Download KINETICS (chap 12)

AP CHEMISTRY First Quarter Test:
A mostly complete List of Topics
STOICHIOMETRY and TYPES OF RXNS (chap 3)
Molar mass
Percent composition
Limiting reactant
Solubility and solubility rules
mole fraction
mole ratios
experimental yield
precipitation rxns
empirical formula
theoretical yield
Avogadro's number
net ionic equations
TYPES of CHEMICAL REACTIONS and SOLUTION STOICHIOMETRY (chap 4)
Redox – know the def’s: xidation, reduction, oxidizing agent, reducing agent, oxidation number
Be able to calculate oxidation number.
Be able to determine what species is reduced and oxidized in a chemical reaction
Be able to identify an oxidizing agent and a reducing agent
Be able to write and balance half-reactions
Be able to balance redox reactions
Electrolytes - weak strong and nonelectrolytes
Solute and solvent
molarity
NUCLEAR CHEMISTRY (chap 21)
Nuclear transformation equations
Know the types of radiation, their symbol and the corresponding changes in mass, Y, and atomic number Z. (see
table in course guide)
Know how to predict if a nucleus is stable, {n:p ratio ~1}
ATOMIC STRUCTURE and PERIODICITY (chap 7)
Know energy level diagrams and electron configurations
Differentiate between excited and ground states
Know how to use the Rydberg equation to calculate wavelength and energy levels of excited states
Know the meanings and values of the quantum numbers: n, l, ml, ms
Be able to give the set of quantum numbers for an electron in a specific orbital with a given spin.
Know the trends for atomic radius, Electronegativity and Ionization Energy.
GASES (chap 5)
Laws – Ideal and van der Waal's
Laws – combined, Boyles, Charles, Avogadro's and Gay-Lusaac's
Laws – Grahams Law and urms
Laws – know the dRT/P to get molar mass and density
KMT – Know the assumptions etc. that make a gas an ideal gas vs a real gas
Laws – partial pressure
Laws – Know the equation for KE and know that at constant Temp, KE is constant
Gas stoichiometry – esp using mole ratios or pressure ratios or volume ratios
BONDING (chap 8 and 9)
Be able to calculate the heat of rxn, H, via bond energies
Know the octet rule and when it is violated
Be able to apply Ionization Energies to successive electron removals realizing that when breaking up stability causes
the greatest jump in the given sequence of ionization energies
Calculate the # of valence electrons
Be able to identify a polar vs nonpolar covalent bond, also covalent vs ionic.
Be able to rank polar bonds in increasing polarity (greatest dipole) based on the greatest electronegativity difference
Know how to write/name ionic formulas. Know the names of polyatomic ions.
Be able to draw structures and give the geometry
Understand resonance of electrons in p-orbitals and in -bonds
AP CHEMISTRY First Quarter Test:
A mostly complete List of Topics
Know the bond angles - tetrahedral is 109.5° (also pyramidal, bent), planar (also equatorial for 5 e-pr’s) is120°, square
planar (also equatorial for 6 e-pr’s) is 90°, linear (also axial for 5 and 6 e-pr’s) is 180°
Covalent Bonding : Orbitals (chap 9)
Be able to determine the hybridization state of a central atom
Know the definition of a hybrid orbital
THERMOCHEMISTRY (chap 6, 16)
Know: units for energy, definitions of system and surroundings, and state function
Be able to solve Hess’ Law problems for H, S or G.
Be able to determine which substance has the greater positional entropy.
Know values of P and T at standard conditions (not the same standard Temp as gases)
Definitions of free energy, entropy and enthalpy and what their signs (+ or -) mean for the reaction
Calculate free energy, entropy and enthalpy from the free energy, entropy or enthalpy of formation, Hf
Use G = H - TS, also be able to predict the sign ofG from the sign of H and S
Determine spontaneity from G
Determine exothermic/endothermic from H
Determine spontaneity from G and in turn from E and K.
