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PSU Freshman > Chem 112B Final > Flashcards

Chem 112B Final Flashcards

1
Q

Collision theory

A

The rate of a chemical reaction is proportional to the number of collisions between reactant molecules.
The more often reactant molecules collide, the more often they react with one another, and the faster the reaction rate

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2
Q

In a reaction profile, peaks are… and valleys are…

A

transition states, intermediate states

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3
Q

Reaction energy (ΔE) is

A

the energy of products minus the energy of the rectants

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4
Q

Activation energy (Ea) is

A

the energy needed to get to the peak, can be either TS-reactant or TS-intermediate

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5
Q

In an elementary reaction, the method of initial rates
Rate = k[A]^x{B}^y

A

x and y are the same as a and b

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6
Q

In a multi-step reaction, the exponents

A

must be determined experimentally

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7
Q

Reaction mechanism consists of

A

elementary steps

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8
Q

Rate law is always based on the

A

slowest step

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9
Q

How do I know if a reaction is elementary or not?

A

All reaction steps in a reaction mechanism are elementary

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10
Q

If the first step is the fast step, will it always be an equilibrium reaction?

A

Yes. For fast first step, use equilibrium to solve for concentration of intermediate

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11
Q

1st order integrated rate law

A

plotting ln[A] vs time gives a straight line. Half-life only depends on k

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12
Q

2nd order integrated rate law

A

plotting 1/[A] vs time gives a straight line. Half life depends on both k and [A]0.

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13
Q

Plotting lnk vs 1/T gives a

A

straight line
slope = -Ea/R
y-intercept = lnA

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14
Q

At two different temperatures, we can determine Ea or ratio of k using which two equations

A

lnk = -Ea/RT + lnA
lnk1/k2 = Ea/R [1/T2 - 1/T1]

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15
Q

At a fixed temp, we can use difference in Ea to determine..

A

ratio of k
kcat/kuncat= e (,..)

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16
Q

H-bond donor

A

strongly electronegative atom such as N, O, or F

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17
Q

H-bond acceptor

A

electronegative atom of a neighboring molecule or ion that contains a lone pair

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18
Q

To be phosphorylated, a side chain must

A

contain alcohol or amine group

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19
Q

if the half-life is constant, the order is

A

1st order

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20
Q

Intermediate

A

Produced, then consumed

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21
Q

Catalyst

A

Consumed, then produced

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22
Q

Rate of forward process=

A

Rate of reverse process

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23
Q

For elementary reactions, Keq=

A

kf/kr, where kf are rate constants for the forward and reverse reaction, respectively

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24
Q

K&raquo_space; 1

A

Products predominate

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25
Q

K &laquo_space;1

A

Reactants predominate

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26
Q

Keq for the reverse reaction is the

A

inverse of Keq for the forward reaction

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27
Q

When a reaction has been multiplied by a number, Keq for the new reaction is the

A

original Keq raised to a power of the multiplication factor

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28
Q

If the net reaction can be obtained by the addition of 2 or more steps, Keq is the

A

product of the individual Keq

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29
Q

Q

A

reaction quotient

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30
Q

Q is calculated using…Keq is calculated using…

A

Any concentrations, equilibrium concentrations

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31
Q

Q< Keq

A

Reaction shifts right (produce more products, consume more reactants)

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32
Q

Q > Keq

A

Reaction shifts left (produce more reactants, consume more products)

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33
Q

At equilibrium, added reactants or products will cause the reaction to shift to

A

consume towards to reestablish equilibrium (balance scale)

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34
Q

Add reactants or remove products

A

Reaction shifts right

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35
Q

Remove reactants or add products

A

Reaction shifts left

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36
Q

Since pressure is increased by disturbance, reaction will shift in direction that

A

reduces pressure

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37
Q

Decreasing the volume shifts the reaction to the side with

A

less moles of gas

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38
Q

If a reaction has the same moles of gas on both sides, changing pressure/volume does

A

NOT have any effect on equilibrium

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39
Q

When heat is added to a system at equilibrium, reaction shifts in the direction that

A

absorbs heat

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40
Q

Spontaneity

A

process proceeds in forward direction to an appreciable extent by itself

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41
Q

Free energy of formation at standard conditions can be calculated using

A

ΔG°f = ΔH°f - (298K)ΔS°

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42
Q

Calculate ΔG° at 25°

A

ΔG° = ΔH° - (298K)ΔS°

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43
Q

Calculate ΔG° at temps besides 25°

A

ΔG° = ΔH° - TΔS°
ΔG° = -RTlnK

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44
Q

ΔG > 0, Q > K

A

System is nonspontaneous in forward direction

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45
Q

ΔG < 0, Q < K

A

System is spontaneous in forward direction (system does work)

