Characteristics of Soft Matter(1) Length scales between atomic and macroscopic

(sometimes called mesoscopic)(2) The importance of thermal fluctuations and Brownian

motion

(3) Tendency to self-assemble into hierarchical structures (i.e. ordered on multiple size scales beyond the molecular)

(4) Short-range forces and interfaces are important.

In the previous lecture:

Lecture 2:

Polarisability and van der Waals’ Interactions:

Why are neutral molecules attractive to each other?

Soft Matter Physics18 February, 2010

See Israelachvili’s Intermolecular and Surface Forces, Ch. 4, 5 & 6

What are the forces that operate over short distances and hold soft matter together?

http://www.cchem.berkeley.edu/rmgrp/about_gecko.jpg

Interaction Potentials

• For two atoms/molecules/segments separated by a distance of r, the interaction energy can be described by an attractive potential energy: watt(r) = - Cr -n = -C/r n, where C and n are constants.

• There is also repulsion because of the Pauli exclusion principle: electrons cannot occupy the same energy levels.

• Treat atoms/molecules like hard spheres with a diameter, s. Use a simple repulsive potential:

wrep(r) = +(s/r)

• The interaction potential w(r) = watt + wrep

r

s

“Hard-Sphere” Interaction Potential

+

w(r)

-

Attractive potential

r

watt(r) = -C/rn

+

w(r)

-

Repulsive potential

rswrep(r) = (s/r)

Hard-Sphere Interaction Potentials

+

w(r)

-Total potential:

r

w(r) = watt + wrep

s

Minimum of potential = equilibrium spacing in a solid = s

The force, F, acting on particles with this interaction energy is:

drdw

F

Interaction Potentials

• Gravity: all atoms/molecules have a mass!• Coulomb: applies to ions and charged molecules;

same equations as in electrostatics• van der Waals: classification of interactions that

applies to non-polar and to polar molecules (i.e. without or with a uniform distribution of charge). IMPORTANT in soft matter!

• How can we describe their potentials?

Gravity: n = 1

r

m1m2

r

mGmrmGmrw 211

21)(

G = 6.67 x 10-11 Nm2kg-1

When molecules are in contact, w(r) is typically ~ 10-52 J

Negligible interaction energy!

Coulombic Interactions: n = 1

r

Q1Q2 rQQ

rwo4

21=)(

• With Q1 = z1e, where e is the charge on the electron, and z1 is an integer value.

• eo is the permittivity of free space and e is the relative permittivity of the medium between ions (can be vacuum with e = 1 or can be a gas or liquid with e > 1).

• The interaction potential is additive in crystals.

• When molecules are in close contact, w(r) is typically ~ 10-18 J, corresponding to about 200 to 300 kT at room temp.

Sign of w depends on whether charges are alike or opposite.

van der Waals Interactions (London dispersion energy): n = 6

r

a1a2

6)(

r

Crw

u2 u1

• Interaction energy (and the constant, C) depends on the dipole moment (u) of the molecules and their polarisability (a).

• When molecules are in close contact, w(r) is typically ~ 10-21 to 10-20 J, corresponding to about 0.2 to 2 kT at room temp., i.e. of a comparable magnitude to thermal energy!

• v.d.W. interaction energy is much weaker than covalent bond strengths.

Covalent Bond Energies

From Israelachvili, Intermolecular and Surface Forces

1 kJ mol-1 = 0.4 kT per molecule at 300 K

(Homework: Show why this is true.)

Therefore, a C=C bond has a strength of 240 kT at this temp.!

Hydrogen bonding

• In a covalent bond, an electron is shared between two atoms.• Hydrogen possesses only one electron and so it can covalently

bond with only ONE other atom.• The proton is unshielded and makes an electropositive end to the

bond: ionic character.• Bond energies are usually stronger than v.d.W., typically 25-100

kT.• The interaction potential is difficult to describe but goes roughly

as r -2, and it is somewhat directional. • H-bonding can lead to weak structuring in water.

HO

HH

HO

d+

d+

d+d+

d-d-

• When w(r) is a minimum, dw/dr = 0.• Solve for r to find equilibrium spacing for a solid, where r = re.• (Confirm minimum by checking curvature from 2nd derivative.)• The force between two molecules is F = -dw/dr• Thus, F = 0 when r = re.• If r < re, F is compressive (+); If r > re, F is tensile (-).• When dF/dr = d2w/dr2 =0, attractive F is at its maximum.

