Chemistry 1201
FINAL EXAM STUDY GUIDE
Chapter 1: Matter and Measurement
know the major metric conversions
Metric System Prefixes
Prefix Magnitude Abbreviation
Pico 10–12 p
nano 10–9 n
micro 10–6 μ (Greek letter “mew”)
milli 10–3 m
centi 10–2 c
deci 10–1 d
BASE 100 g, L, s, m, K, mol, etc.
Deca 101 da
Hector 102 h
Kilo 103 k
Mega 106 M
Giga 109 G
Tera 1012 T
o 1 cm3 = 1 mL
significant figures
o Multiplication and Division: 0.300 × 0.002 = 0.0006 (1 sig-fig)
o Addition and Subtraction: 1.80 + 12.1 = 13.9 (3 sig-figs)
o Mixed Operation: (1.20 ÷ 4.0) – 0.1 = 0.2 (1 sig-fig)
density
mass
o Density =
Volume
1
,Chapter 2: Atoms, Molecules, and Ions
Be able to interpret the information in the periodic table.
o Example: chlorine
chemical symbol: Cl
17 protons (always) and 17 electrons (in a neutral atom)
AVERAGE atomic mass: 35.4527 amu
Be able to identify chemical species from given information.
o Example: 36 electrons, 45 neutrons, and a charge of –1
36 – 1 = 35 protons → MUST be a form of Br
35 amu + 45 amu = 80 amu
80Br–
Ionic vs. Molecular Compounds
o Metal + Nonmetal → Ionic Compound
NaCl
o Nonmetal + Nonmetal → Molecular Compound
SO2
o Polyatomic Ion + Metal → Ionic Compound
Pb(ClO3)2
o Polyatomic Ion + Nonmetal → Ionic Compound
Hg2Br2
o Polyatomic Ion + Polyatomic Ion → Ionic Compound
(NH4)3PO4
Nomenclature
o KNOW THE POLYATOMIC IONS!!!
ClO– hypochlorite PO43– phosphate
ClO2– chlorite NO2– nitrite
ClO3– chlorate NO3– nitrate
ClO4– perchlorate OH– hydroxide
SO32– sulfite H– hydride
SO42– sulfate NH4+ ammonium
CO32– carbonate Hg22+ mercury(I)
2
, o Be able to name inorganic compounds (and vice versa)
Examples
Ca(OH)2 → calcium hydroxide
N2O4 → dinitrogen tetroxide
SO2 → sulfur dioxide
Pb3(PO4)2 → lead(II) phosphate
Average Atomic Mass
o Average Atomic Mass = Σ(Fractional Abundance × Isotopic Mass)
Chapter 3: Stoichiometry
Be able to balance a given chemical equation.
There are three types of reactions for which you will be expected to write
a balanced equation given only the reactants.
o Combustion Reaction
Fuel + O2 → CO2 + H2O
Example: C3H8 + 5O2 → 3CO2 + 4H2O
o Acid-Base Neutralization
Acid + Base → H2O + Salt
Example: Sr(OH)2 + 2HCl → 2H2O + SrCl2
o Double Replacement Reaction (occurs only in aqueous solution)
AB + CD → AD + CB
Example: Fe(ClO)2 + 2NH4I → FeI2 + 2NH4ClO
You should be able to recognize two additional typed of reactions.
o Combination Reaction
A + B → C
Example: C(s) + O2(g) → CO2(g)
o Decomposition Reaction
C → A + B
Example: 2KClO3(s) → 2KCl(s) + 3O2(g)
3
FINAL EXAM STUDY GUIDE
Chapter 1: Matter and Measurement
know the major metric conversions
Metric System Prefixes
Prefix Magnitude Abbreviation
Pico 10–12 p
nano 10–9 n
micro 10–6 μ (Greek letter “mew”)
milli 10–3 m
centi 10–2 c
deci 10–1 d
BASE 100 g, L, s, m, K, mol, etc.
Deca 101 da
Hector 102 h
Kilo 103 k
Mega 106 M
Giga 109 G
Tera 1012 T
o 1 cm3 = 1 mL
significant figures
o Multiplication and Division: 0.300 × 0.002 = 0.0006 (1 sig-fig)
o Addition and Subtraction: 1.80 + 12.1 = 13.9 (3 sig-figs)
o Mixed Operation: (1.20 ÷ 4.0) – 0.1 = 0.2 (1 sig-fig)
density
mass
o Density =
Volume
1
,Chapter 2: Atoms, Molecules, and Ions
Be able to interpret the information in the periodic table.
o Example: chlorine
chemical symbol: Cl
17 protons (always) and 17 electrons (in a neutral atom)
AVERAGE atomic mass: 35.4527 amu
Be able to identify chemical species from given information.
o Example: 36 electrons, 45 neutrons, and a charge of –1
36 – 1 = 35 protons → MUST be a form of Br
35 amu + 45 amu = 80 amu
80Br–
Ionic vs. Molecular Compounds
o Metal + Nonmetal → Ionic Compound
NaCl
o Nonmetal + Nonmetal → Molecular Compound
SO2
o Polyatomic Ion + Metal → Ionic Compound
Pb(ClO3)2
o Polyatomic Ion + Nonmetal → Ionic Compound
Hg2Br2
o Polyatomic Ion + Polyatomic Ion → Ionic Compound
(NH4)3PO4
Nomenclature
o KNOW THE POLYATOMIC IONS!!!
ClO– hypochlorite PO43– phosphate
ClO2– chlorite NO2– nitrite
ClO3– chlorate NO3– nitrate
ClO4– perchlorate OH– hydroxide
SO32– sulfite H– hydride
SO42– sulfate NH4+ ammonium
CO32– carbonate Hg22+ mercury(I)
2
, o Be able to name inorganic compounds (and vice versa)
Examples
Ca(OH)2 → calcium hydroxide
N2O4 → dinitrogen tetroxide
SO2 → sulfur dioxide
Pb3(PO4)2 → lead(II) phosphate
Average Atomic Mass
o Average Atomic Mass = Σ(Fractional Abundance × Isotopic Mass)
Chapter 3: Stoichiometry
Be able to balance a given chemical equation.
There are three types of reactions for which you will be expected to write
a balanced equation given only the reactants.
o Combustion Reaction
Fuel + O2 → CO2 + H2O
Example: C3H8 + 5O2 → 3CO2 + 4H2O
o Acid-Base Neutralization
Acid + Base → H2O + Salt
Example: Sr(OH)2 + 2HCl → 2H2O + SrCl2
o Double Replacement Reaction (occurs only in aqueous solution)
AB + CD → AD + CB
Example: Fe(ClO)2 + 2NH4I → FeI2 + 2NH4ClO
You should be able to recognize two additional typed of reactions.
o Combination Reaction
A + B → C
Example: C(s) + O2(g) → CO2(g)
o Decomposition Reaction
C → A + B
Example: 2KClO3(s) → 2KCl(s) + 3O2(g)
3
