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AP Chemistry > Final AP Test Review > Flashcards

Final AP Test Review Flashcards

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1
Q

distillation: the action of …a liquid by a process of … and …

A

purifying; heating; cooling

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2
Q

law of definite proportions: a given compound always contains the same

A

proportions of elements by mass

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3
Q

law of multiple proportions: when two elements form a series of compounds,, the ratios of the masses of the second element that combine with one gram of the first element can always be reduced to

A

small whole numbers

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4
Q

at the same conditions of temperature and pressure, equal volumes of different gases contain the same

A

number of particles

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5
Q

mass spectrometry is an analytic technique that utilizes the degree of deflection of charged particles by a magnetic field to find the relative masses of

A

molecular ions and fragments

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6
Q

mass spectrometry can be used to determine: …, the … of an unknown substance, and info on ….

A

molecular mass; structure; isotopic abundance

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7
Q

when wavelength increases, … and … decrease

A

frequency; energy

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8
Q

wavelength is the … between two

A

distance; adjacent peaks of waves

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9
Q

frequency is the … that pass a …

A

number of waves; given point per second

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10
Q

excited electrons in an atom return to

A

lower energy states

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11
Q

energy is emitted in the form of a

A

photon of definite wavelength

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12
Q

orbitals are areas of ….

A

probability for locating electrons

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13
Q

heisenberg uncertainty principle: “there is a fundamental limitation on how precisely we can know both the … and … of a particle at a given time”

A

position; momentum

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14
Q

principal quantum number indicates the … from the nucleus

A

distance

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15
Q

angular momentum quantum number (l): varies from … to …. and indicates the … of the orbitals

A

0 to n-1; shape

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16
Q

magnetic quantum number (ml): varies from … to …, and indicates the … of the orbital in space

A

l to -l; orientation

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17
Q

spin quantum number: an orbital can hold only … electrons, and they must have …

A

two electrons; opposite spins

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18
Q

pauli exclusion principle: in a given atom no two electrons can have the

A

same set of four quantum numbers

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19
Q

aufbau principle: electrons fill the lowest available

A

energy levels before filling higher levels

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20
Q

hund’s rule: every orbital in a subshell is singly occupied with one electron before

A

any one orbital is doubly occupied

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21
Q

electron affinity: the energy change associated with the

A

addition of an electron

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22
Q

lattice energy: the energy required to … a mole of an ionic solid into

A

separate; gaseous ions

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23
Q

VSEPR model: the structure around a given atom is determined principally by minimizing ….
non-bonding and bonding electron pairs will be as ….

A

electron-pair repulsions; far apart as possible

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24
Q

hybridization: the mixing of two or more atomic orbitals of similar energies on the same atom to produce

A

new orbitals of equal energies

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25
Q

molecular orbital model: molecular orbitals can hold two electrons with …, explains why O2 is …

A

opposite spins; paramagnetic

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26
Q

paramagnetism: associated with

A

unpaired electrons

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27
Q

diamagnetism: associated with

A

paired electrons

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28
Q

surface tension: the resistance of a liquid to an increase in its …, high surface tensions are due to …. intermolecular forces

A

surface area; strong

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29
Q

capillary action: … forces between molecules of the same substance vs. … forces for molecules of different substances

A

cohesive; adhesive

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30
Q

viscosity: measure of a liquid’s resistance to …

A

flow

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31
Q

viscosity increases with … and …

A

intermolecular forces; molecular size

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32
Q

substitutional alloys: host metal atoms are … in the lattice by other atoms of …

A

replaced; similar size

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33
Q

interstitial alloys: holes in the closest packed metallic structure are filled by …

A

small atoms

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34
Q

vapor pressure: pressure at which the rate of … equals the rate of …

A

condensation; evaporation

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35
Q

vapor pressure increases with … and decreases with … intermolecular forces

A

temperature; stronger

36
Q

for heating cooling curves, steeper slopes mean smaller

A

specific heats

37
Q

for heating cooling curves, the length of the constant lines: longer means more … is needed
it is harder to … than to …

A

energy; boil; melt

38
Q

graham’s law of effusion:

