Matter and Measurements

 Atom  Element  Law Of Definite Proportions

 Mixture  Solution  Physical Properties  Chemical Properties

 Intensive Property  Extensive Property  SI units

 Precision  Accuracy  Significant figures  Dimensional Analysis

 Density = m/v  K = o C + 273

 Solve simple problems using dimensional analysis.  Convert between Celsius and Kelvin

Atoms, Molecules, and Ions

 Nucleus  Proton, Neutron, Electron  Atomic Mass Unit

 Isotope  Group  Period  Metal, nonmetal, metalloid

 Molecule  Compound  Empirical Formula  Molecular Formula

 Ion  Ionic Compound  Polyatomic Ion

 None

 Calculate number of subatomic particles in an atom based on basic information about AMU’s and the type of element the atom is.  Work with empirical and molecular formulas.  Name ionic compounds.  Determine the formula of an ionic compound when given the name.

 20, 22, 47, 53, 69

Stoichiometry

 Chemical Equation  Reactants  Products

 Formula Weight  Mole  Molar Mass  Limiting Reactant

 Theoretical Yield  Percent Yield  Aqueous solution  Sovlent

 Solute  Electrolyte  nonelectrolyte  Strong and weak electrolyte

 Precipitation Reaction  Molecular Equation  Complete Ionic Equation  Net Ionic Equation

 Acid  Base  Neutralization Reaction  Oxidation  Oxidation state

 Reduction  Concentration  Titration  Equivalence Point

 Molarity = moles/L  M 1 V 1 = M 2 V 2

 Balance Equations  Calculate Molar Masses  Convert between moles and mass  Convert between Mass, moles, and number of particles.  Determine percent composition  Determine empirical and molecular formulas from percent composition data.  Calculate percent yeild

 1, 8, 9, 19, 21, 25, 41, 44, 63, 68, 74

Thermodynamics and Thermochemistry

 Thermodynamics  Thermochemistry  Kinetic Energy

 Potential Energy  Joule  Calorie  System

 Surroundings  Heat  First Law Of Thermodynamics  Endothermic

 Exothermic  Enthalpy  Calorimetry  Heat Capacity

 Molar Heat Capacity  Specific Heat  Hess’s Law  Enthalpy Of Formation

 Standard Enthalpy of Reaction  Standard Enthalpy of Formation  Spontaneous  Isothermal

 Second Law Of Thermodynamics  Third Law Of Thermodynamics  Gibbs Free Energy  Standard Free Energy of Formation

 q = C x m x ΔT  ΔH o rxn = sum(nΔH o f products) – sum(ΔH o f reactants)  Δs o = sum(nΔS products) – sum(nΔS reactants)  ΔG = ΔH - TΔS  ΔG o rxn = sum(nΔG o f products) – sum(ΔG o f reactants)  ΔG = ΔG o + RT lnQ  ΔG o =- RT ln k

 Understand the mathematical signs associated with thermodynamics.  Use Hess’s law to determine the heat energy transfer during a chemical reaction.  Calculate the heat transferred in a process using calorimetry.  Use standard enthalpies of formation to determine the standard enthalpy of a reaction.  Qualitatively describe entropy and entropy changes.

 Calculate the standard entropy change for a process using standard molar entropies.  Calculate gibbs free energy from the enthalpy and entropy changes at a given temperature.  Predict the effect of temperature on spontaneity given ΔH and ΔS.  Calculate ΔG under nonstandard conditions.  Relate Δg o and equilibrium constants.

 29, 37, 46, 52,

Electronic Structure Of Matter

 Electron Configuration  Ground State  Excited State  Pauli exclusion principle

 Hunds Rule  Valance Electrons

 None

 Be able to interpret electron energy level diagrams.  Be able to write electron configurations.

 23

Periodic Properties Of The Elements

 Effective Nuclear Charge  Atomic Radius  Isoelectronic

 Ionization Energy  Electron Affinity  Metallic Character

 None

 Understand how effective nuclear charge affects first ionization energy.  Use the periodic table to predict atomic radii, ionic radii, ionization energy, and electron affinity.  Understand how the ionization energy changes as we remove successive electrons.