Significance of Interaction Potentials

re = equilibrium spacing

r

How much energy is required to remove a molecule from the condensed phase?

Q: Does a central molecule interact with ALL the others?

nrCrw =)(

Applies to pairs

L

s = molecular spacing when molecules are in contact

r = density = number of molec./volume

Individual molecules

•

s

Total Interaction Energy, E

Interaction energy for a pair: w(r) = -Cr -n

Volume of thin shell:

Number of molecules at a distance, r :

Total interaction energy between a central molecule and all others in the system (from s to L), E:

drrv 24)4()( 2drrrN

Lr

rnrn

CE

3-

1

)3-(

4- 3-

3)(1

)3(

4 nn Ln

CE

But L >> s! When can we neglect the term?

r -n+2=r -(n-2) System L

nrCrNrwE

24)()(

Conclusions about E

• There are three cases:• When n<3, then the exponent is negative. As L>>s, then

(s/L)n-3>>1 and is thus significant.• In this case, E varies with the size of the system, L! (This

result applies to gravitational potential in a solar system.) • But when n>3, (s/L)n-3<<1 and can be neglected. Then E is

independent of system size, L. • When n>3, a central molecule is not attracted strongly by

ALL others - just its closer neighbours!

[ ]3

33 )3(

4≈)(1

)3(

4n

nn n

CLn

C

E=

33

)(1)3(

4

n

n Ln

CE

The Third Case: n = 33)( Crrw

drrrN 24)(

lnln44

LCrCdr

ELr

r

s will be very small (typically 10-9 m), but lns is not negligible. L cannot be neglected in most cases.

What values of n apply to molecular interaction potentials? Is it >, < or = 3?

Polarity of Molecules• All interaction potentials (and forces) between molecules are

electrostatic in origin.• A neutral molecule is polar when its electronic charge distribution is

not symmetric about its nuclear (+ve charged) centre.• In a non-polar molecule the centre of electronic (-ve) charge does not

coincide with the centre of nuclear (+ve) charge.

+_

_ +

Dipole Moments

A “convenient” (and conventional) unit for polarity is called a Debye (D):

1 D = 3.336 x 10-30 Cm

qu =

The polarity of a molecule is described by its dipole moment, u, given as:

when charges of +q and - q are separated by a distance .

Typically, q is the charge on the electron: 1.602 x10-19 C and the magnitude of is on the order of 1Å= 10-10 m, giving u = 1.602 x 10-29 Cm.

+ -

Examples of Nonpolar Molecules: u = 0

CO2 O-C-O

CH4C

H

H

H

H C

H

HH

H109º

CCl4

ClC

Cl

ClCl

109º

methane

Have rotational and mirror symmetry

120

Top view

Examples of Polar MoleculesCH3Cl CHCl3

Cmxu 301024.6

Cmxu 301054.3

ClC

H

ClCl

C

Cl

HH

H

Have lost some rotational and mirror symmetry!

Unequal sharing of electrons between two unlike atoms leads to polarity in the bond.

Dipole moments

C=O u = 0.11 D

+ -

N

H HH u = 1.47 D

-

+

H

HO

- +

u = 1.85 D

SO Ou = 1.62 D

+

-

Bond moments

N-H 1.31 D

O-H 1.51 D

F-H 1.94 D

What is the S-O bond moment?

Find from vector addition knowing O-S-O bond angle.

V. High!

Vector addition of bond moments is used to find u for molecules.

H H

Given that the H-O-H bond angle is 104.5° and that the bond moment of OH is 1.51 D, what is the dipole moment of water?

q/2

O

1.51 D

uH2O = 2 cos(q/2)uOH = 2 cos (52.25 °) x 1.51 D = 1.85 D

Vector Addition of Bond Moments

Charge-Dipole Interactions

• There is an electrostatic (i.e. Coulombic) interaction between a charged molecule (an ion) and a static polar molecule.

• The interaction potential can be compared to the Coulomb potential for two point charges (Q1 and Q2):

• Ions can induce ordering and alignment of polar molecules.• Why? Equilibrium state when w(r) is minimum. w(r) decreases as q decreases

to 0.

24

cos)(

r

Qurw

o

r

QQrw

o4)( 21

Qqu

r

+

-w(r) = -Cr -2

Dipole-Dipole Interactions

• There are Coulombic interactions between the +ve and -ve charges associated with each dipole.