A

rate1 √M2
——- = ——–
rate 2 √M1

39
Q

tB
— =
tA

A

√Ma

40
Q

(steps in solution formation) ΔH1: expanding the …
ΔH2: expanding the …
ΔH3: interaction of … and … to form the solution

A

solute; solvent; solute and solvent

41
Q

Rate= …

A

Δ[A]/Δt

42
Q

heterogenous catalysis steps:

  1. … and … of the reactants
  2. …. of the adsorbed reactants on the surface
  3. … of the adsorbed substances
  4. …., or desorption, of the products
A

adsorption; activation; migration; reaction; escape

43
Q

specific heat capacity: energy required to raise the

A

temp of 1g of a substance by 1 degree C

44
Q

second law of thermodynamics: in any spontaneous process there is always an

A

increase in the entropy of the universe

45
Q

ΔG=

A

ΔH - TΔS

46
Q

when both ΔH and ΔS are negative, the reaction is spontaneous if temperatures are

A

low

47
Q

when both ΔH and ΔS are positive, the reaction is spontaneous if temps are

A

high

48
Q

ΔG= ΔG∘ +

A

RTlnQ

49
Q

ΔG∘ =

A

-RTlnKeq

50
Q

ΔE=

A

q + w

51
Q

henry’s law: the amount of a gas dissolved in a solution is directly proportional to the

A

pressure of the gas above the solution

52
Q

the solubility of a solid is … if the solution already contains ions …

A

lowered; common to the solid

53
Q

effective buffer concentrations range from

A

.1 to 1.0 M

54
Q

Nernst equation:

A

E= E∘ - .0591/n * logQ

55
Q

(synthesis reactions)

metal oxide + h20 –>

A

metallic hydroxide

56
Q

(synthesis reactions) nonmetal oxide + water –>

A

nonbinary acid

57
Q

(synthesis reactions)

metal oxide + nonmetal oxide –>

A

nonbinary salt

58
Q

(decomposition reactions)

metallic hydroxide –>

A

metal oxide + water

59
Q

(decomposition reactions) nonbinary acid →

A

nonmetal oxide + water

60
Q

(decomposition reactions) nonbinary salt →

A

metal oxide + nonmetal oxide

61
Q

(decomposition reactions) metallic chlorates →

A

metallic chlorides + oxygen

62
Q

(decomposition reactions) electrolysis decomposes compounds into

A

elements

63
Q

(decomposition reactions) metallic carbonates →

A

metal oxides + CO2

64
Q

(decomposition reactions) ammonium carbonate →

A

ammonia, water, CO2

65
Q

factors that increase the rate of reactions:

A

increasing concentration of reactants, increasing temperature, catalysts, increasing surface area

66
Q

a precipitate will form when Q is … than Ksp

A

greater than

67
Q

anode: …, electrons flow … from it

A

oxidation; away

68
Q

cathode: …., electrons flow … it

A

reduction; towards

69
Q

electrolysis involves forcing a current through a cell to produce a chemical change or which the cell potential is

A

negative

70
Q

covalent network: atoms/molecules at …, covalent bonds between all particles, …/…, very high relative … and …
e.g.: …

A

lattice sites; hard/brittle; melting and boiling pts; SiO2

71
Q

MX3:

A

trigonal planar

72
Q

MX2E:

A

bent

73
Q

MX4:

A

tetrahedral

74
Q

MX3E:

A

trigonal pyramidal

75
Q

MX2E2:

A

bent

76
Q

MX5:

A

trigonal bipyramidal

77
Q

MX4E:

A

seesaw

78
Q

MX3E2:

A

t-shaped

79
Q

MX2E3:

A

linear

80
Q

MX6:

A

octahedral

81
Q

MX5E:

A

square pyramidal

82
Q

MX4E2:

A

square planar

83
Q

Kp=

A

Kc(RT)^Δn

84
Q

binary acids become … as you go down a group due to increasing … and …. across a period due to increasing …

A

stronger; size; stronger; electronegativity

85
Q

B + H2O

A

BH+ + OH-

AP Chemistry (24 decks)

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