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Biochemistry I > FINAL - CH2 > Flashcards

FINAL - CH2 Flashcards

1
Q

Bioenergetics is defined as

A

energy conversion in biological

system

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2
Q

Bioenergetics is the study of

A

the various types of energy transformations that occur in living organisms

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3
Q

3 types of work:

A

Osmotic: Maintains varying [solute] across biological
membranes

Chemical: Biosynthesis and degradation of organic
molecules

Mechanical: Muscle contraction in animals

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4
Q

Energy pathway:

A

Solar energy –> Photosynthesis –> Chemical energy –> Work (3 types)

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5
Q

Homeostasis

A

Highly ordered steady state

Requires energy and delays equilibrium

Example: Living organisms

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6
Q

Equilibrium

A

Homeostasis is no longer maintained.

Macromolecules tend to equilibrate to their surroundings.

Example: Non-living organisms

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7
Q

Reduction

A

Gain of electrons

Increase in the number of hydrogens

Decrease in the number of bonds to oxygen***

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8
Q

Oxidation

A

Loss of electrons

Decrease in the number of hydrogens

Increase in the number of oxygens***

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9
Q

System

A

Collection of matter in a defined space

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10
Q

Surroundings

A

All the space not included in the system

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11
Q

Thermodynamics is the study of

A

the changes in energy that accompany events in the universe

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12
Q

System + Surroundings =

A

Universe

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13
Q

Open system

A

Matter and energy are freely exchanged with the

surroundings

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14
Q

Closed system

A

Only energy is exchanged with the surroundings

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15
Q

Isolated system

A

Neither matter nor energy is exchanged with the

surroundings

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16
Q

First law of thermodynamics

A

Energy can be neither created nor destroyed only transformed from one form to another

ΔE = Efinal – Einitial

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17
Q

Descriptions of Enthalpy

A

Exothermic:
Reaction releases heat

Has a –ΔH

Endothermic:
Reaction absorbs heat

Has a +ΔH

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18
Q

2nd law of thermodynamics

A

spontaneous processes in the universe tend toward disorder in the absence of energy input

ΔSuniverse = ΔSsystem + ΔSsurroundings > 0

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19
Q

At equilibrium,

A

ΔG = 0, the rate of formation of products and reactants is equal

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20
Q

Gibbs Free Energy

A

ΔG

Amount of energy capable of doing work

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21
Q

Exergonic vs. Endergonic Reactions

A

Exergonic: ΔG < 0, Reaction is overall favorable and spontaneous

Endergonic: ΔG > 0, Reaction is overall unfavorable and non-spontaneous

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22
Q

Standard Free Energy Change

A

ΔG°

At standard conditions: 1 atm, 298 K, 1M

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23
Q

Keq

A

A + B –> C + D

Keq = [C]eq [D]eq / [A]eq [B]eq

If Keq < 1, favors formation of reactants

If Keq > 1, favors formation of products

If Keq = 1, reaction is at equilibrium

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24
Q

Biochemical Standard Conditions

A

ΔG°’

1 atm, 298 K, 1M
pH = 7
[H2O] = 55.5 M
Mg2+ = 1 mM

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25
Q

A common coupling reaction

A

ATP hydrolysis

26
Q

____ is a carrier of chemical energy

A

ATP

27
Q

EC

A

Energy charge

28
Q

Cells regulate the EC between _____

A

0.7–0.9

29
Q

In catabolic pathways Energy charge (EC) is _____

A

low

30
Q

In anabolic pathways Energy charge (EC) is _____

A

high

31
Q

Water is a ______ and a ______ in

biochemical reactions

A

solvent

reactant

32
Q

Water is ___ of the weight of

most organism

A

70%

33
Q

Angle in water molecules

A

104.5°

34
Q

The typical lifetime of an H-bond is

A

1 x10^-12 s

it is shorter as temperature increases

35
Q

each water molecule can form ____ hydrogen bonds.

A

four

36
Q

__________ occurs between the oxygen atom of one water and the hydrogen of another

A

electrostatic attraction

37
Q

H-bonding is especially strong in water because

A
  1. the O—H bond is very polar
  2. there are 2 lone pairs on the O atom
  3. Each H2O molecule can form four H bonds to other molecules
38
Q

Important property of H2O

A

Ice has a lower density than water

39
Q

Why is ice less dense than liquid water?

A

each water molecule interacts tetrahedrally with four other water molecules

This creates a regular lattice structure, which causes ice to be less dense (expands)

40
Q

__________ gives water its unusual

properties

A

Hydrogen bonding

41
Q

The attraction between the partial electrical charges is

greatest when the three atoms involved lie in _____________

A

a straight line

42
Q

Hydrophobic Effect

A

The tendency of water molecules to minimize their contact with hydrophobic molecules

forming “cages”

43
Q

Dialysis

A

Diffusion of solutes

44
Q

Hemodialysis

A

Acts as an artificial kidney

45
Q

reversible ionization

A

H2O –> H3O+ + OH-

46
Q

Proton jumping:

A

the proton can rapidly
jump from one water molecule to the
next

47
Q

pH + pOH

A

= 14

48
Q

Conjugate Base:

A

base formed by the removal of a proton from an acid

49
Q

Smaller Pka

A

Stronger acid

50
Q

Larger Pka

A

Weaker acid

51
Q

Smaller Ka

A

Weaker acid

52
Q

Larger Ka

A

Stronger acid

53
Q

[H+] [OH-] =

A

1 x 10^-14 = Kw

54
Q

Water density

A

1000 g/L

55
Q

MW of water

A

18 g/mol

56
Q

Buffers

A

solutions that resist changes in pH upon addition of acid or base

57
Q

maximum buffering “capacity”

A

near the pKa of the molecule ± 1 pH

58
Q

Mass-action ratio

A

Q

Keq = [C]i [D]i / [A]i [B]i

59
Q

Removing _____ from the blood helps increase the pH

A

CO2

60
Q

Removing ______ from the blood helps lower the pH

A

HCO3-

61
Q

3 types of membranes

A

Plasma membrane
Endomembranes
Mito/Chlor membranes - required for life

62
Q

Pka =

A

-log Ka

Biochemistry I (13 decks)

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