• In liquids, thermal energy causes continuous motion, i.e. tumbling, of dipoles in relation to each other.

• In solids, dipoles are usually fixed on a lattice with a certain orientation, described by q1 and q2.

q1

q21u

2u

+ +

--

Fixed-dipole Interactions

• The interaction energy, w(r), depends on the relative orientation of the dipoles:

• Molecular size influences the minimum possible r.• For a given spacing r, the end-to-end alignment has a

lower w, but usually this alignment requires a larger r compared to side-by-side (parallel) alignment.

q1

q21u 2u

f

]cossinsincoscos2[4

)( 2121321

r

uurw

o

r

Note: W(r) = -Cr -3

-

+

-

+

w(r)

(J)

r (nm)

At a typical spacing of 0.4 nm, w(r) is about 1 kT. Hence, thermal energy is able to disrupt the alignment.

nm10.=

nm10.=

-10-19

-2 x10-19

0

0.4

kT at 300 K

Dqu 1=||=||

End-to-end

Side-by-side

W(r) = -Cr -3

q1 = q2 = 0

q1 = q2 = 90°

From Israelachvili, Intermol.& Surf. Forces, p. 59

Freely-Rotating Dipoles• In some cases, dipoles do not have a fixed position and

orientation on a lattice but constantly move about.• This occurs when thermal energy is greater than the fixed

dipole interaction energy:

• Interaction energy depends inversely on T, and because of constant motion, there is no angular dependence:

321

4 r

uukT

o>

62

22

21

43 kTr

uurw

o )(_=)(

Note: W(r) = -Cr -6

Polarisability• All molecules can have a dipole induced by an external

electromagnetic field, • The strength of the induced dipole moment, |uind|, is

determined by the polarisability, a, of the molecule:

E

uind

=

Units of polarisability: J

mCNmC

CNCm

CmJCm 222

===

E

Polarisability of Nonpolar Molecules• An electric field will shift the electron cloud of a molecule.

• The extent of polarisation is determined by its electronic polarisability, ao.

+

_E

+_

Initial state In an electric field

Simple Bohr Model of e- Polarisability

eEu oind

==

Force on the electron due to the field: EeFext

=

Attractive Coulombic force on the electron from nucleus:

32

2

2

2

int 4=

4=sin

4=

)(=

R

ueRR

e

R

edR

RdwF

o

ind

oo

At equilibrium, the forces balance:int= FFext

Without a field: With a field:

Fext

Fint

int= FFext

eEu oind

==

34 R

ueEe

o

ind

=Substituting expressions

for the forces:

Solving for the induced dipole moment: ERu oind

34=

So we obtain an expression for the polarisability:34 Roo =

From this crude argument, we predict that electronic polarisability is proportional to the size of the molecule!

Simple Bohr Model of e- Polarisability

Units of Electronic Polarisability

3112

122

mmJC

JmC

Units of volume

Polarisability is often reported as:o

o

4

Electronic Polarisabilities

He 0.20

H2O 1.45

O2 1.60

CO 1.95

NH3 2.3

CO2 2.6

Xe 4.0

CHCl3 8.2

CCl4 10.5Largest

Smallest

Unitsao/(4o): 10-30 m3

Numerically equivalent to ao in units of 1.11 x 10-40 C2m2J-1

ao/(4o) (10-30 m3)

Example: Polarisation Induced by an Ion

Ca2+ dispersed in CCl4 (non-polar).

What is the induced dipole moment in CCl4 at a distance of 2 nm?

- +

By how much is the electron cloud of the CCl4 shifted?

From Israelachvili, Intermol.& Surf. Forces, p. 72

Example: Polarisation Induced by an IonCa2+ dispersed in CCl4 (non-polar). Eu oind

=

Affected by the permittivity of CCl4: e = 2.2

2

24 r

eu

o

oind

=

330105.104

mxo

o From the literature, we

find for CCl4:

24

2

r

eE

o=

Field from the Ca2+ ion:

We find at close contact when r = 2 nm:

uind = 3.82 x 10-31 Cm

Thus, an electron with charge e is shifted by:

02.01038.2 12 mxe

u Å

Polarisability of Polar MoleculesIn a liquid, molecules are continuously rotating and turning, so the time-averaged dipole moment for a polar molecule in the liquid state is 0.

Let q represent the angle between the dipole moment of a molecule and an external E-field direction.

