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CH186—General Chemistry II > Final Exam > Flashcards

Final Exam Flashcards

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1
Q

4 types of IMFs

A

Van der Waals

  • dipole-dipole
  • dispersion
  • hydrogen bonds

Other

  • ion-dipole
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2
Q

dipole-dipole

A

attraction between polar molecules

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3
Q

hydrogen bonds

A

H bound to N, O, F

subset of dipole-dipole

H acquires highly positive charge

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4
Q

dispersion forces

A

result from instantaneous dipoles & induced dipoles

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5
Q

IMF present in all molecules

A

dispersion forces

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6
Q

what kinds of molecules have stronger dispersion forces?

A

larger

linear

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7
Q

ion-dipole interactions

A

ions interacting with neutral polar molecules

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8
Q

determines magnitude of ion-dipole interactions

A

cations are stronger

ions with smaller nuclei are stronger

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9
Q

cohesion

A

attraction of molecules to one another

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10
Q

adhesion

A

attraction of molecules to another surface

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11
Q

1 atm = ____ torr

A

760

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12
Q

4 types of crystals

A

ionic

covalent

molecular

metallic

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13
Q

properties of ionic crystals

A

hard, brittle, high MP, poor conductor, often white/grainlike

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14
Q

properties of covalent crystals

A

hard, brittle, high MP, poor conductor

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15
Q

properties of molecular crystals

A

soft, low MP, poor conductors

more likely to be organic

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16
Q

properties of metallic crystals

A

strong, malleable, good conductors, variable MPs

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17
Q

substance exists in equilibrium of all 3 phases

A

triple point

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18
Q

equilibrium between liquid and gas terminates

A

critical point

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19
Q

3 phase change curves

A
  • Melting curve
  • Vapor pressure curve
  • Sublimation curve
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20
Q

state functions (9)

A

mass

pressure

temperature

volume

particle number

entropy

enthalpy

Gibbs free energy

internal energy

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21
Q

C + ___ = K

A

273

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22
Q

(+) Gibbs means…

A

non-spontaneous

endergonic

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23
Q

(-) Gibbs means…

A

spontaneous

exergonic

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24
Q

standard conditions (6)

A
  • 1 atm
  • 1.00 M
  • pH 7 (biological)
  • 25° C
  • Pure solids & liquids
  • Most stable allotropic form of elements at std conditions
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25
Q

3 laws of TD

A
  1. Energy cannot be created or destroyed, only transduced (changed)
  2. The total entropy of the universe is always increasing
  3. The entropy of a perfect crystalline substance is zero at 0° K (absolute zero)
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26
Q

S° ↑ with… (5)

A

molar mass & molecular complexity, temperature, volume, and when a reaction produces more gas molecules than it consumes

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27
Q

overall reaction order =

A

sum of exponents in the rate law

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28
Q

order of a reaction depends on…

A

concentration of reactants only

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29
Q

elementary reaction

A

single collision of reactant molecules

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30
Q

intermediates

A

species that appear in the mechanism, but not in the products or reactants

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31
Q

molecularity

A

number of reactant molecules involved in the collision

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32
Q

rate-determining step

A

slowest step in the sequence

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33
Q

Rate-determining step must have…

A

the same rate law as that determined by experimental data for the overall reaction

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34
Q

heterogeneous catalyst

A

reactants & catalysts are in different phases

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35
Q

homogeneous catalyst

A

reactants & catalysts are in the same phase - usually in solution

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36
Q

If Kc >> 1, then equilibrium…

A

lies to the right

𝚫G° is negative

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37
Q

If Kc << 1, then equilibrium…

A

lies to the left

𝚫G° is positive

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38
Q

If Kc is between ___ and ___ , product concentration roughly equals reactants’

