Cool video clip! Housekeeping Intro to Electromagnetic Waves and Electrons

› Netbook research activity› Mini presentations

Homework: None for tonight

https://www.youtube.com/watch?v=dmuyLIrSjxI

1. Choose a topic

2. Group up with fellow topic choosers

3. Research your topic

4. Prepare a brief 3 minute presentation about your topic!

1. Fireworks2. Electron Microscope3. Neon Lights4. Lasers5. Microwave Ovens6. Tanning Beds

Finish the presentations from yesterday

Quantum Leap Nova

HW: None, be safe this weekend!!

Review Unit 3 Test› Retakes› The End of the Qurater

Notes on Waves› Structure and Types

Practice Problems with Wave Equation

Spectra Lab

Homework: Complete Practice Problems with Wave Equation

Review Unit 3 Test› Retakes› The End of the Quarter

Notes on Waves› Structure and Types

Practice Problems with Wave Equation

Homework: Complete Practice Problems with Wave Equation

MC Questions:› 10› 5

Retake Policy› End of the Quarter is Thursday› Retakes for any unit taken by

Wednesday!!

What is the electromagnetic spectrum?

How can I calculate the different variables in the wave/energy equation?

https://www.youtube.com/watch?v=uJ3ea9fa6CA

How to use the spectroscope.

Conclusions for the lab.› This conclusion is very important.› Use the format that we have been using all

year› Explain the trends in your graph primarily!!

Check-In HW› Warm-Up

Notes on Bohr Model › His experiment› Electron radiation

Flame Demo

Homework: None

Check-In HW› Warm-Up

Finish notes on Wave and Energy Equations Notes on Bohr Model

› His experiment› Electron radiation

Flame Demo

Spectra Lab (at least start it) Homework: Complete Conclusion and

Analysis of Spectra Lab

Random Follow-up Question of the Day:

How do we know what the Sun is made of?

Wave Equation and Energy Warm-Up

Spectra Lab› Data during 8th Period› Analysis during 9th Period

Homework: Complete Conclusion and Analysis of Spectra Lab

Wave Equation Problems and Energy

Spectra Lab Analysis Work time Calculations and Graphs

Homework: Complete Conclusion and Analysis of Spectra Lab

You need to show all of your work for one line on each of the Samples› The other lines you need to just show your

answers You will be graphing 3 graphs.

› Each are described on the back of the lab› Each graph needs a best-fit line

Answer the analysis questions as a basis for your conclusion.

You will need a complete conclusion describing the three relationships in the three graphs.

Question: From lowest energy to highest energy, what are the different types of radiation that make up the EM Spectrum?

Question: What does the EM Spectrum have to do with atoms????

Bohr realized that atoms could be made to emit light

His explanation was that electrons are assigned to energy levels outside the nucleus

The electrons within these energy levels orbit at certain distinct distances from the nucleus

In order to change its orbital pattern the electron must lose or gain energy. This loss happens in the form of emitted packets of light energy (“Quanta”).

Instead of orbits (as Bohr thought) electrons move within orbitals, which are basically areas around the nucleus where the electrons will most likely be found. The electrons DO NOT stay in set paths within the orbitals!!!

Notice: The p orbitals have the same shape but different orientations

Notice: The d orbitals have the same shape but different orientations

Room 162Science HallwayCrystal Lake Central H.S.45 W. Franklin DriveCrystal Lake, IL 60014

1s2 2s2 2p6

Neon: 1s2 2s2 2p6

Li 1s22s1

C 1s22s22p2

Sc 1s22s22p63s23p64s23d1

On your whiteboards:› Kr› I

Krypton› 1s22s22p63s23p64s23d104p6

Iodine› 1s22s22p63s23p64s23d104p65s24d105p5

[Kr]

Iodine: [Kr]5s24d105p5

Write the FULL electron configuration of:› Sulfur› 1s22s22p63s23p4

Write the shortened E.C. of:› Bromine› [Ar]4s23d104p5

1s2

Principle Quantum #-or-

Energy Level Shape of Orbital-or-

Sublevel

# of electrons in the subshell

• Rows on the periodic table

1s2

Principle Quantum #-or-

Energy Level Shape of Orbital-or-

Sublevel

# of electrons in the subshell

S p d

• Where electrons exist…probably• Each orbital has room for up to…

• 2 electrons

s sublevel = 1 orbitalp sublevel = 3 orbitalsd sublevel = 5 orbitalsf sublevel = 7 orbitals

Each orbital can hold 2 electrons!!!

