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Edexcel A-Level Chemistry > Topic 4: Inorganic Chemistry > Flashcards

Topic 4: Inorganic Chemistry Flashcards

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1
Q

How do you measure atomic radius?

A

Half the distance between the two nuclei of the two identical atoms that are bonded together.

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2
Q

How does the atomic radius change across the period?

A

Decreases

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3
Q

Why does atomic radius decrease across the period?

A

More protons so an increased positive nuclear charge. So an increased attraction between the nucleus and the electrons. Drawing the electrons closer so a smaller atomic radius

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4
Q

What happens to atomic radius down the group?

A

Increases

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5
Q

Why does atomic radius increase down the group?

A

Number of electron shells increases, so that outer electron is further from the nucleus. Increased shielding from shells leads to decreased attraction to the nucleus and an increased atomic radius

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6
Q

What happens to the value of the first ionisation energy across the period?

A

Increases

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7
Q

Why does first ionisation energy increase across the period?

A

More protons means more attraction between the nucleus and electrons. So smaller ionic radius and greater attraction.

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8
Q

What happens to ionisation energy as you enter a new sub shell and why?

A

Drops as the new sub shell is of higher energy level so more energy is needed to remove.
on second filling the electrons are in opposite directions in same filling so repel one another

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9
Q

What happens to the ionisation energy value as you go down the group?

A

Decreases

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10
Q

Why does the Ionisation energy decrease down the group?

A

Atomic radius increases so electrons are further away from the nucleus and more shielding so attraction is less as you descend the group

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11
Q

What happens to the value of successive ionisation energies?

A

It increases

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12
Q

Why do successive ionisation energies increase?

A

when an electron is removed the other ones are pulled closer to the nucleus so more energy is needed to separate the electrons due to increased attraction.

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13
Q

What happens to successive ionisation energy as you drop an electron shell?

A

there is more attraction as you are closer to the nucleus so the ionisation energy increases

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14
Q

how do group 2 oxides react with acids?

A

Forms a salt and water
MgO + 2HNO3 -> Mg(NO3)2 + H2O

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15
Q

How do group 2 hydroxides react with acids?

A

forms the salt and water
Ca(OH)2 + H2SO4 -> CaSO4 + 2H2O

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16
Q

How does magnesium react with water?

A

Reacts with water as steam.
Forms magnesium oxide and hydrogen.
Mg + H2O -> MgO + H2

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17
Q

How do group 2 elements react with water?

A

Produces the metal hydroxide and hydrogen. Group 2 hydroxides can be soluble.
Sr + 2H2O -> Sr(OH) + H2

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18
Q

How does a group 2 element react with chlorine?

A

Forms the metal chloride.
Ca +Cl2 -> CaCl2

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19
Q

What is the general formula for metal chlorides?

A

XCl2
with x being the metal

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20
Q

How does a group 2 element react with oxygen?

A

Forms the metal oxides.
2Mg + O2 -> 2MgO

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21
Q

What colour do group 2 oxides burn?

A

Typically white.
Magnesium oxide is definitely white.

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22
Q

What happens to ionisation energy as you go down group 2? Why?

A

Ionisation energy decreases as the electron is further away from the nucleus and more shielding means less attraction.

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23
Q

What happens to reactivity as you go down group 2? Why?

A

Increases as it is easier to loose the two electrons due to the reduced ionisation energy

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24
Q

Are group 2 elements oxidising or reducing agents?

A

Reducing Agents.
They are oxidised themselves as they loose 2 electrons.

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25
Q

How do group 2 elements react with acids?

A

Produces metal salt and hydrogen gas.
Mg +H2SO4 -> MgSO4 + H2

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26
Q

What happens when an oxide reacts with water?

A

Produces a hydroxide, which dissolves in water.
CaO + H2O -> Ca(OH)2 + H2

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27
Q

What is the trend in solubility of group 2 hydroxides?

