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Bioenergetics Flashcards

(53 cards)

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1
Q

What is the definition of metabolism

A

Sum of anabolic/catabolic reactions in an organism

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2
Q

Why is metabolism important (3)

A

Obtain energy

Convert nutrients into those required by organisms

Needed for cellular work

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3
Q

Define intermediary metabolism

A

Combined activities of all the metabolic pathways that interconvert precursors/metabolites/products of low molecular weight

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4
Q

Catabolism

2 examples

A

Degradative phase of metabolism

ATP —> ADP

NADP —> NADPH

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5
Q

When many macromolecules forms one product

A

Converging

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6
Q

Anabolism

A

Biosynthesis phase of metabolism

ADP —> ATP

NADPH —> NADP+

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7
Q

One micro forms many macromolecules

A

Diverging

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8
Q

Exergonic reaction

A

Catabolism

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9
Q

Endergonic reaction

A

Anabolism

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10
Q

Compartmentalised

A

All work together but need other reactions for it to take place

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11
Q

Amphibolic reactions

A

Serves both anabolic + catabolic reactions

Krebs cycles

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12
Q

How is Krebs cycle amphibolic

A

Catabolism of carbs/FA into the cycle

Anabolic synthesis of precursors for amino acid synthesis

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13
Q

Where can anaplerotic reactions take place

What replenishes it

A

Krebs

Oxaloacetate

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14
Q

Name a negative feedback metabolism reaction

A

ADP activating phosphofructose kinase

As there’s deficiency in ATP

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15
Q

Name a positive feedback system metabolism

A

ATP inhibit phosphofructose kinase

Sufficient ATP is available

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16
Q

Define bioenergetics

A

Quantitative study of energy transductions in living organisms

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17
Q

In isolated systems, what happens with surroundings and exchange of energy

A

No exchange of energy between matter/surroundings

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18
Q

Closed system does what with energy

A

Exchanges energy not matter

No heat loss

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19
Q

Open system

A

All organisms

Exchanges matter/energy in a cell

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20
Q

2nd law of thermodynamics

A

Energy reaction will always lead to unusable energy

Energy able to do work is always less than the original amount of energy

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21
Q

Gibbs free energy definition

A

Amount of energy capable of doing work during a reaction

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22
Q

Negative delta G

23
Q

Positive delta G

24
Q

What is delta G related to

Study These Flashcards
A

Directly related to reactant and product concentrations

25
Gibbs free energy reaction equation
Delta (H) - T delta (S)
26
What is H
Enthalpy Heat content of the reacting system
27
Entropy
Quantitative expression for the randomness or disorder in a system
28
Gain in entropy
Products are less complex / more disordered Sodium chloride in water
29
What amplifies entropy
Temperature
30
What can the Gibbs energy equation say if the value is NEGATIVE
Reaction can occur spontaneously
31
If the delta G is 0
System is equilibrium
32
Positive delta G
Energetically unfavourable
33
catabolic reaction always increase
Entropy As exergonic reaction
34
Endergonic reactions lead to what in terms of entropy
Decrease in entropy
35
Products always start with (3)
More free energy Less stable Greater work capacity
36
Reactants end with (3)
Less free energy More stable Less work capacity
37
ATP hydrolysis is defined as what What bond forms
Transfer of groups from ATP to substrate Covalent bond
38
ATP —> ADP What’s energy then used for
Negative G Cellular work /chemical synthesis
39
ADP —> ATP What’s formed in terms of stability
Positive G More stable products than reactants
40
What 3 things stabilise products
Ionisation Isomerization Resonance
41
ATP provides energy by group transfer through how many reactions
2 step reaction
42
Bisphosphoglycerate forms what
Phosphoglyceric Acid Via hydrolysis
43
Phosphoglyceric Acid forms what
3-phosphoglycerate Ionisation
44
More stable products produced
Catabolic
45
Whats diverging Give an example
Anabolism Acetyl CoA —> cholesterol//phospholipids/tricyclgylcerides
46
What’s converging
Catabolism Glycogen/surcrose/isoleucine —>Acetyl CoA
47
Units of Gibbs
Kj/mol -1
48
With redox potentials Higher redox potential= Lower redox potential =
Higher affinity (accepts electrons) Lower affinity (donates electrons)
49
What does the standard redox potential state
Affinity of substance for electrons
50
If something donates electrons what agent is it
Reducing agent
51
If something accepts electrons what is it
Oxidising agent
52
What do endergonic reactions do to enthalpy and entropy
Decrease entropy Increase enthalpy
53
What do exergonic reactions do to enthalpy and entropy
Increase entropy Decrease enthalpy

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