1.  Naming Formulas  Percent composition  Empirical formulas  Balancing Equations  Types of Reactions  Activity Series

2.  A molecule is held together by covalent bonds.  Valence electrons are shared.  Between non-metals i.e. H 2 O, CO 2, O 2, NO

3.  Use prefixes 1mono- 2di- 3tri- 4tetra- 5penta- 6hexa- 7hepta- 8octa- 9nona- 10deca-

4.  Use prefixes 1mono- 2di- 3tri- 4tetra- 5penta- 6hexa- 7hepta- 8octa- 9nona- 10deca-

5.  Determine the mass percentage of each element in the compound. Mass of element x 100% mass of compound What is the percent composition of Fe 2 O 3 ? 2 Fe 2 x 55.8 = 111.6 3 O 3 x 16.0 = 48.0 Formula mass 159.6 %Fe = 111.6/159.6 = 70.0% % O = 48.0/159.6 = 30.0%

6. X (empirical formula) = molecular formula so x = molecular formula mass empirical formula mass

7.  What is the molecular formula of the molecule that has an empirical formula of CH 2 O and a molar mass of 120.12 g/mol? Empirical formula mass: 12.0 + 2.0 + 16.0 = 30.0 amu X = 120.12 amu = 4 30.0 amu So C 4 H 8 O 4 is the molecular formula.

8.  Find the empirical formula of a compound that contains 53.7% iron and 46.3% sulfur.  % composition  mass of 100 g sample  moles  mole ratio  53.7g x 1 mol/55.8g =.962 mol Fe 46.3g x 1 mol/32.1g = 1.44 mol S.962/.962 = 1, 1.44/.962 = 1.5 1:1.5 ratio x 2 = 2:3 ratio Fe 2 S 3

9.  “Honkle Brif” H2H2 O2O2 N2N2  Cl 2  Br 2 I2I2 F2F2

10.  Yields  Gas(g)  Precipitate  Solid(s) or down arrow  Liquid(l)  Aqueous (aq)

11.  Balancing Equations  Synthesis (Combination)  Decomposition  Single Displacement (Replacement)  Double Displacement (Replacement)  Neutralization  Combustion