A

Increasingly soluble down the group.

Mg(OH)2 - Milk of magnesia, not very soluble.

Ca(OH)2 - Lime Water, very soluble

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28
Q

What effect do hydroxides have on the solution?

A

Makes the solution Alkali. The higher the hydroxide ion concentration the more alkaline it is.

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29
Q

what effect does solubility have on alkalinity?

A

Lower solubility means that there is a low concentration of hydroxide ions so is less alkaline.

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30
Q

What is the trend in solubility of group 2 sulphates?

A

Less soluble down the group.

MgSO4 - Highly soluble in water.

BaSO4 - Insoluble in water - forms a white precipitate

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31
Q

Are group 2 carbonates soluble in water?

A

No - Insoluble

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32
Q

Are group 2 nitrates soluble in water?

A

Yes - Soluble

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33
Q

What happens to the thermal stability of group 2 carbonates and nitrates as you go down the group?

A

Become more thermally stable.

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34
Q

Why do group 2 carbonates and nitrates become more thermally stable as you go down the group?

A

Carbonate and nitrate ions are larger so are more stable with larger ions found towards the bottom of the group.
Smaller ions are more polorising so cause more distortion to the Co or NO ion - making it easier to break bonds.
Larger ions are less polorising so more energy is needed to break the bonds.

35
Q

is group 1 thermally stable?

A

Yes - Stable

36
Q

How do group 1 nitrates decompose?

A

Norm nitrites (XNO2) and O2.

NaNO3 -> NaNO2 + O2

37
Q

What is the exception to the group 1 carbonates and nitrates being stable?

A

Lithium Carbonate

38
Q

Why is lithium carbonate an exception to the stability of group 1 carbonates?

A

Lithium is a small ion.
The carbonate forms lithium oxide and CO2.
The Nitrate forms lithium oxide, NO2 and O2.

39
Q

Why do group 2 nitrates decompose more than group 1?

A

Group 2 has a greater positive charge (charge dencity). So group 2 ions are more polorising and cause more distortion to the nitrate ion.

40
Q

Why is lithium the exception?

A

It is very small - meaning it has a large charge density - so polorises the anion more

41
Q

What colour and state is Fluorine at RTP?

A

Pale yellow gas

42
Q

What colour and state is chlorine at RTP?

A

Pale green gas

43
Q

What colour and state is bromine at RTP?

A

red-brown liquid

44
Q

What colour and state is iodine at RTP?

A

grey-black solid

45
Q

How do melting and boiling points change down the group?

A

Increases down the group

46
Q

Why does the melting and boiling point increase down group 7?

A

a greater number of london forces between the molecules as there are more electrons as you go dow the group

47
Q

What is electronegitivity?

A

The ability of an atom to attract the bionding pair of electrons

48
Q

How does electronegitivity change down group 7?

A

Decreases

49
Q

Why does electronegitivity decrease down group 7?

A

Increased ionic radius so outer electrons are further from the nuclius - also increases sheilding. This reduces the attraction between the nuclius and the bonding pair of electrons

50
Q

What happens when hallogens react?

A

They remove an electron from another species.
Causing the species to be oxidised

51
Q

Are halogens oxidising or reducing agents?

A

Oxidising agents as they are reduced themselves

52
Q

What happens when a halogen is reacted with an aqueous solution of another metal halide?

A

The more reactive halide displaces the halide of the metal halide.

Cl2 + 2NaBr -> 2NaCl +Br

53
Q

What type of reaction is a halogen and aqueous solurion of a metal halide?

A

Displacement

54
Q

What observations can be seen from a displacement reaction?

A

Colour change

55
Q

What is the purpose of a non-polar organic solvent?

A

to distinguish between the different halides present.

56
Q

What non-polar organic solvent is typically used to distinguish between different halides?

A

Cyclohexane

57
Q

What colour is chlorine in water?

A

Pale green/colourless

58
Q

What colour is chlorine in an organic solvent?

