Digital files - genes
Transformation of information
Transformation of energy
Transformation of structure
Text files - proteins
Homeostasis
Electromotive force
Proton-motive force
Molecular ATP machine
Hydrophobic- hydrophilic
balance
Aggregation
Spacio/temporal
organization
Biological space -
aqueous phase
Water as a reactant
C6H12O6 + 6O2 Þ 6H2O + 6CO2 + energy ATP+H2O Þ ADP + H3PO4 + energy
Polimerization,
condensation, hydrolysis
Perception of
water
The water molecule
OH distance = 0.958 Å HOH angle = 104.5o
Oxygen is electronegative it draws the electrons in the
bonds it shares with the hydrogen atoms towards it.
This results in the water molecule having a large dipole moment.
Dipole moment = 1.85 Debye = 6x10
-30Cm
Strength of an H-bond is related to - the D-H---A distance
- the D-H-A angle.
A hydrogen bond consists of a hydrogen atom lying between two small, strongly electronegative atoms with
lone pairs of electrons.
Hydrogen
bonds
Distance Van der Waals radius of
H: 1.1Å, O 1.5 Å.
Intermediate between VdW distance and typical O-H covalent
bond of 0.96Å.
In hydrogen bond separation is about 1 Å less!
It is 1.77 Å.
The closest VdW approach should be 2.6 Å.
The covalent bond between H and O in water (about 492 kJ mol-1).
The van der Waals interaction (about 5.5 kJ mol-1).
The hydrogen bond is
• part electrostatic (90%)
• and part covalent (10%)
The hydrogen bonds is in the range of 0.5 - 100 kJ mol-1.
The hydrogen bond is stronger than typical electrostatic interactions between partial charges, but it is easily disassociated by heat or by
interaction with other atoms.
The strength
Hydrogen bond is directional
( q )
q ' ' 1 cos
cos
12 66
12
÷ -
ø ç ö
è
æ -
÷ + ø ç ö
è
æ -
= r
B r
A r
B r
U A
Hydrogen bond potential energy
can hold two H-bonded molecules or groups in a specific
geometric arrangement
The hydrogen bonds define secondary structure of proteins.
They are
formedbetween the backbone oxygens and
amide hydrogens.
Hydrogen bonds define protein binding
specificity
Solid phase - ice
4 neighbors per molecule
lower density than liquid water H-bonding network
Only 42% of the volume is filled by the van der Waals volumes of the atoms, compared to
74% for spherical close packing.
Solid Ice vs. Solid Benzene
Liquid phase - water
The H-bonding
propensity of the water together with the tetrahedral geometry, leads to a higher entropy
in the bulk phase.
Cooperativity in hydrogen bond formation.
Hydrogen bonds half life = 10
-11– 10
-15sec.
The number of nearest neighbors in water is 4.4 (4 in ice).
Upon breakage of one hydrogen bond,
another hydrogen bond forms, with the
same partner or a new one, within 0.1 ps
High viscosity (0.89 cP, at 25 ° C)
Selected properties of water
High surface tension (72.75 mJ/m
2, at 20 ° C)
High specific heat capacity (C
V=4.18 J g
-1K
-1at 25 ° C) The dielectric constant is high (78.4 at 25 ° C)
Conductivity of protons is anomalously high
A low thermal expansivity (0.00021/ ° C at 20 ° C)
High boiling point
Dissociation
[H2O] ~ 55M and ionization is very weak, then [H2O] ~ constant.
For pure water KW=[H3O+][OH-] = 10-14
[H+] = [H3O+] = [OH-] = 10-7M In a neutral solution
[H
3O
+] = 10
-7M; [OH
-] = 10
-7M
That is only 1 H
+for every
560,000,000 water molecules!
O H
OH O
K H
OH O
H O
H O
H
eq
2 3
3 2
2
] ][
[
+ -- +
=
+
«
+
Acid-base chemistry is centered on water
The acidity of a solution is defined by the concentration of H+ ions.
