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Biology 1010 > Metabolism and ATP > Flashcards

Metabolism and ATP Flashcards

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1
Q

An organism’s metabolism transforms

A

matter and energy,

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2
Q

An organism’s metabolism is
subject to

A

the laws of thermodynamics

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3
Q

The free-energy change of a reaction tells us

A

whether or not the reaction occurs spontaneously

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4
Q

ATP powers cellular work by

A

coupling exergonic reactions to endergonic reactions

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5
Q

Enzymes speed up metabolic reactions by

A

lowering energy
barriers

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6
Q

Regulation of enzyme activity helps

A

control metabolism

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7
Q

A living cell is a

A

miniature chemical factory where
thousands of reactions occur

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8
Q

The cell extracts energy

A

stored in sugars and other
energy-containing organic molecules

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9
Q

The cell extracts energy and applies

A

energy to perform work

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10
Q

Metabolism

A

the totality of an organism’s chemical
reactions

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11
Q

metabolism is an _______ from _____

A

emergent property and interactions between molecules in cell

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12
Q

Metabolic pathways

A

begin with a specific molecule
(substrate or reactant) and end with a product

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13
Q

Each step in the metabolic pathways us

A

catalyzed by a specific enzyme

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14
Q

Catabolic pathways

A

release energy by breaking down
complex molecules into simpler compounds

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15
Q

example of catabolic pathways

A

Cellular respiration

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16
Q

how is Cellular respiration an example of a catabolic pathway

A

breakdown of glucose in the
presence of oxygen

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17
Q

Anabolic pathways

A

consume energy to build complex
molecules from simpler ones

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18
Q

Anabolic pathway example

A

Synthesis of protein from amino acids

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19
Q

Bioenergetics

A

the study of how organisms manage
their energy resources

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20
Q

Energy

A

the capacity to cause change

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21
Q

Energy exists in ______ and some can _____

A

various forms and perform
work

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22
Q

Energy can be converted

A

from one form to another

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23
Q

Kinetic energy

A

energy associated with motion

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24
Q

thermal energy is also known as

A

heat

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25
Q

Heat (thermal energy)

A

kinetic energy associated with
random movement of atoms or molecules

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26
Q

Potential energy

A

energy that matter possesses
because of its location or structure

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27
Q

Chemical energy

A

potential energy available for release
in a chemical reaction

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28
Q

Thermodynamics

A

the study of energy transformations

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29
Q

two types of systems

A
  1. open system
  2. isolated system
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30
Q

isolated system

A

unable to exchange energy or
matter with its surroundings

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31
Q

open system

A

energy and matter can be transferred
between the system and its surroundings

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32
Q

organisms are _____ systems

A

open

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33
Q

first law of thermodynamics

A

the amount of
energy in the universe is constant

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34
Q

how is the amount of
energy in the universe is constant

A

Energy can be transferred and transformed, but it cannot be
created or destroyed

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35
Q

what is first law of thermodynamics also known as

A

principle of conservation of energy

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36
Q

During every energy transfer or transformation, some energy is

A

unusable, and often lost as heat

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37
Q

The second law of thermodynamics

A

Every energy transfer or transformation increases
entropy (disorder) of the universe

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38
Q

Living cells convert what to what

A

organized forms of energy to heat

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39
Q

Spontaneous processes

A

without energy input

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40
Q

For a process to occur without energy input

A

it must increase entropy of universe

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41
Q

Spontaneous processes can happen

A

quickly or slowly

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42
Q

Cells create ordered structures from

A

less ordered materials

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43
Q

Cells create ordered structures from less ordered materials

A

Requires the input of energy

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44
Q

Organisms also replace

A

ordered forms of matter and
energy with less ordered forms

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45
Q
  • Energy flows into an ecosystem in _____ and exits in ____
A

form of light
form of heat

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46
Q

Evolution of more complex organisms

A

does not violate
the second law of thermodynamics

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47
Q

Entropy (disorder) may _____ in an organism, but universe’s total entropy ____

A

decrease and increases

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48
Q

Biologists want to know

A

which reactions occur
spontaneously and which require input of energy

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49
Q

An unstable system is

A

rich in free energy.

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50
Q

An unstable system has a tendency to

A

change spontaneously to a more stable state

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51
Q

how does the free-energy concept apply on a molecular scale

A

to the physical movement of molecules
known as diffusion

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52
Q

less free energy means what (2)

A
  1. more stable
  2. less work capacity
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53
Q

Chemical reactions also involve

A

free energy.

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54
Q

When catabolic pathways break down complex organic molecules what can a cell do

A

harness the free energy stored in the molecules to perform
work

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55
Q

Free energy

A

-It is the amount of energy that is available to do work.

