Chemistry I Review
The following guide is intended to be a study aid for the first exam in AP
Chemistry in September. The exam will cover many of the topics listed below,
although any information you learned in Chem I is potentially on the test. I advise
that if you are unsure of any topic below, look it up over the summer and please
ask during our review time when we return in September. The chapters below
refer to the chapters in the AP Chem text book (Chemistry, Zumdahl & Zumdahl,
9th edition). You can use the internet sources such as Google or Youtube.com,
Chemtutor.com, Khanacademy.org to help you with these topics.
Good luck with your studies!
Know the definitions of:
Chem/Science Basics (Ch. 1)
Scientific Method
Substance
Hypothesis
Matter
Experiment
Element
Theory
Compound
Law
Physical Property
Independent Variable
Extensive Property
Dependent Variable
Intensive Property
Scientific Notation
Chemical Property
Significant Figures
States of Matter
Accuracy
Solid
Precision
Liquid
Certainty
Gas
Unit Analysis
Vapor
Conversion Factor
Physical Change
Law of Definite Proportions
Chemical Change
Density
Law of Conservation of Mass
Pressure
Barometer
Vapor Pressure
STP
Boyle’s Law
Charles’s Law
Gay-Lussac’s Law
The Gas Laws (Ch. 5.1 – 5.5)
Combined Gas Law
Ideal Gas Law (PV = nRT)
Ideal Gas Constant (R)
Gas Stoichiometry
Avogadro’s Principle
Dalton’s Law of Partial Pressure
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Chemistry I Review
Know also:
 Components of the scientific method: observation, hypothesis, experiment,
conclusion.
 Determine precision and certainty (Percent error); I’ll give you the formula of
Experimental Value - Accepted value
Accepted value
x 100 = % Error
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Apply the law of Conservation of Mass
Apply the law of Definite Proportions
Density is mass/volume
Use the Gas Laws (Boyle, Charles, Gay-Lussac, Combined)
Determine the number of moles (or mass) of gas given mass, T, & P
Ideal Gas Law: PV = nRT; how to work with this formula
Determine density or molar mass of a gas using M=dRT/P
Determine the partial pressure of a gas given its mole fraction and vice-versa.
Convert units of pressure and temperature.
Apply the law of conservation of mass
How to add, subtract, multiply, divide numbers and get proper number of
significant figures.
 Dimensional analysis to solve problems.
Know the Definitions of:
Atomic Nucleus (Ch. 2)
Dalton’s Atomic Theory
Atomic Number
Nucleus
Isotope
Proton
Mass Number
Neutron
Atomic Mass Unit (amu)
Electron
Atomic Mass
Electrons in Atoms (Ch. 7)
Electromagnetic Radiation
Quantum Mechanical Model of atom
Atomic Orbital
Wavelength (λ)
Principal Quantum Number
Frequency (ν)
Amplitude
Principal Energy Level
Electromagnetic Spectrum
Energy Sublevel
Quantum
Electron Configuration
Planck’s Constant
Aufbau Principle
Photoelectric Effect
Pauli Exclusion Principle
Photon
Hund’s Rule
Atomic Emission Spectrum
Valence Electron
Ground State
Electron (Lewis) Dot Structure
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Chemistry I Review
Know also:
 Dalton’s Atomic Theory
 Charge on a Proton, Neutron, and Electron
 What makes up the nucleus
 Rutherford’s Experiment and what that showed about the nucleus
 Atomic Number = Number of Protons = Number of Electrons
 Mass number = Number of Protons + Number of Neutrons; know how to
find any one given the other two.
 What shorthand notation means. i.e. C-14 means Carbon has 14 protons +
neutrons, Carbon (C) is element #6 so it has 6 protons.
C-14 than has 8
neutrons.
 Know how to calculate the atomic mass of an element given the mass and
the abundance of the isotopes.
 Photons are bundles of energy and the units are Joules (J)
 Calculate the energy of an electromagnetic wave (E=hν)
 The atomic orbitals (s, p, d, f)
 How to fill the atomic orbitals of a element
 Number of orbitals in an energy level, n. (# orbitals = n2)
 Number of electrons in an energy level, n (#electrons = 2n2)
 Electron orbital notation. Ex. B = 1s22s22p1
 Orbital Box Diagram. Example: Carbon
o
1s
2s
2p
↑↓
↑↓
↑
↑
 How to spot violations of Aufbau Principle, Hund’s rule, and the Pauli
Exclusion Principle
Know Definitions of:
The Periodic Table & Periodic Trends (Ch. 7)
Periodic Law
Transition element/metal
Group, Family, Column
Metal
Period
Alkali Metal
Representative Element
Alkaline Earth Metal
Inner Transition Metal
Nonmetal
Halogen
Noble Gas
Metalloid
Ion
Ionization Energy
Octet Rule
Electronegativity
Z*(Zeff) = Z – S
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Chemistry I Review
Know also:
 The classification of an element (metal, nonmetal, metalloid)
 How to locate an element by period, group, and block
 Whether the element is a representative element or a transition element
 Trends of Zeff, atomic radius, ionic radius, ionization energy,
electronegativity, and metallic character as you move across and down the
periodic table.
 Size relationship between a neutral atom its corresponding ion
Know the definitions of:
Ionic Compounds & Metals (Ch. 2 & Chem I notes)
Binary compound
Oxidation number
Chemical Bond
Polyatomic ion
Cation
Electron sea model
Anion
Delocalized electrons
Ionic bond
Metallic bond
Lattice Energy
Alloy
Formula unit
Interstitial alloy
Monoatomic Ion
Substitutional alloy
Hydrate
Know how to:
 Make a compound neutral when you have positive and negative ions.
 Show that column (group) of the element effects its oxidation number.
