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, 21, 25, 41, 44, 63,

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

 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.