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Eleanor Rowe Chemistry GCSE > Chemical Changes > Flashcards

Chemical Changes Flashcards

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1
Q

Metal + oxygen =

A

Metal oxide

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2
Q

Metal + water =

A

Metal hydroxide + hydrogen

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3
Q

What can you use the metal plus water reaction to find

A

Where metals lie on the reactivity series

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4
Q

What does the reactivity of a metal depend on

A

It’s ability to lose electrons and form a positive ion

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5
Q

Where are unreactive metals found

A

In the earth in a pure state

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6
Q

Where are reactive metals found and what can you do to extract them

A

They are found in the ground reacted with oxygen to form compounds
you use displacement reactions to extract the metal

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7
Q

What is oxidation

A

Loss of electrons

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8
Q

What is reduction

A

Gain of electrons

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9
Q

Are all acids aqueous

A

Yes

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10
Q

What ions do acids produce in aqueous solutions

A

H+ ions

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11
Q

What is a base

A

A chemical that neutralises acid and produces a salt and water

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12
Q

Give examples of a base

A

Metal oxide and metal hydroxide

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13
Q

What is a base that is soluble in water called

A

An alkali

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14
Q

What ions do alkalis produce in aqueous solutions

A

OH- ions

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15
Q

What is the formula for a neutralisation reaction

A

H+ + OH- —> H2O

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16
Q

What are the formulas for three main acids

A

HCl is hydrochloric acid
H2SO4 is sulphuric acid
HNO3 is nitric acid

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17
Q

Why is a salt formed when metals react with acid

A

Most metals are more reactive than hydrogen so when they react with acid they displace the H plus ions forming a salt

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18
Q

Metal plus acid =

A

Salt + hydrogen

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19
Q

Acid + base =

A

Salt plus water

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20
Q

Acid plus metal carbonate =

A

Salt plus water plus co2

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21
Q

Method for required practical of making soluble salt using sulphuric acid and copper oxide

A
  1. Sulphuric acid in beaker over Bunsen with other equipment
  2. Heat until almost boiling
  3. Add copper oxide in excess until it stops dissolving in acid
  4. Filter solution
  5. Place in Evap basin on Bunsen until half has evaporated, leave in warm room for 48 hours until all evaporates
  6. Pat dry crystals with towel
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22
Q

What is a strong acid

A

One that fully ionises in aqueous solutions

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23
Q

Examples of strong acids

A

HCl, H2SO4, HNO3

24
Q

What is a weak acid

A

One that partially ionises in aqueous solutions, shown by reversible reactions

25
Q

Examples of weak acids

A

Carbonic acid
Ethanoic acid
Citric acid

26
Q

As the pH scale decreases by 1 unit, how does the conc of H+ ions change?

A

It increases by 10 times

27
Q

Titration required practical method

A
  1. Use a pipette to put 25 cm³ of sodium hydroxide into conical flask
  2. Add five drops of methyl orange indicator
  3. Place flask on a white tile to see the colour change clearly
  4. Fill the burette with sulphuric acid
  5. Add acid to the alkali until solution turns neutral and keep swirling the flask whilst adding it
  6. Once neutral read the volume of acid added from the right and calculate concentration,
28
Q

How does the orange indicator change from acidic to neutral in the titration reaction

A

Methyl orange goes from yellow when acidic to red when neutral

29
Q

How can you read the volume of acid added from the burette correctly

A

Making sure your eye is at the surface of the meniscus and read it multiple times and calculate the mean

30
Q

Why can solid ionic compounds not conduct electricity

A

The ions are locked in place and not free to move due to the electrostatic forces

31
Q

What is a melted ionic compound called

A

An electrolyte

32
Q

What material are the electrodes made out of

A

Graphite a form of carbon

33
Q

What is the negative electrode called

A

The cathode

34
Q

What is the positive electrode called

A

The anode

35
Q

What happens to the positive ions in the solution during electrolysis

A

They are attracted to the negative cathode and gain electrons that surround it to form a stable atom through reduction

36
Q

What happens to the negative ions in the solution during electrolysis

A

They are attracted to the positive anode and lose electrons to form stable atoms through oxidation

37
Q

How do you extract metals less reactive than carbon from their compounds

A

By reduction with carbon through a displacement reaction

38
Q

How are metal is more reactive than carbon extracted from their compounds

A

By electrolysis

39
Q

Does aluminium oxide have a low or high melting point and how is this overcome for electrolysis

A

High

It is mixed with cryolite which lowers it so the ions can move

40
Q

What happens to the aluminium ions in electrolysis of aluminium oxide

A

They go to the cathode and gain three electrons forming aluminium through reduction

41
Q

What happens to the oxygen ions in electrolysis of aluminium oxide

A

They go to the Arnold lose two electrons and form oxygen through oxidation

42
Q

What happens at the anode in electrolysis of aluminium oxide following the formation of oxygen

A

The oxygen reacts with the graphite in the anode forming carbon dioxide gas

43
Q

Why is aluminium extraction through aluminium oxide electrolysis expensive

A

Melting the aluminium oxide compound requires lots of energy which is expensive and lots of energy is needed to produce the electric current

44
Q

What ions to water molecules form

A

H+ and OH-

45
Q

What for ions are involved in electrolysis of copper sulphate in an aqueous solution

A

Cu2-
So42-
H+
Oh-

46
Q

In what circumstances will hydrogen be produced at the cathode in electrolysis of aqueous solutions

A

If the metal that would be produced is more reactive than hydrogen, hydrogen is produced

47
Q

In electrolysis of copper sulphate in aqueous solution what is produced at the cathode

A

Copper

48
Q

In electrolysis of copper sulphate in aqueous solution what is produced at the anode

A

Oxygen has

49
Q

Half equation for the anode in electrolysis of copper sulphate in aqueous solution

A

4OH- —> O2 + 2H2O + 4e-

50
Q

What ions are present in the electrolysis of sodium chloride in aqueous solution

A

Na+
Cl-
H+
OH-

51
Q

What element is formed at the cathode and electrolysis of sodium chloride in aqueous solution and why

A

Hydrogen is produced as sodium is more reactive

52
Q

What element is produced at the anode during electrolysis of sodium chloride in aqueous solution and why

A

Chlorine gas is produced because if the aqueous solution contains halite ions the halogen is produced at the anode

53
Q

What does inert mean

A

Not reactive

54
Q

What is the method for the copper 2 chloride and sodium chloride electrolysis required practical

A

Pour 50cm³ of copper to chloride into beaker
Place plastic dish with two holes on top with graphite electrodes through each hole
Attach wires and full circuit to electrodes
Repeat but with sodium chloride instead

55
Q

What will the results be for the copper 2 chloride and sodium chloride electrolysis required practical

A

For copper chloride at the cathode copper is formed and At the anode chlorine gas is formed
For sodium chloride at the cathode hydrogen is formed as sodium is more reactive and at the anode chlorine gas is formed as a halide present

Eleanor Rowe Chemistry GCSE (9 decks)

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