2. Matter and Measurements

3.  Atom  Element  Law Of Definite Proportions

4.  Mixture  Solution  Physical Properties  Chemical Properties

5.  Intensive Property  Extensive Property  SI units

6.  Precision  Accuracy  Significant figures  Dimensional Analysis

7.  Density = m/v  K = o C + 273

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

9. Atoms, Molecules, and Ions

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

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

12.  Molecule  Compound  Empirical Formula  Molecular Formula

13.  Ion  Ionic Compound  Polyatomic Ion

14.  None

15.  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.

16.  20, 22, 47, 53, 69

17. Stoichiometry

18.  Chemical Equation  Reactants  Products

19.  Formula Weight  Mole  Molar Mass  Limiting Reactant

20.  Theoretical Yield  Percent Yield  Aqueous solution  Sovlent

21.  Solute  Electrolyte  nonelectrolyte  Strong and weak electrolyte

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

23.  Acid  Base  Neutralization Reaction  Oxidation  Oxidation state

24.  Reduction  Concentration  Titration  Equivalence Point

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

26.  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

27.  1, 8, 9, 19, 21, 25, 41, 44, 63, 68, 74

28. Thermodynamics and Thermochemistry

29.  Thermodynamics  Thermochemistry  Kinetic Energy

30.  Potential Energy  Joule  Calorie  System

31.  Surroundings  Heat  First Law Of Thermodynamics  Endothermic

32.  Exothermic  Enthalpy  Calorimetry  Heat Capacity

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

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

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

36.  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

37.  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.

38.  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.

39.  29, 37, 46, 52,

40. Electronic Structure Of Matter

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

42.  Hunds Rule  Valance Electrons

43.  None

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

45.  23

46. Periodic Properties Of The Elements

47.  Effective Nuclear Charge  Atomic Radius  Isoelectronic

48.  Ionization Energy  Electron Affinity  Metallic Character

49.  None

50.  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.

51.  18, 57, free response question 6

52. Basic Chemical Bonding

53.  Chemical Bonds  Ionic Bonds  Covalent Bonds

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

55.  Lewis Structure  Sigma Bond  Pi Bond  Bond Polarity

56.  Nonpolar Covalent Bond  Polar Covalent Bond  Electronegativity  Polar Molecule

57.  Formal Charge  Resonance Structure  Bond Enthalpy

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

59.  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.

60.  4, 5, 47, 71, 73,

61. Molecular Geometry and Bonding Theories

62.  VSEPR  Electron Domain  Bonding Pair

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

64.  None

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

66.  6, 7, 24

67. Gases

68.  Pressure  STP  Boyles Law

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

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

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

72.  15, 16, 17, 28, Free response question 2

73. Intermolecular Forces, Liquids, Solids

74.  Intermolecular Forces  Dipole-Dipole Forces  LDF

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

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

77.  Covalent-Network Solid  Ionic Solids  Metallic Solids

78.  None

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

80.  42, 54, 55, 66,

81. Reaction Rates

82.  Reaction Rate  Rate Law  Rate Constant

83.  Reaction Order  Overall Reaction Order  First Order Reaction  Second Order Reaction

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

85.  Elementary Reaction  Molecularity  Intermediate  Rate Determining Step

86.  Catalyst

87.  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

88.  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.

89.  32, 51, 62, 67, Free response question 3.

90. Equilibrium

91.  Chemical Equilibrium  Equilibrium constant expression  Equilibrium constant

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

93.  K p = K c (RT) Δn

94.  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.

95.  26, 30, 60, Free response question 1

96. Acids and Bases and Solubility Equilibria

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

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

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

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

102.  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

103.  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

104.  40, 45, 56, Free response 1 e and f.

105. Electrochemistry

107.  Half-Reactions

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