 Explain that lattice energy is affected by ion size and charge
 Identify elemental ions like oxide (O2-) and polyatomic ions like carbonate
(CO32-)
 Write out a formula from the name of the compound (Ex. potassium nitrate
is KNO3), and what to do when you have a transition element (Ex. Cobalt(II)
chloride is CoCl2) and a hydrated compound (Ex. Barium iodide dihydrate is
BaI2•2H2O).
 Write out a name when you have a formula. Ex. PbSO4 is lead(II) sulfate.
Same ideas as previous bullet point, just in reverse.
 Note: You do NOT have to know the nomenclature rules for the oxyanions
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Chemistry I Review
Know the definitions of:
Covalent Bonding (Chem I notes)*
Covalent Bond
Structural formula
Molecule
Polar covalent bond
Lewis Structure
Electronegativity
Sigma (σ) bond
Bond dissociation energy
Pi (π) bond
Lone pair electrons
Endothermic
Allotrope
Exothermic
* This material is covered in greater detail in Ch. 8, which we will formally cover later in the
year. The summary here are topics you should know from Chem I.
Know how to:
 Write the formula for covalent compounds (e.g. carbon dioxide)
 Draw Lewis structures of simple compounds and ions, be able to label
bonding electrons and lone pair electrons
 Determine type of bond between the two elements based on their
electronegativity difference
 Qualitatively determine how number of bonds and bond length affects bond
strength (i.e. double bonds are shorter and take more energy to break them
than single bonds)
Know the Definitions of:
Chemical reaction
Reactant
Product
Chemical equation
Coefficient
Precipitate
Solute
Solvent
Aqueous Solution
Le Chatelier’s Law
Chemical Reactions (Ch. 3)
Types of Reaction
Synthesis
Decomposition reaction
Single-Replacement reaction
Double-Replacement reaction
Combustion Reaction
Complete ionic equation
Net ionic equation
Spectator ion
Chemical Equilibrium (Notes)
Equilibrium
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Chemistry I Review
Know how to:
 Balance simple reactions
 Identify simple reactions as decomposition, synthesis, single replacement,
double replacement or combustion.
 Recall the seven diatomic elements (H2, N2, O2, F2, Cl2, Br2, I2)
 Decomposition of carbonates yields a metal oxide and carbon dioxide (eg.
CaCO3  CaO(s) + CO2(g))
 Decomposition of chlorates yields a metal chloride and oxygen gas (eg.
2Al(ClO3)3  2AlCl3(s) + 9O2(g))
 Identify the physical states of reactants and products (s= solid, aq=aqueous,
l=liquid, g=gas)
 Write the reaction using formulas if you are given the names and states of
the compounds
 Write the net ionic equation given the complete ionic equation
Know the Definitions of:
Mole
Avogadro’s Constant
Molar mass
The Mole (Ch. 3)
Percent Composition
Empirical formula
Molecular formula
Hydrate
Know how to:
 Determine the molar mass of a substance (element or compound).
 Change grams to moles to number of atoms, molecules or formula units and
back
 Determine the empirical formula of a compound given the elemental mass
percentages (or masses) of the compound
 Determine the molecular formula of a compound given the elemental mass
percentages (or masses) and the molar mass
 Determine the empirical formula of a hydrated compound given the mass
percentages of salt and water in the compound
Know the Definitions of:
Stoichiometry
Mole ratio
Limiting reactant
Stoichiometry (Ch. 3)
Excess reactant
Theoretical yield
Actual yield
Percent yield
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Chemistry I Review
Know how to:
 Perform mol-mol, mol-mass, mass-mol, and mass-mass stoichiometry
calculations
 Determine the limiting reactant in a reaction
 Determine the amount of product(s) (mass or moles) formed in a limiting
reactant problem
 Determine the mass (or moles) of excess reactant leftover in a limiting
reactant problem
 Use gas volumes like moles in a gas stoichiometry problem
 Determine the volume of gas produced in a reaction at STP or other
conditions
 Determine the percentage yield, theoretical yield, and actual yield of a
reaction
Know the Definitions of:
Solutions (Ch. 11.1 & Notes)
Molarity
Solution
Mass percent: %(m/m) & %(m/v)
Soluble/Insoluble
Saturated/Unsaturated Solutions
Miscible/Immiscible
Concentration (of a solution)
Dissolve
Parts per Million (ppm)
Mole Fraction
Colligative Properties
Freezing point depression
molality
Boiling point elevation
Acids & Bases (Ch. 4.8, 14.3, 14.4 & Notes)*
Acid
pH
Base
pOH
Neutralization
[H+]
Strong Electrolyte
[OH-]
* This material is covered in greater detail in Ch. 14 and 15, which we will formally cover later
in the year. The summary here are topics you should know from Chem I.
Solutions
Know how to:
 Calculate the %(m/m) of a solution
 Calculate the %(m/v) of a solution
 Calculate the mole fraction of a solution
 Calculate the ppm concentration
 Calculate the molarity of a solution
 Convert between %(m/v) and molarity of a solution
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Chemistry I Review
 Prepare a solution of a certain molarity and volume (i.e. how many grams of
solute to weigh)
 Determine the new concentration %(m/v) of a solution if it is diluted
(CV=CV)
 Determine the new molarity of a solution if it is diluted (MV=MV)
 Determine the molality of a solution
 Determine the new boiling point or freezing point of a solution with a
nonvolatile solute (∆T=Kb*m or ∆T=Kf*m)
 Use colligative properties to find the molar mass of a solute (we’ll go over
this in September)
Acids and Bases
Know how to:
 Determine pH from [H+] or [OH-]; pH = -log[H+], pOH = -log[OH-]
 Determine [H+] from pH ([H+] = 10-pH)
 Determine an unknown molarity by titration (neutralization)
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