2. Ionic Compounds composed of cations + anions electrically neutral
the total positive charge equals the total negative charge
formula units
usua lly solid at room temperature
have high melting points

3. Simple Ionic Compounds
Metal ion + Nonmetal ion  salt
Examples
Be+2 + N -3  Be3N2
Fe+3 + Cl -1  FeCl3
Subscript shows
number of atoms
present in formula
unit

4. Polyatomic Ions
Collections of tightly bound atoms that behave as a unit and carry a charge
examples
SO3-2 sulfite ion SO4-2  sulfate ion
NO2 -2  nitrite ion NO3-1  nitrate ion
ClO2-1  chlorite ion ClO3-1  chlorate ion

5. Ionic Compounds with Polyatomic Ions
Metal ion + Polyatomic ion or
Polyatomic ion + nonmetal ion
examples
Na+1 + SO4-2 Na2SO4
Mg+2 + NO3-1  Mg(NO3)2
NH N -3  (NH4)3 N
Oh no parentheses!

6. Given a formula, what’s the compound’s name?
e.g. Be2C
NH4MnO4
Al2(C2O4)3
H2SO4

7. Given a compound’s name, what is its formula?
e.g. ammonium sulfite
phosphoric acid
calcium chloride
iron (III) nitrite

8. Practice, practice, practice
name  formula
formula  name

9. Simple Molecular Compounds
Composed of two non-metallic compounds
Uses prefixes to indicate the number of atoms in the molecule
mono, 1
di, 2
tri, 3
tetra, 4
penta, 5
hexa, 6
hepta, 7
octa, 8
nona, 9
deca

10. Simple Molecular Compounds
examples: formula name
CO carbon monoxide
CO2 carbon dioxide
N2O dinitrogen monoxide
Cl2O3 dichloro trioxide
SF6 sulfur hexafluoride

11. More Simple Molecular Compounds
examples: name formula
nitrogen trifluoride NF3
phosphorus trichloride PCl3
carbon tetrachloride CCl4