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chem final Flashcards

1
Q

What is meant by the term oxidation?

A

The loss of electrons by the compounds in chemical reactions.

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2
Q

On which side of an oxidation half-reaction do the electrons appear?

A

On the right side (products).

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3
Q

What is meant by the term oxidant?

A

It is the species that’s being reduced.

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4
Q

What is meant by the term oxidizing agent?

A

The compound which gains electrons in the redox reaction.

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5
Q

What is meant by the term reduction?

A

The gain of electrons by the compounds in chemical reactions

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6
Q

On which side of a reduction half-reaction do the electrons appear?

A

On the left side (reactants)

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7
Q

What is meant by the term reductant?

A

It is the species that’s being oxidized.

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8
Q

What is meant by the term reducing agent?

A

The compound that loses electrons in the redox reaction.

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9
Q

For a reduction potential to be a standard reduction potential, the substances in the reaction or half-reaction must be at _________, _______M aqueous solutions and ____ atm
gas pressures.

A

standard conditions
1
1

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10
Q

What is the standard reduction potential of a standard hydrogen electrode?

A

0 V

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11
Q

It is not possible to measure the standard reduction potential of a single half-reaction because each voltaic ____ consists of _____, half-reaction(s) and only the potential of a ____________ can be measured.

A

cell
2
complete cell

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12
Q

What is electrolysis?

A

The process of using an electric current to break up an ionic compound and form elements.

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13
Q

Are electrolysis reactions thermodynamically spontaneous?

A

no
Spontaneous reactions don’t include an external source or agent, and the electrolysis reactions involve electricity. So, they are not spontaneous.

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14
Q

What is an electrolytic cell?

A

An electrolytic cell is an electrochemical cell that uses electricity to make a non spontaneous redox reaction.

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15
Q

The negative terminal of a voltage source is connected to an electrode of an electrolytic cell. Is the electrode the anode or the cathode of the cell?

A

The electrode is the cathode.
The electrode connected with the negative terminal of a battery is defined as a cathode.

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16
Q

The electrolysis of water is often done with a small amount of sulfuric acid added to the water. What is the role of the sulfuric acid?

A

The ions in sulfuric acid will increase the conductivity of water, and help the electrolysis of water to happen more quickly.

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17
Q

Is lightening spontaneous or non-spontaneous?

A

spontaneous

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18
Q

Is ripe banana spontaneous or non-spontaneous?

A

spontaneous

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19
Q

Is sugar dissolving in hot coffee spontaneous or non-spontaneous?

A

spontaneous

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20
Q

Is Nitrogen forming N2 spontaneous or non-spontaneous?

A

spontaneous

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21
Q

Is the formation of CH4 and O2 molecules from CO2 and H2O at room temp, spontaneous or non-spontaneous?

A

non-spontaneous

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22
Q

Is the vaporization of liquid water to steam at a pressure of 1 atm endothermic or exothermic>

A

endothermic

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23
Q

At what temp is the vaporization of liquid water to steam at a pressure of 1 atm a spontaneous process>

A

above 100 deg C

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24
Q

At what temp is the vaporization of liquid water to steam at a pressure of 1 atm a non-spontaneous process>

A

below 100 deg C

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25
Q

At what temp is the vaporization of liquid water to steam at a pressure of 1 atm, at what temp are the stages in equilibrium

A

at 100 deg C

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26
Q

A system goes from state 1
to state 2
and back to state 1.
Is ΔE the same in magnitude for both the forward and reverse processes?

A

yes

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27
Q

A system goes from state 1 to state 2 and back to state 1.
Without further information, can you conclude that the amount of heat transferred to the system as it goes from state 1 to state 2 is the same or different as compared to that upon going from state 2 back to state 1 ?

A

no

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28
Q

A system goes from state 1
to state 2 and back to state 1
Suppose the changes in state are reversible processes. Can you conclude anything about the work done by the system upon going from state 1
to state 2
as compared to that upon going from state 2
back to state 1
?

A

The magnitudes of the work are equal, but the signs are opposite.

