another representation of the atomic orbitalshellip
• Slide 36
• Slide 37
• Slide 38
• Slide 39
• Homework
• Electron Configurations
• Slide 42
• Slide 43
• Slide 44
• Slide 45
• Slide 46
• Slide 47
• Slide 48
• Slide 49
• Slide 50
• Slide 51
• Physics and the QMM
• Slide 53
• Anatomy of a Wavelength
• Take 3 minutes only for quiz ndash hand in when finished
• ν ldquotimesrdquo λ = speed of light
• Every element bends light in a specific wayhellip
• Another idea that came about through the study of lighthellip

ν ldquotimesrdquo λ = speed of light

bull Every time

bull Light bends through prisms to create thehellip

Electromagnetic Spectrum = relative size

Every element bends light in a specific wayhellip

Open book and complete sample 132 and practice problem 11

Another idea that came about through the study of lighthellip

bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo

bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos

constant bull E = bull Problem 13 on page 379

• Chapter 4 Electrons in Atoms
• Chapter 4 Arrangement of Electrons in Atoms
• If + and ndash charges attract why donrsquot e- collapse into the nucleus
• Slide 5
• Slide 6
• Slide 7
• Slide 8
• Slide 9
• Slide 10
• Slide 11
• Slide 12
• Slide 13
• Slide 14
• Slide 15
• Slide 16
• Slide 17
• Slide 18
• Slide 19
• Slide 20
• Slide 21
• Slide 22
• Slide 23
• Slide 24
• Slide 25
• Slide 26
• ldquoRungs of a ladderrdquo
• The Quantum Mechanical Model (QMM)
• Slide 29
• Atomic Orbitals
• Slide 31
• Do Now
• Basicallyhellip
• Slide 34
• Another representation of the atomic orbitalshellip
• Slide 36
• Slide 37
• Slide 38
• Slide 39
• Homework
• Electron Configurations
• Slide 42
• Slide 43
• Slide 44
• Slide 45
• Slide 46
• Slide 47
• Slide 48
• Slide 49
• Slide 50
• Slide 51
• Physics and the QMM
• Slide 53
• Anatomy of a Wavelength
• Take 3 minutes only for quiz ndash hand in when finished
• ν ldquotimesrdquo λ = speed of light
• Every element bends light in a specific wayhellip
• Another idea that came about through the study of lighthellip

Every element bends light in a specific wayhellip

Open book and complete sample 132 and practice problem 11

Another idea that came about through the study of lighthellip

bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo

bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos

constant bull E = bull Problem 13 on page 379

• Chapter 4 Electrons in Atoms
• Chapter 4 Arrangement of Electrons in Atoms
• If + and ndash charges attract why donrsquot e- collapse into the nucleus
• Slide 5
• Slide 6
• Slide 7
• Slide 8
• Slide 9
• Slide 10
• Slide 11
• Slide 12
• Slide 13
• Slide 14
• Slide 15
• Slide 16
• Slide 17
• Slide 18
• Slide 19
• Slide 20
• Slide 21
• Slide 22
• Slide 23
• Slide 24
• Slide 25
• Slide 26
• ldquoRungs of a ladderrdquo
• The Quantum Mechanical Model (QMM)
• Slide 29
• Atomic Orbitals
• Slide 31
• Do Now
• Basicallyhellip
• Slide 34
• Another representation of the atomic orbitalshellip
• Slide 36
• Slide 37
• Slide 38
• Slide 39
• Homework
• Electron Configurations
• Slide 42
• Slide 43
• Slide 44
• Slide 45
• Slide 46
• Slide 47
• Slide 48
• Slide 49
• Slide 50
• Slide 51
• Physics and the QMM
• Slide 53
• Anatomy of a Wavelength
• Take 3 minutes only for quiz ndash hand in when finished
• ν ldquotimesrdquo λ = speed of light
• Every element bends light in a specific wayhellip
• Another idea that came about through the study of lighthellip

Another idea that came about through the study of lighthellip

bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo

bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos

constant bull E = bull Problem 13 on page 379

• Chapter 4 Electrons in Atoms
• Chapter 4 Arrangement of Electrons in Atoms
• If + and ndash charges attract why donrsquot e- collapse into the nucleus
• Slide 5
• Slide 6
• Slide 7
• Slide 8
• Slide 9
• Slide 10
• Slide 11
• Slide 12
• Slide 13
• Slide 14
• Slide 15
• Slide 16
• Slide 17
• Slide 18
• Slide 19
• Slide 20
• Slide 21
• Slide 22
• Slide 23
• Slide 24
• Slide 25
• Slide 26
• ldquoRungs of a ladderrdquo
• The Quantum Mechanical Model (QMM)
• Slide 29
• Atomic Orbitals
• Slide 31
• Do Now
• Basicallyhellip
• Slide 34
• Another representation of the atomic orbitalshellip
• Slide 36
• Slide 37
• Slide 38
• Slide 39
• Homework
• Electron Configurations
• Slide 42
• Slide 43
• Slide 44
• Slide 45
• Slide 46
• Slide 47
• Slide 48
• Slide 49
• Slide 50
• Slide 51
• Physics and the QMM
• Slide 53
• Anatomy of a Wavelength
• Take 3 minutes only for quiz ndash hand in when finished
• ν ldquotimesrdquo λ = speed of light
• Every element bends light in a specific wayhellip
• Another idea that came about through the study of lighthellip