A

0.01 and 100

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39
Q

Law of mass action

A

Kc = Qc at equilibrium

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40
Q

If Qc > Kc…

A

reactants favored

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41
Q

If Kc > Qc…

A

products favored

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42
Q

In the Kp equation, 𝚫n =

A

moles gaseous product - moles gaseous reactant

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43
Q

If you reverse the reaction, Kc…

A

becomes 1/Kc = Kc*

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44
Q

If you multiply the equation, Kc…

A

is raised to the power of what you multiplied by

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45
Q

if you divide the reaction, Kc…

A

the root of the divisor is taken on Kc

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46
Q

if you add 2 reactions, the Kc’s…

A

are multiplied together

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47
Q
  • Increase [reactants] =
  • Increase [products] =
  • Decrease [reactants] =
  • Decrease [products] =
A
  • Increase [reactants] = Q < K, shift to right
  • Increase [products] = Q > K, shift to left
  • Decrease [reactants] = Q > K, shift to left
  • Decrease [products] = Q < K, shift to right
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48
Q
  • Decrease volume =
  • Increase volume =
  • Decrease pressure =
  • Increase pressure =
  • 𝚫 in pressure or volume =
  • Adding an inert gas to the reaction at fixed volume & pressure =
A
  • Decrease volume = shift to side with fewer particles
  • Increase volume = shift to side with more particles
  • Decrease pressure = shift to side with more particles
  • Increase pressure = shift to side with fewer particles
  • 𝚫 in pressure or volume = no change if both sides have equal particle number
  • Adding an inert gas to the reaction at fixed volume & pressure = no change
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49
Q
  • Increase heat in an exothermic rxn =
  • Decrease heat in an endothermic rxn =
  • Increase heat in endothermic rxn =
  • Decrease heat in endothermic rxn =
A
  • Increase heat in an exothermic rxn = shift to left
  • Decrease heat in an endothermic rxn = shift to right
  • Increase heat in endothermic rxn = shift to right
  • Decrease heat in endothermic rxn = shift to left
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50
Q

amphoteric

A

acts as acid or base

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51
Q

Kw =

A

Kw = [H3O][OH] = 10-14 @ 25° C

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52
Q

Hydrohalic acid strength

A

HF << HCl < HBr < HI

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53
Q

oxoacids

A

contain H, O and a central nonmetal atom

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54
Q

examples of oxoacids

A

Chloric acid HClO3; bromic acid HBrO3; carbonic acid H2CO3; nitrous acid HNO2; nitric acid HNO3; phosphorous acid H3PO3; phosphoric acid H3PO4; sulfuric acid H2SO4

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55
Q

more oxygen in an oxoacid =

A

stronger acid

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56
Q

more electronegative central atoms in an oxoacid =

A

stronger acid

57
Q

carboxylic acids

A

include C bound to 2 O and an R group

58
Q

examples of strong acids

A
  • Hydrochloric acid HCl
  • Hydrobromic acid HBr
  • Hydroiodic acid HI
  • Nitric acid HNO3
  • Chloric acid HClO3
  • Perchloric acid HClO4
  • Sulfuric acid H2SO4
59
Q

examples of strong bases

A
  • Group 1A hydroxides
    • LiOH
    • NaOH
    • KOH
    • RbOH
    • CsOH
  • Group 2A hydroxides
    • Ca(OH)2
    • Sr(OH)2
    • Ba(OH)2
60
Q

Percent ionization =

A

100([H3O]eq / [HA]0)

61
Q

larger Ka =

A

stronger acid

62
Q

lewis acid

A

accepts pair of electrons

63
Q

lewis base

A

donates pair of electrons

64
Q

when can the H-H equation no longer be used?

A

at the equivalence point and beyond

65
Q

to find a suitable buffer…

A

find an acid w/ pKa within a unit of the pH

66
Q

“acid + base → …….”

A

salt + water

67
Q

not included in Ksp equation

A

solids

68
Q

molar solubility:

mass solubility:

A

mol/L (M)

g/L

69
Q

what does common ion effect have on the ICE table?

A

changes the initial value of the ion present in the “other” solution

the spectator ion doesn’t matter

70
Q

oxidation

A

loss of e-

71
Q

reduction

A

gain of e-

72
Q

charge of H with a nonmetal

A

positive

73
Q

charge of H with a metal

A

negative

74
Q

oxidation state rule about oxygen

A

usually 2-, except in molecules with O-O bonds

75
Q

elements in bottom left corner more likely to have ___ charge

A

positive

76
Q

11 oxidation state rules

A
  1. 0 charge in substance with atoms of one element
  2. simple ions’ charge is their OS
  3. H+ with a nonmetal
  4. H- with a metal
  5. Group 1A = 1+
  6. Group 2A = 2+
  7. Oxygen usually 2-, except in O-O molecules
  8. Group VIIA = 1-
  9. sum of OS in neutral compound is 0
  10. sum of states in polyatomic ion is that ion’s charge
  11. elements in bottom left more likely to be +
77
Q

10 steps to balance redox rxns

A
  1. split into ½ reactions
  2. balance all atoms except O and H
  3. balance O with H2O
  4. balance H with H+
  5. balance charge with e-
  6. (bases) balance H+ with OH- on BOTH sides
  7. (bases) combine H+ with OH- to form water
  8. cancel all e- via multiplication
  9. combine equations - cancel anything you can
  10. check charges & balancing
78
Q

cell notation

A

(anode reactant) | (anode product) || (cathode reactant) | (cathode product)

79
Q

cell potential

A

Ecell

80
Q

E =

(redox)

A

electron motive force

81
Q

cathode

A

reductive process

gain of electrons

becoming more negative

82
Q

anode

A

oxidative process

loss of electrons

becoming more positive

83
Q

rule about Ecell under std conditions

A

must be +

84
Q

E of H2

A

0 V

85
Q

strongest reducing agents are…

strongest oxidizing agents are…

A

most negative anodes

most positive cathodes

86
Q

n (electrochem) =

A

moles of electrons transferred

87
Q

3-way relationship in electrochem

A

E° — 𝚫G° — K

88
Q

if we are setting up a galvanic cell, we want E° to be…

A

positive (spontaneous)

