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GCSE Chemistry > Topic 4- Extracting Metals And Equilibra > Flashcards

Topic 4- Extracting Metals And Equilibra Flashcards

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1
Q

What is oxidation?

A

The Loss of electrons

Or the gain of oxygen

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2
Q

What is reduction ?

A

The gain of electrons

The loss of oxygen

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3
Q

What’s a good way to remember the difference between oxidation and reduction?

A

OIL RIG

oxidation is loss (of electrons)
Reduction is gain (of electrons)

Oxidation
Is
Loss
Reduction
Is
Gain
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4
Q

What’s an example of oxidation?

A

E.g. when metals react with oxygen, metal oxides are produced:
Magnesium + oxygen → magnesium oxide
2Mg + O2 → 2MgO

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5
Q

What’s an example of reduction ?

A

E.g. when metal oxides lose oxygen and return to their atomic form:
Iron oxide + carbon monoxide → iron + carbon dioxide
Fe2O3 + 3CO → 2Fe + 3CO2

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6
Q

Sodium + oxygen —> ?

A

Sodium oxide

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7
Q

Mg(s) + 2H+(aq) + 2Cl-(aq) → Mg2+(aq) + 2Cl-(aq) + H2(g)

In this ionic equation, what’s being oxidised and what’s being reduced?

A

Mg2+ is being oxidised

H+ is being reduced

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8
Q

Mg(s) + 2H+(aq) + 2Cl-(aq) → Mg2+(aq) + 2Cl-(aq) + H2(g)

In this ionic equation, what is are the spectator ions ?

A

2Cl-(aq) ions

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9
Q

When reacting with other substances, what ions do metal atoms always become ?

A

metal atoms always form positive ions.

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10
Q

What is the reactivity of a metal linked to ?

A

how easy it is for a metal to form its positive ion

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11
Q

What order can metals be arranged in ?

A

in order of their reactivity.

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12
Q

What are examples of highly unreactive metals ?

A

Gold and platinum

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13
Q

Where are gold and platinum found ?

And what do we call them ?

A

These metals are found in the Earth’s crust as pure metals. We call them native metals.

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14
Q

Which non-metals are often included in the reactivity series of metals for reference?

A

Carbon

Hydrogen

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15
Q

What is a displacement reaction ?

A

A more reactive metal (one that forms positive ions more easily) can remove a less reactive metal from a compound.

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16
Q

When can a metal displace another metal from a compound ?

A

A metal can only displace another metal from a compound if it is located above it in the reactivity series.

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17
Q

What’s an example of a displacement reaction ?

Calcium + copper sulfate → calcium sulfate + copper

A

Calcium is higher in the reactivity series than copper. This means that calcium is able to displace copper from a copper sulfate solution to create calcium sulfate.
Calcium + copper sulfate → calcium sulfate + copper
Ca(s) + CuSO4(aq) → CaSO4(aq) + Cu(s)
Platinum, on the other hand, is less reactive than copper and so would not be able to displace copper from a copper sulfate solution.

18
Q

What are redox reactions ?

A

Displacement reactions are examples of redox reactions.
In metal displacement reactions, the more reactive metal loses electrons (oxidised) and the less reactive metal gains electrons (reduced).

19
Q

What are the products of the reaction between magnesium and copper sulfate ?

A

Magnesium sulfate and copper

20
Q

What is the word and symbol equation for the displacement reaction :

Sodium bromide + chlorine → ? + ?
2NaBr + Cl2 → ? + ?

A

Sodium bromide + chlorine → sodium chloride + bromine.

2NaBr + Cl2 → 2NaCl + Br2

21
Q

What is the half equation for bromine ions in displacement reactions ?

A

Bromide ions are oxidised (electrons are lost):

2Br- → Br2 +2e-.

22
Q

What is the half equation for chlorine ions in displacement reactions ?

A

Chlorine is reduced (electrons are gained):

Cl2 + 2e- → 2Cl-.

23
Q

What are the spectator ions in the displacement reaction-

Sodium bromide + chlorine → sodium chloride + bromine.
2NaBr + Cl2 → 2NaCl + Br2

A

Sodium ions

24
Q

What are spectator ions ?

A

A spectator ion is an ion that doesn’t change during a chemical reaction.

25
Q

What is the reactivity series order ?

Order From most reactive to least

A 
Potassium 
Sodium
Lithium 
Calcium
Magnesium 
Aluminium 
CARBON - not a metal
Zinc 
Iron
HYDROGEN - not a metal 
Copper
Silver 
Gold
Platinum
26
Q

2NaBr(aq) + Cl2(g) → 2NaCl(aq) + Br2(l)

Which is the spectator ion in this equation?

A

Na +

27
Q

When Potassium, sodium and lithium all react quickly with cold water to produce what ?

A

a metal hydroxide and hydrogen gas

28
Q

What happens to potassium when reacted with cold water ?

A

Potassium is the most reactive so reacts very quickly.

The hydrogen produced ignites instantly and the metal also sets alight, sparking and burning with a lilac flame

29
Q

What colour is the flame of potassium when it reacts with water ?

A

lilac flame

30
Q

What happens to sodium when reacted with cold water ?

A

Sodium fizzes rapidly and melts to form a ball that moves around on the water surface.

31
Q

What happens to lithium when reacted with cold water ?

A

Lithium fizzes steadily and floats, becoming smaller until it eventually disappears

32
Q

Most metals react with dilute acids to give what ?

A

a salt (e.g. copper chloride) and hydrogen gas

33
Q

What metals don’t react with dilute acids ?

A

copper, silver, gold and platinum.

34
Q

What metals react with dilute acids but not cold water ?

A

magnesium, aluminium, zinc, iron and lead (iron and lead react slowly).

Metals don’t have to be that reactive to react with dilute acids.

35
Q

Why is carbon used to extract metals?

A

Reducing a metal with carbon will result in the extraction of the metal if the metal is lower in the reactivity series than carbon.

Carbon is used because it is cheap and abundant.

36
Q

How is carbon used to extract metals?

A

In the reduction, the metal oxide loses oxygen to form a pure metal.

Reduction with carbon normally involves heating the metal oxide in the presence of the carbon, which is often used in the form of coal.

37
Q

What form is carbon often used in when reducing metal oxides?

A

Coal

38
Q

metal+acid→?+?

A

metal+acid→salt+hydrogen

39
Q

Fact about reactivity series’s

A

Potassium down to aluminium are more reactive than carbon and so cannot be extracted by reduction with carbon.

Silver, gold and platinum are either found as natural elements or can be simply extracted by heating directly in air.

The remaining metals - zinc, iron, and copper - are all commonly extracted by reduction with carbon.

40
Q

What type of reaction is used when extracting metals using carbon ?

A

Reduction

GCSE Chemistry (10 decks)

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