AP Chemistry Test Review



AP Chemistry Test Review

Besides doing the multiple choice practice tests and free-response questions, you should know/review the following items…

1) Give all answers to 3 sig. figs. when in doubt and label the answer correctly.

2) how to calculate the empirical formula given % composition data…(Rhyme: “% to mass, mass to mole, divide by small, times ‘til whole.”)

3) how to determine the limiting reactant for a reaction

4) Re-memorize the list of strong acids and bases…HF is a weak acid!

5) Re-memorize the ions and their charges

6) Re-memorize the shapes of molecules: sp, sp2, sp3, sp3d, sp3d2

7) be able to draw dot notations to determine if a molecule is polar or nonpolar based on its symmetry

8) know the dot notations/shapes of these common molecules: H2O, CO2, NH3, BF3, O2, N2.

9) how to calculate the % composition by mass of a compound

10) “PTV” PV=nRT MM=dRT/P (Remember the correct units needed for each variable!)

11) mole fraction & partial pressure calculations P1 =XPt

12) Graham’s Law of diffusion…given on the AP Equation Sheet

13) q=mc∆T

14) Hess’s Law

15) ∆Hrxn= ∆Hf products – ∆Hf reactants…a pure element has no ∆Hf

16) Periodic trends: atomic radius of atoms vs. ionization energy vs. electron affinity

17) calculate formal charges

18) ∆Hrxn= energy of bonds broken – energy of bonds formed

19) sigma vs. pi bonds

20) bond order calculation

21) odd # of electrons or 12 or 16 electrons are paramagnetic

22) determining the intermolecular forces in a molecule…L.D. dip-dip, H-bonds

23) interpreting phase diagrams

24) ∆T= K*m*i

25) determining the Rate Law based on lab data

26) graphs of 0, 1st, and 2nd order rate laws…[A], ln[A], 1/[A] vs. time

26) Units on the rate constant, k

27) energy “hill” diagrams…finding A.E., ∆H, effect of catalysts.

28) determine the intermediate or catalyst in a multi-step mechanism

29) Keq expressions…products/reactants…only (g) or (aq) appear!

30) Remember that K doesn’t change unless the temperature changes!

31) Le Chatlier’s principle…(+) or (-) heat; ∆P; ∆V; (+) or (-) reactants and products; inert gases have no effect.

32) Q>K…the reaction goes backwards to the reactants

33) for Ksp, Q>K means a precipitate will form (see topic #45)

34) Calculate K by doing ICE box problems

35) acid/base definitions…Bronsted-Lowry = acids donate protons; Lewis= acids accept e- pair

36) calculate pH, pOH, [H+], [OH−]

37) acid equilibrium problems…ICE box…remember pH can be used to find [H+].

38) salt pH…example: Na2CO3 = slightly basic; Al(NO3)3 = slightly acidic

39) more O’s in the oxy-acid means easier to lose the H+, therefore it is a stronger acid

40) salts made of metals in the d-block that have multiple charges are usually colorful solutions

41) common ion effect…less likely to ionize or dissolve

42) NaHCO3 is baking soda and releases CO2(g) in most reactions.

43) use H-H to solve buffer problems

44) acid base titrations MV=MV at equilibrium…be careful with Ba(OH)2 …you get 2[OH-] when in solution

45) AB2(s) ⇓⋄ A+(aq) + 2B-(aq) Ksp= [A][B]2 and Ksp = (x)(2x)2 when setting up an ICE box.

46) know the signs for ∆S, ∆G, and ∆H and when each of the values are zero

47) spontaneous reactions have −∆G or + E°cell

48) ∆G° = zero for pure elements in their standard state

49) LEO- ANO; CPR-GER…how to balance redox reactions and find ox. agents or red. agents

50) calculate E°cell and be able to use the Nernst equation if not at standard conditions.

51) Electrolysis only switches the sign of the cathode and anode.

52) calculate grams or time doing a conversion problem from amps and time and 96500 C/mole e-

53) organic names of –ane, -ene, -yne, alcohols (-ol), ketones (-one), etc. (See “quickie review sheet”)

54) draw an isomer…same formula, but a different arrangement of the atoms

55) types of radioactive particles and their symbols: α, β, γ , protons, neutrons…(See “quickie review sheet”)

56) balance nuclear reactions…top and bottom #’s must be balanced on each side of the equation.

Other Stuff: 1) I suggest that you look over your AP Equations Sheet to re-familiarize yourself with what formulas and constants are given. 2) Look over the “Writing and Predicting Chemical Reactions” review sheet. The more reactions you practice, the better you will do, and the faster you will get. My website has a link of tons of old chemical equations to complete from previous AP tests. 3) Look over the “Colors” review sheet. There’s an interactive quiz on my website that you can do for practice problems. 4) Use my website links for many more helpful hints and strategies to use.

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