Crystal Structures Flashcards

1
Q

What is a Crystal?

A

Solids that contain particles in a regular arrangement known as a lattice.

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2
Q

What are the 4 groups crystal lattices are classified in to?

A

Ionic Crystals
Metallic Crystals
Molecular (Simple Covalent) Crystals
Macromolecular (giant covalent) structures

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3
Q

How are ionic crystals structured?

A

Positive and Negative Ions, held together in a giant ionic lattice by strong electrostatic attraction between oppositely charged ions.

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4
Q

What are the properties of Ionic Crystals and why?

A
  • Hight m.p: Strong electrostatic attraction between oppositely charged ions
  • Only conduct molten/ in solution: Ions free to move and carry a charge in liquid state
  • Hard, but brittle: Force can move ions and produce contact between like charges causing repulsion
  • Often dissolve in water: Ions become solvated and surrounded by water molecules.
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5
Q

What is a metallic crystal?

A

A giant lattice of positive ions held together by a sea of delocalised electrons

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6
Q

What are the properties of metallic crystals and why do they have them?

A
  • High m.p & b.p: Strong electrostatic attraction between metal ions and the delocalised sea of electrons
  • Conduct electricity solid: Free moving electrons that can carry a charge through the structure.
  • Malleable and Ductile: Metal ions slide past each other, but retain lattice structure and metallic properties.
  • Insoluble: Water molecules can’t break up the metallic bonding, so metal ions can’t become solvated.
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7
Q

What is a molecular crystals (simple covalent)?

A

Individual molecules held together by weak intermolecular forces.

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8
Q

Properties of molecular crystals?

A
  • Low m.p, soft and easily breakable: Only weak van der waals forces between molecules so only a small amount of energy is needed to overcome these.
  • Doesn’t conduct electricity: No free moving electrons/ions so nothing can carry the charge.
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9
Q

What is a macromolecular (giant covalent) structure?

A

A giant arrangement of atoms joined by covalent bonds.

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10
Q

What is the structure of Diamond?

A

Interlocking tetrahedra of Carbon atoms

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11
Q

Properties of Diamond?

A

V.High m.p & Very Hard: many strong covalent bonds holding structure together, so lots of energy needed to break these bonds
- Non-conductor: No free moving electrons/ ions so nothing to carry charge.

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12
Q

Structure of Graphite?

A

Layered structure of Carbon atoms

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13
Q

Properties of Graphite?

A
  • Very high m.p: Many strong covalent bonds holding structure together, so takes lots of energy to break these bonds.
  • Soft, flaky & slippery: Has a layered structure with delocalised electrons between layers, so layers can slide.
  • Conducts electricity: Delocalised electrons between layers that are free to move & carry a charge.
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