Ch1. Structure of Solid

Instructor: Dr. Indranil Bhaumik

 Three (/four) states of matter:  Why to study Solids? Amorphous: lacks a systematic atomic arrangement (no long range order) Crystalline material: atoms organized in a periodic array (long range order)

SiO2 (quartz) crystal (2d projection)

SiO2 glass (amorphous)

CRYSTAL STRUCTURE A crystal is constructed by infinite repetition of identical structural units in space. Crystal structure = Lattice + Basis ‘Lattice’ is a regular periodic arrangement of points in space. ‘Basis’ is the collection of atoms attached identically* to each lattice point (*identical in composition, arrangement and orientation)

1

Periodicity is the main key!! Solid materials possess crystalline structure that means: It has: spatial periodicity or translation symmetry.

1D:

2D:

In 3D: We assume that there are 3 non-coplanar vectors a1, a2, and a3 that leave all the properties of the crystal unchanged after the shift as a whole by any of those vectors. As a result, any lattice point R' could be obtained from another point R as R' = R +m1a1 + m2a2 + m3a3 = R + T where, mi are integers, T= m1a1 + m2a2 + m3a3 is called the translational vector. (bold are vectors) Such a lattice is called the Bravais lattice.

2

UNIT CELL: Contains all the necessary points on the lattice that can be translated to repeat itself in an infinite array. In other words, the unit cell defines the basic building blocks of the crystal, and the entire crystal is made up of repeatedly translated unit cell. Choice of unit cell is not unique! Unit cell containing lattice point only at the corner is called Primitive unit cell. Non-primitive unit cell

Examples One dimensional lattices

Two-Dimensional Lattices (hypothetical)

The are 5 basic classes of 2D lattices 3

Three-Dimensional Lattices (real case): Crystal system (7) - Primitive unit cells 1. Cubic a=b=c

2. Tetragonal

α =β=γ =9 0 °

a =b ≠ c

3. Orthorhombic: a≠b≠c

4. Hexagonal

a=b≠c

5. Rhombohedral (Trigonal)

6. Monoclinic:

7. Triclinic

a≠b≠c

a≠b≠c

α = β=γ =9 0 °

α=β=γ=90°

α=β=90°, γ=120°

a=b=c

α =β=γ ≠ 9 0 °

α=γ=90°, β ≠ 90°

α ≠β ≠γ ≠ 90°

4

More Bravais lattice ? Can we add more points at judicious locations to any of the 7 crystal system and get other distinct lattice? Condition : Translational symmetry still maintained. Rotation and reflection symmetry in the crystal system need to be preserved. Possibilities:

• • • •

Primitive (P) At body centre (I) At all face centres (F) At c / a / b face centre (base centerd)

In cubic system: P, I, F are distinct. Base centred lattice violates the symmetry (3 fold symmetry along body diagonal is lost) consideration hence not a valid one.

In tetragonal:

Only P and F are distinct.

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Total no. of Bravais lattice: 14 (a) cubic (3): Primitive, body centred (BCC), face centred (FCC) (b) tetragonal (2): Primitive, centered tetragonal (c) orthorhombic (4): Primitive, base centered, body centered, face centered. (d) monoclinic (2): Primitive, centered monoclinic (e) triclinic (1): Primitive (f) trigonal (1): Primitive (g) hexagonal (1): Primitive

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Note: After adding extra lattice point translational symmetry still holds (ex:BCC) with new sets of translation vectors.

Some terminologies: 1. Number of lattice points/ unit cell: Counting the number of lattice points within the unit cell Many atoms are shared between unit cells Simple cubic structure: 8 corners x 1/8 = 1 lattice point Body-centered cubic structure: (8 corners x 1/8) + 1 body = 2 lattice points For Face-centered cubic structure? 7

2) Fractional coordinates Used to locate lattice points within unit cell

2`

FC C :

1. 0,0,0

1. 2. 3. 4.

0, 0, 0 ½, ½, 0 ½, 0, ½ 0, ½, ½

3` 4

3. Nearest distance between lattice points: Distance between two closest existing lattice points. Simple cubic: a 4. Packing density: Pack with biggest possible hard spheres of equal size placing them in each lattice point in the unit cell. Packing density = total volume occupied by ‘them’/ total volume of the unit cell (Important: keep in mind the share of lattice points to each unit cell!!!) First thing: Find out the biggest possible sphere that can be accommodated in the lattice. Example: For SC: radius of biggest possible sphere that can be accommodated = a/2. 1 sphere share/unit cell The packing density:

. FCC ?? 8

Lattice type Simple cubic

Number of lattice points unit cell 1

Nearest distance Maximum packing between lattice Example density points a Phosphor π/6 = 52 %

