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Eleanor Rowe Chemistry GCSE > Chemical Changes > Flashcards

Chemical Changes Flashcards

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
Examples of weak acids
Carbonic acid Ethanoic acid Citric acid
26
As the pH scale decreases by 1 unit, how does the conc of H+ ions change?
It increases by 10 times
27
Titration required practical method
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
How does the orange indicator change from acidic to neutral in the titration reaction
Methyl orange goes from yellow when acidic to red when neutral
29
How can you read the volume of acid added from the burette correctly
Making sure your eye is at the surface of the meniscus and read it multiple times and calculate the mean
30
Why can solid ionic compounds not conduct electricity
The ions are locked in place and not free to move due to the electrostatic forces
31
What is a melted ionic compound called
An electrolyte
32
What material are the electrodes made out of
Graphite a form of carbon
33
What is the negative electrode called
The cathode
34
What is the positive electrode called
The anode
35
What happens to the positive ions in the solution during electrolysis
They are attracted to the negative cathode and gain electrons that surround it to form a stable atom through reduction
36
What happens to the negative ions in the solution during electrolysis
They are attracted to the positive anode and lose electrons to form stable atoms through oxidation
37
How do you extract metals less reactive than carbon from their compounds
By reduction with carbon through a displacement reaction
38
How are metal is more reactive than carbon extracted from their compounds
By electrolysis
39
Does aluminium oxide have a low or high melting point and how is this overcome for electrolysis
High | It is mixed with cryolite which lowers it so the ions can move
40
What happens to the aluminium ions in electrolysis of aluminium oxide
They go to the cathode and gain three electrons forming aluminium through reduction
41
What happens to the oxygen ions in electrolysis of aluminium oxide
They go to the Arnold lose two electrons and form oxygen through oxidation
42
What happens at the anode in electrolysis of aluminium oxide following the formation of oxygen
The oxygen reacts with the graphite in the anode forming carbon dioxide gas
43
Why is aluminium extraction through aluminium oxide electrolysis expensive
Melting the aluminium oxide compound requires lots of energy which is expensive and lots of energy is needed to produce the electric current
44
What ions to water molecules form
H+ and OH-
45
What for ions are involved in electrolysis of copper sulphate in an aqueous solution
Cu2- So42- H+ Oh-
46
In what circumstances will hydrogen be produced at the cathode in electrolysis of aqueous solutions
If the metal that would be produced is more reactive than hydrogen, hydrogen is produced
47
In electrolysis of copper sulphate in aqueous solution what is produced at the cathode
Copper
48
In electrolysis of copper sulphate in aqueous solution what is produced at the anode
Oxygen has
49
Half equation for the anode in electrolysis of copper sulphate in aqueous solution
4OH- —> O2 + 2H2O + 4e-
50
What ions are present in the electrolysis of sodium chloride in aqueous solution
Na+ Cl- H+ OH-
51
What element is formed at the cathode and electrolysis of sodium chloride in aqueous solution and why
Hydrogen is produced as sodium is more reactive
52
What element is produced at the anode during electrolysis of sodium chloride in aqueous solution and why
Chlorine gas is produced because if the aqueous solution contains halite ions the halogen is produced at the anode
53
What does inert mean
Not reactive
54
What is the method for the copper 2 chloride and sodium chloride electrolysis required practical
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
What will the results be for the copper 2 chloride and sodium chloride electrolysis required practical
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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