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TPS Science New Spec > Chemical changes > Flashcards

Chemical changes Flashcards

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1
Q

What type of separation process would you use to separate a soluble salt?

A

Crystallisation

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2
Q

When there are several ions in solution, which ion will collect at the anode?

A

At the cathode: Hydrogen is produced if the metal is more reactive than Hydrogen

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3
Q

Write the formulae of Magnesium Chloride

A

MgCl2

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4
Q

Higher What is a ‘weak’ acid?

A

An acid that is only partially ionised in water.

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5
Q

Describe how you would make a pure, dry sample of a soluble salt using an insoluble base and an acid.

A
  • Add base in excess to acid.
  • Filter excess base.
  • Crystallisation – to separate salt from its solution.
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6
Q

What is the name for the reaction when an acid reacts with an alkali to make a salt + water?

A

Neutralisation reaction

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7
Q

Higher Explain why the reaction below is a redox reaction. Zn (s) + 2HCl (aq) → ZnCl2 (aq) + H2 (g)

A

• Zinc atoms are oxidised. • Hydrogen atoms are reduced. • Hence reduction and oxidation happen at the same time so it’s called a redox reaction.

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8
Q

Higher Fill in the blanks: Oxidation is the _____ of electrons. Reduction is the _____ of electrons.

A

• Oxidation is the loss of electrons • Reduction is the gain of electrons

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9
Q

Complete the general equation

Acid + Metal Carbonate →

A

Acid + Metal carbonate → Salt + Water + carbon dioxide

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10
Q

Why is cryolite used in the electrolysis of aluminium oxide?

A

To lower the melting point of aluminium oxide (to save energy and costs)

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11
Q

Higher In the following equation, state which species are oxidised and which are reduced? 2Fe2O3 + 3C → 4Fe + 3CO2

A

• 2Fe2O3 (Iron oxide) is reduced • 3C (carbon) is oxidised

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12
Q

Name the ‘salt’ produced when the following chemicals react

Magnesium oxide + sulfuric acid

A

Magnesium sulfate

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13
Q

If an atom is very reactive, is it more or less likely to turn into an ion?

A

More likely

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14
Q

What is that name for the reaction that involves the removal of oxygen?

A

Reduction

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15
Q

Write an ionic equation for neutralisation

A

H+ (aq) + OH- (aq) → H2O (l)

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16
Q

In electrolysis, what is the negative electrode called?

A

Cathode

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17
Q

Why is gold found naturally in the Earth, but other metals are locked up in compounds?

A

Gold is unreactive

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18
Q

In the electrolysis of lead bromide, what collects at The negative electrode (the cathode)

A

Lead (at the cathode)

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19
Q

Name the ion found in acidic solutions

A

Hydrogen ion, H+

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20
Q

Write the formulae of the following salts using the formulae of ions provided below. Sodium Chloride

A

NaCl

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21
Q

Higher During electrolysis, what happens to ions at the Anode?

A

At the Anode: Ions lose electrons and turn into atoms (Oxidation)

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22
Q

Complete the general equation

Metal + Acid →

A

Metal + Acid → Salt + Hydrogen

23
Q

In the electrolysis of lead bromide, what collects at The positive electrode (the anode)

A

Bromine (at the anode)

24
Q

Higher During electrolysis, what happens to ions at the Cathode?

A

At the Cathode: Ions gain electrons and turn into atoms (Reduction)

25
Q

What is the name of the liquid that is electrolysed.

A

Electrolyte

26
Q

Higher If you compared the pH of a 1M Strong Acid and a 1M Weak acid, which would have the higher pH and why?

A

The weaker acid will have the higher pH because it only partially ionises in water (or vice versa).

27
Q

What is the name for the reaction that involves the gaining of oxygen?

A

Oxidation

28
Q

Name the ‘salt’ produced when the following chemicals react

Iron hydroxide + hydrochloric acid

A

Iron chloride

29
Q

Complete the general equation

Metal + Water →

A

Metal + Water → Metal hydroxide + Hydrogen

30
Q

Higher In the following equation, state which species are oxidised and which are reduced? a) Mg (s) + 2HCl (aq) → MgCl2 (aq) + H2 (g)

A

• Magnesium atoms (Mg) are oxidised. • Hydrogen ions (H+) are reduced.

31
Q

When there are several ions in solution, which ion will collect at the cathode?

A

At the anode: Oxygen is produced unless the solution contains halide ions, then the halogen is produced.

32
Q

What type of separation process would you use to separate an insoluble salt?

A

Filtration

33
Q

In electrolysis, what is the positive electrode called?

A

Anode

34
Q

Higher Write half equations at the anode and cathode for the electrolysis of water.

A

• Anode: 4OH- - 4e- → O2 + 2H2O or 4OH- → O2 + 2H2O + 4e- • Cathode: 2H+ + 2e- → H2

35
Q

What type of reaction is shown by the equation below? magnesium + oxygen → magnesium oxide

A

Oxidation

36
Q

What is the pH of a neutral solution?

A

7

37
Q

Complete the general equation

Acid + Metal oxide →

A

Acid + Metal oxide → Salt + Water

38
Q

To which electrode are negative ions attracted to?

A

Positive electrode (opposites attract)

39
Q

Name the ‘salt’ produced when the following chemicals react

Sodium carbonate + nitric acid

A

Sodium nitrate

40
Q

Why can’t aluminium be extracted by reduction with carbon?

A

Aluminium is more reactive than carbon

41
Q

Higher Write the half equations at the anode and cathode for the electrolysis of lead bromide.

A

• Anode: 2Br- - 2e- → Br2 or 2Br- → Br2 + 2e- • Cathode: Pb2+ + 2e- → Pb

42
Q

Higher Write an ionic equation for each of the displacement reactions below: Fe + CuCl2 → Cu + FeCl2

A

Fe(s) + Cu2+ (aq) → Cu(s) + Fe2+ (aq)

43
Q

What is the pH range of acids?

A

0-6

44
Q

What chemical reaction is shown by the equation below to extract iron from iron oxide?

Iron oxide + carbon → iron + carbon dioxide

A

Reduction (with carbon)

45
Q

What two non-metals are often included in the reactivity series?

A

Hydrogen and Carbon

46
Q

To which electrode are positive ions attracted to?

A

Negative electrode (opposites attract)

47
Q

What is the pH range of alkalis?

A

8-14

48
Q

Why does the positive electrode have to be regularly replaced in the extraction of aluminium oxide?

A

Because oxide ions react with the carbon electrode… • Releasing CO2… • Meaning the electrodes gradually degrade

49
Q

Why does a metal compound have to be molten or dissolved for electrolysis to work?

A

Because the ions need to be free to flow

50
Q

Why must aluminium be extracted by electrolysis?

A

It is more reactive than carbon (and therefore can’t be extracted by reduction with carbon)

51
Q

What is the name for the liquid that contains the ions in the electrolysis process?

A

Electrolyte

52
Q

Higher Write an ionic equation for each of the displacement reactions below: Mg + CuSO4 → Cu + MgSO4

A

Mg(s) + Cu2+ (aq)→ Cu(s) + Mg2+ (aq)

53
Q

Higher Give two examples of strong acids and two examples of weak acids.

A

• Strong acids include: Hydrochloric, Nitric and Sulfuric • Weak acids include: Carbonic, Ethanoic and Citric

54
Q

Put the following elements in order of reactivity from least to most reactive: iron / lithium / zinc / copper / potassium / calcium / sodium / magnesium

A

(least reactive) copper – iron – zinc – magnesium – calcium – lithium – sodium – potassium (most reactive)

TPS Science New Spec (14 decks)

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