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A Level Chemistry - Inorganic Chemistry > Group 7 The Halogens > Flashcards

Group 7 The Halogens Flashcards

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1
Q

Colour of fluorine + state

A

Pale yellow
Gas

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2
Q

Chlorine colour + state

A

Pale green gas

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3
Q

Bromine colour and state

A

Brown -orange
Liquid

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4
Q

Iodine colour and state

A

Grey
Solid

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5
Q

Trend in boilings points group 7

A

Increase down the group
Increase Van Der waals due to increasing size and relative mass of atoms

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6
Q

Trend in electronegativity group 7

A

This decreases going down the group
As the atoms get larger the distance between positive nucleus and bonding electron increases + more shielding

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7
Q

Displacement rule in halogens

A

A more reactive halogen will displace a less reactive halogen

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8
Q

What colour is iodine solution

A

Brown

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9
Q

Standard equation of halogens displacing each other half/ ionic equation

A

X2 + 2Y- —> 2X- + Y2

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10
Q

How is bleach made which reaction

A

Disproportionating reaction

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11
Q

Equation for making bleach

A

2NaOH + Cl2 —> NaClO + NaCl + H2O

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12
Q

Uses of bleach

A

Cleaning agents
Treating water
Bleaching fabrics

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13
Q

What happens in a disproportionation reaction w chlorine

A

The chlorine is reduced and oxidised simultaneously

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14
Q

Why is chlorine added to water

A

To kill bacteria

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15
Q

Reaction when water is added to chlorine

A

H2O + Cl2 —> 2H+ + Cl- + ClO-

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16
Q

Reaction when chlorine is added to water but in sunlight ionic

A

2H2O + Cl2 —> 4H+ + 2Cl- + O2

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17
Q

Advantages of chlorinating drinking water x4

A

Destroys microorganisms that causes diseases
Long lasting so reduces bacteria build up
Reduces the growth of algae
Not doing it can lead to cholera epidemic

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18
Q

Disadvantages of chlorinating drinking water x3

A

Chlorine gas is toxic
Liquid chlorine causes chemical burns
Chlorine could react with organic compounds to make chloroalkanes. These can cause cancer.

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19
Q

Are halides oxidising or reducing agents

A

Reducing agents

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20
Q

Trend in reducing ability of halides review

A

Increase going down
They are reducing agents so oxides themselves so they lose electrons
Going down distance between outer electron and nucleus increases and more shielding so attraction is weaker.

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21
Q

Test for halide ions

A

1) add dilute nitric acid to remove the any ions that could give false results
2) add silver nitrate
3) further test with ammonia

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22
Q

Chloride ions form what colour precipitate

A

White

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23
Q

Bromine produce what coloured ions..

A

Cream

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24
Q

Iodine produce what coloured ions

A

Yellow

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25
Q

Half equation standard for halide test with silver nitrate

A

Ag+(aq) + X-(aq) —> AgX(s)

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26
Q

Cl- white precipitate with ammonia observation

A

Dissolves in dilute ammonia

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27
Q

I- yellow precipitate with ammonia observation

A

Insoluble in concentrated ammonia

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28
Q

Br- cream precipitate with ammonia observation

A

Insoluble in concentrated ammonia

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29
Q

How to test for group 2 ions

A

Flame test
Dip wire in hydrochloric acid
Place loop into blue flame

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30
Q

What colour calcium on flame test

A

Dark red

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31
Q

What colour strontium in flame test

A

Red

32
Q

What colour barium in flame test

A

Green

33
Q

How to test for ammonium compounds

A

Add sodium hydroxide
Heat gently
Positive - ammonia gas produced bleaches litmus paper blue

34
Q

Test for hydroxide + problem

A

They are alkaline so will turn red litmus paper blue
However lots of thing turn litmus paper blue so need to do further tests

35
Q

Test for carbonates

A

Add acid E.g. hydrochloric acid
Fizzing and Produces CO2 gas ( if positive)
Limewater turns cloudy if CO2 is present