Be able to calculate/interconvert between G, E and K (remember n = # of moles of e's)
Know paramagnetic vs diamagnetic
LIQUIDS/SOLIDS AND SOLUTIONS (chap 10, 11)
IMF's - know the def and be able to identify the predominant IMF in a molecule
ionic; network covalent; H-bond; dipole-dipole; LD, London Dispersion;
IMF's and relation to boiling point, melting point and vapor pressure.
Types of phase changes
Be able to label and read a heating/cooling curve and a phase diagram
Know the definitions of boiling point and melting point.
Concentration - mass percent; mole fraction ; molarity and molality
Colligative properties – boiling point elevation and freezing point depression by the presence of a solute.
Be able to calculate the change in boiling or freezing point.
Raoult's Law
Know all solubility rules and that ionic compounds dissociate when dissolved.
Apply mole ratios to dissociation equations and calculate the concentration of an ion in solution prior to and following
a precipitation
KINETICS (chap 12)
Rate
rate law
rate constant
Rate determining step
half life
mechanism
Integrated rate laws
overall order
Intermediates
Determining order
-graphically
-from rate data (with and without showing all the work the long way
-from the mechanism (RDS)
Be able to write rate laws and be able to solve for any possible variable.
Know the units of the rate constant.
Be able to calculate the rate of appearance/disappearance of a molecule in a rxn based on another’s rate via mole ratios.
Be able to manipulate the integrated rate law to solve for any variable, particularly time, t.
Know the relationship between activation energy, temperature and the rate constant - Arhenius equation.
AP CHEMISTRY First Quarter Test:
A mostly complete List of Topics
EQUILIBRIUM (chap 13, 15)
Write equilibrium expressions: K, Kp, Ka, Kb, Ksp
Know when products or reactants are favored by the magnitude of K.
Apply le Chatelier's principle – particularly it’s impact on K or the conc of a molecule after an add/loss of another
molecule or a temperature or pressure change.
Be able to use H (heat and temp) in le Chatelier's principle and K.
Solve I.C.E. problems. Also know how to do ICE if your given amounts for two molecules and not just one.
Interconvert between Kp and Kc
Use Q to determine if equilibrium has been achieved or in which direction a shift would have to occur, and the
resulting impact on the concentration of products and reactants.
Apply the common ion effect
Buffers (a good buffer is one that is used at a pH that is less than 1 pH of the pKa of the acid, and is a weak acid with
its conjugate base)
Be able to solve for anything in the Henderson-Hasselbach equation
ACID - BASE (chap 14, 15)
Types of acid/base - Bronsted-Lowry, Arrhenius, Lewis: (Remember Lewis is the opposite of Bronsted-Lowry)
Know formulas of strong acids and bases
Be able to calculate the Ka for either a strong or weak acid/base dissociation
Know the chemical equation for either a strong or weak acid/base dissociation
Be able to calculate the percent dissociation (this is the same as percent ionization)
Know the math to calculate the pH, pOH, [H+] and [OH-]
Be able to predict which molecule is a stronger acid based on Lewis Structure (see the course guide)
Be able to fully apply the Henderson-Hasselbach eq.
Be able to identify what kind of acid/base (weak/strong) is being used in a pH titration curve.
Furthermore, be able to identify the parts of a pH titration curve (see fig 15.1-5)
Be able to use ICE, acid/base dissociation eq’s, mole ratios and molarities to calc the amount of a molecule in solution
after a volume of acid or base has been added. (The text has good ex’s in sec 15.4) [I don’t expect you to do the
whole titration, just after one addition.]
ELECTROCHEMISTRY (chap 17)
Identify the components of a half cell or a voltaic cell, see sec 17.2. (also from the line equations)
oxid at anode; red at cathode (Redcat)
Be able to calc oxid numbers and identify reduction and oxidation
Be able to add half-rxns and E’s to get the overall rxn and E, E°
Nernst Equation
Calculate the cell potential, E
Use standard reduction potentials to write redox rxns from 2 half rxns both written for a reduction and predict the
course of a rxn
Determine spontaneity from G and in turn from E and K.
Balance redox rxns
Be able to calculate/interconvert between G, E and K (remember n = # of moles of e's)
Know what Q is and be able to use it.
Apply Faraday’s law.