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56
Q

what is a criterion for spontaneous change

A

Free energy

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57
Q

G

A

Free energy

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58
Q

Free energy is related to the systems

A

total energy and entropy

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59
Q

H

A

enthalpy of total energy

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60
Q

S

A

entropy

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61
Q

T

A

Temperature in K

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62
Q

Free Energy equation

A

G = H-TS

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63
Q

Free energy (g) is proportional to the

A

system’s energy available to do work

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64
Q

free energy is the difference between

A

the total energy (enthalpy) and
the energy not available for doing work (TS)

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65
Q

The maximum amount of usable energy that can be harvested from a particular reaction is

A

the system’s free energy change from the
initial to the final state.

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66
Q

Gibbs-Helmholtz equation

A

change in free energy (ΔG) at a constant Temp and pressure

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67
Q

ΔG

A

change in free energy

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68
Q

ΔH

A

change in total energy

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69
Q

the total energy is also known as

A

enthalpy

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70
Q

ΔS

A

change in entropy

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71
Q

T

A

absolute temp in K

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72
Q

how to calculate Kalvins

A

(Degree Celius + 273)

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73
Q

ΔG equation

A

ΔG = ΔH – TΔS

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74
Q

The living system’s free energy is

A

the energy that can do work
when temperature and pressure are uniforms,

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75
Q

spontaneous processes have a

A

negative ∆G

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76
Q

what can spontaneous processes be harnessed to do

A

perform work

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77
Q

During a spontaneous change, free energy ____ and the stability of a system ____

A

decreases and increases

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78
Q
  • Free energy is a measure of a
A

system’s instability

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79
Q

system’s instability

A

tendency to change to a more stable state

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80
Q

Equilibrium is a state

A

of maximum stability

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81
Q

A process is spontaneous and can perform work only

A

when it is moving toward equilibrium

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82
Q

more free energy =

A
  1. higher G
  2. less stable
  3. greater work capacity
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83
Q

In a spontaneous change

A
  1. free energy of the system decreases
  2. system becomes more stable
  3. released free energy can be used to do work
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84
Q

the final result of the change

A
  1. less free energy
  2. lower G
  3. more stable
  4. less work capacity
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85
Q

Based on their free energy changes, all chemical reactions

A

classified as exergonic or endergonic

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86
Q

relationship between chemical equilibrium and the free energy change (ΔG) of a reaction

A
  1. As a reaction approaches equilibrium, the free energy of the system decreases
  2. When a reaction is pushed away from equilibrium, the free energy of the system increases
  3. When a reaction reaches equilibrium, ΔG = 0
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87
Q

When a reaction reaches equilibrium, ΔG = 0

A

no net change in the system

88
Q

When a reaction is pushed away from equilibrium, the free energy of the system increases

A

non-spontaneous and
endergonic reaction

89
Q

As a reaction approaches equilibrium, the free energy of the system decreases

A

spontaneous and exergonic reaction

90
Q

Reactions can be classified based on their free energy changes

A

Exergonic reaction
Endergonic reaction

91
Q

Exergonic reaction

A

a reaction that proceeds with a net
loss of free energy.

92
Q

Endergonic reaction

A

an energy-requiring reaction that
proceeds with a net gain of free energy;

93
Q

a reaction absorbs free energy from its surroundings

A

Endergonic reaction

94
Q

Chemical products have less free energy than the reactant molecules

A

Exergonic reaction

95
Q

Reaction is energetically downhill

A

Exergonic reaction

96
Q

Spontaneous reaction

A

Exergonic reaction

97
Q

ΔG is negative

A

Exergonic reaction

98
Q

ΔG is the maximum amount of work the reaction can perform

A

Exergonic reaction

99
Q

Products store freer energy than reactants

A

Endergonic reaction

100
Q

The reaction is energetically uphill

A

Endergonic reaction

101
Q

Non-spontaneous reaction
requires energy input

A

Endergonic reaction

102
Q

ΔG is positive.

A

Endergonic reaction

103
Q

+ΔG is the minimum amount of work required to drive the reaction

A

Endergonic reaction

104
Q
  • An exergonic reaction proceeds
A

with a net release of free energy and is spontaneous

105
Q
  • Exergonic reaction is
A

spontaneous

106
Q

Energy is released during

A

the progress of an exergonic reaction.