36
Q

What order to test ions + why

A

1) carbonates
2) sulfates
3) halides
To prevent false positives

37
Q

Ionic equation for carbonate test

A

CO3 -2 + 2H+ —> CO2 + H2O

38
Q

Nitrogen gas formula

A

N2

39
Q

Forulma bleach

A

NAClO

40
Q

Half equation to show oxidation of halide ion to halogen

A

2X- —> X2 +2e-

41
Q

How to test for barium

A

Add any sulphate E.g. SO42-
White precipitate

42
Q

Bromine is what colour solution

A

Yellow

43
Q

Reaction when chlorine is added to water not ionic

A

2Cl2 + 2H2O —> 4HCl +O2

44
Q

Ionic equation test for barium with…

A

Sulfates
Ba2+ + SO4-2 —> BaSO4

45
Q

Equation when chlorine is added to drinking water

A

2Cl2 + 2H2O —> 4HCl +O2

46
Q

Why is catalyst used in equilibrium

A

No effect on yield
Lowers temperature used
Lowers cost

47
Q

State why not more than the minimum ionisation energy is used to ionise a sample

A

To prevent further ionisation

48
Q

Explain why sodium oxide forms alkali solution when reacts with water

A

Contains O2- ions
React with water to form OH- ions
O2- + H2O —> 2OH-

49
Q

Metal oxide + hydroxide

A

Metal oxide ion + water

50
Q

Why is second ionisation energy higher than first ionisation energy

A

More energy to remove an electron from a more positive ion

51
Q

Which element in period 2 has the highest 2nd ionisation energy

A

Li

52
Q

Chlorine + aqueous sodium hydroxide cold dilute

A

2NaOH + Cl2 —> NaCl + NaOCl + H2O

53
Q

Ionic equation w state symbols of metal reacting with water group 2

A

X (s) + 2H2O(l) —> X+2(aq) + 2OH- (aq) +H2(g)

54
Q

Practical steps to determine solubility of solution

A

Take a known volume of saturated solution
Evaporate to filtrate dryness
Weigh the residue

55
Q

Equation metal hydroxide + sulfuric acid

A

X(OH)2 + H2SO4 —> XSO4 + 2H2O

56
Q

Reactivity with water down group 2

A

Increases

57
Q

Why should you not add water to burning magnesium

A

Forms hydrogen
Which is flammable

58
Q

Strontium chloride + sodium sulfate

A

Sodium chloride + strontium sulfate

59
Q

How to test for presence of bromide ions w ammonia

A

Add nitric acid then silver nitrate
Then add dilute ammonia
Cream precipitation forms
No visible change

60
Q

Why does calcium have higher melting point than strontium

A

Delocalised electrons are closer to positive nucleus because atomic radius is smaller
This means stronger metallic bonding

61
Q

Equation chlorine redissolving in ammonia

A

AgCl(s) + 2NH3 (aq) —> Ag(NH3)2 + (aq) + Cl-

62
Q

Why is chlorine added to water even though it is toxic

A

Not harmful in low concentration

63
Q

Sulfur if acid formula

A

H2SO4

64
Q

Which halide ion with sulphuric acid is not a redox equasion

A

Chlorine + fluorine

65
Q

In the tests for halides why is excess silver nitrate used

A

To ensure ALL the halide ions precipitate out

66
Q

Reaction sodium halide and sulfuric acid + what do you see

A

H2SO4 + NaX —> NaHSO4 + HX
Misty fumes

67
Q

Reaction concentrated sulphuric acid with fluorine and chlorine + why

A

No reaction
Sulfuric acid is not a strong enough oxidising agent to oxides chloride or fluoride ions.

68
Q

Bromide and concentrated sulfuric acid + which oxidised and reduced + what observation

A

2Br- —> Br2 + 2e- (oxidised)
H2SO4 + 2H+ + 2e- —> SO2 + 2H2O (reduced)
Combine for overall equations
Orange vapour

69
Q

Iodine ions with concentrated sulfuric acid

A

1) NaI + H2SO4 —> NaHSO4 + HI
2) 2H+ + 2I - + H2SO4 —> I2 + SO2 + 2H2O
3) 6HI + SO2 —> H2S + 3I2 + 2H2O

70
Q

Role of chloride ions in NaCl + H2SO4 —> NaHSO4 + HCl

A

Base

71
Q

Bromine colour in solution

A

Orange

72
Q

Iodine colour in solution

A

Brown

73
Q

As you move from HCl to HI
The bond dissociation energy…
The bond polarity …..

A

Decreases
Decreases

74
Q

As you move from HCl to HI they are more/less easily oxidised in aqueous solutions

A

More

75
Q

Role of chlorine in NaCl + H2SO4 —> NaHSO4 + HCl

A

Proton donor

76
Q

Colour magnesium hydroxide

A

White

77
Q

What colour are the hydroxides of group 2

A

WHITE ALL

A Level Chemistry - Inorganic Chemistry (4 decks)

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