If the changes of state are reversible, the two paths are different, w(1→2)=−w(2→1).

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29
Q

Is this process spontaneous or non spontaneous?
alignment of iron fillings in a magnetic field

A

spontaneous

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30
Q

Is this process spontaneous or non spontaneous?
the dissolving of HCl in water to form hydorchloric acid.

A

spontaneous

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31
Q

Is this process spontaneous or non spontaneous?
rxn of H gas w O2 gas to form water vapor at room temp

A

spontaneous

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32
Q

Is this process spontaneous or non spontaneous?
melting of ice cubes at -10 deg C and 1 atm

A

non spontaneous

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33
Q

Is this process spontaneous or non spontaneous?
seperating a mixture of N2 and O2 into 2 seperate samples, one with pure N2 and one with pure O2.

A

non spontaneous

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34
Q

Do you need to specify the temperature to calculate the entropy change?

A

Yes, because entropy is thermodynamic. Since entropy is a thermodynamic property, its value is related to the temperature of the system.

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35
Q

Label CH3COO−
as being a strong base, a weak base, or a species with negligible basicity.

A

weak base

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36
Q

Write the formula of CH3COO−
conjugate acid

A

CH3COOH

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37
Q

Indicate whether the conjugate acid of CH3COO−
is a strong acid, a weak acid, or a species with negligible acidity.

A

weak acid

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38
Q

Label HCO3−
as being a strong base, a weak base, or a species with negligible basicity.

A

weak base

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39
Q

Write the formula of HCO3−
conjugate acid

A

H2CO3

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40
Q

Indicate whether the conjugate acid of HCO3−
is a strong acid, a weak acid, or a species with negligible acidity.

A

weak acid

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41
Q

Label O2−
as being a strong base, a weak base, or a species with negligible basicity.

A

strong base

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42
Q

Write the formula of O2−
conjugate acid

A

OH−

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43
Q

Indicate whether the conjugate acid of O2−
is a strong acid, a weak acid, or a species with negligible acidity.

A

species with negligible acidity

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44
Q

Label Cl−
as being a strong base, a weak base, or a species with negligible basicity.

A

species with negligible basicity

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45
Q

Write the formula of Cl−
conjugate acid

A

HCl

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46
Q

Indicate whether the conjugate acid of Cl−
is a strong acid, a weak acid, or a species with negligible acidity.

A

strong acid

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47
Q

Label NH3
as being a strong base, a weak base, or a species with negligible basicity.

A

weak base

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48
Q

Write the formula of NH3
conjugate acid

A

NH4+

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49
Q

Indicate whether the conjugate acid of NH3
is a strong acid, a weak acid, or a species with negligible acidity.

A

weak acid

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50
Q

Based on the ion-product constant for water, Kw
, the product of the [H+]
and [OH−]
concentrations is

A

10 ^ -14

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51
Q

In a neutral water solution, the concentration of H+ and OH- would both be….

A

10 ^ −7

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52
Q

if a water solution has an OH- value less than _____ than the solution is … if the OH value is more… than it is

A

10 ^ −7
acidic
basic

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53
Q

If a neutral solution of water, with pH=7.00
, is cooled to 10 ∘C, the pH rises to 7.27.
H = ……

A

H+ = OH-

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54
Q

Ammonia, NH3, acts as an Arrhenius base because it _____
the concentration of hydroxide ion, OH−
in aqueous solution.

A

increases

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55
Q

It acts like a Br ø
nsted-Lowry base because it is a proton, H+…

A

acceptor

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56
Q

It acts like a Lewis base because it is an electron pair…

A

donator

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57
Q

If a substance is an Arrhenius base, it _____ be a Brønsted-Lowry base _____ a Lewis base.

