The Periodic TableThe Periodic Table

The Periodic TableThe Periodic Table• Understand the rationale behind the periodic table; view the table as an ordered database of element properties. • Explain how the periodic table reflects the quantum mechanical structure of the atom. • Explain and use periodic trends in: atomic radius ionic radius ionization energy • Explain the connection between ionization energy and metallic character.

Quick ReviewQuick Review

Quantum Numbers (4)Quantum Numbers (4) Represent or describe the space orbital in Represent or describe the space orbital in

which the ewhich the e-- moves or may be found. moves or may be found.

1.1. DistanceDistance from nucleus from nucleus

2.2. ShapeShape of the orbital of the orbital

3.3. PositionPosition or locationor location with respect to the 3 axes with respect to the 3 axes in spacein space

4.4. Direction of spinDirection of spin of the e of the e-- in the orbital in the orbital

Quantum NumbersQuantum Numbers11stst Quantum Number: Quantum Number:

Principle Quantum # (n) – avg. distance of ePrinciple Quantum # (n) – avg. distance of e--

from nucleus. Positive whole # 1,2,3, etc. from nucleus. Positive whole # 1,2,3, etc.

The main The main energy levelenergy level designation equal to designation equal to

K,L,M, etc. shellsK,L,M, etc. shells

Quantum # 2Quantum # 2

Orbital Quantum # (l) – Orbital Quantum # (l) – shapeshape of orbital in which of orbital in which the ethe e-- moves. # of possible shapes = the moves. # of possible shapes = the value of the principal quantum #. value of the principal quantum #.

11stst energy level = 1 shape energy level = 1 shape

22ndnd energy level = 2 shapes energy level = 2 shapes

33rdrd energy level = 3 shapes, etc energy level = 3 shapes, etc

Letter designations for shapes are s,p,d,f. These Letter designations for shapes are s,p,d,f. These are also sublevels or sub orbitalsare also sublevels or sub orbitals

S – Sphere, P – 8 ( 3 - one on each axis x,y,z)S – Sphere, P – 8 ( 3 - one on each axis x,y,z)

33rdrd Quantum # - Magnetic (m) – indicates Quantum # - Magnetic (m) – indicates the position about the three axes in the position about the three axes in space of the orbital.space of the orbital.

1 position for s orbital1 position for s orbital

3 positions for p orbitals (p3 positions for p orbitals (pxxppyyppzz))

5 positions for d orbitals5 positions for d orbitals

7 positions for f orbitals7 positions for f orbitals

44thth Quantum Number Quantum Number

Spin (s) – right hand or left hand, clockwise Spin (s) – right hand or left hand, clockwise or counter-clockwiseor counter-clockwise

Therefore 2 eTherefore 2 e-- can occupy any space can occupy any space designated by the first 3 quantum #’s but designated by the first 3 quantum #’s but they will have opposite spins.they will have opposite spins.

No 2 eNo 2 e-- have the same quantum #’s have the same quantum #’s

No 2 eNo 2 e-- have the same energy have the same energy

In 1859 Mendeleyev devised the periodic table of In 1859 Mendeleyev devised the periodic table of elements.elements.

“ “Properties of the elements are in periodic Properties of the elements are in periodic dependence on their atomic weights.”dependence on their atomic weights.”

Ramsay discovered the noble gases: Ne, Ar, Kr, Xe. Ramsay discovered the noble gases: Ne, Ar, Kr, Xe. Noble or inert: will not react with others.Noble or inert: will not react with others.

Periodic Law: Periodic Law: The physical & chemical properties of The physical & chemical properties of the elements are periodic functions of their atomic #’s.the elements are periodic functions of their atomic #’s.

1. Period/Series – horizontal rows1. Period/Series – horizontal rows

2. Group/Family – vertical columns2. Group/Family – vertical columns

a. elements with similar properties have a similar a. elements with similar properties have a similar

arrangement of outer-shell earrangement of outer-shell e-- (same group in the (same group in the

periodic table) or valence eperiodic table) or valence e--..

Most active metal – lower leftMost active metal – lower left Most active non-metal – upper rightMost active non-metal – upper right Transition elements are metallic & have either 1 Transition elements are metallic & have either 1

or 2 eor 2 e-- in their outer shell (generally) in their outer shell (generally) Rare Earth elements are basically identical. Rare Earth elements are basically identical.

The outer shell contains 2 eThe outer shell contains 2 e--

Zigzag line: separates metals from the non-Zigzag line: separates metals from the non-metals. Those touching are metalloids, have metals. Those touching are metalloids, have both or either characteristics of metals and non-both or either characteristics of metals and non-metals.metals.

Atomic RadiiAtomic Radii

The radius of an atom The radius of an atom does not increase does not increase with atomic #.with atomic #.

