1. The Chemistry of the Periodic Table
Key points:
How the periodic table is arranged (groups, periods, electron configurations)
Trends in the periodic table (atomic radius, ionization energy, electron affinity, electronegativity)
What is ionization and which atoms gain/lose electrons to become stable
Properties of metals/non-metals

2. Vocabulary
Ionization Energy Oxidation Atomic Radius Reduction Electron Affinity Stable Electronegativity Unstable
Electron Shell Inert
Valence Shell
Valence Electrons
Cation
Anion

3. Trends in the periodic table:
Ionization Energy Atomic Radius Electron Affinity Electronegativity

4. Atomic Radius

5. Going down the periodic table means going to outer shells so the radius increases
protons

6. Going across the periodic table means adding electrons to the same shell and increasing the positive charge of the nucleus so the radius decreases as the shell is pulled in.
The shell is pulled in 6+ 4+ 3+ 5+

8. Ionization Energy and Electron Affinity
Electrons can jump between shells (Bohr’s model supported by line spectra)
The electrons can be pushed so far that they escape the attraction of the nucleus
Losing an electron is called ionization
The amount of energy required to remove 1 electron (the outermost e-) from an atom (g) is called the ionization energy

9. Going down the periodic table means going to outer shells so the radius increases. The outer electrons are not attracted as strongly to the nucleus, so require less energy to remove
Elements at the top have the highest ionization energy in each group.
Elements at the bottom have the lowest ionization energy in each group.

10. Going across the periodic table means adding electrons to the same shell. Filled valence shells are more stable, and require more energy to remove an electron. Thus, ionization energy increases as you move across to the right.
Noble gases have filled valence shells, so are very stable and have the highest ionization energy in each period.
Alkali metals have only 1 valence electron, so have the lowest ionization energy in each period

11. When one atom loses an electron, another atom gains that electron.
The receiving atom can gain or lose energy when the electron is added.
If energy is released, the negatively charged ion will be stable.
The energy absorbed or released during the addition of an electron is the electron affinity.
Electron affinities are expressed as negative values.

12. The ability of an atom to attract shared electrons is called its electronegativity.
When one atom has lost an electron and another has gained an electron, they become oppositely charged ions that attract each other.
Noble gases have no value for electronegativity (they do not need to share electrons as their valence shells are full).

14. s max. = 2
p max. = 6
d max. = 10
p max. = 14

15. Metals
Left side of the periodic table
Lose electrons
Form positive ions called cations
Shiny
Malleable
Conduct electricity

16. +1
Alkali Metals
Brainiac Rhubium

17. We can show how a metal loses electrons to form a cation using a half reaction.
When the electron is lost it is on the right and it is called oxidation.
LEO goes GER
Loss of Electrons is Oxidation
Gain of Electrons is Reduction Li
 Li+
+ e-

18. Alkaline Earth Metals +2 Sr Ba Ra

19. Group 2
Alkaline Earth Metals.
2 valence electrons.
They lose two electrons to form 2+ ions.

20. Ca
20p
20n
2e-
2e- 2 valence electrons- Unstable
8e-

21. Ca2+
8 valence electrons- Full Shell
-Stable
20p
20n
2e-
8e-

22. Ca
 Ca2+
+ 2e-

23. Transition Metals- Groups 3 - 12

24. Boron Family +3 In Ti

25. Boron Family.
3 valence electrons.
Lose three electrons to form 3+ ions.

26. Al
 Al3+
+ 3e-

27. Nonmetals
Right side of the periodic table
Gain electrons
Form negative ions called anions
Dull
Brittle
Do not conduct electricity

29. Group 15
Nitrogen Family.
5 valence electrons.
gain 3 to form 3- ions.

30. P
5 valence electrons- Full Shell
-unstable
15p
16n
2e-
8e-
5e-

31. P3-
8 valence electrons- Full Shell
-Stable
15p
16n
2e-
8e-

32. We can show how a nonmetal gains electrons to form an Anion using a half reaction.P
+ 3e-
 P3-
GER
Gain of Electrons is Reduction

34. Oxygen Family.
6 valence electrons.
gain 2 electrons to form 2- ions.

35. S
6 valence electrons- Full Shell
-unstable
16p
16n
2e-
8e-
6e-

36. S2-
8 valence electrons- Full Shell
-Stable
16p
16n
2e-
8e-

37. S
+ 2e-
 S2-

39. Halogens.
7 valence electrons.
Gain 1 electron to form 1- ions.

40. Cl2
+ 2e-
 Cl- 2 O2
+ 4e-
 O2- 2 N2
+ 6e-
 N3- 2

41. Brainiac

42. Noble or Inert Gases.
8 valence electrons.
Do not form compounds.