1. Ions, Charges, and Metallic Bonds

2. Types of Ions
Polyatomic - a covalently bonded group of atoms that lost or gained e-
Sulfate: SO42-
Monoatomic - one atom that lost or gained valence e-
Sulfide: S2-

3. Monoatomic Ions
The representative groups form ions with predictable charges (oxidation number).
Electrons are lost/gained so atoms can be isoelectric with the nearest noble gas
You must to know the charge formed by each group

4. CATIONS (+) [Ne] 3s1  Na+ + e- Na  [Ne]
A metal atom loses all its valence e- in a process called oxidation forming a positive ion
Go backward on the table to determine the noble gas
[Name is same as neutral element] e-
Notice that Na+ has the same configuration as neon
[Ne] 3s1 
[Ne]
Na e-
Na 
Sodium ion

5. ANIONS (-)
A nonmetal atom gains enough valence e- in a process called reduction to have 8 total
Go forward on the table to determine the noble gas
[Name ends with -ide] e-
Which noble gas does chloride become isoelectric with?
 1s22s22p6
1s22s22p5
[Ne] F
+ e-  F-
Fluoride ion

6. The charges on groups of the periodic table
+/- 4 N O B L E
G A S +2
(most)
Lose e-
Gain e-

7. Metallic Bonds
Metallic elements exist as cations (the atoms lose their valence e-)
This “sea of e-” belong to all the atoms; this is why metals are malleable and conductive