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Proteins > Bioenergetics > Flashcards

Bioenergetics Flashcards

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

A

Exergonic

23
Q

Positive delta G

A

Endergonic

24
Q

What is delta G related to

A

Directly related to reactant and product concentrations

25
Q

Gibbs free energy reaction equation

A

Delta (H) - T delta (S)

26
Q

What is H

A

Enthalpy

Heat content of the reacting system

27
Q

Entropy

A

Quantitative expression for the randomness or disorder in a system

28
Q

Gain in entropy

A

Products are less complex / more disordered

Sodium chloride in water

29
Q

What amplifies entropy

A

Temperature

30
Q

What can the Gibbs energy equation say if the value is NEGATIVE

A

Reaction can occur spontaneously

31
Q

If the delta G is 0

A

System is equilibrium

32
Q

Positive delta G

A

Energetically unfavourable

33
Q

catabolic reaction always increase

A

Entropy

As exergonic reaction

34
Q

Endergonic reactions lead to what in terms of entropy

A

Decrease in entropy

35
Q

Products always start with (3)

A

More free energy

Less stable

Greater work capacity

36
Q

Reactants end with (3)

A

Less free energy

More stable

Less work capacity

37
Q

ATP hydrolysis is defined as what

What bond forms

A

Transfer of groups from ATP to substrate

Covalent bond

38
Q

ATP —> ADP

What’s energy then used for

A

Negative G

Cellular work /chemical synthesis

39
Q

ADP —> ATP

What’s formed in terms of stability

A

Positive G

More stable products than reactants

40
Q

What 3 things stabilise products

A

Ionisation

Isomerization

Resonance

41
Q

ATP provides energy by group transfer through how many reactions

A

2 step reaction

42
Q

Bisphosphoglycerate forms what

A

Phosphoglyceric Acid

Via hydrolysis

43
Q

Phosphoglyceric Acid forms what

A

3-phosphoglycerate

Ionisation

44
Q

More stable products produced

A

Catabolic

45
Q

Whats diverging

Give an example

A

Anabolism

Acetyl CoA —> cholesterol//phospholipids/tricyclgylcerides

46
Q

What’s converging

A

Catabolism

Glycogen/surcrose/isoleucine —>Acetyl CoA

47
Q

Units of Gibbs

A

Kj/mol -1

48
Q

With redox potentials

Higher redox potential=

Lower redox potential =

A

Higher affinity (accepts electrons)

Lower affinity (donates electrons)

49
Q

What does the standard redox potential state

A

Affinity of substance for electrons

50
Q

If something donates electrons what agent is it

A

Reducing agent

51
Q

If something accepts electrons what is it

A

Oxidising agent

52
Q

What do endergonic reactions do to enthalpy and entropy

A

Decrease entropy

Increase enthalpy

53
Q

What do exergonic reactions do to enthalpy and entropy

A

Increase entropy

Decrease enthalpy

Proteins (13 decks)

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