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Chemistry Paper 1 > Topic 5 Using Spec > Flashcards

Topic 5 Using Spec Flashcards

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1
Q

What are electrolytes

A

Ionic compounds that dissolve in water to make a solution that conducts electricity

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2
Q

What happens when ionic compounds are melted or dissolved in water

A

The ions are free to move around and the liquids will conduct electricity

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3
Q

What are positively charged ions attracted to

A

Negative electrode ( cathode)

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4
Q

What are negatively charged ions attracted to

A

Positive electrode (anode)

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5
Q

When do ions attract to the electrode

A

When a voltage is applied an electrolyte

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6
Q

What happens when an ion touches an electrode

A

Electrons can be transferred producing elements

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7
Q

What is electrolysis used for

A

Extracting reactive metals from molten ores

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8
Q

What is the anode usually made of and why

A

Carbon because it is a good conductor and is cheap

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9
Q

What happens at the cathode

A

Aluminium is formed

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10
Q

What are disadvantages of electrolysis

A

Lots of energy needed to produce the electric current

Costs money

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11
Q

Describe copper chloride solution in electrolysis

A

Applying electricity across copper chloride solution with graphite electrodes produces copper at the cathode and chloride gas at the anode

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12
Q

Describe molten lead bromide in electrolysis

A

When we use graphite electrodes to apply electricity across molten lead bromide, we form lead (metal) at the cathode and bromine (non-metal) at the anode.
Lead is present if a shiny metal forms around the cathode
Bromine is observed as a brown gas

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13
Q

Describe sodium chloride in electrolysis

A

Chloride produces hydrogen gas at cathode and chlorine gas at anode
Electrodes are graphite or platinum
Hydrogen can be detected using lit splint and squeaky pop sound
Chlorine gas detected by smell

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14
Q

Describe sodium sulfate in electrolysis

A

Graphite electrodes
Hydrogen and cathode and oxygen at anode
Hydrogen detected by split and squeaky pop
Oxygen detected by glowing splint

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15
Q

What is produced when halide ions are present at the anode

A

Respective halogen

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16
Q

What happens if there are no halide ions in the anode

A

Oxygen forms

17
Q

What is produced in the cathode when a metal is higher than oxygen in the reactivity series

A

Hydrogen

18
Q

What is produced in the cathode when metal is lower than hydrogen in the reactivity series

A

The metal is produced

19
Q

In the cathode what half question takes place

A

Pb2(+) - 2e(-) -> Pb

20
Q

What half equations takes place at the anode

A

2Br(-) -> Br2 + 2e(-)

21
Q

How can you purify copper using copper sulfate in electrolysis

A

Copper ions will go into the electrolyte solid copper sulfate
The Cu2+ ions will be attracted to the cathode and pure copper will form

22
Q

What metals are found in the earths crust

A

Gold and platinum (highly unreactive metals )

23
Q

What is oxidation

A

Gain of oxygen and loss of electrons

24
Q

What is reduction

A

Loss of oxygen and gain of electrons

25
Q

What is a displacement reaction

A

Where a more reactive metal that forms positive ions more easily can remove a less reactive metal from a compound

26
Q

Describe displacement in terms of oxidation and reduction

A

More reactive metal loses electrons (oxidation) and the less reactive metal gains electrons (reduction)

27
Q

What are the 4 stages of life cycle assessment

A

Collecting the raw materials needed
Making and packaging the product
Product use
Disposal of the product

28
Q

What are benefits of recycling metals

A

Less burning of fossil fuels
Less energy used
Conserves finite resources
Fewer waste rock heaps

29
Q

What does oxidation of metals result In

A

Corrosion

30
Q

How can the rusting of iron be prevented

A

Exclusion of oxygen
Exclusion of water
Sarcrifical protection

31
Q

What are the three methods to stops metals from corroding

A

Coatings - apply a coating witch acts like a barrier such as greasing, painting or electroplating
Sarcrifical method - metal that that requires protection will have a more reactive metal attached to it
Galvanising - metal that needs protecting is sprayed With a more reactive metal

32
Q

Disadvantages of coating

A

If the coating gets damaged, the metal becomes exposed so corrosion can take place

33
Q

How can electroplating be used to improve the appearance of a metal

A

coat a cheaper metal with a more expensive one. This gives the cheaper metal the appearance of the more expensive metal, which could be gold or silver. This gives us the option of buying cheaper jewellery.

34
Q

How is electroplating used in electrolysis

A

placing the metal to be electroplated at the negative electrode (cathode) and the coating metal at the positive electrode (anode).

Chemistry Paper 1 (4 decks)

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