 18, 57, free response question 6

Basic Chemical Bonding

 Chemical Bonds  Ionic Bonds  Covalent Bonds

 Metallic Bonds  Lewis Symbol  Octet Rule  Lattice Energy

 Lewis Structure  Sigma Bond  Pi Bond  Bond Polarity

 Nonpolar Covalent Bond  Polar Covalent Bond  Electronegativity  Polar Molecule

 Formal Charge  Resonance Structure  Bond Enthalpy

 ΔH rxn = Sum(bond enthalpies of bonds broken) – Sum(Bond enthalpies of bonds formed)

 Write Lewis symbols for atoms and ions.  Understand lattice energy and arrange compounds in order of lattice energy.  Draw Lewis structures for molecules and compounds.  Calculate formal charges.  Use formal charges to select the best possible Lewis structure.  Understand the relationship between bond type, bond strength, and bond length.  Use bond enthalpies to determine the enthalpy of a reaction.

 4, 5, 47, 71, 73,

Molecular Geometry and Bonding Theories

 VSEPR  Electron Domain  Bonding Pair

 Non Bonding Pair  Electron-Domain Geometry  Molecular Geometry  Polar Bond

 None

 Describe the three dimensional shapes of molecules using VSEPR.  Determine whether a molecule is polar or nonpolar.

 6, 7, 24

Gases

 Pressure  STP  Boyles Law

 Charles Law  Avogadros Law  Ideal Gas Law  Partial PRessure

 Mole Fraction  Kinetic-Molecular Theory  Effusion  Diffusion

 PV = nRT  P1V1/T1 = P2V2/T2  d = (P)(molar mass)/RT  Pt = P1 + P2 + P3…..

 15, 16, 17, 28, Free response question 2

Intermolecular Forces, Liquids, Solids

 Intermolecular Forces  Dipole-Dipole Forces  LDF

 Hydrogen Bonding  Ion-Dipole Forces  Polarizability  Heat of fusion

 Heat of vaporization  Vapor Pressure  Phase Diagram  Molecular Solids

 Covalent-Network Solid  Ionic Solids  Metallic Solids

 None

 Describe different intermolecular forces.  Understand polarizability.  Describe how the strength of intermolecular forces affect the macroscopic properties of matter.

 42, 54, 55, 66,

Reaction Rates

 Reaction Rate  Rate Law  Rate Constant

 Reaction Order  Overall Reaction Order  First Order Reaction  Second Order Reaction

 Half Life  Activation Energy  Transition State  Reaction Mechanism

 Elementary Reaction  Molecularity  Intermediate  Rate Determining Step

 Catalyst

 aA + bB  cC + dD  Rate =  ln[A] t – ln[A] o = -kt  1/[A] t – 1/[A] o = kt  lnk = (-E a /R)(1/T) + lnA

 Understand the factors that affect the rate of chemical reactions.  Be able to determine the rate of a reaction.  Be able to determine the rate law of a reaction.  Be able to determine the rate law constant for a reaction.  Be able to use the integrated rate laws.  Be able to use the Arrhenius equation.

 32, 51, 62, 67, Free response question 3.

Equilibrium

 Chemical Equilibrium  Equilibrium constant expression  Equilibrium constant

 Homogeneous Equilibrium  Heterogeneous Equilibrium  Reaction Quotient  Le Chatelier’s Principle

 K p = K c (RT) Δn

 Understand what equilibrium means  Write equilibrium constant expressions for any reaction.  Relate K p and K c.  Calculate equilibrium constants from concentration measurements.  Use ICE charts.  Be able to predict how a reaction will change if a stress is applied.

 26, 30, 60, Free response question 1

Acids and Bases and Solubility Equilibria

 Bronsted-Lowry acids and bases  Conjugate acid and bases  Ion-Product constant of water

 pH  Acid dissociation constant  Percent Ionization  Polyprotic Acids

 Base dissociation constant  Hydrolysis  Common ion effect  buffer

 Henderson-Hasselbalch equation  pH titration curve  Solubility product constant  Complex ions

 Understand the difference between an acid and a base.  Identify conjugate acid/base pairs  Calculate the pH of a solution when given [OH-] or [H 3 O+]  Calculate the pH of a strong acid or base when given its concentration  Calculate k a or k b for an acid or base when given its concentration and the pH of the solution.  Calculate the pH of a solution when given its k a or k b.  Calculate k a when given k b or vice versa

 Describe the common ion effect  Explain how to make a buffer  Calculate the pH of a buffer  Calculate the pH of a buffer after small amounts of acid or base are added.  Calculate the pH at any point of a titration  Calculate k sp from molar solubility and vice versa.  Predict the effect of pH on solubility  Predict whether a precipitate will form when solutions are mixed

 40, 45, 56, Free response 1 e and f.

Electrochemistry

 Half-Reactions

 The energy released in a spontaneous redox reaction can be used to perform electrical work.