Free Webs



AP Chem Unit 4: Intermolecular Forces (Tro Chapters 9-12)

Key Concepts and Definitions

Types of bonds, valence e-, ionic Lewis models, lattice E, covalent bonding, bond strength, bond length, electronegativity and covalent bonds, dipole moment, % ionic character, resonance, resonance structures, resonance hybrid, formal charge, exceptions to Lewis model, using FC to determine stability, bond E (breaking +, forming -), VSEPR, e- group, electron geo. vs molecular geo., effect of lone pairs on geo., bond angles, polarity, hybridization, molecular orbital theory, solid, liquid, gas, intermolecular forces (dispersion/dipole-diploe/H-bonding/ion-dipole), vapor pressure, dynamic equilibrium, volatile v. nonvolatile, boiling pt, normal boiling pt, soln, solute, solvent, entropy, miscibility, soln equil., saturate/unsaturated/supersaturated, soln conc, dilute/concentrated

Be able to Determine/Calculate/Know

FC=#val e- - (#nonbond e- + ½ # bond e-)

ΔHrxn=Σ(ΔH all bonds broken) + Σ(ΔH all bonds formed)

Polarity of molecular shape

IMF v. surface tension/viscosity/capillary action(cohesion/adhesion)/boiling pt/solubility

Rate of evap v. temp/surface area/IMF

Change in phase v. endo/exo ΔH

Heating curves

Soln formation v endo/exo ΔH

Like dissolves like, ΔHsoln = ΔHsolute + ΔHsolvent + ΔHmix

ΔHhydration (it’s in the book, you read about it)

Solubility v. temp/

Molarity/mol fraction/mol %

Problems

Ch 9 RQ #3, 6, 11-15, 19-22, 26-28, 31-39, 43-45, 48-60, 63-65, 72, 75, 78, 82, 85-87, 91, 98-99, 114, 119 pg 418 - 423

Ch 10 RQ #3-9, 15-17, 27, 30, 33-35, 43-44, 47-48, 51, 67, 77, 80, 87-92, 109-111 pg 474-480

Ch 11 RQ #10, 15-19, 22-32, 49, 54, 60-62, 67, 72, 79-80, 84, 94 pg 535-539

Ch 12 RQ #5, 7, 10-14, 26, 29, 33, 35, 43, 46, 48, 61a, 134-135 pg 588-594

AP Chem Unit 1: General Chemistry (Tro Chapters 1 – 5)

Key Concepts and Definitions

Physical change vs. Chemical change sigfigs accuracy vs. precsision error subatomic part. chem. symbols isotope mass # vs. ave. atomic mass ion mol Avogadro’s # molar mass ionic vs covalent nomenclature percent comp. types of rxn

chemical formula/empirical form./molec. form./ structural form. balancing eqns stoich.

LR/% Yield/Actual Yield soln molarity electrolyte vs nonelectrolyte solubility ppt rxn molec. eqn/complete ionic eqn/net ionic eqn spectator ion acid-base rxn gas-evol rxn polyprotic acid salt titration equivalence pt indicator redox rxn oxidation vs reduction oxidation state pressure Boyle’/Charles’s/Avogadro’s/Dalton’s ideal gas law molar vol. STP vapor pressure kinetic molec. theory mean free path diffusion vs. effusion Graham’s Law van der Waals

Be able to Determine/Calculate/Know

density, K (( ˚C, metric conv., mass #, complete chem. symb, #e-, p+, no, predict ion, ave atom. mass, % abund., molar mass, molar conv, chem. form. (( name, emp. form., molec. form., predict rxn prod., LR, stoich., % yield, M, M1V1=M2V2, solubility, ox. state w/in cmpd, redox rxn, P conv, use gas laws, root mean sq veloc., rate of effusion