A

MUST
AND

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58
Q

Predict whether the equivalence point of each of the following titrations is below, above, or at pH=7

NaHCO3 titrated with NaOH

A

above PH 7

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59
Q

Predict whether the equivalence point of each of the following titrations is below, above, or at pH=7

NH3 titrated with HCl

A

below pH=7

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60
Q

Predict whether the equivalence point of each of the following titrations is below, above, or at pH=7

KOH titrated with HBr

A

at pH=7

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61
Q

what are the strong acids (7)

A

HCl
HNO3
H2SO4
HBr
HI
HClO4
HClO3

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62
Q

what are the strong bases (6)

A

LiOH
NaOH
KOH
Ca(OH)2
Sr(OH)2
Ba(OH)2

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63
Q

sucrose is made of…

A

glucose and fructose

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64
Q

in addition to alcohols, a molecule of glucose contains which functional group?

A

aldehyde.

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65
Q

Which are the groups NOT functional in 2-propanol?

A

hydroxyl
alcohol

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66
Q

which functional groups always contain Nitrogen?

A

amines and amides.

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67
Q

amines are…

A

a derivative of ammonia NH3

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68
Q

aldehydes have…

A

carbonyl group at the end of their chain.

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69
Q

carbonyl group

A

a double bond between C and O … C=O

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70
Q

which group has a CARBONYL?
alcohol
ether
carboxylic acid
amine

A

carboxylic acid

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71
Q

which functional group does NOT contain oxygen?
amine
amide
ester
ether

A

Amine

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72
Q

the major organic product formed when 2-butene reacts with excess Br2 is….

A

2, 2, 3, 3 - tetrabromobutane

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73
Q

the major organic product formed when HBr reacts with 2-Butane is….

A

2-Bromobutane

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74
Q

the correct IUPAC name for CH3-CH2-CH2-CH=CH2 is…

A

1-Pentene

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75
Q

which term describes at least one carbon-carbon bond in 2,4-dimethyl-1-hexene?

A

double. (ends in ‘ene’, alkene)

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76
Q

which term describes the carbon-carbon bonds in Benzene?

A

delocalized pi bonds

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77
Q

C10H22 is the molecular formula of…

A

alkane

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78
Q

C3H6 is the molecular formula of…

A

alkene (double bonds on either ends)

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79
Q

Aromatics have _______ because theyre more stable

A

substitution

80
Q

molecule names containing ‘ol’ have…

A

OH groups wherever the ‘ol’ is

81
Q

ethers have…

A

oxygen in the middle of the chain

82
Q

most common substance in vinegar?

A

acetic acid

83
Q

why cant spontaneous radioactive decay be a zero-order or second-order kinetic process?

A

spontaneous radioactive processes are unimolecular processes leading only to a first order kinetic process

84
Q

which particles have no change in nuclear charge when emitted in nuclear decay?

A

neutron

85
Q

the atomic number is equal to the number of…..

A

protons

86
Q

the number of protons + neutrons

A

mass number

87
Q

If Ecell is a negative number…

A

cell is electrolytic

88
Q

If Ecell is a positive number…..

A

cell is volatile

89
Q

Ecell=…

A

Ecell = cathode - anode

90
Q

a volatile cell converts …

A

chemical energy to electricity

91
Q

cation going to cathode

A

reduction

92
Q

anion going to anode

A

oxidation

93
Q

in a redox reaction, e- moves from…

A

high potential to low potential

94
Q

cell potential is the

A

Ecell

95
Q

in a oxidation reaction, e- moves from…

A

low to high potential

96
Q

O charge is

A

-2

97
Q

H charge is

A

+1

98
Q

Cl charge is

A

-1

99
Q

oxidation state of nitrogen in (NH4)+ is….

A

-3

100
Q

Oxidation state of Mn in (MnO4)- is….

A

+7

101
Q

the element being reduced is the …

A

oxidizing agent

102
Q

oxidation is when the element

A

gains more pos charge in from reactants to products

103
Q

oxidation is…

A

loss of electrons

104
Q

reduction is….

A

gain of electrons

105
Q

reduction is when the element

A

loses positive charge, becomes more negative in the products

106
Q

if the cell potential for a reaction is large and positive then the reaction is…

A

spontaneous

107
Q

the purpose of the salt bridge in the voltaic cell is…

A

to maintain neutrality by allowing the flow of ions.

