1. Periodic Law - The properties of the elements are periodic functions
electron has Wavefunction quantum electron
wavelike (Shrödinger Equation) numbers configuration
behavior
predicted properties (periodicity)
Periodic Law - The properties of the elements are periodic functions
of their atomic numbers (# of protons)
Atomic Radii Ionization Energy
Electron Affinity Electronegativity

2. Cl Cl
Atomic Radii
Effective Nuclear Charge - Nuclear charge experienced
by the outer shell electrons 2r
The inner shell electrons shield the outer shell electrons from the
full effect of the nuclear charge.
Increase
Increase
Increase

3. Ionic Radii
Neutral Atom  Anion  size
Neutral Atom  Cation  size

4. Isoelectronic - species that have the same number of electrons
The species with the most protons will have the smallest radius

5. First Ionization Energy - The minimum amount of energy required
to remove the most loosely bound electron from an isolated gaseous
atom to form an ion with a 1+ charge
X(g) + 1st Ionization Energy  X+(g) + e-

6. First Ionization
Energy Trend
Increase
Increase
Increase

7. Electron Affinity - the amount of energy absorbed when an
electron is added to an isolated gaseous atom to form an ion with a 1-
charge.
X(g) + e-(g) X-(g)
Increases = less negative or
more positive
Increase
Increase
Increase
Book pg 247

8. Electronegativity - measure of the relative tendency of an atom
to attract electrons to itself when it is chemically combined with
another atom. (qualitative)
Increase
Increase
Increase

9. Reactions of Hydrogen Displacement Reactions:
3Fe(s) + 4H2O  Fe3O4(s) + 4H2(g)
Zn(s) + 2HCl(aq)  ZnCl2(s) + 4H2(g)
Electrolysis:
2H 2O(g) 2H2(g) + O2(g)
Combustion:
2H2(g) + O2(g) 2H 2O(g) + Energy
Electricity
Spark or heat

10. Preparation & Rxn’s of Hydrides (Binary H containing compound)
Ionic hydrides - MH M=group IA
MH2 M=heavier group IIA (Ca, Sr, Ba)
2Li(l) + H2(g)  2LiH(s)
Ca(l) + H2(g)  CaH2(s)
LiH(s) + H2O  Li(OH)(s) + H2(g)
CaH2(s) + 2H2O  Ca(OH)2(s) + 2H2(g)
Molecular hydrides -
X2 + H2(g) HX(g) X=halogen (F,Cl,Br,I) (acidic)
Combination:
Ionic hydrides
are basic in water
Combination:
H2O, H2S, H2Se, H2Te
Figure 6-4 (pg. 253)

11. Oxygen Oxides - Binary compounds that contain oxygen
Normal oxides - (O2-) ox # O = -2
Peroxides - (O22-) ox # O = -1
Superoxides - (O2-) ox # O = -(1/2)
Rxn of oxygen with metals:
4Li(s) + O2(g) (excess)  2Li2O(s)
2Na(s) + O2(g) (excess) Na2O2(g)
M(s) + O2(g) (excess) MO2(s) M=K, Rb & Cs
M(s) + O2(g) (excess)  MO(s) M=Be, Mg, Ca, Sr
Ba(s) + O2(g) (excess) BaO2(s)
Basicity
Increases
pg. 257

12. Rxn of oxygen with metals (cont.):
2Fe(s) + O2(g) FeO(s) iron (II) oxide (ferrous oxide)
6FeO(s) + O2(g) Fe3O4(s) magnetic iron oxide (mixed oxide)
4Fe3O4(s) + O2(g) Fe2O3(s) iron (III) oxide (feric oxide)
Rxn of oxygen with nonmetals:
2C(s) (excess) + O2(g) 2CO(s) ox # C in CO = +2
C(s) + O2(g) (excess) CO2(g) ox # C in CO2 = +4

13. Rxn of non-metal oxides (acid anhydrides or acidic oxides)
CO2(g) + H2O 2H2CO3(aq)
Acidity Increases +4 +4
Ternary Acid
non-metal oxides combine with water to form ternary acids without a
change in oxidation state of the non-metal
Rxn of metal oxides with non-metal oxides:
CaO(s) + SO3(l) CaSO4(s)
metal oxides combine with non-metal oxides to produce salts without
a change in oxidation states.

14. Combustion Reactions - combination reaction with oxygen.
Combustion of fossil fuels:
2C8H18(l) + 25O2(g)(excess)  16CO2(g) + 18H2O(l)
2C8H18(l) + 17O2(g)  16CO(g) + 18H2O(l)
2C8H18(l) + 9O2(g)(excess)  16C(s) + 18H2O(l)
S8(s) + 8O2(g)  8SO2(g)
2SO2(g) + O2(g)  2SO3(l)
SO3(l) + H2O  H2SO4(l)
N2(g) + O2(g) NO(g)
2NO(g) + O2(g)  2NO2(g)
3NO2(g) + H2O  HNO3(aq) + NO(g)
slow
reddish-brown
gas UV
light
Acid Rain
Acid Rain