Metals Flashcards

1
Q
A

Body Centred Cubic (BCC)

More open structure

Coordination number- 8

Packing Density- 68%

Slip systems- 48 (planes are not close packed needing high temp. or force to activate)

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2
Q
A

Hexagonal Close Packing (HCP)

Each atom is surrounded by 6 more

Coordination number- 12

Packing Density- 74%

Slip systems- 3 (brittle)

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3
Q

How do you reduce slip in metals and why?

A
  1. Alloying
  2. Decrease grain size

Makes a metal harder/stronger or more brittle

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4
Q

Elastic Deformation

A

Stress is proportional to strain, is reversible

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5
Q

Malleability

A

The ability of a solid material to deform under compression

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6
Q

Types of Alloys

A
  1. Interstitial- Alloying atoms fit between metal atoms (Carbon in Steel)
  2. Substitutional- Alloying atoms replace other metal atoms (Brass with Copper and Zinc)
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7
Q

How does Grain Size affect the mechanical properties of metals?

A

Less slip across grain boundaries

Smaller grain means more boundaries which means harder to slip which means harder/stronger metal

Small grains are obtained by fast cooling, use of chemical agents, or application of physical treatment

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8
Q

Coordination Number?

A

Amount of neighbour atoms

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9
Q

Suitability of a metal

A

CASE

Cheap

Abundant

Suitable for the task

Easy to extract

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10
Q

Brittle

A

Materials considered this if they fracture at less than 5% strain

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11
Q

Ductility

A

A measure of the extent of plastic deformation a material can sustain before fracturing. Can be drawn into wires

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12
Q

Metallic Glass

A

Disordered structure like a liquid

High strength and elastic limit

Resistant against corrosion/scratches/dents/wear

Brittle

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13
Q
A

Cubic Close Packing (CCP)

Each atom is surrounded by 6 others in each layer

Coordination number- 12

Packing Density- 74%

Slip systems- 12 (4 slip planes, 3 directions) (ductile)

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14
Q

How do Metallic Grains form?

A
  1. As a metal solidifies, crystals start to grow in all different directions
  2. These merge to give a grain structure where each grain has its own crystalline orientation
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15
Q

Where are small grains not wanted?

A

High temp. strength

Temp-induced slip/failure more likely along the grain boundaries

Jet Turbines

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16
Q

Plastic Deformation

A

Deformation in which stress and strain are no longer proportional, not reversible

17
Q

Anode and Cathode (metal corrosion)

A

The anode defines the area at which oxidation takes place

The cathode defines the area at which reduction takes place (where oxide layer forms)

This is always true!

18
Q

Example of REDOX reactions

A
  • Corosion
  • Extraction of metals
  • Batteries/Fuel Cells
  • Burning of fuels
19
Q

Transistion Metals

A

d-block elements lose the valence s-electrons when they form compounds but most can also lose a variable number of d-electrons. Explains mulitiple oxidation states

20
Q

Trends across a Period

A

Atomic Radius- Increases

Ionisation energy- Decreases

Oxidising Strength- Decreases

Reducing Strength- Increases

21
Q

Ionisation energy

A

The energy required to remove one electron from an atom of the element in the gas phase

22
Q

Metals in Nature

A

Generally form positive ions which combine non metal negative ions, forming ores

23
Q

Electrochemical Potential

A

It is a measure of the chemical potential of compounds which takes electrostatic forces into account