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46
Q

Endothermic ΔH

A

positive

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47
Q

Exothermic ΔH

A

negative

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48
Q

Molar entropy increases when

A

Gaseous, largest molar mass, most molecular complexity, volume increases, pressure decreases

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49
Q

Increased Kd means

A

Weaker binding

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50
Q

Decrease in entropy of a reaction

A

Decrease is numbers of gaseous or aqueous molecules

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51
Q

Increase in entropy of a reaction

A

Solids dissolve
Endothermic (s->l->g)
Volume increase

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52
Q

7 strong acids

A

HClO4, HI, HBr, HCl, H2SO4, HNO3, HClO3

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53
Q

8 strong bases

A

KOH, LiOH, NaOH, Ca(OH)2, Ba(OH)2, RbOH, Sr(OH)2, CsOH

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54
Q

Group 1A and heavy group 2A hydroxides are

A

strong bases

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55
Q

Amines are

A

weak bases

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56
Q

Carboxylic acids and thiols are

A

weak acids

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57
Q

The conjugate base of a strong acid is

A

a negligible base

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58
Q

The conjugate base of a weak acid is a

A

weak base

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59
Q

For weak acids and bases, the stronger the acid, the

A

weaker its conjugate base

60
Q

Within the same group,

A

larger atoms means stronger acid

61
Q

Within the same period, higher electronegativity means

A

stronger acids

62
Q

The more electrognegative the central atom, he higher the

A

number of oxygen atoms attached, the stronger the acid

63
Q

Non-metal oxides/hydroxides are

A

acidic

64
Q

For pure water,

A

[OH] = [H]

65
Q

Strong acids and strong bases are strong electrolytes, so they

A

dissociate completely in water

66
Q

Larger Ka, smaller pKa

A

Stronger acid

67
Q

Smaller Kb, larger pKb

A

Weak base

68
Q

Addition of a common ion decreases

A

ionization

69
Q

Buffer

A

solution that contains a weak acid and salt of its conjugate base
solution that contains a weak base and salt of its conjugate acid

70
Q

To make/produce buffer

A

Combine weak acid and salt of conjugate base/ vice versa
OR use neutralization to combine excess weak acid with a strong base

71
Q

Optimal pH of a buffer =

A

pKa

72
Q

More concentrated buffer solution has

A

greater capacity

73
Q

Equivalence point is when

A

stoichiometrically equivalent quantities of acid and bASE REACTED

74
Q

At half eq point, pH=

A

pKa

75
Q

Solubility

A

Maximum amount of solid that will dissolve under a given condition, forms a saturated solution

76
Q

If Q > Ksp

A

precipitate will form

77
Q

If Q < Ksp

A

More solid can be dissolved

78
Q

Chelating ligands have

A

two or more donor atoms

79
Q

Larger Kf (more stable) is mostly due to the

A

entropy effect

80
Q

Electrode of a voltaic cell

A

GRedCat, LAnOx

81
Q

Salt bridge of voltaic cell

A

to neutralize excess charges (anions to anode, cations to cathode)

82
Q

External circuit of a voltaic cell

A

e- flow from anode to cathode

83
Q

Oxidizing agent

A

Gains e-, gets reduced

84
Q

Reduction agent

A

Loses e-, gets oxidized

85
Q

The more positive E°red

A

the more spontaneous and one will undergo reaction (at cathode)

86
Q

Determine which electrode is cathode and anode

A
  • Write reduction half rxns,
  • Compare E° red , the more positive (spontaneous) one will undergo reduction (at cathode)
87
Q

Calculate standard cell potential

A
  • Write oxidation and reduction half rxns,
  • E° cell = E° ox + E° red
88
Q

Connect free energy (and work) to cell potential

A
  • ∆G = –nFEcell and ∆G o = –nFE°cell
  • Ecell is (+), ∆G is (–), rxn/process is spontaneous
89
Q

Describe electrolysis and electrolytic cell (Drive nonspontaneous rxns by
applying electrical energy.)