89
Q

used for non-std conditions in galvanic cells

A

Nernst equations

90
Q

2 types of Nernst equations

A

2 for non-std temp (involving RT)

1 for std temp (omits RT)

91
Q

to find variables for Nernst equation…

A

find ½ reactions

use E° values given for each

balance to find n (electrons transferred)

use [products]/[reactants] to find Q (omitting water)

92
Q

if Q > 1, E __ E°

A

E < E°

93
Q

if Q < 1, E __ E°

A

E > E°

94
Q

radioactivity

all ___ elements

A

spontaneous emission of particles or electromagnetic energy

elements >83

95
Q

proton symbol

A

1/1 P

1/1 H

96
Q

neutron symbol

A

1/0 n

97
Q

electron symbol

A

0/-1 e

0/-1 B

98
Q

positron symbol

A

0/+1 e

99
Q

alpha particle symbol

A

4/2 a

(He)

100
Q

top number in notation for subatomic particles

A

mass #

101
Q

bottom number in notation for subatomic particles

A

atomic #

102
Q

“belt of stability”

A

stable nuclei - 2, 8, 20, 50, 82, 126 protons/neutrons

103
Q

4 types of nuclear decay

A

beta emission

electron capture

positron emission

alpha decay (releases He)

104
Q

gamma radiation

A

emits photons

105
Q

notation for nuclear transmutation

A

14/7 N + 4/2 H → 17/8 O + 1/1 H

14/7N (a, p) 17/8O

parent nucleus (bombarding particle, emitted particle) product nucleus

106
Q

higher E; more likely to be ______

lower E; more likely to be _______

A

reduced

oxidized

107
Q

E of strongest reducing agents

A

more negative

108
Q

E of strongest oxidizing agents

A

more positive

109
Q

“what is the name of a thin film of water contracting and adhering to the wall of a glass cylinder?”

A

capillary action

110
Q

“which of the following has the highest surface tension at a given temp?”

A

two molecules with O by double bonds

111
Q

“location at which two phases can exist in equilibrium”

A

phase boundary

112
Q

what forces hold each type of solid together?

A

ionic crystals: attractions between anions and cations

metallic crystals: IMFs & sharing of electrons throughout

covalent crystals: covalent bonds

molecular crystals: IMFs

113
Q

O – C – O

IMFs

A

dispersion

114
Q

3H - C —— C - 2H - OH

IMFs

A

dispersion

hydrogen bonds

dipole-dipole

115
Q

H —— S — 3Cl

IMFs

A

dispersion

dipole-dipole

116
Q

“highest boiling point”

NH3 or CH4

A

NH3

117
Q

“highest vapor pressure”

A

smaller molecule - C3H8

118
Q

“highest surface tension”

A

CH3COOH

OH group present

119
Q

“order of reaction of decomposition of sulfuryl chloride (SO2Cl2)”

A

first (see units)

120
Q

“for reaction A + 2B → C, which expression is correct?”

A

𝚫[C]/𝚫t = -½𝚫B/𝚫t

121
Q

steps to find rate law given a table of experimental data

A

take initial concentration of one trial divided by another (where other reactant is constant concentration)

take same given initial rates divided by one another

the rate quotient = the concentration quotientx

repeat for other reactant(s)

122
Q

equation to use for finding concentration of dimerizing butadiene after 3 hours

A

integrated rate law for second order rxns

(0.0052 M)

123
Q

number of elementary steps =

A

number of “hills” on the potential energy profile

124
Q

“what will decrease the entropy of an inert gas system?”

A

decreasing volume

125
Q

entropy increases with…

A

more particles

more energy

higher temperature

greater molecular mass

more even distribution of particles among cells

126
Q

what is larger: joule or kilojoule

A

kilojoule

127
Q

joule to kilojoule

A

divide by 1000

128
Q

kilojoule to joule

A

multiply by 1000

129
Q

conjugate base of sulfuric acid?

A

HSO4 -

130
Q

“Kc of decomposition of HI”

A

0.26

131
Q

“concentration of N2 for nitrogen fixation reaction”

A

2.7 M

132
Q

“[H3O] concentration in formic acid”

A

4.2 x 10^-3

133
Q

“Kp of nitric oxide and bromine”

A

134

134
Q

“Ka of butyric acid”

A

1.5 x 10^-5

135
Q

question to go straight to QF after ICE table

[H3O]

A

piric acid in the leather industry

0.15 M

136
Q

“cartoon of weak acid at equilibrium”

“solvent water molecules omitted for clarity”

A

Ka = 10^-3

137
Q

“polyprotic acid malonate ion [] “

A

2 x 10^ -6 M

138
Q

pH of malonic acid problem

A

1.8 (-log0.016)

139
Q

difference between the mass of an atom and the sum of the masses of its constituent nucleons

A

mass defect

CH186—General Chemistry II (6 decks)

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