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MCB II Block 2 > Biochemistry: Introductory principles > Flashcards

Biochemistry: Introductory principles Flashcards

1
Q

draw base of alcohol

A

pg 5

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2
Q

draw base of aldehyde

A

pg 5

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3
Q

draw base of ketone

A

pg 5

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4
Q

draw base of carboxylic acid

A

pg 5

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5
Q

draw base of ether

A

pg 5

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6
Q

draw base of acid anhydride

A

pg 5

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7
Q

draw base of sulfhydryl group

A

pg 5

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8
Q

draw base of a disulfide group

A

pg 5

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9
Q

draw base of amino group

A

pg 5

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10
Q

draw base of quaternary amine group

A

pg 5

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11
Q

draw base of ester

A

pg 5

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12
Q

draw base of thioester

A

pg 5

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13
Q

draw base of phosphoester

A

pg 5

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14
Q

draw base of amide

A

pg 5

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15
Q

an aldehyde is more ____ than an alcohol

A

oxidized

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16
Q

a carboxylic acid is more _____ than a keton

A

oxidized

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17
Q

generally, double bonds are more _____ than single bonds

A

oxidized

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18
Q

describe properties of C-C and C-H bonds

A

electrons shared equally, non-polar, unreactive

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19
Q

describe properites of C-O & C-N bonds

A

electrons shared unequally, polar reactive

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20
Q

when we eat we do what to food

A

oxidize the food

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21
Q

when we oxidize the food we are creating

A

energy

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22
Q

what is oxidation

A

loss of electrons

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23
Q

mneominc for oxidation

A

OIL RIG
oxidation is loss
reduction is gain
(of electrons)

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24
Q

when alcohol is oxidized what does it become

A

aldehyde

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25
Q

what is reduction

A

gain of electrons

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26
Q

oxidation generally release

A

energy

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27
Q

reduction generally absorb

A

energy

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28
Q

what is another word for energy release

A

exergonic

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29
Q

what is another name for absorbing energy

A

endergonic

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30
Q

which is more oxidized, C=C or C-C

A

C=C

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31
Q

if there is loss of hydrogen and gain of oxygen it is

A

oxidation

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32
Q

if there is gain of hydrogen and loss of oxygen it is

A

reduction

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33
Q

a reducing agent is also called a

A

reductant

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34
Q

reducing agent is something that is going to

A

reduce something else but itself will be oxidized

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35
Q

what happens to a reducing agent

A

donate an electron

it has lower electron affinity than the other

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36
Q

an oxidizing agent is also called

A

oxidant

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37
Q

a reducing agent compared to oxidizing agnet

A

reducing agent has lower electron affinity, oxidizing agent has higher electron affinity

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38
Q

oxygen has the highest

A

reduction potential of any molecule we know of!!!

it is being reduced

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39
Q

oxygen is a good example of a

A

oxidizing agent

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40
Q

reduction potential of oxygen

A

high - it has highest reduction potential. it has more affinity to electrons than any other molecule

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41
Q

lower reduction potential is synonymous with saying

A

lower affinity for electrons

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42
Q

using the table on pg 7 which one has the lower reduction potential

A

NADH

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43
Q

the one with the highest E number is the one that

A

will be more likely to take the electrons

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44
Q

What does E stand for

A

standard reduction potential

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45
Q

what is the standard reduction potential

A

quantitative measure of the tendency of redox pairs to lose electrons

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46
Q

The lower the E the greater the tendency to

A

lose electrons

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47
Q

the greater the E the greater the tendency to

A

accept electrons

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48
Q

draw a carboxylate group

A

pg 9

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49
Q

draw a phosphate group

A

pg 9

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50
Q

draw a sulfate group

A

pg 9

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51
Q

acidic groups contain what that make them acidic

A

proton that may dissociate

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52
Q

any acid to be deprotenated you form

A

conjugate base

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53
Q

draw acetic acid

A

pg 9

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54
Q

explain a conjugate base and acid

A

aceitc acid is the acid, acetate would be the conjugate base.