107
Q

The amount of energy released is delta G
less than zero

A

Exergonic reaction

108
Q

The exergonic reaction is the
difference between the ____ free energy of
the reactants and the ____ free energy of
the products

A

higher and the lower

109
Q

An endergonic reaction

A

absorbs free energy from its
surroundings and is nonspontaneous

110
Q

nonspontaneous

A

Endergonic reaction

111
Q

Energy is required during the progress

A
  • Endergonic reaction
112
Q

The amount of energy required is delta G
greater than zero

A
  • Endergonic reaction
113
Q

Endergonic reaction is the
difference between the ____ free energy
of the reactants and the ____ free energy
of the products

A

lower and higher

114
Q

Reactions in a closed system

A

eventually, reach equilibrium
and then do no work

115
Q

Cells are

A

not in equilibrium and open systems
experiencing a constant flow of energy and matter

116
Q
  • Defining feature of life
A

is that metabolism is never at
equilibrium

117
Q

Catabolic pathway in a cell

A

releases free energy in a series
of reactions

118
Q

If a chemical process is exergonic the reverse process

A

must be endergonic

119
Q

For each mole of glucose oxidized in the exergonic process of cellular respiration

A

2870 kJ are released

120
Q

To produce a mole of glucose, the endergonic process of photosynthesis requires

A

energy input of 2870 kJ

121
Q

The individual steps of respiration in isolation would

A

come to equilibrium and the cellular work would cease

122
Q

in respiration, there is a series of drops in free energy between

A

glucose, the start material and the metabolic wastes at the end

123
Q

with the steps, respiration will

A

never reach equilibrium as long as the organism lives

124
Q

with multiple steps, the _____ becomes the _____ for the next and the _____ are expelled from the cell

A
  1. product
  2. waste
  3. metabolic wasts
125
Q

three kinds of cellular work

A
  1. chemical
  2. transport
  3. mechanical
126
Q

To do work, cells manage energy resources by

A

energy coupling

127
Q

energy coupling

A

use of an exergonic process to drive an endergonic one

128
Q

Most energy coupling in cells is mediated by

A

ATP (adenosine triphosphate)

129
Q

cell’s energy shuttle

A

ATP

130
Q

ATP has what nitrogen base

A

adenine

131
Q

Bonds between the phosphate groups of A T P can be broken

A

by hydrolysis

132
Q
  • Energy is released from ATP with
A

the terminal phosphate bond of ATP broken

133
Q

The release of energy comes from the ATP molecule is

A

chemical change to a state of lower energy, not from the phosphate bonds themselves

134
Q

cilia beating

A

mechanical work

135
Q

the contraction of the muscle cells

A

mechanical work

136
Q

the movement of the chromosomes during
cellular reproduction

A

mechanical work

137
Q

the pumping of substances across
membranes against the direction of spontaneous movement

A

transport work

138
Q

the pushing of endergonic reactions that would
not occur spontaneously

A

chemical work

139
Q

synthesis of polymers from monomers

A

endergonic

140
Q

ATP drives endergonic reactions by

A

phosphorylation

141
Q

phosphorylation

A

transferring a phosphate group to some other molecule

142
Q

phosphorylated intermediate

A

The recipient molecule after receiving the phosphate group

143
Q

ATP is a ______ regenerated from _____

A

renewable resource and adenosine
diphosphate ADP

144
Q

Energy to phosphorylate ADP comes

A

catabolic reactions in the cell

145
Q

Catalyst

A

chemical agent that accelerate a reaction without being permanently changed in the process

146
Q

Enzymes

A

are catalytic proteins that change the rate of a
reaction without being consumed by the reaction

147
Q

Are all enzymes catalysts

A

YES

148
Q

Are all catalysts enzymes

A

NO

149
Q

Transition state

A

unstable condition of reactant molecules
that have absorbed sufficient free energy to react

150
Q

energy of activation, or activation
energy

A

The initial investment of energy for starting a reaction – the energy required to break bonds in the reactant molecules

151
Q

example of an enzyme-catalyzed reaction

A

Hydrolysis of sucrose by sucrase

152
Q

Every chemical reaction between molecules involves

A

bond breaking and bond forming

153
Q

Initial energy needed to start a chemical reaction

A

activation energy

154
Q

Activation energy is often supplied in form of

A

thermal energy that reactant molecules absorb from their surroundings

155
Q

Enzymes catalyze reactions

A

by lowering activation energy barrier

156
Q

Enzymes do not affect

A

change in free energy (∆G)

157
Q

The reactant that an enzyme acts

A

substrate

158
Q

An enzyme binds to its substrate to form an

A

enzyme-substrate complex

159
Q

the reaction catalyzed by each enzyme is very specific

A

from the enzyme-substrate complex

160
Q

The active site

A

is the region on an enzyme where the
substrate binds

161
Q

Induced fit

A

a substrate brings chemical groups of active
site into positions that enhance their ability to catalyze reaction

