CHAD’S ULTIMATE GENERAL CHEMISTRY REVIEW
Table of Contents
Chapter 1: Matter and Measurement Page 1
Chapter 2: Atoms, Molecules, and Ions Page 3
Chapter 3: Stoichiometry Page 5
Chapter 4: Aqueous Reactions and Solution Stoichiometry Page 8
Chapter 5: Thermochemistry Page 11
Chapter 6: Electronic Structure Page 15
Chapter 7: Periodic Properties of the Elements Page 19
Chapter 8: Bonding and Lewis Structures Page 21
Chapter 9: Molecular Geometry and Bonding Page 24
Chapter 10: Gases Page 26
Chapter 11: Intermolecular Forces and Phase Diagrams Page 29
Chapter 12: Colligative Properties Page 31
Chapter 13: Kinetics Page 32
Chapter 14: Equilibrium Page 35
Chapter 15: Acids and Bases Page 37
Chapter 16: Solubility Equilibria Page 43
Chapter 17: Thermodynamics Page 45
Chapter 18: Electrochemistry Page 47
Chapter 19: Nuclear Chemistry Page 51
Chapter 20: Coordination Chemistry Page 54
0
, Chapter 1 – Matter and Measurement
Matter
Elements (Na, Si, H2, S8) vs. compounds (CO2, NaCl, NaHCO3)
Pure substances vs. mixtures (more than one element and/or compound)
Homogeneous vs. heterogeneous mixtures
Chemical vs. physical properties and changes
Intensive vs. extensive properties
Precision vs. accuracy
1
,Units of Measurement
Convert 1500g to kilograms. SI Units
10
Terra Giga Mega kiloLength
12 centi milli m
109 pico femtoMass
icro nano kg
106 Time s
103 Temperature K
10-2
10-3 Derived Units
Convert 3200m to miles (1in = 2.54cm, 1mile = 5280ft).
10-6 Volume
10-9 m3
Energy/Work J
10-12 Pressure Pa
10-15
A hose fills your swimming pool at a rate of 1,000.0 gallons per hour. How much is this in
mL per second? (1 gal=3.785L)
Density calculations (d=m/v)
A cube with 2.00cm edges weighs 10.0 grams. What is its density?
How much would a cube of the same substance with 5.00cm edges weigh?
Significant Figures
Zeroes in between significant figures are significant
Zeroes right of the decimal, at the end are significant
-Multiplication/division vs addition/subtraction
2
, Chapter 2 – Atoms, Molecules, and Ions
Atomic Structure - nucleus composed of protons and neutrons surrounded by an electron cloud
Dalton proposed his atomic theory.
Thompson discovered electrons.
Millikan determined the mass of an electron (oil drop experiment).
Rutherford discovered the nucleus (scattering of alpha particles in thin gold foil).
Isotope symbols (atomic number, mass number, isotopes)
Atomic Weights
Chlorine has two abundant isotopes; 75% have a mass of 35a.m.u, 25% have a mass of 37 a.m.u. What is the
atomic mass (also called atomic weight) of chlorine?
Periodic Table
Periods vs. groups
metals, non-metals, and metalloids
Group names
3
Table of Contents
Chapter 1: Matter and Measurement Page 1
Chapter 2: Atoms, Molecules, and Ions Page 3
Chapter 3: Stoichiometry Page 5
Chapter 4: Aqueous Reactions and Solution Stoichiometry Page 8
Chapter 5: Thermochemistry Page 11
Chapter 6: Electronic Structure Page 15
Chapter 7: Periodic Properties of the Elements Page 19
Chapter 8: Bonding and Lewis Structures Page 21
Chapter 9: Molecular Geometry and Bonding Page 24
Chapter 10: Gases Page 26
Chapter 11: Intermolecular Forces and Phase Diagrams Page 29
Chapter 12: Colligative Properties Page 31
Chapter 13: Kinetics Page 32
Chapter 14: Equilibrium Page 35
Chapter 15: Acids and Bases Page 37
Chapter 16: Solubility Equilibria Page 43
Chapter 17: Thermodynamics Page 45
Chapter 18: Electrochemistry Page 47
Chapter 19: Nuclear Chemistry Page 51
Chapter 20: Coordination Chemistry Page 54
0
, Chapter 1 – Matter and Measurement
Matter
Elements (Na, Si, H2, S8) vs. compounds (CO2, NaCl, NaHCO3)
Pure substances vs. mixtures (more than one element and/or compound)
Homogeneous vs. heterogeneous mixtures
Chemical vs. physical properties and changes
Intensive vs. extensive properties
Precision vs. accuracy
1
,Units of Measurement
Convert 1500g to kilograms. SI Units
10
Terra Giga Mega kiloLength
12 centi milli m
109 pico femtoMass
icro nano kg
106 Time s
103 Temperature K
10-2
10-3 Derived Units
Convert 3200m to miles (1in = 2.54cm, 1mile = 5280ft).
10-6 Volume
10-9 m3
Energy/Work J
10-12 Pressure Pa
10-15
A hose fills your swimming pool at a rate of 1,000.0 gallons per hour. How much is this in
mL per second? (1 gal=3.785L)
Density calculations (d=m/v)
A cube with 2.00cm edges weighs 10.0 grams. What is its density?
How much would a cube of the same substance with 5.00cm edges weigh?
Significant Figures
Zeroes in between significant figures are significant
Zeroes right of the decimal, at the end are significant
-Multiplication/division vs addition/subtraction
2
, Chapter 2 – Atoms, Molecules, and Ions
Atomic Structure - nucleus composed of protons and neutrons surrounded by an electron cloud
Dalton proposed his atomic theory.
Thompson discovered electrons.
Millikan determined the mass of an electron (oil drop experiment).
Rutherford discovered the nucleus (scattering of alpha particles in thin gold foil).
Isotope symbols (atomic number, mass number, isotopes)
Atomic Weights
Chlorine has two abundant isotopes; 75% have a mass of 35a.m.u, 25% have a mass of 37 a.m.u. What is the
atomic mass (also called atomic weight) of chlorine?
Periodic Table
Periods vs. groups
metals, non-metals, and metalloids
Group names
3