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55
Q

ionizable group

A

contains acid and amino group

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56
Q

basic groups can

A

acquire a proton

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57
Q

if it can be protonated

A

it is a base. once it is protonated it forms the conjugate acid

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58
Q

what is a polar group

A

unequal sharing of electrons b/w atoms

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59
Q

if a molecule is polar what will happen in water

A

it will dissolve

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60
Q

if a molecule is charged and dissolves in water it is

A

polar

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61
Q

what happens to large nonpolar compounds in water

A

pushed together by water

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62
Q

what are examples of large nonpolar groups

A

fat droplets
cholesterol
lipid micelles

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63
Q

ionizable groups are examples of

A

bases and acids

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64
Q

nitrogen containing groups are usually: acidic or basic?

A

basic

65
Q

if something is basic it means it can acquire

A

proton

66
Q

when a base acquires a proton it becomes

A

positively charged cation

67
Q

what is the name for the positively charged cation as a result of a base acquiring a proton

A

conjugate acid

68
Q

Besides N what can act as a base

A

S or P with functional groups

69
Q

look up electronegativity in the biochem book

A

ppt pg 11, just refresh what it means

70
Q

what is a nucleophile

A

“nucleus or positive-charge loving”
provide an electron pair to form a covalent bond
electron donating

71
Q

what is an electrophile

A

“electron or negative-charge loving”
accept an electron pair to form a covalent bond
electron accepting

72
Q

nucleophiles and electrophiles have a tendancy to form what kind of bond

A

covalent bonds w/ each other

73
Q

what is another name of a nucleophile

A

lewis base

74
Q

what is another name of an electrophile

A

lewis acid

75
Q

it has reqched equilibrium when

A

rate of forward and reverse reactions are equal

76
Q

Keq stands for the

A

equilibrium constant

77
Q

at equilibrium, describe the ratio nof products to reactants

A

it is constant

78
Q

write out the equilibrium constant equation

A

Keq = [C]c[D]d/[A]a[B]b

pg 15

79
Q

polar molecules and electrolytes do what in water

A

dissolve, form either hydrogen bonds or hydration shells

80
Q

describe hydorgen bond and hydration shell

A

pg 17

81
Q

water dissociates

A

weakly

82
Q

nitrogen containing groups are usually

A

basic

83
Q

S or P with functional groups can act as

A

bases

84
Q

What is ion product of water? (Kw)

A

10^-14

85
Q

What does Kw stand for

A

ion product of water

86
Q

what is the pH of water

A

7

87
Q

acid

A

proton donor

88
Q

base

A

proton acceptor

89
Q

strong acid

A

completely dissociate in water

90
Q

weak acid

A

partially dissociate in water or low ph

91
Q

conjugate acids are

A

protonated

92
Q

conjugate bases are

A

deprotonated

93
Q

what is Ka

A

dissociation constant of acid

94
Q

what is pKa

A

is the pH at which the protonated and unprotonated species are present at equal concentrations

95
Q

if pH is 7 what is concentration hydrogen

A

10^-7

96
Q

write out henderson-hasselbach equation

A

pH = pKa + log [A-]/[HA]

97
Q

Ka =

A

[H+][A-]/[HA]

H is acid A is base

98
Q

If pKa < pH, then

A

A- > HA

which means it is strongly dissociated

99
Q

what does it mean that A- > HA

A

strongly dissociated

100
Q

if pKa > pH, then

A

HA > A-

which means it is not dissociated or weakly dissociated

101
Q

what does it mean that HA > A-

A

not dissociated or weakly dissociated

102
Q

the greater the difference b/w pKa and pH in either direction, the greater the

A

degree of deprotonation or protonation

103
Q

when ration = 1, then pH =

A

pKa

104
Q

when acid is half-neutralised, A- =

A

HA

105
Q

do notecard and get help for

A

pg 23

106
Q

what is log 1

A

0

107
Q

what is log 10

A

1

108
Q

10^0 is

A

0

109
Q

what is log 100

A

2

110
Q

what is antilog 1

A

10

111
Q

what is antilog -1

A

1/10

112
Q

what is antilog 2

A

100

113
Q

what is antilog -2

A

1/100

114
Q

what is a buffer solution

A

has weak acid & its conjugate base

115
Q

what do buffers resist

A

changes in pH when acid or base is added to the solution

116
Q

at pH +- 1 around pKa, what happens to pH with addition of acid or base

A

it remains relatively constant

117
Q

there is maximum buffering capacity when pH =

A

pKa

118
Q

small changes in pH may drastically affect what

A

the protonation (or otherwise) of molecules and therefore their function

119
Q

what is normal blood pH

A

7.4

120
Q

pH of blood reflects the pH of

A

interstitial fluid

121
Q

what is the main acid produced by the body

A

CO2

122
Q

what is the buffer of the blood

A

bicarbonate

123
Q

CO2 is its own

A

buffer

124
Q

if bicarbonate is low what would pt do to compensate

A

breathe more

125
Q

why do we breath more when we work out

A

the body creates lactic acid when it is working out which lower the pH so we need to breathe more to bring the pH back up - helps body get rid of hydrogen