The spatially-averaged value of <cos2q> = 1/3

The induced dipole moment is: 22

cos=kT

Euuind

An external electric field can partially align dipoles:

E +

-

The molecule still has electronic polarisability, so the total polarisability, a, is given as:

kTu

o 3

2

+= Debye-Langevin equation

kTu

orient 3

2

=As u = aE, we can define an orientational polarisability.

Origin of the London or Dispersive Energy• The dispersive energy is quantum-mechanical in origin, but we can treat it

with electrostatics.• Applies to all molecules, but is insignificant in charged or polar molecules.

• An instantaneous dipole, resulting from fluctuations in the electronic distribution, creates an electric field that can polarise a neighbouring molecule.

• The two dipoles then interact.

1 2

2- +1u

+ +- - 2u

1u

r

Origin of the London or Dispersive Energy

+ +- - 2u

1u

r

2123

1 314

/)cos+(= r

uE

o

u1

u2

The field produced by the instantaneous dipole is:

)(===

fr

uEuu

o

ooind 3

12 4

So the induced dipole moment in the neighbour is:

62

21

3

31

1

21321

444

4 ru

rr

uu

fr

uurw

o

o

o

o

o

o )(

)(),,()(

We can now calculate the interaction energy between the two dipoles (using the equation for permanent dipoles - slide 27):

Instantaneous dipole

Induced dipole

Origin of the London or Dispersive Energy

+ +- - 2u

1u

r

62

21

)4()(

r

urw

o

o

This result:

compares favourably with the London result (1937) that was derived from a quantum-mechanical approach:

62

2

)4(4

3)(

r

hrw

o

o

h n is the ionisation energy, i.e. the energy to remove an electron from the molecule

London or Dispersive Energy

62

2

)4(4

3)(

r

hrw

o

o

The London result is of the form: 6

)(r

Crw

In simple liquids and solids consisting of non-polar molecules, such as N2 or O2, the dispersive energy is solely responsible for the cohesion of the condensed phase.

where C is called the London constant:

2

2

)4(4

3

o

o hC

Must consider the pair interaction energies of all “near” neighbours.

SummaryType of Interaction Interaction Energy, w(r)

Charge-charge rQQ

o421 Coulombic

Nonpolar-nonpolar 62

2

443

r

hrw

o

o

)(_=)(

Dispersive

Charge-nonpolar 42

2

42 rQ

o )(_

Dipole-charge24 r

Qu

ocos_

42

22

46 kTruQ

o )(_

Dipole-dipole

62

22

21

43 kTruu

o )(_

Keesom

321

22

21

4 rfuu

o ),,(_

Dipole-nonpolar

62

2

4 ru

o )(_

Debye

62

22

4231

ru

o )()cos+(_

In vacuum: e=1

van der Waals’ Interactions

• Refers to all interactions between polar or nonpolar molecules, varying as r -6.

• Includes Keesom, Debye and dispersive interactions.

• Values of interaction energy are usually only a few kT.

Comparison of the Dependence of Interaction Potentials on r

Not a comparison of the magnitudes of the energies!

n = 1

n = 2

n = 3n = 6

Coulombic

van der Waals

Dipole-dipole

Charge-fixed dipole

Interaction energy between ions and polar molecules

• Interactions involving charged molecules (e.g. ions) tend to be stronger than polar-polar interactions.

• For freely-rotating dipoles with a moment of u interacting with molecules with a charge of Q we saw:

42

22

46 kTruQ

o )(_

• One result of this interaction energy is the condensation of water (u = 1.85 D) caused by the presence of ions in the atmosphere.

• During a thunderstorm, ions are created that nucleate rain drops in thunderclouds (ionic nucleation).

+Q

Measuring Polarisability• Polarisability is dependent on the frequency of the E-field. • The Clausius-Mossotti equation relates the dielectric constant

(permittivity) e of a molecule having a volume v to a:

43

21

4v

o

)(

43

21

4 2

2 vnn

o

o )(

• At the frequency of visible light, however, only the electronic polarisability, ao, is active.• At these frequencies, the Lorenz-Lorentz equation relates the refractive index, n (n2 = e) to ao:

So we see that measurements of the refractive index can be used to find the electronic polarisability.

