✅ 616 - extracting metals Flashcards

Ores + copper

1
Q

define an ore

A

a mineral or rock that contains a enough metal/metal compound to make it economical to extract the metal

(= the value of the metal is more than the cost of extracting it)

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2
Q

what is the ore to extract copper (carbonate)?

A

malechite

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3
Q

what is the ore to extract iron(III) (oxide)?

A

haematite

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4
Q

what is the ore to extract aluminium (oxide)?

A

bauxite

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5
Q

describe the 3 main stages to extract a metal

A

1) ore is mined

2) ore is processed
(metal compound separated from other substances in the ore)

3) metal is extracted from the pure metal compound using chemical reactions

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6
Q

what is the mneunomic to remember the metal reactivity series?

(and what does each stand for - in terms of elements)

A

cute - carbon (NOT METAL)

has - hydrogen (NOT METAL, USED FOR REFERENCE)

Please stop calling me a (cute) zebra, I think love has copper silver gold platinum

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7
Q

What extraction methods are there - when are they used

A
  • in principle, all metals could be extracted from their compounds using electrolysis, but electricity is expensive
  • if metal is less reactive than carbon, cheaper methods are used instead
  • copper + iron are less reactive than carbon, so they can be extracted by heating their compounds with carbon or with carbon monoxide
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8
Q

all metals can be extracted from their compounds using …… but is expensive

A

electrolysis (electricity is expensive)

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9
Q

why can copper be extracted using carbon, but not sodium?

A

as copper is less reactive than carbon
- wheras sodium is too reactive to be extracted by reduction

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10
Q

describe the 2 main steps of how copper is extracted from copper sulfide

(and the word and symbol equation for each one)

A

1) copper sulfide (II) is ‘roasted’ in air
(to get it into metal oxide form for carbon to reduce later) :

copper(II) sulfide + oxygen -> copper(II) oxide + sulfur dioxide
2CuS(s) + 3O2 (g) -> 2CuO(s) + 2SO2 (g)

2) copper(II) oxide is heated with carbon:

copper (II) oxide + carbon -> copper + carbon dioxide
2CuO(s) + C(s) -> 2Cu(s) + CO2 (g)

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11
Q

explain how the extraction of copper sulfide is a redox reaction
- and what is the reducing agent

A
  • copper(II) oxide loses oxygen and is reduced
  • carbon gains oxygen and is oxidised
  • carbon is acting as a reducing agent (reduced copper oxide to copper)
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12
Q

what form of carbon is used when extracting copper from copper sulfide?

A

charcoal

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13
Q

What does the method chosen to extract a metal depend upon

A

Its position in the reactivity series

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14
Q

Extracting metals topic:

Copper(II) oxide can also be reduced to copper by heating it with __ or with __
(Rather than carbon)

A

Methane, hydrogen

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15
Q

5 steps to reduce copper(II) oxide using charcoal, which is mostly carbon.

+ 2 considerations

A

1 - mix the two powders in a crucible, replace the lid. The lid must be kept on the crucible during heating to stop the powders escaping and to stop air getting in (because then the carbon would burn)

2- heat it strongly

3 - after several minutes, allow the crucible to cool

4 - when the crucible is cool, transfer its contents to a beaker of water. The copper sinks to the bottom while excess charcoal is suspended in the water

5 - separate the copper by washing it

  • excess charcoal powder is used to ensure that all of the copper(II) oxide is reduced to copper
  • eye protection should be worn throughout this practcial
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16
Q

Overall extracting copper - pb

A