126
Q

what does it mean that pKa of H2CO3 ≈ 3.8, it will completely dissociate at

A

pH 7.4

127
Q

draw out the bicarbonate system

A

pg 29

128
Q

what cooperate in the blood to buffer it

A

HCO3- and haemoglobin (Hb)

129
Q

draw out the bicarbonate in blood from a hepatic cell

A

pg 31

130
Q

when pH decreases, breathing

A

increases

131
Q

carbonic anhydrase plays important role in

A

kidney, pancreas, RBC, stomach

132
Q

when we eat, the stomach uses what strategy to digest foo

A

low pH

133
Q

where does stomach obtain acid

A

they can take carbon dioxide and hydraget to carbolic acid, which dissociates and then yoou have hydrogen and bicarbonate. the bicarbonate is pulled out and is exhcnaged for chloride in the stomach.
so this is coming from carbonic anhydrase

134
Q

describe carbonic anhydrase role in pancreas

A

bile ducts produce basic cocktail. they take carbon dioxide, water, make carbon anhydrase, carbonic acid, then it dissociates, HCo3 go into pancreatic duct and H+ goes into blood

135
Q

what happens to pH in body if I vomit

A

pH increases b/c there is extra amounts of bicarbonate

136
Q

what happens to pH in body if diarrhea

A

pH decrease - b/c you are getting rid of bicarbonate and keeping hydrogen

137
Q

describe carbonic anhydrase in kidney

A

carbon dioxide hydrognaed wit water → carbonic acid → dissociates → secreted into the lumen of the tubules in the kidney and it acidifies the kidney and at the same time it rescues bicarbonate (

138
Q

what is alkalosis

A

ph increases

139
Q

what is important buffer in cells outside of blood

A

phosphate

140
Q

when acid is half neutralized, [A-]=

A

[HA]

141
Q

the stronger the base, what happens to pKa

A

larger pKa

142
Q

the stronger the acid, what happens to pKa

A

smaller pKa

143
Q

what is the main acid produced by the body

A

CO2

144
Q

CO2 is its own

A

buffer

145
Q

pKa of H2CO3 is

A

3.8

146
Q

H2CO3 will completely dissociate at pH

A

7.4

147
Q

H2CO3 is

A

carbonic acid

148
Q

draw out the bicarbonate buffer system

A

pg 29

149
Q

What is SLC4A3

A

chloride-bicarbonate exchanger

150
Q

as bicarbonate ions are released from RBC they are replaced by

A

chloride ions

151
Q

acetoacetic acid & β-hydroxybutyric acid are what kind of bodies

A

ketone

152
Q

describe diabetic ketoacidosis

A

Basically, regarding pH: so much ketone is produced, it makes blood acidic, too much for bicarbonate to buffer it.

Diabetic patient (Type I)
Insufficient insulin

Fatty acid released from adipocytes

Converted to acetoacetic acid & β-hydroxybutyric acid by liver

Metabolic acidosis (diabetic ketoacidosis, DKA)
As pH decreases
Breathing increases - rapid, deep and labored (Kussmaul respiration)
Results in loss of CO2 so pH increases
Depending on degree of acidosis Kussmaul repsiration may be insufficient

153
Q

if someone is hyperventilating what happens to pH

A

increases

154
Q

what is alkalosis

A

pH increases

155
Q

describe what happens with hyperventilation and how to treat

A

taking in too much air so CO2 levels in body decrease, which means pH increases. if pt breathes in paper bag they are breathing back in their own CO2 and can lower their pH

156
Q

Name three other important buffer systems in body besides bicarbonate

A

H2PO4-
NH3 + H+
serum and intracellular proteins containing His

157
Q

drug will absorb where dissociated acid is

A

more abundant

158
Q

absorption of drugs is most efficient where and why?

A

in stomach and small intesting

b/c it will be primarily deprotonated

159
Q

if pH is lower than pKa then what happens to dissociation

A

it is abundant

MCB II Block 2 (10 decks)

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