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Chemistry CGP Paper 2 > Section 1 > Flashcards

Section 1 Flashcards

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1
Q

What do compounds with ionic bonding always have?

A

Giant ionic structures.

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2
Q

How are giant ionic structures held together?

A

Closely packed 3D lattice arrangement by the attraction between oppositely charged ions.

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3
Q

What is the electrostatic attraction between oppositely charged ions?

A

Very strong.

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4
Q

Why is the boiling point of giant ionic structures so high?

A

A lot of energy is required to overcome the strong attraction.

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5
Q

How do the charges of the ion affect the structure?

A

It affects the strength of the ionic bonding. 2+ or 2- is stronger than 1+ or 1-.

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6
Q

What do higher charged ions mean?

A

Higher melting and boiling points.

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7
Q

In diamond what does each carbon atom form?

A

Four covalent bonds in a very rigid giant covalent structure.

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8
Q

What is the hardest natural substance?

A

Diamond.

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9
Q

What is diamond used for?

A

Drill tips and cutting tools.

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10
Q

In graphite what does each carbon atom form?

A

Three covalent bonds creating layers.

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11
Q

What do the layers in graphite allow?

A

Free to slide over one another.

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12
Q

What does this mean graphite is good for?

A

A good lubricant.

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13
Q

What does the sliding also do?

A

Leaves free electrons, so graphite is the only non-metal which is a good conductor of electricity.

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14
Q

How can the theoretical yield be calculated?

A

From the balanced equation.

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15
Q

Percentage yield =

A

actual yield / theoretical yield x 100

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16
Q

What does 100% yield mean?

A

You got all the product you expected to get.

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17
Q

What is 6.023 x 10 to the 23?

A

Avogadro’s number or the Avogadro constant.

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18
Q

What can you think of a mole as?

A

The Avogadro number of particles in a substance, where the particles are atoms, molecules, ions or electrons.

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19
Q

One does one mole of any gas occupy at room temperature and pressure?

A

24 dm3.

20
Q

Volume =

A

moles of a gas x 24

21
Q

Volume =

A

mass of a gas / Mr of gas x 24

22
Q

In electrolysis what will be produced at the cathode in an aqueous solution with sodium?

A

Hydrogen.

23
Q

In electrolysis what will be produced at the cathode in an aqueous solution with copper?

A

Copper.

24
Q

In electrolysis what will be produced at the anode if a halide is present?

A

The halide.

25
Q

In electrolysis what will be produced at the anode if no halide is present?

A

Oxygen.

26
Q

What ions are in sulphuric acid solution?

A

SO42-, H+, OH-.

27
Q

What is formed at the cathode in sulphuric acid?

A

Hydrogen.

28
Q

What is the half equation for the production of hydrogen?

A

2H+ + 2e- -> H2

29
Q

In sulphuric acid what is formed at the anode?

A

Oxygen and water.

30
Q

What is the half equation for the production of oxygen and water?

A

4OH- -> O2 + 2H20 + 4e-

31
Q

What ions are in sodium chloride solution?

A

Na+, Cl-, OH- and H+.

32
Q

What is formed at the cathode in sodium chloride?

A

Hydrogen.

33
Q

What is formed at the anode in sodium chloride?

A

Chlorine gas.

34
Q

What is the half equation for the production of chlorine gas.

A

2Cl- -> Cl2 + 2e-

35
Q

What ions are in copper (II) sulphate solution?

A

Cu2+, SO42-, H+ and OH-

36
Q

What is produced at the cathode in copper sulphate?

A

Copper metal.

37
Q

What is produced at the anode in copper sulphate?

A

Oxygen and water.

38
Q

What is the half equation for the production of copper metal?

A

Cu2+ + 2e- -> Cu.

39
Q

What does the amount of product made by electrolysis depend on?

A

The number of electrons that are transferred.

40
Q

What happens if you increase the number of electrons?

A

You increase the mount of substance produced.

41
Q

How can you increase the number of electrons?

A

Electrolysing for a longer time, increasing current.

42
Q

What does one amp flowing for one second mean?

A

A charge of one coulomb has moved.

43
Q

Q =

A

It.

44
Q

What does 1 faraday contain?

A

One mole of electrons.

45
Q

When working out the mass of something in electrolysis what are the steps?

A
  1. Write balanced half equation for cathode.
  2. Calculate number of faradays (amps x time (s)) .
  3. Calculate number of moles of substance produced (faradays divided by number of electrons in half equation).
  4. Work out mass = Mr x moles.

Chemistry CGP Paper 2 (14 decks)

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