topic 5 - transition metals, alloys and corrosion Flashcards

1
Q

where are transition metals found

A

in the middle of the periodic table

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2
Q

typical properties of transition metals (4)

A
  • high melting point (apart from mercury)
  • high density
  • make good catalysts (eg iron is used in the haber process)
  • form colourful compounds
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3
Q

what colour compounds do Fe^2+ ions form

A

light green

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4
Q

what colour compounds do Cu^2+ ions form

A

blue

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5
Q

what colour compounds do Fe^3+ ions form

A

orange/brown

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6
Q

alloy

A

a mixture of metals / the addition of another element to a metal

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7
Q

why are alloys stronger

A

they contain different elements with different sized atoms making it difficult for layer to slide over each other

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8
Q

steels

A

alloys of iron

used more often than pure iron

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9
Q

how is steel made

A

small amount of carbon are added to iron

other metals are added to make alloy steels

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10
Q

general differences steel vs iron (2)

A
  • steels are harder than iron

- iron is more likely to rust than steel

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11
Q

3 types of steel

A

low carbon steel
high carbon steel
stainless steel

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12
Q

low carbon steel (make-up and properties)

A

0.1-0.3% carbon

malleable

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13
Q

high carbon steel (make-up and properties)

A

0.22-2.5% carbon

very strong, brittle and inflexible

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14
Q

stainless steel (properties)

A

corrosion resistant

strong

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15
Q

copper alloy examples

A

bronze

brass

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16
Q

bronze (makeup)

A

copper + tin = bronze

17
Q

bronze (properties and uses)

A

bronze is much harder than copper

made into medals, statues and decorative ornaments

18
Q

brass (makeup)

A

copper + zinc = brass

19
Q

brass (properties and uses)

A

brass is more malleable than bronze

used in situations where less friction is needed such as water taps and door fittings

20
Q

gold alloys (makeup and uses)

A

zinc, copper and silver used to strengthen the very soft and malleable gold
used to make jewellery

21
Q

aluminium alloy example

A

magnalium

22
Q

aluminium alloys (properties and uses)

A

low density and stronger than regular aluminium

used to make aircraft

23
Q

magnalium (makeup)

A

aluminium + magnesium = magnalium

24
Q

low magnesium content magnalium (properties and uses)

A

light strong and corrodes less easily than pure aluminium

used for cars and aeroplanes

25
Q

high magnesium content magnalium (properties and uses)

A

more reactive, burns brightly and is more stable than magnesium
used for fireworks

26
Q

corrosion

A

a process where something is slowly damaged or destroyed by a chemical process

27
Q

rusting

A

the corrosion of iron

28
Q

what is corrosion (reaction)

A

corrosion is caused by redox reactions
metals corrode in the presence of water and oxygen
metal is oxidised
oxygen is reduced

29
Q

how to prevent rusting (what are you blocking)

A

coating iron with a barrier to keep out oxygen or water or both

30
Q

how can you prevent rusting (techniques)

A

painting
oiling or greasing (especially on moving parts)
sacrificial protection

31
Q

sacrificial protection

A

placing a more reactive metal with iron so it is corroded instead

32
Q

galvanisation

A

an example of sacrificial protection where a coat of zinc is placed on an iron object
often done to corrugated iron roofing

33
Q

electroplating

A

coating the surface of a metal with another metal using electrolysis

34
Q

what should the cathode, anode and electrolyte be in electroplating

A

cathode - the object to be electroplated
anode - bar of metal being used as plating
electrolyte - solution containing metal ions of the plating metal

35
Q

2 examples of when we use electroplating

A

we electroplate household items such as cutlery/cooking utensils to stop corrosion (protective metals used are unreactive and don’t corrode easily)

jewellery and decorative items may be electroplated gold or silver to make them look shiny

36
Q

what happens in terms of movement of ions in electroplating

A

metal ions from electrolyte move to the cathode, where they are reduced and the metal is deposited on the object
the anode keeps the metal ions ‘topped up’