BCC

2

a√3/2

π√3/8 = 68 %

Tungsten

FCC

4

a/√2

π√2/3 = 74 %

Aluminum

A few (real) structures as example: NaCl (Sodium Chloride) Bravais lattice: Face centred cubic (FCC ) with Na-Cl as basis. Lattice points: 0,0,0; 0,1/2,1/2; 1/2,0,1/2; and 1/2,1/2,0. Atoms: Cl-: 0,0,0; 0,1/2,1/2; 1/2,0,1/2; and 1/2,1/2,0 + Na : ½, ½, ½; ½,0,0; 0, ½,0; 0,0, ½

Diamond lattice Bravais lattice: Face centered cubic, contains two identical atoms per lattice point. The distance between the two atoms equals one quarter of the body diagonal of the cube. Ex: diamond(C), germanium (Ge) and silicon (Si).

Zinc-blende lattice . as diamond with two different atoms per lattice point. Same Example:Zinc blende (ZnS), gallium arsenide, Cu/Fe Bravais lattice: FCC Look for more examples. 9

Index system for crystal planes (Miller Index): Aim: to identify planes in crystal Written as (hkl); h,k,l are integer values, called Miller indices. 1. Find intercepts on x,y,z: Example: 1/4, 2/3, ½ 2. Take reciprocals 4, 3/2, 2 3. Multiply up to integers: (8 3 4) [if necessary] Miller index of the plane 4. Replace negative integers with bar over the number, i.e. we replace -h by

Plane perpendicular to y cuts at ∞, 1, ∞ → (0 1 0) plane

This diagonal cuts at 1, 1, ∞ → (1 1 0) plane

d-spacing The perpendicular distance between pairs of adjacent planes is the d-spacing For cubic crystals: a=b=c

e.g. for (1 0 0) d=a (2 0 0) d = a/2 (1 1 0) d = a/√2 etc. 10

DIRECTIONS IN A LATTICE 1. Vector components of the direction are resolved along each of the coordinate axes and reduced to the smallest integers. 2. All parallel directions have the same direction indices. 3. Equivalent directions have the same atom spacing.

?

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Addition Reading: The Reciprocal Lattice Direct lattice  Fourier transformation  reciprocal lattice Reciprocal space is also called Fourier space, k- space, or momentum space The concept of the reciprocal lattice was devised to tabulate two important properties of crystal planes: their slopes and their interplanar distances. Let n(x) is function (say, electron density) which is periodic in one dimensional space with periodicity ‘a’.

Fourier series : n( x ) = ∑ nm e imx m

n( x + a ) = ∑ nm e im ( x + a ) = n( x) m

because of spacial periodicity ma = p.2π ⇒ m = p. 2π

a

n( x ) = ∑ n p e

i

2πp .x a

p

In one dimension these points lies in a line. Implies that in the Fourier space the function n(x) will have nonzero coefficients only at these points, other points are not allowed in F-expansion of any periodic function.

a 2π/a (Magnitude not shown) 12

ρ In 3 - D we find a set of vectors G such that ρρ ρ iG . r n ( r ) = ∑ nG e G ρ is invarient under all lattice translations T which leaves crystal invarient. r r r r r r r r r r iG .( r +T ) iG . r iG .T n(r + T ) = ∑ nG e = ∑ nG e .e = n( r ) G

G

r r iG .T

⇒⇒ e = 1 r* r* r r* G = ha + kb + lc with above criteria is called reciprocal lattice vector

ρ* ρ* ρρ ρ ρ ρ ρ* G.T = (ha + kb + lc ).(ua + vb + wc) = 2π

New sets of axis for reciprocal unit cell So that, a.a* = 2π

a*.b = 0

a*.c = 0

etc.

This concept and the relation of the direct and reciprocal lattices through the Fourier transform was first introduced in crystallography by P. P. Ewald (1921).

13

G102

• G002



G101

c* • G001

• a*

G100 •

β*

a) from this origin, lay out the normal to every family of parallel planes in the direct lattice; b) set the length of each normal equal to 2π π times the reciprocal of the interplanar spacing for its particular set of planes; c) place a point at the end of each normal.

G102 •

• G002 dh k l

G101 • G100 • a*

• G001c* β*

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Ch1. Structure of Solid → Three

Example:Zinc blende (ZnS), gallium arsenide,. Atoms: Cl. -. : 0,0,0;. 0,1/2,1/2; 1/2,0,1/2; and 1/2,1/2,0. Na. +. : ½, ½, ½; ½,0,0;. 0, ½,0;. 0,0, ½. Cu/Fe. Bravais ...

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