Biochemistry: Introductory principles Flashcards
1
Q
draw base of alcohol
A
pg 5
2
Q
draw base of aldehyde
A
pg 5
3
Q
draw base of ketone
A
pg 5
4
Q
draw base of carboxylic acid
A
pg 5
5
Q
draw base of ether
A
pg 5
6
Q
draw base of acid anhydride
A
pg 5
7
Q
draw base of sulfhydryl group
A
pg 5
8
Q
draw base of a disulfide group
A
pg 5
9
Q
draw base of amino group
A
pg 5
10
Q
draw base of quaternary amine group
A
pg 5
11
Q
draw base of ester
A
pg 5
12
Q
draw base of thioester
A
pg 5
13
Q
draw base of phosphoester
A
pg 5
14
Q
draw base of amide
A
pg 5
15
Q
an aldehyde is more ____ than an alcohol
A
oxidized
16
Q
a carboxylic acid is more _____ than a keton
A
oxidized
17
Q
generally, double bonds are more _____ than single bonds
A
oxidized
18
Q
describe properties of C-C and C-H bonds
A
electrons shared equally, non-polar, unreactive
19
Q
describe properites of C-O & C-N bonds
A
electrons shared unequally, polar reactive
20
Q
when we eat we do what to food
A
oxidize the food
21
Q
when we oxidize the food we are creating
A
energy
22
Q
what is oxidation
A
loss of electrons
23
Q
mneominc for oxidation
A
OIL RIG
oxidation is loss
reduction is gain
(of electrons)
24
Q
when alcohol is oxidized what does it become
A
aldehyde
25
what is reduction
gain of electrons
26
oxidation generally release
energy
27
reduction generally absorb
energy
28
what is another word for energy release
exergonic
29
what is another name for absorbing energy
endergonic
30
which is more oxidized, C=C or C-C
C=C
31
if there is loss of hydrogen and gain of oxygen it is
oxidation
32
if there is gain of hydrogen and loss of oxygen it is
reduction
33
a reducing agent is also called a
reductant
34
reducing agent is something that is going to
reduce something else but itself will be oxidized
35
what happens to a reducing agent
donate an electron
| it has lower electron affinity than the other
36
an oxidizing agent is also called
oxidant
37
a reducing agent compared to oxidizing agnet
reducing agent has lower electron affinity, oxidizing agent has higher electron affinity
38
oxygen has the highest
reduction potential of any molecule we know of!!!
| it is being reduced
39
oxygen is a good example of a
oxidizing agent
40
reduction potential of oxygen
high - it has highest reduction potential. it has more affinity to electrons than any other molecule
41
lower reduction potential is synonymous with saying
lower affinity for electrons
42
using the table on pg 7 which one has the lower reduction potential
NADH
43
the one with the highest E number is the one that
will be more likely to take the electrons
44
What does E stand for
standard reduction potential
45
what is the standard reduction potential
quantitative measure of the tendency of redox pairs to lose electrons
46
The lower the E the greater the tendency to
lose electrons
47
the greater the E the greater the tendency to
accept electrons
48
draw a carboxylate group
pg 9
49
draw a phosphate group
pg 9
50
draw a sulfate group
pg 9
51
acidic groups contain what that make them acidic
proton that may dissociate
52
any acid to be deprotenated you form
conjugate base
53
draw acetic acid
pg 9
54
explain a conjugate base and acid
aceitc acid is the acid, acetate would be the conjugate base.
55
ionizable group
contains acid and amino group
56
basic groups can
acquire a proton
57
if it can be protonated
it is a base. once it is protonated it forms the conjugate acid
58
what is a polar group
unequal sharing of electrons b/w atoms
59
if a molecule is polar what will happen in water
it will dissolve
60
if a molecule is charged and dissolves in water it is
polar
61
what happens to large nonpolar compounds in water
pushed together by water
62
what are examples of large nonpolar groups
fat droplets
cholesterol
lipid micelles
63
ionizable groups are examples of
bases and acids
64
nitrogen containing groups are usually: acidic or basic?
