Final AP Test Review Flashcards

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
molecular orbital model: molecular orbitals can hold two electrons with ..., explains why O2 is ...
opposite spins; paramagnetic
26
paramagnetism: associated with
unpaired electrons
27
diamagnetism: associated with
paired electrons
28
surface tension: the resistance of a liquid to an increase in its ..., high surface tensions are due to .... intermolecular forces
surface area; strong
29
capillary action: ... forces between molecules of the same substance vs. ... forces for molecules of different substances
cohesive; adhesive
30
viscosity: measure of a liquid's resistance to ...
flow
31
viscosity increases with ... and ...
intermolecular forces; molecular size
32
substitutional alloys: host metal atoms are ... in the lattice by other atoms of ...
replaced; similar size
33
interstitial alloys: holes in the closest packed metallic structure are filled by ...
small atoms
34
vapor pressure: pressure at which the rate of ... equals the rate of ...
condensation; evaporation
35
vapor pressure increases with ... and decreases with ... intermolecular forces
temperature; stronger
36
for heating cooling curves, steeper slopes mean smaller
specific heats
37
for heating cooling curves, the length of the constant lines: longer means more ... is needed it is harder to ... than to ...
energy; boil; melt
38
graham's law of effusion:
rate1 √M2 ------- = -------- rate 2 √M1
39
tB --- = tA
√Mb ------ √Ma
40
(steps in solution formation) ΔH1: expanding the ... ΔH2: expanding the ... ΔH3: interaction of ... and ... to form the solution
solute; solvent; solute and solvent
41
Rate= ...
Δ[A]/Δt
42
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
adsorption; activation; migration; reaction; escape
43
specific heat capacity: energy required to raise the
temp of 1g of a substance by 1 degree C
44
second law of thermodynamics: in any spontaneous process there is always an
increase in the entropy of the universe
45
ΔG=
ΔH - TΔS
46
when both ΔH and ΔS are negative, the reaction is spontaneous if temperatures are
low
47
when both ΔH and ΔS are positive, the reaction is spontaneous if temps are
high
48
ΔG= ΔG∘ +
RTlnQ
49
ΔG∘ =
-RTlnKeq
50
ΔE=
q + w
51
henry's law: the amount of a gas dissolved in a solution is directly proportional to the
pressure of the gas above the solution
52
the solubility of a solid is ... if the solution already contains ions ...
lowered; common to the solid
53
effective buffer concentrations range from
.1 to 1.0 M
54
Nernst equation:
E= E∘ - .0591/n * logQ
55
(synthesis reactions) | metal oxide + h20 -->
metallic hydroxide
56
(synthesis reactions) nonmetal oxide + water -->
nonbinary acid
57
(synthesis reactions) | metal oxide + nonmetal oxide -->
nonbinary salt
58
(decomposition reactions) | metallic hydroxide -->
metal oxide + water
59
(decomposition reactions) nonbinary acid →
nonmetal oxide + water
60
(decomposition reactions) nonbinary salt →
metal oxide + nonmetal oxide
61
(decomposition reactions) metallic chlorates →
metallic chlorides + oxygen
62
(decomposition reactions) electrolysis decomposes compounds into
elements
63
(decomposition reactions) metallic carbonates →
metal oxides + CO2
64
(decomposition reactions) ammonium carbonate →
ammonia, water, CO2
65
factors that increase the rate of reactions:
increasing concentration of reactants, increasing temperature, catalysts, increasing surface area
66
a precipitate will form when Q is ... than Ksp
greater than
67
anode: ..., electrons flow ... from it
oxidation; away
68
cathode: ...., electrons flow ... it
reduction; towards
69
electrolysis involves forcing a current through a cell to produce a chemical change or which the cell potential is
negative
70
covalent network: atoms/molecules at ..., covalent bonds between all particles, .../..., very high relative ... and ... e.g.: ...
lattice sites; hard/brittle; melting and boiling pts; SiO2
71
MX3:
trigonal planar
72
MX2E:
bent
73
MX4:
tetrahedral
74
MX3E:
trigonal pyramidal
75
MX2E2:
bent
76
MX5:
trigonal bipyramidal
77
MX4E:
seesaw
78
MX3E2:
t-shaped
79
MX2E3:
linear
80
MX6:
octahedral
81
MX5E:
square pyramidal
82
MX4E2:
square planar
83
Kp=
Kc(RT)^Δn
84
binary acids become ... as you go down a group due to increasing ... and .... across a period due to increasing ...
stronger; size; stronger; electronegativity
85
B + H2O
BH+ + OH-