162
Q

The active site can lower an EA barrier by

A
  • Orienting substrates correctly
    – Straining bonds in the substrate molecule
    – Providing a favourable microenvironment
    – Covalently bonding to the substrate
163
Q

In an enzymatic reaction, the substrate

A

binds to the active site of the enzyme

164
Q

how are substrates held together in the active site

A

by weak interactions
hydrogen or ionic bonds

165
Q

An enzyme’s activity can be affected by

A

temperature
pH
pressure
Chemicals that specifically influence the enzyme

166
Q

Optimal conditions favour the most

A

active conformation (shape) for the enzyme

167
Q

optimal temp for typical human enzyme

A

37 degree Celcius

168
Q

Stomach enzyme (Pepsin) optimal PH

A

2

169
Q

Intestinal enzyme (Tryposin) optimal PH

A

8

170
Q

Cofactors

A

nonprotein enzyme helpers

171
Q

cofactors may be

A

inorganic
or organic

172
Q

inorganic cofactor

A

such as a metal in ionic form

173
Q

coenzyme

A

organic cofactor

174
Q

coenzyme example

A

vitamins

175
Q

Competitive inhibitors

A

bind to the active site of an
enzyme, competing with substrate

176
Q

Noncompetitive inhibitors

A

bind to an enzyme at a
separate site from the active site

177
Q

Noncompetitive inhibitors results in

A

a conformational change in the enzyme that makes the active site less effective

178
Q

Examples of inhibitors include

A

toxins, poisons, pesticides,
and antibiotics

179
Q

antibiotics works more on

A

bacteria

180
Q

ANIMAL intermediate energy

A

glucose and sugar

181
Q

ANIMAL immediate energy

A

ATP

182
Q

ANIMAL long-term energy

A

Fat and adipose cells

183
Q

PLANT intermediate energy

A

Glucose

184
Q

PLANT immediate energy

A

ATP

185
Q

PLANT long-term energy

A

oils

186
Q

photosynthesis is endergonic or exergonic

A

endergonic reaction

187
Q

cellular respiration is endergonic or exergonic

A

exergonic reaction

188
Q

more complex molecules have more energy because

A

the energy stored is in the bonds

189
Q

Downhill metabolic pathway

A

Energy is released by the downhill reactions of catabolic pathways

190
Q

uphill metabolic pathway

A

energy is stored and then used to drive uphill reactions of anabolic pathways

191
Q

a process on its own that leads to a decrease in entropy

A

Nonspontaneous process

192
Q

Organisms are ____ entropy

A

low

193
Q

The greater the decrease in free energy,

A

the greater the amount of work that can be done

194
Q

Why does heat not work well in biological systems?

A

a. High temps denature proteins and kill cells
b. Heat would speed up ALL reactions not just specific ones

195
Q

Inhibitors can attach to the enzyme by covalent bonds

A

irreversible

196
Q

Most bind to the enzyme by weak interactions

A

reversible

197
Q

A cell must be able to control when and where its various enzymes are active

A

Either by switching on and off the genes that encode specific enzymes

Regulating the activity of enzymes once they are made

198
Q

Endergonic or Exergonic

A

Endergonic

199
Q

Endergonic or Exergonic

A

Exergonic

200
Q

enzymes are _____ encoded by ____

A

proteins and genes

201
Q

changes or _____ leads to changes in enzyme’s ______

A

mutations and amino acids

202
Q

altered amino acids may alter enzyme’s

A

substrate specificity

203
Q

what would result if a cell’s metabolic pathways were not regulated

A

chemical chaos

204
Q

how does a cell regulate its metabolism

A
  1. switching on or off genes that encode specific enzymes
  2. regulating activity of enzymes
205
Q

Allosteric regulation

A

may either inhibit or stimulate an enzymes activity

206
Q

Allosteric regulation occurs when a

A

regulatory molecule binds to a protein at one site and affects the protein’s functionm at another site

207
Q

Most allosterically regulated enzymes contain

A

multiple polypeptide subunits

208
Q

Each enzyme has

A

active and inactive forms

209
Q

Binding of an activator

A

stabilizes the active form of an enzyme

210
Q
  • Binding of an inhibitor
A

stabilizes the inactive form of an enzyme

211
Q

Cooperativity

A

is a form of allosteric regulation that can
amplify enzyme activity

212
Q

In feedback inhibition,

A

the end product of a metabolic pathway shuts down the pathway

213
Q

ATP powers cellular work by

A

coupling exergonic
reactions to endergonic reactions

214
Q

ATP drives endergonic reactions by

A

transfer of the phosphate group to specific reactants

215
Q

cell respiration (catabolic pathway) drives the

A

regeneration of ATP from ADP

Biology 1010 (14 decks)

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