pH = - log
10[H
+]
For pure water [H+] = 10-7 moles/L
Acid precipitation refers to rain, snow, or fog with
a pH lower than 5.6
The Acid Precipitation
Ocean acidification impacts shell formation of planktonic organisms
Definition of pK
a( )
( K H)e
aH
ln10 p p1
p
-1
-= + q
Titration curve:
One state transition
The pKa of a titrating site is defined as the pH for which the site is 50% occupied,
HA + H
2O Û A
-+ H
3O
+Deprotonation reaction
+ +
+ = = -
= H O H O
HA A HA
O H A
3 3
3 -
- 1
a a a
a a
a Ka a
q
q
θ is degree of protonation or occupancy:number of bound protons as a function of pH
% 11 90
1 = 10 » +
= pKa fA-
pH
% 9
1 »
-
= pKa fA-
pH
% 9 . 0
2 »
-
= pKa fA-
pH
pKa = 4.0
18
Different pathways of viral entry
Protomer
Pentamer
Capsid
(contains RNA genome)
FMDV Assembly
Acid sensitivity of Foot-and-Mouth Disease Virus (FMDV)
Histidine is a prime suspect
+ 0
Virus Capsid
Inter-pentamer interface
+ +
pH 7.0 pH 3.0
+
Proton transport in bulk water
The diffusion coefficient of each is similar to that of hydrated ion such
as Na
+Perception of
water
Water in
biological systems
• Intracellular water very close to any membrane or organelle (sometimes called vicinal water).
• The density of bound water is 10% higher and it has a 15%
greater heat capacity suggesting
much reduced molecular motion.
The whole cell water (70–80% of the total mass) is distributed into
only two to three
hydration layers around
macromolecules.
Representation of the first layer of interfacial water at
the surface of a protein.
Its highly heterogeneous structure reflects the
heterogeneity of the macromolecule surface.
Bound water ’ in
biological systems
Water molecules connecting the haem groups and protein residues of the two
identical subunits of Scapharca inaequivalvis haemoglobin. Note the symmetry of the two pentameric rings. On binding oxygen, the water molecules transfer
information between the subunits before the water cluster is disrupted .
Some surface water is well ordered
Royer et al. Proc. Natl Acad. Sci. USA 93, 14526 (1996).
A single water molecule in the ligand-binding site of concanavalin A functions as a link between Asp14, Asn16 and Arg228 of the protein and the 2'-OH hydroxyl group of the trimannoside ligand.
Some water is required for structure (function)
Li & Lazaridis, J. Phys. Chem. B 109, 662 (2005).
Retinal
LYS216
ASP85
ASP212
TYR57
THR205
TYR79 ARG82
GLU204
GLU194
Water molecules in bacteriorhodopsin; photoisomerization of all-trans-retinal (pKa 13) to 13-cis-retinal (pKa 8.45), drives a proton from its Lys216-Schiff base to Asp85
releasing the pentagonal hydrogen-bonded ring, flipping the Arg82 towards the
(arrowed) protonated water molecule, releasing a proton through a water wire) to the extracellular space. The Schiff base is reprotonated from the cytoplasm through
another associated water wire.
Some water is required for proton transfer
Garczarek & Gerwert, Nature 439, 109 (2005).
Rapid electron transfer between two molecules of bovine liver cytochrome b5. The electrostatic interactions of the water molecules provide a large donor-to-acceptor coupling that produces a smooth distance dependency for the electron-transfer rate.
Only the water cluster and the cytochromes are shown, and the protein residues are hidden.
Some water is required for electron transfer
Lin et al. Science 310, 1311 (2005).
Solubility in water
Water structure is different around the solute molecules:
DG = DH - TDS
Formation of ordered structure
hydrogen bonds
DG < 0 Soluble compound DG > 0 Hydrophobic/ insoluble compound
Water is a polar solvent: dissolves charged or polar compounds by replacing solute-solute H-bonds with solute-water H-bonds.
Non-polar molecules such as lipids and side chains of some amino acids
are hydrophobic
Amphipathic molecules have polar or charged regions, as well as non-polar regions.
Compounds that dissolve easily in water are hydrophilic.
Entropy increases as crystalline substances dissolve
Water interacts
electrostatically with charged solutes
Argon
Hydrophobic and hydrophilic hydration
33
Types of ions
Ion Surface charge
density Intra-cellular Extra-cellular Water preference
Ca2+ 2.11 10 nM 2.5 mM High density
Na+ 1.00 10 mM 150 mM High density
K+ 0.56 159 mM 4 mM Low density
• Structure-breaking ion 'chaotrope' (disorder-maker) (Na
+)
• structure-forming ion 'kosmotrope' (order-maker) (K
+)
• Kosmotropes shift the local equilibrium to the right.
• Chaotropes shift it to the left.
more dense water « less dense water
Moisture Sorption Isotherm
aw
Moisture content (d.w.b.)