108
Q

which of the following is the strongest oxidizing agent?

A

always F2, fluorine.

109
Q

which is the strongest reducing agent?

A

Li. because it is always losing electrons.

110
Q

gibbs formula?

A

delta G = nFE

111
Q

nernst equation

A

E cell = E0 - (RT/ nF) ln Q

112
Q

nernst equation is used for?

A

ion concentration

113
Q

in a concentration cell, the half reactions are…

A

the same.

114
Q

electrolyte in lead-acid car battery is

A

H2SO4

115
Q

a cell that uses external energy to produce an oxidation-reduction reaction is a ______ cell

A

electrolytic

116
Q

reduction occurs at the ______ in both Galvanic and electrolytic cells

A

cathode.

117
Q

oxidation occurs at the _______ in both Galvanic and electrolytic cells

A

anode.

118
Q

corrosion of metals can be prevented by the following: (but never by salt bridge)

A

-sacrificial anode
-oxide coating
-paint

119
Q

delta G = -nFE =…..

A

-RT*lnK

120
Q

the F in delta G = -nFE is

A

96485 C/ mol

121
Q

E = ….

A

E = (RT / nF) * ln K

122
Q

delta G = -RT *…..

A

ln K

delta G= -RT* ln K

123
Q

corrosion is..

A

oxidation / rust.

124
Q

which radiation is able to penetrate human tissue?

A

gamma

125
Q

nuclear fusion is a _______ reaction, reaction by which the ____ produces energy, and not yet practical as an energy source.

A

thermonuclear
sun

126
Q

nuclear fission is the

A

splitting of the nucleus

127
Q

mass defect and binding energy are related by

A

e = mc^2

128
Q

all radioactive decay processes follow

A

first order reaction kinetics

129
Q

a cyclotron is a

A

particle accelerator

130
Q

the half life of a radioisotope is the…

A

time required for one half of the atoms to undergo radioactive decay

131
Q

iodine 131 is transmuted to xenon 131 by

A

beta emission

132
Q

polonium 212 is transmuted to lead 208 by

A

alpha emission

133
Q

when an atom of cobalt 60 undergoes beta decay the product is

A

nickel 60

134
Q

when an atom of U238 undergoes alpha decay the product is

A

Th 234

135
Q

when an atom emits gamma radiation, the energy of the nucleus

A

decreases.

136
Q

during conversion of uranium 238 to lead 206, X alpha emissions and Y beta emissions occur… what will X and Y equal?

A

X= 8 Y= 6

137
Q

all spontaneous processes are…

A

irreversable

138
Q

entropy is the ____ in a system

A

randomness

139
Q

entropy is a state function.
change in entropy is given by…

A

S final - S initial

140
Q

the 2nd law of thermodynamics says

A

entropy of the universe increases when spontaneous processes occur.

141
Q

if a forward reaction is spontaneous….

A

the reverse reaction will be non-spontaneous

142
Q

a car is being driven from west to east is experiencing…

A

translational motion.

143
Q

change in molecule bond length or bond angles, are examples of….

A

vibrational motion.

144
Q

when a molecule spins, this is…

A

rotational motion.

145
Q

entropy of CO2 increases upon heating because all three types of molecular motion increase (t/f)

A

true

146
Q

entropy of neon increases upon heating because all 3 types of molecular motions increase (t/f)

A

false.
its just a single atom, it will not undergo vibration

147
Q

which is true:
s = k * w
s = k / w
s = k *ln w
s = k ^ w

A

S= k * ln w

148
Q

entropy decreases when…

A

a gas becomes a solid

149
Q

at equilibrium free energy, AKA delta G =

A

0

150
Q

Gibbs free energy formula

A

delta G = delta H - T* delta S

151
Q

if enthalpy is positive and entropy is negative, the reaction is

A

non spontaneous at all temps.