Problems

Ch 1. Review Questions 35-36, 41-60, 68, 73-88 pg 37-40

Ch 2. Review Questions 41-42, 47-48, 51-54, 57-58, 71-86 pg 80-82

Ch 3. Review Questions 23-32, 37-54, 59-62, 65-66, 71-72, 79-84, 87-88, 99-110, 125-126, 131-132 pg 130-135

Ch 4. Review Questions 25-30, 35-44, 49-98, 101-102, 108, 116, 119-120, 136-138 pg 186-192

Ch 5. Review Questions 29-38, 43-46, 48-54, 57-58, 61-62, 65-68, 71-72, 77-78, 81-82, 85-90, 97, 102, 107, 139, 143-145 pg 238-244

AP Chem Unit 2: Thermochemistry (Tro Chapters 6 and 17)

Key Concepts and Definitions

energy, work, heat, KE, PE, chemical energy, conservation of energy, system, surroundings, units of E, state function, ΔEsys=-ΔEsurr., sign convention for q w and ΔE, identify change in q w and ΔE relative to a system, heat capacity (C), specific heat capacity (Cs), calorimetry, pressure-vol. work, enthalpy (H), endothermic rxn vs. exothermic rxn, intensive properties vs. extensive properties, constant-P calorimetry, Hess’s Law, standard heat of formation, enthalpy (H), entropy (S), entropy v. phases, Gibbs free energy (ΔG), spontaneous = -ΔG, effect of ΔH/ΔS, and T on spontaneity, standard state (ΔS˚/ΔG˚),

Be able to Determine/Calculate/Know

KE=mv2, ΔE=Eprod-Ereact. (ΔE=Efinal-Einitial), ΔE=q+w, q=mCsΔT, qsoln=msolnCs,solnΔT, qmet.=-qH2O, mmetalCs,metalΔTmetal=-mH20Cs,H2OΔTH2O, w=-PΔV, ΔH as conv. factor, qsoln=msolnCs,solnΔT, qrxn=-qsoln, ΔH/n, ΔHrxn=ΔH1+ΔH2+ΔH3, ΔH˚rxn=ΣnpΔH˚f(prod)-ΣnrΔH˚f(react), ΔG=ΔH-TΔS

ΔS˚rxn=ΣnprodS˚prod - ΣnreactS˚react, ΔG˚rxn=ΔH˚rxn-TΔS˚rxn, ΔG˚rxn=ΣnprodG˚prod - ΣnreactG˚react

Problems

Ch 6 RQ #8, 10, 11, 12, 14, 15, 21, 23, 25, 33-34, 37-38, 41-42, 45-50, 55-60, 65-66,

75-84, 87-88, 99-100, 113-114, 123, 128, 131, 136, 138 pg 287-293

Ch 17 RQ #6, 13, 16, 27-32, 37-38, 43-44, 49-50, 57-58, 67-68, 79-84, 107-113 pg 852-858

AP Chem Unit 3: Quatum #’s and Periodicity (Tro Chapters 7-8)

Key Concepts and Definitions

electromagnetic radiation, photon, pulse, photoelectric effect, EMS, Bohr model of an atom, Heisenburg uncertainty principle, Coulombic force, 4 quantum numbers, e- config., aufbau Pauli Hund’s, Coulomb’s Law, shielding, effective nuclear charge, valence e-,

periodic trends in atomic radius effective nuc. charge ionization E electronegativity e-affinity

Be able to Determine/Calculate/Know

E=(hc)/λ, E=hv, #photons=Epulse/Ephoton, n ℓ mℓ ms,

Problems

Ch 7 Rev Quest #6, 7, 10, 11, 14, 23, 45, 51, 57, 69, 70, 80, 85, 103, 104 pg 329-333

Ch 8 Rev Quest #8, 9, 17, 20, 21, 25, 27, 28, 30, 31, 35, 36, 41, 42, 50, 55, 65, 67, 78, 85, 87-91, 131 pg 374-379

................
................

In order to avoid copyright disputes, this page is only a partial summary.

Google Online Preview   Download