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PHY1039
Properties of Matter
6 February, 2012
Lecture 1
Why Study Matter? Understanding Gases
http://www.jamie.aarontastic.com/Low%20Pressure%20Example.JPG
Meteorology: high and low pressure
Measuring Lung Capacity
http://www.heart-watch-blog.com/images/blogs/7-2007/lung-
capacity-7810.jpg
Ideal Gas:
Pressure, Volume,
Temperature
relationships
http://www.teslasociety.com/mars2.htm
Atmospheres of Planets
Thermal expansion of girders was
restricted by frictional forces. They could
not expand lengthwise, so they buckled!
Joints in bridges are used to
enable thermal expansion.
Why Study the Properties of Matter? Thermal Expansion
Pressure, volume and temperature are interrelated in solids.
http://communication.howstuffworks.com/laptop.htm/printable
Why Study the Properties of Matter? Heat Dissipation
Heat sinks, heat spreaders, and fans remove heat from the CPU of a laptop computer.
(The objective is to do electrical work, but heat is also given off in the process.)
Double-walled Multi-walled Single-walled
Carbon Nanotubes
Why Study the Properties of Matter?
Underlies (Nano)Technology
Electron microscope image of multi-walled carbon nanotubes
S. Iijima, Nature 354 (1991) 56.
Is it possible to construct a lift to satellites orbiting the Earth?
What Happens when Thermal Properties Go Wrong?
A failed O-ring allowed the escape of H2 gas. The result was an explosion = sudden release of heat
Challenger Space Shuttle Disaster
http://www.ssqq.com/archive/disasters.htm
Columbia Space Shuttle Disaster
Damage to the wing caused over-heating on re-entry into the atmosphere
Thermodynamics Provides Equations to Describe Properties of Matter
Properties are inter-related:
• Mechanical (elastic modulus and compressibility)
• Thermo-mechanical (expansivity)
• Thermal (heat capacity)
• Flow (viscosity)
A Typical Phase Diagram for the Three States of Matter
Figure from “Understanding Properties of Matter” by M. de Podesta
Solid Liquid: Melting (heat in) Liquid Solid: Freezing (heat out) Liquid Gas: Boiling (heat in) Gas Liquid: Condensation (heat out) Solid Gas: Sublimation (heat in) Gas Solid: Deposition (heat out)
Phase Transitions
Lines represent conditions where two phases co-exist. Three phases co-exist at the triple point.
Importance of Phase Transitions:
Laser Annealing
Laser annealing to create metal nanoparticles
Intense laser beam can melt
metals. The liquid metal flows and
makes small droplets on the
surface.
If the metal liquid is hot enough, it
evaporates into the air where it
forms nm-sized solid particles when
cooled.
Image: http://wps.prenhall.com/wps/media/objects/602/616516/Chapter_10.html
Phase Diagram for Carbon Dioxide
atm = atmospheres (a unit of pressure)
Image: http://wps.prenhall.com/wps/media/objects/602/616516/Chapter_10.html
Phase Diagram for Water
States of Matter Gas • Atoms/molecules randomly distributed
throughout their container. • Have a distribution of mean speeds. • Travel in all directions. • Low density: the mean free path is about
l= 3 nm in air under standard conditions.
Liquids • Atoms/molecules randomly distributed
throughout their container (like gas). • Have a distribution of mean speeds. • Vibrate in all directions. • Density is higher than in a gas. • Separated from gas by a meniscus.
Crystalline Solids • Atoms/molecules arranged on a periodic
array in three dimensions (a lattice) • Vibrate in all directions • Density is usually higher than the liquid’s.
Atoms are in close contact.
Figures from “Understanding Properties of Matter” by M. de Podesta
Mean Free Path of Gas Molecules
Molecules travel a distance of l in between collisions.
Bonds in Solids
In simple cubic packing, each atom has six nearest neighbours.
The bond between two atoms with a mass of m can be modelled as springs, with a spring constant, K, showing simple harmonic motion with a resonant frequency of f0:
When the atoms vibrate and stretch the springs, the potential energy rises. The kinetic energy also oscillates as the velocity changes during the vibrations.
Figures from “Understanding Properties of Matter” by M. de Podesta
𝑓0=1
2𝜋
𝐾
𝑚
“Sea of electrons”: electrons are shared between all atoms, i.e. delocalised
Ionic bonds: Coulombic attraction between cations (+ve) and anions (-ve)
Weak van der Waals’ attraction between individual charge-neutral molecules; No sharing of electrons
Classification of Solids
(2) Ionic (1) Molecular
(4) Metal (3) Covalent
Electrons are shared in bonds between neighbouring atoms Bonds extend in prescribed directions
Figure from “Understanding Properties of Matter” by M. de Podesta
Potential Energy, u, between Ions
For a singly-charged cation (+ve) and an anion (-ve) at a distance of ro, the potential energy is:
u = −𝑒2
4𝜋𝜀𝑜𝑟𝑜
In an ionic solid, there are interactions between ions in three dimensions and at regularly spaced distances.
Figure from “Understanding Properties of Matter” by M. de Podesta
e = charge on the electron: 1.602 x10-19 C
eo = permittivity of free space:
8.854 x10-12 Fm-1
Potential Energy, u, between Neutral Atoms
Averaged over time, electrons are uniformly distributed around an atom’s nucleus.
But at any given instant, the electron charge distribution is non-uniform.
There is an attraction between the oppositely-charged sides of atoms:
Electron distribution at intervals of 10-16 seconds
Potential energy: r
𝑢~−1
𝑟6
Potential Energy for Non-Charged Atoms/Molecules
r
s
r/s r/s
Po
ten
tial
En
erg
y
Potential Energy
varies with the
separation distance, r. There is also kinetic
energy, which is the
energy of motion.
Figure from “Understanding Properties of Matter” by M. de Podesta
~ r -6