A
  • Consist electrodes in either aqueous solutions or molten salts.
  • Oxidation still at anode, reduction still at cathode.
  • Be able to differentiate voltaic cell and electrolytic cell.
90
Q

Predict products at cathode or anode of electrolytic cell

A
  • Identify all species in solution
  • Write half reactions with species as reactants
  • Compare potentials to predict products
91
Q

Do quantitative calculations involving electrolysis

A
  • Write balanced half reactions
  • Use datasheet conversions for amps, volts, Faradays, etc.
92
Q

Linear combinations of wavefunctions to create molecular orbitals

A
  • Same number of MOs created: bonding and antibonding
  • Each MO holds maximum of 2 electrons
93
Q

Bonding orbitals (lower energy)

A
  • Sigma (σ) : e density on axis
  • Pi (π): e density above and below
  • Subscript of original AO
94
Q

Anti-bonding orbitals (higher energy):

A
  • Node between nuclei
  • Star superscript
95
Q

Fill MOs of diatomic molecules/ions:

A
  • Fill lower MOs first.
  • For degenerate MOs, singly occupy first before doubly up.
96
Q

Predict bond order using MO diagram:

A
  • BO = ½(#BE - #AE)
  • Bond order of zero means substance is very unstable (does not exist)
97
Q

Coordination compound is a

A

neutral compound of the metal complex ion + counter
ion(s)

98
Q

Inside the bracket of the coordination compound is the

A

metal complex (ion),
which has a transition metal cation + ligands covalently bond (coordinated) to it.

99
Q

Outside the bracket is the

A

counter ion(s)

100
Q

The charge of the metal complex =

A

– (total charge of counter ions)

101
Q

In water, coordination compound fully dissociates into

A

the metal complex and counter ions

102
Q

The coordination number of the metal is

A

the number of donor atoms (from the ligand) that are bonded/coordinated to the metal cation

103
Q

Describe metal complex

A
  • Transition metal act as Lewis acids (accept e – pair);
  • Ligands act as Lewis bases (donate e – pair)
104
Q

Crystal field theory

A

Δ = Crystal field splitting energy
Large Δ ->Strong Field -> Low spin
Small Δ -> Weak Field -> High spin

105
Q

Paramagnetic

A

have unpaired electrons

106
Q

Diaamagnetic

A

No unpaired electrons

107
Q

Units of 0 order

A

Ms^-1

108
Q

Units of 1st order

A

s^-1

109
Q

Units of 2nd order

A

M^-1s^-1

110
Q

4 factors that affect reaction rates

A

Inc contact area = faster
Inc concentration = faster
Inc temp = faster
Catalyst lowers Ea = rate faster

111
Q

Small Km,

A

strong binding

112
Q

Inc kCat, small Km,

A

Efficient enzyme

113
Q

Q < Keq

A

Reaction proceeds reverse, more reactant produced

114
Q

Q > Keq

A

Reaction proceeds forward, more product produced

115
Q

Endothermic heat is the

A

reactantE

116
Q

Exothermic heat is the

A

product

117
Q

Kb =

A

Kon/Koff

118
Q

Kd =

A

Koff/Kon

119
Q

Large Koff=

A

weak binding

120
Q

Large Kb=

A

Strong binding

121
Q

Small Kd =

A

Strong binding

122
Q

nm to um

A

divide by 1000

123
Q

Ki =

A

Koff/Kon

124
Q

Competitive inhibition

A

Vmax not affected
Km increases

125
Q

Noncompetitive inhibition

A

Vmax decreases
Km stays same

126
Q

Fewer H-bonds raises

A

Ki

127
Q

Weaker interactions, Ki

A

increases

128
Q

For a process to be spontaneous, ΔS must be

A

+

129
Q

When ΔH and ΔS is negative,

A

ΔG is negative at low T (spontaneous)
ΔG is positive at high T (nonspontaneous)

130
Q

When ΔH and ΔS is positive,

A

ΔG is negative at high T (spontaneous)
ΔG is positive at low T (nonspontaneous)

131
Q

When ΔH is negative and ΔS is positive,

A

ΔG is negative (spontaneous)

132
Q

When ΔH is positive and ΔS is negative,

A

ΔG is positive (nonspontaneous)

133
Q

Arrhenius acids produce

A

H+ when dissolved in water

134
Q

Arrhenius bases produce

A

OH- when dissolved in water

135
Q

Bronsted acids

A

donate H+

136
Q

Bronsted bases

A

accept H+

137
Q

Ka increases

A

acidity increases

138
Q

Stability of conjugate base factors

A

larger atom
electronegative
resonance
inductive effect (electronegativity)

139
Q

Lewis acids

A

accept e- (incomplete octets)

140
Q

Lewis bases

A

donate e- (at least 1 lone pair)

141
Q

Ligand is the molecule or ion that

A

bonds to a metal or ion

142
Q

Coordination number

A

The number of atoms bonded to the metal (# of bonds metal forms)

143
Q

Acidic

A

H > OH

144
Q

Basic

A

H < OH

145
Q

Cation

A

positive charge

146
Q

Anion

A

negative charge

147
Q
A

PSU Freshman (12 decks)

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