Zone 3 Bulk water Zone 2
Loosely bound water Zone 1 Tightly bound water
- Activity – “effective concentration”
- Ion-ion and ion-H
2O interactions (hydration shell) cause number of ions available to react chemically ("free" ions) to be less than the number present
- Concentration can be related to activity using the activity coefficient g, where [a] = g (c)
The value of g depends on:
- Concentration of ions - Charge of the ion
- Diameter of the ion
Hydrophobic effect is crytical for biological systems
This is not an intermolecular force, but rather
the effect due to the peculiar solvent – water.
Glucose Aspartate Glicine
Lactate Glycerol
Hydrophilic molecules
Phenylalanine
Phosphatidylcholine
Hydrophobic molecules
Amphiphilic molecules
Arrangement of water molecules is barely disturbed
5
Polar molecule dissolved in water
Non-polar
molecule dissolved in water
Introduction of a hydrocarbon molecule creates a unfavourable cavities in water.
By clumping together in water hydrophobic molecules can reduce the total surface area of the cavity (ΔS > 0).
q System explores different conformations through diffusion and random thermal motion.
There is no “ hydrophobic force ” !!!
Lipid supension
v Water concentration – 55 M v Lipid concentration < 1 µM
107
5 . 5 ´ molecules »
lipid
molecules water
q The water molecules easily change orientations, or move to new neighboring locations.
q System will stay with the lowest energy conformation it encounters.
Alcohol dehydrogenase (homodimer)
Dimer
A B
B A
90°
Hydrophobic
sidechains coloured yellow
The strength of the hydrophobic interaction is
proportional to the total hydrophobic surface area
buried.
Exterior (hydrophilic)
A subunit
180°
Interior (hydrophobic)
A subunit
Amphipatic
compounds in
aqueous solution
The hydrophobic effect can be used for creating well- defined supramolecular assemblies.
Spherical Micelle
(zero-dimensional ensemble)
Cylindrical Micelle (one-dimensional ensemble)
Vesicle
(two-dimensional ensemble)
Spherical micelles of PS-PAA amphiphile
Cylindrical micelles of PS-PAA amphiphile
Perception of
water
Diffusion
Thermal fluctuations Low Reynold’s number
The radius of a water molecule is about 0.1 nm.
Protein radius is in the range 2 - 10 nm.
Fluid can be considered as a continuum
A system is not in equilibrium when the macroscopic parameters (T, P, etc.) are not constant throughout the system.
To approach equilibrium, these non-uniformities have to be dissipated through the transport of energy, momentum, and mass.
The mechanism of transport is molecular movement.
Transport Phenomena
2 1
2
3 2 1 2
3
÷ ø ç ö
è
= æ
=
M v kT
v M kT
For T = 300 K
500 Da (ATP) – v = 70 m/s
50 000 Da (protein) – v = 7 m/s
6.25 GDa (200 nm diameter vesicle) – v = 600 µm/s
Molecular speed
Actual velocity Þ Maxwell ’ s distribution
RT Mv
e RT v
v M
f
2 22 /
3 2
4 2 )
( ÷
-ø ç ö
è
= æ
p p
Macroscopic theory of diffusion:
x
Assumptions:
1. conservation of mater
2. the relation between gradient and flux is linear
0
dx
Adolf Eugen Fick (1829-1901)
x D C
t C
2 2
¶
= ¶
¶
¶
Jx in Jx out
x D C Jx
¶ - ¶
=
Fick’s 1st law:
x J t
C
¶ - ¶
¶ =
From the ¶
conservation of mater: Fick’s 2nd law:
In thermodynamic terms, we're watching the increase in entropy within a small, isolated system without an input of
energy.
Units m
2s
-1The solution which corresponds to an initial condition that all particles are at x =0 at t =0:
n x, t
( )
= kDt exp − x2 4Dt
"
#$ %
&
'
k is a normalization factor
The rms displacement of particles:
Dt x
2»
dc(x, y, z)
dt x,y,z = D d2C
dx2 + d2C
dy2 + d2C dz2
!
"
# $
%&
t
C t D
and C C
D
J = Ñ
2¶ Ñ ¶
-
! =
In three dimensions:
= 0 x
The random walk of a large number of particles results with
deterministic flow of particles.