152
Q

if volume inc…

A

entropy inc, and microstates inc

153
Q

if atoms inc…

A

microstates inc

154
Q

if temp inc…

A

entropy and microstates inc

155
Q

vibration is

A

simulstaneous oscillations

156
Q

if gas moleculs inc…

A

entropy inc

157
Q

if no. moles inc, entopy

A

increases

158
Q

if molecules become bigger, entropy

A

increases

159
Q

what is the value of entropy of a perfect pure crystalline substance at absolute zero

A

0

160
Q

what is the third law

A

cannot reach absolute zero in any number of processes

161
Q

what happens when NaOH is added to buffer

A

the NaOH will react with conjugate acid and convert some of it.

162
Q

what happens when HCl acid is added to buffer

A

it will react with the conjugate base, and convert some of it.

163
Q

what will be the ksp expression for dissolution of silver sulfate Ag2SO4

A

[Ag]^2[SO4]

164
Q

silver bromide is insoluble in water, but dissolves in aq. ammonia due to formation of…

A

Ag(NH3)2+ complex to remove silver ions from soln

165
Q

adding a bromide ion to an aq. soln of ____ will decrease its solubility in water.

BaSO4
Li2CO3
PbS
AgBr

A

AgBr
find the common ion.

166
Q

which mixture will form a good buffer,
HCl and KCl
HNO3 and KNO3
HCl and NH4Cl
NH3 and NH4Cl

A

NH3 and NH4Cl

167
Q

a buffer is…

A

weak acid + salt
weak base + salt

168
Q

strong acid + strong base leads to

A

-bad buffer
-electrolyte
-dissolves in water

169
Q

which solution has a better buffer capacity?

A

1 L solution of 0.5 N NH3 and 0.5M of NH4Cl
this is because this option had higher Molarity than the others.

170
Q

what is the henderson hasselbach eq?

A

pH = pKa + log (base / acid)

171
Q

strong acid + weak base
what is pH

A

lower than 7

172
Q

strong base + weak acid
what is pH

A

higher than 7

173
Q

bronsted lowry acid

A

proton H+ donor

174
Q

bronsted lowry base

A

proton H+ acceptor

175
Q

lewis acid

A

electron pair acceptor

176
Q

lewis base

A

electron pair donor

177
Q

what is the conjugate base of HPO4) -2

A

PO4)^ -3

178
Q

conjugate acid of SO4)2-

A

HSO4)1-

179
Q

the stronger the acid, the ____ the conjugate base

A

weaker

180
Q

acids and bases react to form their ____ conjugate

A

weaker

181
Q

conjugate base pair kw =

A

kw = ka * kb

182
Q

value of ion product constant for water is

A

10^-14

183
Q

all spontaneous processes are

A

irreversible

184
Q

which process is NOT spontaneous at 25 deg C?
melting of ice cube
boiling of liquid n2
sublimation of dry ice
freezing of ethyl alcohol

A

freezing of ethyl alcohol

185
Q

in spontaneous reaction..
entropy of universe ____
free energy of a system _____

A

inc
dec

186
Q

what kind of motion can molecules do, that an atom cant>

A

a molecule can vibrate and rotate
a single atom cant do either one.

187
Q

Bolzmanns entropy eq, S=….

A

S= k ln W

188
Q

if enthalpy change is pos, and entropy change is neg, reaction is

A

non spon at all temps

189
Q

if enthalpy change is neg, and entropy change is pos, reaction is

A

spontaneous at all temps

190
Q

what will be the pH change as NaOH is added to an HCl soln?

A

increase

191
Q

why will the equilibrium conc of a weak acid equal its initial conc?

A

because most weak acids of low to moderate concentration undergo very little ionization, often less than 1% in soln, so the extent of ionization can be neglected.

192
Q

at mid equivalence point,

A

pH = pKa

193
Q

2^x = 7

A

x ln 2= ln 7

194
Q

O2 is a strong base (t/f)

A

true

195
Q

kw=

A

10^-14

196
Q

amphoteric

A

soluble in strong acids/bases, bc they can act either as acids OR bases.

197
Q

ksp

A

the []*[] of REACTANTS, not products, no dividing.

Flash Cards (21 decks)

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