Quantum Refrigeration & Absolute Zero Temperature Yair Rezek Tova Feldmann Ronnie Kosloff.
PX3012 The Solid State Course coordinator: Dr. J. Skakle CM3020 Solid State Chemistry Course...
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Transcript of PX3012 The Solid State Course coordinator: Dr. J. Skakle CM3020 Solid State Chemistry Course...
PX3012
The Solid State
Course coordinator:
Dr. J. Skakle
CM3020
Solid State Chemistry
Course coordinator:
Dr. J. Feldmann
SOLID STATECrystals
Crystal structure basics unit cells symmetry lattices
Some important crystal structures and properties close packed structures octahedral and tetrahedral holes basic structures ferroelectricity
Diffraction how and why - derivation
Objectives
By the end of this section you should:• be able to identify a unit cell in a symmetrical
pattern• know that there are 7 possible unit cell shapes• be able to define cubic, tetragonal,
orthorhombic and hexagonal unit cell shapes
Why Solids?
most elements solid at room temperature
atoms in ~fixed position
“simple” case - crystalline solid
Crystal Structure
Why study crystal structures?
description of solid
comparison with other similar materials - classification
correlation with physical properties
Crystals are everywhere!
More crystals
Early ideas• Crystals are solid - but solids are not
necessarily crystalline• Crystals have symmetry (Kepler) and long
range order• Spheres and small shapes can be packed to
produces regular shapes (Hooke, Hauy)
?
Group discussionKepler wondered why snowflakes have 6 corners,
never 5 or 7. By considering the packing of polygons in 2 dimensions, demonstrate why pentagons and heptagons shouldn’t occur.
Definitions1. The unit cell
“The smallest repeat unit of a crystal structure, in 3D, which shows the full symmetry of the structure”
The unit cell is a box with:
• 3 sides - a, b, c
• 3 angles - , ,
Seven unit cell shapes
• Cubic a=b=c ===90°
• Tetragonal a=bc ===90°
• Orthorhombic abc ===90°
• Monoclinic abc ==90°, 90°
• Triclinic abc 90°
• Hexagonal a=bc ==90°, =120°
• Rhombohedral a=b=c ==90°
Think about the shapes that these define - look at the models provided.
2D example - rocksalt (sodium chloride, NaCl)
We define lattice points ; these are points with identical environments
Choice of origin is arbitrary - lattice points need not be atoms - but unit cell size should always be the same.
This is also a unit cell - it doesn’t matter if you start from Na or Cl
- or if you don’t start from an atom
This is NOT a unit cell even though they are all the same - empty space is not allowed!
In 2D, this IS a unit cellIn 3D, it is NOT
All M.C. Escher works (c) Cordon Art-Baarn-the Netherlands.All rights reserved.
Examples
The sheets at the end of handout 1 show examples of periodic patterns. On each, mark on a unit cell. [remembering that there are a number of different (correct) answers!]
SummarySummary
Unit cells must link up - cannot have gaps between adjacent cells
All unit cells must be identical
Unit cells must show the full symmetry of the structure next section