1. Intramolecular Bonds
Ionic Bonds – metal (gives e-, cation) with non-metal (takes e-, anion)
- GLUE: electrostatic attraction
Covalent Bonds – non-metal atoms
(polarity of bond depends on electronegativity difference of atoms)
- GLUE: share e-
Metallic Bonds –metal atoms
- GLUE: sea of electrons e-

2. Names/Formulas of Compounds
Ionic Compounds : (Note: 1st atom is metal OR ammonium)
Atom + Atom-ide
If 1st atom is a metal you don’t know the charge of…use Roman Numerals
If you cross charges, SIMPLIFY
If you cross a 2 charge or higher next to a polyatomic ion…use parentheses!
Know Polyatomic Ions:
Ammonium – NH Carbonate – CO32-
Hydroxide – OH- Chromate – CrO42-
Cyanide – CN- Dichromate – Cr2O72-
Nitrite – NO Sulfite – SO32-
Nitrate – NO3 - Sulfate – SO4 2-
Bicarbonate - HCO Phosphate – PO43-
Acetate – C2H3O2-
Permanganate – MnO4-
Write the formula:
Magnesium chloride  d. Aluminum hydroxide 
Iron (III) phosphide  e. Calcium bicarbonate 
Lead (IV) sulfate  f. Gold nitrite 
Write the name:
Cu2O  c. Zn3(PO4)2 
KCl  d. Ag2Cr2O7 

3. Names/Formulas of Compounds
Covalent Compounds : (Note: 1st atom is non-metal, prefixes are present)
Prefix-Atom + Prefix-Atom-ide
Never use mono- on 1st atom
NEVER SIMPLIFY
Don’t think!!!... Just do what it says!!!
Know Prefixes:
1 – mono 6 – hexa
2 – di 7 – hepta
3 – tri 8 – octa
4 – tetra 9 – nona
5 – penta 10 – deca
Write the formula:
tetraphosphorus octaoxide c. Disulfur monophosphide
Carbon trioxide d. Hexafluorine decabromide
Write the name:
SO4  c. N5H9 
CO3  d. P7Cl10 

4. Dot Diagrams Rules: Draw the dot diagrams: F2 b. O2 c. N2 d. HF
Put the atom by itself in the middle.
Surround it by the other atoms. Hydrogen goes on the outside ALWAYS!
Atoms want to maximize electron repulsion and get as far away from each other as possible.
Draw the dot diagrams:
F2 b. O2 c. N2 d. HF
H2O f. CO2 g. SiS2 h. BCl3
i. CBr4 j. C2H6 k. C2H4 l. C2H2

5. VSEPR Practice Compound Dot Diagram Shape Name Bond Angle(s) Polarity
Hybridization H2
HCl
SiO2
CF4
H2S
PH3
Si2H4