Diffusive transport in biology
dx D dC J
x= -
A concentration penalty
The time penalty – <X2> = 4Dt
No directional specificity D ~ 10 -5 for most small molecules in water
Perception of
water
Forces acting on a particle due to the solvent:
(i) Stochastic thermal (Langevin) force:
Averageing over a large number of particles
The Langevin approach – dissipative force
changes direction and magnitude averages to zero over time
0 )
( t =
x
(ii) a viscous drag force that always slows the motions.
v
f = - z
friction (damping) coeff.viscosity
Stokes law
ph R
z = 6
The thermal forces
nN f » 4 . 5
The gravitational force
F
g» 10
-14nN << f
Newton’s law for the protein motion in a one-dimensional domain of length L, x(t):
L t
x t
f dt v
m dv dt v
dx
B
£ £
+ -
=
= , z ( ) 0 ( )
) ) (
( 2
) (
2
2 2 2
2 2
t dt xf
x mv d
dt x d
m
+
B-
=
- z
The average over a large number of proteins
) 2 (
2
2 2
2 2 2
t dt xf
x mv d
dt x m d
+
B-
=
- z
Integrating twice between t = (0, t) with x(0) = 0:
[ ( 1 ) ]
), 2 1
2 (
22
t
t
t
z z
B t
B t
k T t e
x T e
k dt
x
d
- -- -
= -
=
where t = m/z.
The protein behaves as a ballistic particle moving with a velocity v = (kBT/m)1/2. For a protein with m = 10-21 kg, v = 2 m/s.
In a fluid the protein moves at this velocity only for a time t ~ m/z = 10 -13 sec – shorter than any motion of interest in a molecular motor.
During this time the protein travels a distance v · t ~ 0.01 nm before it collides with another molecule.
For
t << t
, the exponential can be expand to secondorder:
)
2
(
2
= t t << t
m T x k
B[ ( 1 ) ]
2
2 t
tz
B
T t e
tx = k - -
-) 2 (
2
t
z >>
= k T t t
x
BWhen
t >> t
, the exponential term disappears and:For protein typically D ~ 10-11 m2/sec.
Because <x2> = 2Dt (Einstein relation – 1905):
z
T
D = k
BFriction is quantitatively related to diffusion
[ ( 1 ) ]
2
2 t
tz
B
T t e
tx = k - -
-Brownian motion
Brown (1827): observed irregular movement of pollens in water under microscope.
Major contribution of Brown: made sure non-organic particles also have Brownian motion, confirmed that Brownian motion is not a manifestation of life.
Robert Brown
The random impulses from the water molecules are uncorrelated with position.
0 )
( )
( t × f t =
x B
Einstein, Brownian motion, and atomic hypothesis
Albert Einstein published 4 papers in the Annalen der Physik in 1905.
– Photoelectric effect – Brownian motion
– Special theory of relativity
Albert Einstein, 1905
• Drag force: f = gv
• Diffusion due to random walk: d
2= 6Dt
• To reach equilibrium: Dg = kT
• Random collisions (random walk) are related to the
dissipation of kinetic energy to solvent molecules.
External forces acting on macromolecules
) ) (
,
( f t
t t x dt
dx
+ B
¶ - ¶
= f
z
Langevin equation
The inertial term is neglected.
) ( )
,
( x t f t dt F
dx
+
B=
z ×
Forces acting on proteins can be characterized by a potential
x t t x
x
F ¶
- ¶
= ( , ) )
,
( j
Perception of
water
(1) Fluids have density ( r ), and thus moving fluids have momentum (requires a force to start or stop them).
(2) Fluids have viscosity
(1) Viscosity changes with temperature and salinity (2) When fluids contact a solid, there is a thin layer
that sticks very tightly to the solid surface. = “No- slip condition”.
Characteristics of Fluids
Momentum Transfer, Viscosity
vx
Drag – transfer of the momentum in Dz
the direction perpendicular to velocity.
Laminar flow between two surfaces moving with respect to each other.
Δ px
Δ t ≡ Fx ∝ A ⋅ v
(
x, top − vx, bottom)
Δ z
z u d A
F
x x= h D
Fx – the viscous drag force, h - the coefficient of viscosity Fx/A – shear stressShear viscosity h is the proportionality between the velocity
gradient and the force required, per area, to keep the plates moving at constant velocity.
h(kg/m•sec at 20o C)
Water 10-3
Olive oil 0.084
Glycerine 1.34
Glucose 1013
Dimensionless constant
The Reynolds Number
108 1000
103 years 109
10 m Whale
10-5 10-3
1 msec 10-12
1 µm Bacterium
Reynolds number Swimming
speed [cm/s]
Diffusion time Mass
[g]
When the Reynolds number ‘R’ is small the viscous forces dominate.
Shark skin delays transition to turbulence