A

Pale Green/colourless

59
Q

What colour is bromine in water?

A

Orange

60
Q

What colour is bromine in an organic solvent

A

orange/red

61
Q

What colour is iodine in water?

A

Brown

62
Q

What colour is iodine in an organic solvent

A

pink/violet

63
Q

What is a disproportionation reaction?

A

When the same element undergoes both oxidation and reduction simultaniouesly.

64
Q

How does chlorine react with water?

A

Produces Chloric (I) acid and hydrochloric acid.

Cl2 + H2O -> HCl + HClO

65
Q

How does chlorine react with cold aqueous sodium hydroxide?

A

produced sodium chloride (NaCl) and sodium chlorate (I) (NaClO) and water

Cl2 + 2NaOH -> NaCl + NaClO + H2O

66
Q

How does chlorine react with hot concentrated sodium hydroxide?

A

Produces sodium chloride (NaCl). Also Water.
Chlorate (I) undergoes further decomposition and forms the chlorate (V) ion (NaClO3)

3Cl2 + 6NaOH -> 5NaCl + NaClO3 + 3H2O

67
Q

What happens in the reaction between a halide and sulfuric acid?

A

The halide ions are oxidised. They cause sulpher to be reduced.
e.g.

2Br- + x -> Br2 + x-

68
Q

What happens to group 7’s reducing ability as you go down the group?

A

Become better reducing agents

69
Q

Why does the reducing ability of group 7 become better as you go down the group?

A

Small atomic radius and little shielding mean that it is hard for elements at the top to lose electrons.

70
Q

What happens in the reaction with concentrated sulfuric acid and sodium chloride?

A

Makes Sodium Hydrogen sulphate and HCl.

NaCl + H2SO4 -> NaHSO4 + HCl

misty fumes of HCl are seen

71
Q

What happens after the reaction of concentrated sulfuric acid and sodium chloride?

A

Chlorine ions have a low reducing power so the reaction stops. There is not change in oxidation states.

72
Q

What happens in the reaction with concentrated sulfuric acid and sodium bromide?

A

Makes Sodium Hydrogen sulphate and HBr.

NaCl + H2SO4 -> NaHSO4 + HBr

See misty fumes of HBr followed by brown gas of bromine

73
Q

What happens after the reaction of concentrated sulfuric acid and sodium bromide?

A

Bromine reduces the sulpher to form H2O, SO2 and Br2.

2Br- + H2SO4 + 2H+-> SO2 + Br2 + H2O

74
Q

What happens in the reaction with concentrated sulfuric acid and sodium iodide?

A

Makes Sodium Hydrogen sulphate and HI.

NaCl + H2SO4 -> NaHSO4 + HI

See purple fumes of HI

75
Q

What happens after the reaction of concentrated sulfuric acid and sodium iodide?

A

Iodine reduces the sulphur to an oxidation state of either 0 or -2. it forms either sulphur or hydrogen sulphate,

H2SO4 + 6HI -> 3I2 + 4H2O + S
or
H2SO4 + 8HI -> 8I2 + 4H2O + H2S

purple fumes of iodine are seen.

H2S produces an eggy smell

76
Q

How can the produced halide solution be identified?

A

By adding silver nitrate (AgNO3) to the solution to cause the precipitation of a silver halide

77
Q

What precipitate does AgCl produce?

A

White

78
Q

What colour precipitate does AgBr produce?

A

Cream

79
Q

What colour precipitate does AgI produce?

A

Yellow

80
Q

How can the silver halide precipitate be tested to further aid identification?

A

Dissolving in dilute and concentrated ammonia

81
Q

What does AgCl dissolve in?

A

Dilute ammonia solution

82
Q

What does AgBr dissolve in?

A

Concentrated ammonia

83
Q

What does AgI dissolve in?

A

Does not dissolve in ammonia

Edexcel A-Level Chemistry (9 decks)

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