biophysics Flashcards

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
KE relation to accessible microstates
as KE decreases so does number of accessible microstates
26
entropies of perfectly crystalline substances at 0K
0
27
Gibbs free energy function
determines whether reaction is favourable
28
Gibbs free energy equation
free energy change = enthalpy change - temperature*entropy change
29
Gibbs free energy change at constant temp and pressure
- temperature * change in total entropy
30
when is a reaction feasible?
when free energy change is negative
31
when is a reaction not feasible?
when free energy change is positive?
32
G in relation to useful work
what's left from internal energy and entropy changes in system after taking away wasted work
33
ATP synthesis favourability
unfavourable as gibbs energy change is + couple to H+ transport
34
when do molecules react in a collision
if KE > Ea
35
what does most probable speed depend on?
mass/ temp
36
kinetic energy formula
1/2 m v^2
37
Kinetic energy average formula
3/2KbT
38
what does RoR depend on?
temp enzymatic catalysis concentration
39
first order reactions
single atom or molecule determines rate e.g decomposition
40
rate of decomposition
k[A]
41
2nd order reactions
when 2 molecules collide to determine rate
42
rate of 2nd order reactions
k[A]^2
43
rate of bimolecular reaction
k[A][B]
44
how are orders of reaction found?
experimentally or by full knowledge of the kinetic pathway
45
what's order of a reaction controlled by?
the slowest, rate-limiting step of a reaction
46
Kc
[AB]/[A][B]
47
Kc effect on product yield
Kc >> 1 (mostly product) Kc << 1 (mostly reactant) Kc = 1 (mixture)
48
Le Chatelier's principle
"when a system at eq is disturbed, system composition adjusts to minimise the disturbance"
49
equilibrium formula for gibbs free energy change
-RTlnKeq R= gas constant
50
exponential effect on equilibrium constant
makes v sensitive to small changes in gibbs free energy
51
pH formula
-log10[H+]
52
pH effects
affects protein solvation enzyme activity
53
pH effect on cells
6-7 death 7-7.35 acidosis 7.45-7.8 alkalosis 7.8-9 death
54
2H2O dissociation
H3O+ + OH- hydroxonium doesn't exist in water
55
equilibrium constant of water
([H+][OH-])/[H2O]^2 H2O doesn't change in aq solutions so Kw = [H+][OH-]
56
Kw at 25 degrees celcius
1*10^-14 therefore [H+]=[OH-]=1*10^-7
57
free energy
weighted sum of partial molar Gibb's energy
58
entropic effect of mixing A with other components
RTln[A]
59
conc difference enthalpy balancing reverse
electrical potential difference
60
Nernst potential
electrical potential difference required to stop flow of ions arising from conc difference
61
change in potential energy
q*change in v
62
chemical potential difference
zFchange inV
63
F
Faraday's constant
64
impermeable macromolecule charge density
125mM conc of e-=
65
Donnan equilibrium
equilibrium internal concentration of each ion and membrane potential difference
66
sodium anomaly
Nernst potential of Na is far more + than membrane potential cellular osmolytes required so cell doesn't burst
67
how does pH imbalance store free energy
chemical contribution (concentration gradient) electrostatic contribution (potential difference)
68
combination of chemical and electrostatic contribution
proton motive force -200mV
69
rotary motors powered by proton flux
ATP synthase and bacterial flagellar motor