So how many electrons can fit in each sublevel?

Neon: 1s2 2s2 2p6

Write the FULL electron configuration of:› Sulfur› 1s22s22p63s23p4

Krypton› 1s22s22p63s23p64s23d104p6

Iodine› 1s22s22p63s23p64s23d104p65s24d105p5

[Kr]

Iodine: [Kr]5s24d105p5

Write the FULL electron configuration of:› Phosphorus› 1s22s22p63s23p3

Write the shortened E.C. of:› Bromine› [Ar]4s23d104p5

What is the significance of the electron configuration? (Quantum Numbers)

1s2

Principle Quantum #-or-

Energy Level Shape of Orbital-or-

Sublevel

# of electrons in the subshell

• Rows on the periodic table• Tells us how far from the nucleus each electron is

• The larger the energy level the further the electron is from the nucleus

• Which electron is furthest from the nucleus?• 1s• 2p• 3d• 4s

1s2

Principle Quantum #-or-

Energy Level Shape of Orbital-or-

Sublevel

# of electrons in the subshell

S p d

• Orbitals are the place where electrons are housed in an atom• Probably…

• Each orbital only has room for…• 2 electrons

s sublevel = 1 orbitalp sublevel = 3 orbitalsd sublevel = 5 orbitalsf sublevel = 7 orbitals

Each orbital can hold 2 electrons!!!

So how many electrons can fit in each sublevel?

s sublevel = 2 electronsp sublevel = 6 electronsd sublevel = 10 electronsf sublevel = 14 electrons

Remember: Each orbital can hold 2 electrons!!!

Sodium: 1s2 2s2 2p6 3s1

Energy Level # of Sublevels

Total # of Orbitals

Total # of Electrons

1 1 1 2

2 2 4 8

3 3 9 18

4 4 16 32

5 4 16 32

Sublevel # of Orbitals # of Electrons

per Orbital

Total # of Electrons in

Sublevel

s 1 2 2

p 3 2 6

d 5 2 10

f 7 2 14

Energy Level # of Sublevels

Total # of Orbitals

Total # of Electrons

1 1 1 2

2 2 4 8

3 3 9 18

4 4 16 32

5 5 25 50

Each group gets 1 marker and 1 white board

You have 10 mins to answers these questions.

Please do not write on the paper.

Make Sure Mr. Gustin checks your answers before you erase them.

s sublevel = 1 orbitalp sublevel = 3 orbitalsd sublevel = 5 orbitalsf sublevel = 7 orbitals

Can we think of a simple way to draw orbitals?

Electrons are drawn as arrows, either up or down.

Aufbau Principle:› Each orbital in a subshell must have one

electron in it before a second electron can be added.

Hund’s Rule:› Electrons must be drawn going the same

direction until the subshell is full. Pauli Exclusion Principle:

› Each orbital can only contain one up and one down arrow.

1s22s22p63s23p5

Draw the Orbital Diagram for Chlorine.

Same rules as before!!

In your group draw the orbital diagrams for the following:› H› O› Si› Br› Now use the shorthand and Draw Br

Valence electrons are the electrons that exist in the outermost energy level in an electron configuration.

These are the electrons that “do” chemistry

How many valence electrons does _____ have?› Beryllium (Be)› Oxygen (O)

Li› 1s22s1

Na› 1s22s22p63s1

K› 1s22s22p63s23p64s1

F› 1s22s22p5

Cl› 1s22s22p63s23p5

Br› 1s22s22p63s23p64s23d104p5

Depicts the valence electrons of different atoms.

Another way to model the electron configuration of atoms.

Represent paired and unpaired electrons.

Draw the Valence Dot Structure for:› H› O› Si› Br› Cl› F

Write the electron configuration of Lithium. 1s22s1

Write the electron configuration of Fluorine. 1s22s22p5

Write the electron configuration of the Fluoride Ion (F-)

1s22s22p6

Charged atoms that contain a different number of electrons than protons.

For each + charge an electron is subtracted. For each – charge an electron is added.

Calcium Ion (Ca2+). 1s22s22p63s23p6

Bromide Ion (Br-). 1s22s22p63s23p64s23d104p6