Part 3 Flashcards

1
Q

What is an important factor in SCM phase transitions?

A

the dynamics of the transition

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What are the most common transition types?

A
  • liquid liquid

- melting and crystallisation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is used to predict phase coexistence?

A

mean field theory

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

How are liquid-liquid transitions described?

A
  • quantum behaviour is not important
  • use mean field theory to calculate free energy of mixing
  • assume no concentration fluctuations
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Entropy of liquid-liquid mixing

A
  • consider atoms and molecules to be arranged on a lattice
  • in mean field theory sites a and b are independent of each other
  • P(a next to b) = P(b next to b) providing the concentrations of a and b are equal
  • use Boltzmann equation to calculate the entropy of mixing
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Energy of liquid liquid mixing

A
  • maximum a,b interaction occurs when their mole fractions are 0.5
  • an ideal entropy situation is described where ab> aa and bb interactions
  • if X> 2 there are two coexisting phases with minimal free energy
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

When is a system spinodal?

A
  • when the curve of free energy is zero

- beyond this the system is unstable to small composition fluctuations

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

When is a system metastable?

A
  • when fluctuations in composition increase the free energy

- to achieve phase separation the system must go through an energy barrier

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

When is a system unstable?

A
  • when fluctuations in composition reduce the free energy of the system
  • the system phase separates
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What liquid demixing mechanism occurs below the spinodal curve?

A
  • unstable composition
  • phase separation occurs by continual composition change
  • results in an irregular structure
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What liquid demixing mechanism occurs in the metastable region?

A
  • nucleation of one phase into the other

- often involves an activation energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Why is the mixture unstable within the spinodal curve?

A
  • all composition changes reduce the free energy

- fluctuations are amplified

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What does the strange free energy curvature cause?

A
  • flow of matter from areas of low concentration to areas of high concentration
  • fast diffusion has a higher energy cost
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

How are droplets formed?

A

by large fluctuation in mole fraction

- small droplets formed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

How is the decomposition process characterised?

A
  • by a length scale
  • optimum size of droplets formed fastest
  • forms patterns in the decomposition process
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

How do domain sizes change?

A
  • size of domain changes with time
  • as q increases do does domain size
  • coarsening occurs when a system grows into large domains to minimise the total interfacial energy
17
Q

Why is classical nucleation theory needed?

A
  • nucleation of a new phase into an existing one often involves an energy barrier and is an activated process
  • The more molecules involved lead to higher energy clusters with higher interface energies
18
Q

How are freezing and melting described?

A
  • No simple mean field theory for these transitions
  • There is a change in symmetry going from liquid with local order to a solid with global order
  • Kinetics is similar to liquid liquid demixing
19
Q

How are heterogenous and homogenous nucleation different?

A
  • homogeneous nucleation which occurs in pure solution

- heterogeneous nucleation which involves a 3rd species in addition to the melt solid

20
Q

Describe Homogenous Nucleation

A

• An activated process due to the energy cost associated with the increased interfacial area when a crystal is grown

  • Requires high activation energy and nucleation often occurs through heterogeneous nucleation
  • Tend to form spheres, unless crystals are involved in which case specific faces grow first
  • Free energy change depends on the degree of supercooling,
21
Q

How does a crystal form in homogenous nucleation?

A
  • As you move down in temperature the free energy barrier decreases until at some point it can be overcome by thermal fluctuations, causing the formation of a crystal
  • As soon as a crystal forms the rest of the molecules have a lattice template and can also from crystal as there is no longer a free energy barrier
22
Q

Describe Heterogenous nucleation

A
  • Activation energy is reduced
  • Described using a contact angle model
  • The affinity of a solid towards a surface depends on the contact angle, depending on 3 surface tensions
  • Critical radius is independent of a solid and liquid affinity of the mould but free energy is very dependent
  • If the contact angle is 180o nucleation will happen in bulk solution “drying transition” and is effectively homogeneous in nature
  • As you decrease the contact angle the free energy of heterogenous nucleation becomes more favourable/ larger

Free energy is proportional to surface tension, therefore large areas cause large free energies which lead to aggregation