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Paper 1 CHEM MMS EXAM > ✅4 - Inorganic Chemistry and the Period Table > Flashcards

✅4 - Inorganic Chemistry and the Period Table Flashcards

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1
Q

How does ionisation energy change down group 2?

A

It decreases

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2
Q

Why does ionisation energy decrease down Group 2?

A

The extra inner shells shield electrons

Nucleus is further away from outer electrons due to more shells

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3
Q

How does reactivity change down group 2?

A

Reactivity increases

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4
Q

Why does reactivity increase down group 2?

A

It becomes easier for the outer electrons to be lost, as they have lower ionisation energies

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5
Q

What do group 2 elements react with?

A

Water, oxygen and chlorine

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6
Q

What are the group 2 elements?

A

Beryllium, Magnesium, Calcium, Strontium, Barium (Radium)

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7
Q

What do group 2 elements produce when they react with water?

A

Hydroxides and hydrogen

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8
Q

Which group 2 elements react with water?

A

All except Be, Mg reacts very slowly

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9
Q

What do group 2 elements produce when they react with oxygen?

A

Oxides

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10
Q

What colour are group 2 oxides?

A

White

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11
Q

What do group 2 elements produce when they react with chlorine?

A

Chlorides

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12
Q

What colour are group 2 chlorides?

A

White

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13
Q

Oxides and hydroxides are…

A

…bases

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14
Q

What happens when group 2 oxides dissolve in water?

A

They form a strongly alkaline solution due to OH-

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15
Q

What happens when beryllium oxide is added to water?

A

It doesn’t dissolve, it is insoluble

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16
Q

What happens when magnesium oxide is added to water?

A

It reacts slowly and isn’t very soluble

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17
Q

When oxides and hydroxides are added to acid, what do they form?

A

They neutralise the acid to form salts

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18
Q

What is the equation for the reaction between MgO and H2O?

A

MgO + H2O —-> Mg(OH)2

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19
Q

What is the equation for the reaction between MgO and HCl?

A

MgO + 2HCl —-> MgCl2 + H2O

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20
Q

Solubility trends of group 2 depend on…

A

…the anion

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21
Q

If a group 2 compound has a singly charged anion (OH-) how does the solubility change down the group?

A

It increases

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22
Q

If a group 2 compound has a doubly charged anion (SO4 2-) how does the solubility change down the group?

A

It decreases

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23
Q

Which group 2 sulfate is insoluble?

A

Barium Sulfate

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24
Q

How does thermal stability change down group 1 and 2 carbonates and nitrates?

A

It increases

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25
Q

Why do carbonates and nitrates become more stable down the group?

A

Large ions have less polarising power so distort the electron cloud less and have a lower charge density. Therefore, they distort the carbonate or nitrate less

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26
Q

Which of group 1 and group two compounds are more thermally stable?

A

Group 1

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27
Q

Why are Group 1 compounds more stable than group 2?

A

They have a lower charge, so a lower charge density and therefore less polarising power

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28
Q

What do group 2 carbonates decompose to form?

A

An oxide and carbon dioxide

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29
Q

What is the equation for thermal decomposition of CaCO3?

A

CaCO3 —-> CaO + CO2

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30
Q

Do group 1 carbonates decompose?

A

No

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31
Q

What do group 1 nitrates decompose to form?

A

The Nitrite (NO2) and oxygen

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32
Q

What is the equation for decomposition of Potassium nitrate?

A

2KNO3 —-> 2KNO2 + O2

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33
Q

What is the exception to the group 1 nitrate decomposition?

A

Lithium

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34
Q

What does lithium nitrate decompose to form?

A

LiO2, NO2 and O2

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35
Q

What doe group 2 nitrates decompose to form?

A

The oxide, nitrogen dioxide and oxygen

36
Q

What is the equation for the decomposition of Ca(NO3)2?

A

2Ca(NO3)2 —-> 2CaO + 4NO2 + O2

37
Q

How can the thermal stability of nitrates be tested?

A

Measuring how long it takes for a certain amount of oxygen to be produced
OR
How long it takes for brown gas (NO2) to be produced

38
Q

How can the thermal stability of carbonates be tested?

