Topic 4 - Metals Flashcards

1
Q

Properties of metals

A
  • Conductivity
  • Shiny
  • Malleable
  • Solid (mostly)
  • High melting point and boiling point
  • High density
  • low ionisation energies
  • low electronegativities
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2
Q

Cations

A

Metals, lose electrons so they have a positive charge

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3
Q

Transition metals

A

harder, higher density, higher melting points, strong magnetic properties, bright coloured

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4
Q

Alloys

A
  • metals are mixed with small amounts of another substance usually another metal or carbon. They are melted together, mixed and then allowed to cool. An alloy is harder and melts at a lower temperature than a pure metal.
  • Steel = Transition metals + carbon
  • Copper is one of the few metals that s mainly used in pure form.
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5
Q

In what order do you write the number and charge of an ion

A

Number then charge

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6
Q

Metals are usually hard and tend to have high boiling points

A

the forces between the particles must be strong

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6
Q

Metals are usually hard and tend to have high boiling points

A

the forces between the particles must be strong

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7
Q

Metals conduct electricity in the solid state and in the modern liquid state

A

metals have charged particles that are free to move

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8
Q

metals are malleable and ductile

A

the attractive forces between the particles must be stronger than the repulsive forces between the particles when the layers of particles are moved

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9
Q

Metals generally have high densities

A

The particles are closely packed in a metal

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10
Q

Metals are good conductors of heat

A

there must be a way of quickly transferring energy throughout a metal object

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11
Q

Metals are lustrous or reflective

A

free electrons are present, so metals can reflect light and appear shiny

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12
Q

Metals tend to react by losing electrons

A

electrons must be relatively easily removed from metal atoms.

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13
Q

The metallic bonding model must include:

A

charged particles that are free to move and conduct electricity

strong forces of attraction between particles throughout the metal structure

some electrons that are relatively easily removed

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14
Q

A metal crystal:

A

a region of solid where the particles
are arranged regularly.

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15
Q

Lattice:

A

Tightly packed regular arrangement.

16
Q

The reactivity of a metal depends

A

on how easily electrons can be removed from their atoms.

17
Q

Metals can react with

A

water, oxygen, acids

18
Q

what is the trend of reactivity to water, oxygen and acids

A

Group 1, group 2, transition metals

19
Q

Metals are normally more reactive with

A

acids than with water. More metals react with acids and
the reactions tend to be more energetic.

20
Q

Gold and platinum are essentially unreactive and are described as

A

inert.

21
Q

The Reactivity Series

A
  • Please
  • Send
  • Charlie’s
  • Monkey
  • And
  • Zebras
  • In
  • Lead
  • Cages
  • Securely
  • Guarded

Potassium
Sodium
Calcium
Magnesium
Aluminium
zinc
iron
lead
copper
Silver
gold

potassium highest, gold lowest

22
Q

Atoms of metals

A

are generally larger than the atoms of non-metallic elements within a period.

have lower effective nuclear charge (core charge)

have lower ionisation energy (it takes less energy to remove electrons from an outer shell)

Metals tend to lose their outer shell electrons to form positive ions, called ions

23
Q

The reactivity of a metal depends on how…

A

easily electrons can be removed from its atoms

24
Q

Circular economy

A

a continuous cycle where the extracted material is reused after initial use, waste is minimum and can be recycled, or re-purposed

sustainable

25
Q

most metals in the earths crust form…

A

oxides, sulphides or silicates

26
Q

when the concentration of mineral in rock is high enough to be extracted it is called…

A

an ore

27
Q

Mining

A

the first step in metal production from ores
involves the removal of surface vegetation, soil and bedrock to reach the ore deposits. Underground mining - digging a vertical shafts into the group then tunnels are dug to reach the ore

in-situ leaching, injecting solutions into holes to resolve the minerals and then pumping them to the surface where the minerals can be recovered, cheaper.

28
Q

Ore processing

A

the second step in metal production from ores

processed to separate the valuable minerals from the waste rock.

29
Q

metal extraction

A

the thirds step in metal production from ores

the method to extract the metals changes based on the reactivity. All metals can be extracted by passing an electric current through the liquid compound, electrolysis. Uses lots of energy. expensive, only used for very reactive elements

iron can be extracted by heating it at a high temperature with carbon, and smelting.

30
Q

environmental issues

A

land, water, air, biodiversity.

31
Q

Linear Economies

A

you use it then dispose of it. take make dispose

32
Q

metal recycling…

A

save up to 20 times the energy needed to extract metals
avoids using metals as landfill
reduces CO2 emmisons

33
Q

Recycling process

A

collection
preparation for recovery
smelting
purification

34
Q

haematite

A

Fe 2 O 3

35
Q

extraction of iron

A

materials used = iron ore, coke, limestone and air

To extract iron, blast furnace
- different reactions in different temperature zones

part 1
- coke reacts with oxygen to produce carbon dioxide which reacts with carbon to form carbon monoxide

Part 2
- carbon monoxide reacts with iron ore
- carbon monoxide + iron oxide = iron + carbon dioxide

limestone
- limestone breaks down, to form calcium oxide and carbon dioxide with reacts with the unwanted materials to form slag

collection of iron
- holes at the base of the furnace are opened and the molten iron and slag are drained out and separated.