1. Atomic radius increases with atomic # 1. Atomic radius increases with atomic #

in a particular group/family. (increased in a particular group/family. (increased

shells)shells)

2. From group 1 to 18 (I to VIII) in a 2. From group 1 to 18 (I to VIII) in a

period, there is a general decrease in period, there is a general decrease in

the atom radii. (increase in pthe atom radii. (increase in p++, increase , increase

attraction of the eattraction of the e--))

Atomic radius Atomic radius

Ionization EnergyIonization Energy Energy required to remove an eEnergy required to remove an e-- from an from an

atom.atom. normally, ionization removes valence normally, ionization removes valence

electrons first electrons first valence electrons are farthest from valence electrons are farthest from

nucleus on average, so they feel the least nucleus on average, so they feel the least attraction for the nucleus and are easiest attraction for the nucleus and are easiest to remove to remove

end of valence electrons is marked by a end of valence electrons is marked by a big jump in ionization energies big jump in ionization energies

AAo o (nuetral) + Energy = A (nuetral) + Energy = A + + (positive ion) + e(positive ion) + e-- kJ – kilo joules or kcal – kilo calories may be kJ – kilo joules or kcal – kilo calories may be

the energy unit of measure used per mole of the energy unit of measure used per mole of substance.substance.

Ex: It takes 124 kcal to remove the outer shell Ex: It takes 124 kcal to remove the outer shell ee-- from 6.02 X 10 from 6.02 X 102323 atoms of Li. atoms of Li.

Mole: amount of the substance equal to aMole: amount of the substance equal to a

Avogadro Number: 6.02 X 10Avogadro Number: 6.02 X 102323atoms atoms Mole: may also equal that substances atomic Mole: may also equal that substances atomic

weight in grams.weight in grams.

Quick Check for understandingQuick Check for understanding normally, ionization removes valence electrons normally, ionization removes valence electrons

first first valence electrons are farthest from nucleus on valence electrons are farthest from nucleus on

average, so they feel the least attraction for the average, so they feel the least attraction for the nucleus and are easiest to remove nucleus and are easiest to remove

end of valence electrons is marked by a big end of valence electrons is marked by a big jump in ionization energies jump in ionization energies

Low ionization energy is characteristic of a Low ionization energy is characteristic of a metal. metal.

High ionization energy is characteristic of a non-High ionization energy is characteristic of a non-metal metal

Intermediate ionization energy for metalloidsIntermediate ionization energy for metalloids

Within a group/family ionization energy generally Within a group/family ionization energy generally decreases with increasing atomic #decreases with increasing atomic #

Ionization energy does not vary uniformly within a Ionization energy does not vary uniformly within a period/series as a result of filled or unfilled period/series as a result of filled or unfilled sublevels.sublevels.

To remove successive eTo remove successive e-- from the same atom from the same atom becomes progressively more difficult due to the becomes progressively more difficult due to the closeness of the remaining ecloseness of the remaining e-- to the nucleus. to the nucleus.

Na + Energy = NaNa + Energy = Na++ + + e-e- +496 kJ 1+496 kJ 1stst ionization energy ionization energy Na + Energy = NaNa + Energy = Na++++ + 2 + 2e-e- +4560 kJ 2+4560 kJ 2ndnd ionization energy ionization energy

Electron AffinityElectron Affinity

Energy released when an eEnergy released when an e-- is added to a is added to a neutral atom.neutral atom.

A + eA + e-- = A = A-- + energy (kcal) Note: + energy (kcal) Note: EE on on Product side of the equationProduct side of the equation

Low electron affinity – weak bondingLow electron affinity – weak bonding High electron affinity – strong bondingHigh electron affinity – strong bonding Electron affinities decrease in Electron affinities decrease in

groups/families due to additional shellsgroups/families due to additional shells Electronegativity: ability to attract eElectronegativity: ability to attract e--

Additional TermsAdditional Terms

Ion – an atom which has become charged Ion – an atom which has become charged by either gaining or losing electrons.by either gaining or losing electrons.

Anion – negatively charged atom, Anion – negatively charged atom, characteristic of the non-metals.characteristic of the non-metals.

Cation – positively charged atom, Cation – positively charged atom, characteristic of the metals.characteristic of the metals.

Group or Family Names:

1 Alkali metals, 2 Alkaline earth metals, 3-12 transition metals, 13 Boron-Aluminum,

14 Carbon, 15 Nitrogen, 16 Chalcogen, 17 Halogens (salt formers), 18 Noble (Inert) or Group O

Rare Earth Elements

Ionic Bonding

Covalent Bonding

Electron donor, lender

Electron acceptor, borrower

CHEMICAL FAMILIES:ALKALI METALS: GROUP IA (1)All alkali metals react with H2O to form an alkaline (Basic)

Solution. ** Hydrogen is NOT considered an alkaline metal in this case.ALKALINE EARTH METALS: GROUP IIA (2)All alkali earth metals also react with H2O to form a basic solution.HALOGENS: GROUP VIIA (17)Salt FormersNOBLE GASES: GROUP VIIIA (18)Noble Gases have all their orbitals Filled.

The other groups are identified by the element at the top of the column. Example, GROUP IVA is the called the Carbon Family (or Group).

Lanthanide Series: Fourteen elements beginning with lanthanum in which the highest energy electrons to be in the 4f sublevel.Actinide Series: Fourteen elements beginning with actinium in which the highest energy electrons to be in the 5f sublevel.

Rare Earth Elements – Inner Transition Elements