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Cell biology semester 1 > biophysics > Flashcards

biophysics Flashcards

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1
Q

water characteristics

A

dipolar (H-bonding) > high bp
hydration cell of interactions

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2
Q

solubility of larger biological molecules

A

more polar / charged side groups = higher solubility

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3
Q

charged side groups

A

amino
carboxyl
phosphate

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4
Q

polar side groups

A

alcohol
thiol
carbonyl
ester
amide

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5
Q

hydrophibicity

A

apolar groups disrupt H-bonding
drives protein folding

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6
Q

ampiphatic

A

both polar and non-polar end

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7
Q

brownian motion

A

thermal energy moving molecules in solution

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8
Q

diffusion

A

net flux of molecules down a concentration gradient due to random thermal motion

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9
Q

what drives passive transport across membranes

A

steady state diffusion

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10
Q

flux equation

A

J = P (C1-C2)
J= flux
P= permeability

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11
Q

time scale to transverse distance R with diffusion coefficient D

A

T=R^2/6D

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12
Q

U/ internal energy

A

capacity of a system to do work

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13
Q

chemical potential

A

determined by:
chemical bonds within
intermolecular bonding

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14
Q

1st law of thermodynamics

A

change in H = change in U + p (change in V)
enthalpy change = energy released by a reaction - work

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15
Q

ammonium nitrate solution

A

favourable but has positive enthalpy change

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16
Q

entropy

A

measure of system disorder

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17
Q

2nd law of thermodynamics

A

entropy of an isolated system will either increase or remain the same

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18
Q

entropy vs enthalpy

A

large change in entropy can drive a reaction despite enthalpic favourability

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19
Q

positive change in enthalpy

A

order to disorder

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20
Q

high to low enthalpy

A

negative change in enthalpy of system

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21
Q

Boltzmann formula

A

entropy = boltzmann constant *ln(number of accessible microstates)

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22
Q

Boltzmann constant

A

1.3*10^-23 J/K

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23
Q

minimum entropy

A

0

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24
Q

entropy relation to microstates

A

less entropy = less translational microstates accessible

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25
Q

KE relation to accessible microstates

A

as KE decreases so does number of accessible microstates

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26
Q

entropies of perfectly crystalline substances at 0K

A

0

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27
Q

Gibbs free energy function

A

determines whether reaction is favourable

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28
Q

Gibbs free energy equation

A

free energy change = enthalpy change - temperature*entropy change

29
Q

Gibbs free energy change at constant temp and pressure

A
  • temperature * change in total entropy
30
Q

when is a reaction feasible?

A

when free energy change is negative

31
Q

when is a reaction not feasible?

A

when free energy change is positive?

32
Q

G in relation to useful work

A

what’s left from internal energy and entropy changes in system after taking away wasted work

33
Q

ATP synthesis favourability

A

unfavourable as gibbs energy change is +
couple to H+ transport

34
Q

when do molecules react in a collision

A

if KE > Ea

35
Q

what does most probable speed depend on?

A

mass/ temp

36
Q

kinetic energy formula

A

1/2 m v^2

37
Q

Kinetic energy average formula

A

3/2KbT

38
Q

what does RoR depend on?

A

temp
enzymatic catalysis
concentration

39
Q

first order reactions

A

single atom or molecule determines rate
e.g decomposition

40
Q

rate of decomposition

A

k[A]

41
Q

2nd order reactions

A

when 2 molecules collide to determine rate

42
Q

rate of 2nd order reactions

A

k[A]^2

43
Q

rate of bimolecular reaction

A

k[A][B]

44
Q

how are orders of reaction found?

A

experimentally or by full knowledge of the kinetic pathway

45
Q

what’s order of a reaction controlled by?

A

the slowest, rate-limiting step of a reaction

46
Q

Kc

A

[AB]/[A][B]

47
Q

Kc effect on product yield

A

Kc&raquo_space; 1 (mostly product)
Kc &laquo_space;1 (mostly reactant)
Kc = 1 (mixture)

48
Q

Le Chatelier’s principle

A

“when a system at eq is disturbed, system composition adjusts to minimise the disturbance”

49
Q

equilibrium formula for gibbs free energy change

A

-RTlnKeq
R= gas constant

50
Q

exponential effect on equilibrium constant

A

makes v sensitive to small changes in gibbs free energy

51
Q

pH formula

A

-log10[H+]

52
Q

pH effects

A

affects protein solvation
enzyme activity

53
Q

pH effect on cells

A

6-7 death
7-7.35 acidosis
7.45-7.8 alkalosis
7.8-9 death

54
Q

2H2O dissociation

A

H3O+ + OH-
hydroxonium doesn’t exist in water

55
Q

equilibrium constant of water

A

([H+][OH-])/[H2O]^2
H2O doesn’t change in aq solutions so
Kw = [H+][OH-]

56
Q

Kw at 25 degrees celcius

A

110^-14
therefore [H+]=[OH-]=110^-7

57
Q

free energy

A

weighted sum of partial molar Gibb’s energy

58
Q

entropic effect of mixing A with other components

A

RTln[A]

59
Q

conc difference enthalpy balancing reverse

A

electrical potential difference

60
Q

Nernst potential

A

electrical potential difference required to stop flow of ions arising from conc difference

61
Q

change in potential energy

A

q*change in v

62
Q

chemical potential difference

A

zFchange inV

63
Q

F

A

Faraday’s constant

64
Q

impermeable macromolecule charge density

A

125mM conc of e-=

65
Q

Donnan equilibrium

A

equilibrium internal concentration of each ion and membrane potential difference

66
Q

sodium anomaly

A

Nernst potential of Na is far more + than membrane potential
cellular osmolytes required so cell doesn’t burst

67
Q

how does pH imbalance store free energy

A

chemical contribution (concentration gradient)
electrostatic contribution (potential difference)

68
Q

combination of chemical and electrostatic contribution

A

proton motive force
-200mV

69
Q

rotary motors powered by proton flux

A

ATP synthase and bacterial flagellar motor

Cell biology semester 1 (6 decks)

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