1. Part B. Definitions
Empirical Formula = a formula giving the ratios (proportions) of the elements present in a compound but not the actual numbers or arrangement of atoms… aka the reduced/simplest form
Examples:
CH2O --- this is the empirical form for glucose, C6H12O6
C3H4O --- the subscripts cannot be simplified so must be in their reduced form, making this empirical

2. Part B. Definitions
Molecular Formula = a formula giving the number of atoms of each of the elements present in one molecule of a specific compound (not necessarily the reduced form, but it could be)
Examples:
C6H12O6 (sugar) --- Dividing all subscripts by 6 would give the empirical form, CH2O
N2O4 --- dividing all subscripts by 2 would give the empirical form NO2
H2O --- this is the molecular and empirical form because this is actually what the H2O molecule looks like

3. Part B. Definitions
Mole Ratio = ratio of atoms within a compound or the ratio of compounds in a reaction
Examples:
H2O has a 2:1 ratio of
hydrogen to oxygen.
C6H12O6 (sugar) has a 6:12:6 ratio of carbon to hydrogen to oxygen.

4. PART C. Identify the following as empirical or molecular
1. Formaldehyde
CH2O
2. dinitrogen tetroxide
N2O4
3. carbon monoxide CO
4. acetic acid
C2H4O2
5. Hydrogen peroxide
H2O2

5. PART C. Identify the following as empirical or molecular
6. Acetylene
C2H2
7. Water
H2O
8. Carbon dioxide
CO2
9. Butene
C4H8
10. glucose
C6H12O6