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Materials Chemistry 1 > Intro to solid state chemistry > Flashcards

Intro to solid state chemistry Flashcards

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1
Q

Crystalline solid

A

a solid material whose constituents are arranged in a highly ordered microscopic structure, forming a crystal lattice that extends in all directions

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2
Q

Amorphous solid

A

a solid that lacks long-range order and doesn’t organise into a definite lattice pattern

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3
Q

2D lattice counting: atoms in centre of cell

A

1

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4
Q

2D lattice counting: atoms on edge of cell

A

1/2

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5
Q

2D lattice counting: atoms at a corner of cell

A

1/4

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6
Q

3D lattice counting: atoms in centre of cell

A

1

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7
Q

3D lattice counting: atoms on edge of cell

A

1/4

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8
Q

3D lattice counting: atoms at a corner of cell

A

1/8

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9
Q

3D lattice counting: atoms on face of cell

A

1/2

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10
Q

Packing efficiency formula

A

Natoms*Vatom / Vunit cell

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11
Q

Laves Principles

A

regarding the packing of spheres

  • space
  • symmetry
  • connection
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12
Q

Two types of close packing

A
  • Hexagonal close packing (hcp); ABABAB…
  • Cubic close packing (ccp); ABCABC…
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13
Q

Coordination no. of close packing

A

12

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14
Q

Packing efficiency of close packing

A

74%

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15
Q

Primitive cubic packing

(sites of atoms, packing efficiency, coordination number, points of contact)

A
  • M at (0,0,0)
  • 52% of volume occupied
  • coordination no. = 6
  • spheres in contact along cell edges
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16
Q

Body centred cubic packing

(sites of atoms, packing efficiency, coordination number, points of contact)

A
  • M at (0,0,0) and (1/2, 1/2, 1/2)
  • 68% of volume occupied
  • coordination no. = 8
  • spheres in contact along body diagonal
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17
Q

CsCl structure

A

Cl at (0,0,0)
Cs at (1/2, 1/2, 1/2)
two interpenetrating primitive cubic lattices

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18
Q

Are Oh or Td holes bigger

A

Oh

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19
Q

If there are n spheres, how many Oh holes are there?

A

n

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20
Q

If there are n spheres, how many Td holes are there?

A

2n

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21
Q

NaCl structure

A
  • Na in all Oh holes of a CCP of Cl
  • 6:6 coordination
  • 2 interpenetrating CCP arrays
22
Q

Rutile

A

TiO 2

  • distorted HCP of O with Ti in half Oh holes
  • edge and corner sharing TiO 6 octahedra
23
Q

Fluorite

A

CaF 2

  • all tetrahedral holes in CCP
  • Ca is surrounded by 8 F
  • F is surrounded by 4 Ca
  • 8:4 coordination
24
Q

NiAs

A
  • all octahedral holes in HCP
  • HCP of As with Ni in Oh holes
  • As in trigonal prism of Ni
  • 6:6 coordination
  • Ni octahedra share faces
25
Q

Perovskite

A

ABO 3

  • ideal cubic structure
  • Ti octahedrally coordinated
  • Ca is 12 coordinated
  • Ti in Oh holes
  • corner sharing BO 6 octahedra
26
Q

What are the allowed oxidation states in perovskite

A

3+ / 3+
2+ / 4+
1+ / 5+

27
Q

Ferroelectric Material

A

dielectric materials in which polarisation remains permanently, even after removing the applied electric field

28
Q

Crystal polymorphism

A

compound can crystallise into more than one crystal structure

29
Q

Spinel

A

AB 2 O 4

  • Mg in MgO 4 tetrahedra
  • Al in AlO 6 octahedra
  • close packed O layers
  • A and B are in some of the Td and Oh holes
30
Q

Allowed Oxidation states of spinels

A

2+ / 3+
1+ / 4+

31
Q

Most favourable conditions for radius ratio rules

A
  • ions treated as hard spheres
  • cation-anion contact
  • no anion-anion contact
  • coordination no. is max possible
32
Q

Lattice energy

A

the change in internal energy when 1 mole of an ionic compound at 1 bar is formed from infinitely separated gaseous ions

33
Q

What is the madelung constant?

A

the sum of the partial madelung constants which represent the contributions of the individual ions to the total lattice energy

34
Q

How does Born-Lande Equation differ from Born-Mayer?

A

Born-Mayer uses density as measuring the repulsion term

35
Q

How does Born-Lande Equation differ from Kapustinkii?

A

Kapustinkii can be used to estimate lattice energy without the knowledge of the structure type (i.e. the madelung constant)

36
Q

How types of polycrystalline materials are formed

A
  • conventional solid state reactions
  • precursor methods
  • hydrothermal / solvothermal methods
  • intercalation ion exchange
37
Q

How types of single crystals are formed

A
  • single crystal growth from melt
  • single crystal growth from fluxes
  • floating zone furnace (large) crystal growth
38
Q

How thin films are formed

A
  • chemical vapour deposition
  • sputtering
39
Q

Why is grinding needed in ‘shake and bake’?

A
  • produces an intimate mixture of reactants
  • reduces reactant particle size
40
Q

Why are high temperatures required for ‘shake and bake’?

A
  • generally leads to thermodynamically stable products
41
Q

What method is used to deduce crystal structures?

A

x-ray diffraction

42
Q

Solid oxide fuel cells: positives and negatives

A

+ve = clean and efficient energy generation, fuel flexibility, zero CO 2 emissions
-ve = device cost and reliability

43
Q

Solid oxide fuel cells: electrolyte used

A

YSZ
Yttria-stabilised zirconia

44
Q

Isovalent Substitution

A

the ion that is substituting the original ion is of the same oxidation state as the ion replacing it

45
Q

Aliovalent Substitution

A

the ion that is substituting the original ion is of a different oxidation state than the ion it is replacing

46
Q

Two mechanisms for ionic conduction

A
  • Vacancy-hopping oxide ion conductors
  • Interstitial oxide ion conductors
47
Q

Example of other ionic conductor

A

Layered materials containing mobile cations

used in rechargeable battery materials

48
Q

Superconductors

A

a type of material that conducts electricity with zero energy loss or resistance when cooled to a certain temperature

49
Q

Example of molecular superconductors

A

Alkali fullerides, A 3 C 60

50
Q

Factors for elements replacing one another in doping

A
  • Oxidation state (similar oxidation state is favourable)
  • Ionic radii (similar sizes is favourable)
  • Coordination preferences (geometry)

Materials Chemistry 1 (4 decks)

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