basic
65
if something is basic it means it can acquire
proton
66
when a base acquires a proton it becomes
positively charged cation
67
what is the name for the positively charged cation as a result of a base acquiring a proton
conjugate acid
68
Besides N what can act as a base
S or P with functional groups
69
look up electronegativity in the biochem book
ppt pg 11, just refresh what it means
70
what is a nucleophile
"nucleus or positive-charge loving"
provide an electron pair to form a covalent bond
electron donating
71
what is an electrophile
"electron or negative-charge loving"
accept an electron pair to form a covalent bond
electron accepting
72
nucleophiles and electrophiles have a tendancy to form what kind of bond
covalent bonds w/ each other
73
what is another name of a nucleophile
lewis base
74
what is another name of an electrophile
lewis acid
75
it has reqched equilibrium when
rate of forward and reverse reactions are equal
76
Keq stands for the
equilibrium constant
77
at equilibrium, describe the ratio nof products to reactants
it is constant
78
write out the equilibrium constant equation
Keq = [C]c[D]d/[A]a[B]b
| pg 15
79
polar molecules and electrolytes do what in water
dissolve, form either hydrogen bonds or hydration shells
80
describe hydorgen bond and hydration shell
pg 17
81
water dissociates
weakly
82
nitrogen containing groups are usually
basic
83
S or P with functional groups can act as
bases
84
What is ion product of water? (Kw)
10^-14
85
What does Kw stand for
ion product of water
86
what is the pH of water
7
87
acid
proton donor
88
base
proton acceptor
89
strong acid
completely dissociate in water
90
weak acid
partially dissociate in water or low ph
91
conjugate acids are
protonated
92
conjugate bases are
deprotonated
93
what is Ka
dissociation constant of acid
94
what is pKa
is the pH at which the protonated and unprotonated species are present at equal concentrations
95
if pH is 7 what is concentration hydrogen
10^-7
96
write out henderson-hasselbach equation
pH = pKa + log [A-]/[HA]
97
Ka =
[H+][A-]/[HA]
H is acid A is base
98
If pKa < pH, then
A- > HA
| which means it is strongly dissociated
99
what does it mean that A- > HA
strongly dissociated
100
if pKa > pH, then
HA > A-
| which means it is not dissociated or weakly dissociated
101
what does it mean that HA > A-
not dissociated or weakly dissociated
102
the greater the difference b/w pKa and pH in either direction, the greater the
degree of deprotonation or protonation
103
when ration = 1, then pH =
pKa
104
when acid is half-neutralised, A- =
HA
105
do notecard and get help for
pg 23
106
what is log 1
0
107
what is log 10
1
108
10^0 is
0
109
what is log 100
2
110
what is antilog 1
10
111
what is antilog -1
1/10
112
what is antilog 2
100
113
what is antilog -2
1/100
114
what is a buffer solution
has weak acid & its conjugate base
115
what do buffers resist
changes in pH when acid or base is added to the solution
116
at pH +- 1 around pKa, what happens to pH with addition of acid or base
it remains relatively constant
117
there is maximum buffering capacity when pH =
pKa
118
small changes in pH may drastically affect what
the protonation (or otherwise) of molecules and therefore their function
119
what is normal blood pH
7.4
120
pH of blood reflects the pH of
interstitial fluid
121
what is the main acid produced by the body
CO2
122
what is the buffer of the blood
bicarbonate
123
CO2 is its own
buffer
124
if bicarbonate is low what would pt do to compensate
breathe more
125
why do we breath more when we work out
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
what does it mean that pKa of H2CO3 ≈ 3.8, it will completely dissociate at
pH 7.4
127
draw out the bicarbonate system
pg 29
128
what cooperate in the blood to buffer it
HCO3- and haemoglobin (Hb)
129
draw out the bicarbonate in blood from a hepatic cell
pg 31
130
when pH decreases, breathing
increases
131
carbonic anhydrase plays important role in
kidney, pancreas, RBC, stomach
132
when we eat, the stomach uses what strategy to digest foo
low pH
133
where does stomach obtain acid
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
describe carbonic anhydrase role in pancreas
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
what happens to pH in body if I vomit
pH increases b/c there is extra amounts of bicarbonate
136
what happens to pH in body if diarrhea
pH decrease - b/c you are getting rid of bicarbonate and keeping hydrogen
137
describe carbonic anhydrase in kidney
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
what is alkalosis
ph increases
139
what is important buffer in cells outside of blood
phosphate
140
when acid is half neutralized, [A-]=
[HA]
141
the stronger the base, what happens to pKa
larger pKa
142
the stronger the acid, what happens to pKa
smaller pKa
143
what is the main acid produced by the body
CO2
144
CO2 is its own
buffer
145
pKa of H2CO3 is
3.8
146
H2CO3 will completely dissociate at pH
7.4
147
H2CO3 is
carbonic acid
148
draw out the bicarbonate buffer system
pg 29
149
What is SLC4A3
chloride-bicarbonate exchanger
150
as bicarbonate ions are released from RBC they are replaced by
chloride ions
151
acetoacetic acid & β-hydroxybutyric acid are what kind of bodies
ketone
152
describe diabetic ketoacidosis
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
if someone is hyperventilating what happens to pH
increases
154
what is alkalosis
pH increases
155
describe what happens with hyperventilation and how to treat
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
Name three other important buffer systems in body besides bicarbonate
H2PO4-
NH3 + H+
serum and intracellular proteins containing His
157
drug will absorb where dissociated acid is
more abundant
158
absorption of drugs is most efficient where and why?
in stomach and small intesting
| b/c it will be primarily deprotonated
159
if pH is lower than pKa then what happens to dissociation
it is abundant