Frequency dependence of polarisability

From Israelachvili, Intermol. Surf. Forces, p. 99

it.wikipedia.org/wiki/Legge_di_Van_der_Waals

PV diagram for CO2

RTnbVV

aP ))(( 2

Non-polar gasses condense into liquids because of the dispersive (London) attractive energy.

Van der Waals Gas Equation:

Measuring Polarisability• The van der Waals’ gas law can be written (with V = molar

volume) as:

RTnbVV

aP ))(( 2

33

2

C

a

The constant, a, is directly related to the London constant, C:

where s is the molecular diameter (= closest molecular spacing). We can thus use the C-M, L-L and v.d.W. equations to find values for ao and a.

Measuring Polarisability

From Israelachvili, Intermol.& Surf. Forces

Problem Set 11. Noble gases (e.g. Ar and Xe) condense to form crystals at very low temperatures. As the atoms do not undergo any chemical bonding, the crystals are held together by the London dispersion energy only. All noble gases form crystals having the face-centred cubic (FCC) structure and not the body-centred cubic (BCC) or simple cubic (SC) structures. Explain why the FCC structure is the most favourable in terms of energy, realising that the internal energy will be a minimum at the equilibrium spacing for a particular structure. Assume that the pairs have an interaction energy, u(r), described as

where r is the centre-to-centre spacing between atoms. The so-called "lattice sums", An, are given below for each of the three cubic lattices.

SC BCC FCC A6 8.40 12.25 14.45A12 6.20 9.11 12.13

Then derive an expression for the maximum force required to move a pair of Ar atoms from their point of contact to an infinite separation.

2. (i) Starting with an expression for the Coulomb energy, derive an expression for the interaction energy between an ion of charge ze and a polar molecule at a distance of r from the ion. The dipole moment is tilted by an angle q with relation to r, as shown below.

(ii) Evaluate your expression for a Mg2+ ion (radius of 0.065 nm) dissolved in water (radius of 0.14 nm) when the water dipole is oriented normal to the ion and when the water and ion are at the point of contact. Express your answer in units of kT.

Is it a significant value? (The dipole moment of water is 1.85 Debye.)

3. Show that 1 kJ mole-1 = 0.4 kT per molecule at 300 K.

,2)(6

6

12

12

rA

rAru

rq

ze

Interaction betw een ions andpolar molecules

• Interactions involving charged molecules (e.g. ions)tend to be stronger than polar-polar interactions.

• For freely-rotating dipoles with a moment of uinteracting with molecules with a charge of Q we saw:

42

22

46 kTruQ

o )(_

• One result of this interaction energy is the condensation ofwater (u = 1.85 D) caused by the presence of ions in theatmosphere.

• During a thunderstorm, ions are created that nucleate raindrops in thunderclouds (ionic nucleation).

Hydrogen bonding

• In a covalent bond, an electron is shared between two atoms.

• Hydrogen possesses only one electron and so it can covalently bond with only ONE other atom.

• The proton is unshielded and makes an electropositive end to the bond: ionic character.

• Bond energies are usually stronger than v.d.W., typically 25-100 kT.

• The interaction potential is difficult to describe but goes roughly as r-2, and it is somewhat directional.

• H-bonding can lead to weak structuring in water.

HO

HH

HO

d+

d+

d+d+

d-d-

Hydrophobic Interactions

• “Foreign” molecules in water can increase the local ordering - which decreases the entropy. Thus their presence is unfavourable.

• Less ordering of the water is required if two or more of the foreign molecules cluster together: a type of attractive interaction.

• Hydrophobic interactions can promote self-assembly.

A water “cage” around another molecule

Hydrophobic Interactions• The decrease in entropy (associated with the ordering of molecules)

makes it unfavourable to mix water with “hydrophobic molecules”.

• For example, when mixing n-butane with water: DG = DH - TDS = -4.3 +28.7 = +24.5 kJ mol-1. Unfavourable (+ve DG) because of the decrease in entropy!

• This value of DG is consistent with a “surface area” of n-butane of 1 nm2 and g 40 mJ m-2 for the water/butane interface; an increase in DG = gDA is needed to create a new interface!

• Although hydrophobic means “water-fearing”, there is an attractive van der Waals’ force (as discussed later in this lecture) between water and other molecules - there is not a repulsion! Water is more strongly attracted to itself, because of H bonding, however, in comparison to hydrophobic molecules.

De-wetting

“Froth flotation”

Protein folding

Adhesion in water

ImmiscibilityMicellisation

Association of molecules

Coagulation