AP CHEMISTRY EXAM PREP

AP CHEMISTRY EXAM PREP

• Color of solutions: Fe2+: pale green solid
• Color of solutions: Group 1 and 2 solids and solutions: Solids: white, solutions: colorless
• Common spectators:: all group 1 cations, NH4+, Cl- (except AgCl)
• Molar Mass using Ideal gas law:: M=mRT/PV
• Graham's Law of Diffusion and Effusion (formula): rate1/rate2 = sqrt(molar mass2/molar

mass1) ~Heavier particles diffuse slower

• Dalton's law of partial pressures:: Ptotal = P1 + P2 + P3...
• Speed of gases at the same temp:: gases with smaller molar masses are faster
• KE of gases at the same temp:: equal
• Rates of effusion and diffusion at the same temp:: smaller molar mass = faster
• Density of gases at the same temp:: larger molar mass = higher density when volume is

equal

11. 7 Strong Acids: HI, HCl, HBr, HNO3, HClO3, HClO4, H2SO4

12. HNO2: nitrous acid (weak)

13. H2SO3: sulfurous acid (weak)

14. CH3COOH: acetic acid (weak)

15. HF: hydrofluoric acid (weak)

16. H3PO4: phosphoric acid (weak)

17. H3PO3: phosphorous acid (weak)

• 4 pH equations:: 1) pH + pOH = 14

2) pH = -log[H+]

3) 10^-14 = [H+][OH-]

4) pOH = -log[OH-]

19. Bronsted-Lowry acid: proton donor and becomes conjugate base

20. principal quantum number: n=1-7, main energy level

• angular momentum quantum number: l=0 through (n-1), shape of orbital 1 / 2

22. magnetic quantum number: m sub l= -l through l, orientation

23. spin: m sub s= +0.5 through -0.5, spin of e-

24. Lyman series: n=1, ultraviolet

25. Paschen series: n=3, infrared

26. Balmer series: n=2, visible light

27. Aufbau Principle: Always fill lowest energy level first

28. Hund's Rule: E- fill one at a time before pairing

29. Pauli Exclusion Principle: Max 2 e- in an orbital and spinning away

30. metal + nonmetal: salt

31. metal oxide + water: base

32. nonmetal oxide + water: acid

33. acid + base: salt + water

• Atomic Radius: Increases down and decreases across; more p+ in the nucleus (Eff

increases)

• Ionization energy: Increases across and decreases down; energy required to remove

outermost e- from the ground state. ALWAYS forms a cation

• Electron affinity: Increases to the right and up, group 2, 12, and 18 don't have it; the

energy change that happens when an atom gains an e-. ALWAYS forms an anion

• Effective nuclear charge (Zeff=Z-S): Measures how strongly the valence e- are attracted to

the nucleus

38. mL to L: 1000 mL = 1 L

39. mg to g: 1000 mg = 1 g

40. nm to m: 10^9nm=1m

41. Specific heat units: J/gC or J/gK

42. Avogadro's number: 6.022 x 10^23 molecules or particles

• Isotopes are:: atoms of an element with different masses (neutrons)
• Average atomic mass formula:: sum of abundancy x amu = mass on periodic table

45. Light calculations units: hz, s^-1, m

46. Light constants: speed of light and planck's constant (on formula sheet)

• Difference in Ionization energy to remove inner shell e- versus outer shell e-: Each

successive e- is harder to remove-->more p+ are pulling versus the remain- ing e-, and the size shrinks and is closer to the nucleus

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