A

Measuring how long it takes for a certain amount of CO2 to be produced using lime water

39
Q

What is the flame colour for Lithium?

A

Red

40
Q

What is the flame colour for Sodium?

A

Orange/Yellow

41
Q

What is the flame colour for Potassium?

A

Lilac

42
Q

What is the flame colour for Rubidium?

A

Red

43
Q

What is the flame colour for Caesium?

A

Blue

44
Q

What is the flame colour for Calcium?

A

Brick red

45
Q

What is the flame colour for Strontium?

A

Crimson

46
Q

What is the flame colour for Barium?

A

Apple green

47
Q

Why is a colour produced during a flame test?

A

The electrons are excited to a higher energy level and then as they drop back down, they release the energy in the form of light.

48
Q

What determines the wavelength of light produced in a flame test?

A

The difference between the higher and lower energy levels

49
Q

What is the solubility of halogens?

A

Low, as they are non polar

50
Q

What do halogens dissolve easily in?

A

Cyclohexane

51
Q

How can halogens be identified when dissolved in organic compounds?

A

They have distinctive colours

52
Q

What colour is bromine in hexane?

A

Orange/Red

53
Q

What colour is iodine in hexane?

A

Purple

54
Q

How does the reactivity of halogens change down the group?

A

It decreases

55
Q

How do the melting and boiling points of halogens change down the group?

A

They increase

56
Q

Why do melting and boiling points increase down group 7?

A

There are more electron shells, so greater London forces

57
Q

What can chlorine displace?

A

Br- and I-

58
Q

What can bromine displace?

A

I-

59
Q

What redox property do halogens have?

A

They are reducing agents

60
Q

How do halogens react with group 1 metals?

A

They produce halide salts, so the metal is reduced and the halogen oxidised

61
Q

What is the equation for the reaction between Li and F?

A

2Li + F2 —-> 2LiF

62
Q

How do halogens react with group 2 metals?

A

They form halide salts, where the metal is reduced and the halogen oxidised

63
Q

What type of reaction occurs between halogens and cold alkalis?

A

Disproportionation

64
Q

What is the equation for the reaction between I2 and NaOH?

A

I2 + 2NaOH —-> NaOI + NaI + H2O

65
Q

What type of reaction do halogens undergo with hot alkali?

A

Disproportionation

66
Q

What compound is used to kill bacteria?

A

Chlorate (I) - ClO-

67
Q

How does the reducing power of halides change down the group?

A

It increases

68
Q

What is the equation for the reaction between KCl and H2SO4?

A

KCl + H2SO4 —-> KHSO4 + HCl

69
Q

What happens during the reaction between KCl and H2SO4?

A

HCl gas is given off as misty fumes
Cl- aren’t strong enough reducing agents to reduce sulfuric acid, so reaction stops there
Not a redox reaction

70
Q

What are the equations for the reaction between KBr and H2SO4?

A

KBr + H2SO4 —-> KHSO4 + HBr

2HBr + H2SO4 —-> Br2 + SO2 + 2H2O

71
Q

What happens during the reaction between KBr and H2SO4?

A

The first reaction gives misty fumes of HBr
Br- are stronger reducing agents so react with H2SO4 in a redox reaction
The reaction produces fumes of sulfur dioxide and orange fumes of Br2

72
Q

What are the equations for the reactions between Kl and H2SO4?

A

KI + H2SO4 —-> KHSO4 + HI
2HI + H2SO4 —-> I2 + SO2 + 2H2O
6HI + SO2 —-> H2S + 3I2 + 2H2O

73
Q

What happens during the reactions between Kl and H2SO4?

A

HI gas is produced in the initial reaction
Iodide ions then reduce H2SO4 as before
I- is a strong reducing agent and reduced the SO2 to H2S

74
Q

What are hydrogen halides?

A

Acidic gases

75
Q

How do hydrogen halides behave in water?

A

The dissolve

76
Q

How do hydrogen halides react with ammonia?

A

They give off white fumes of ammonium halides

77
Q

What colour precipitate does Chlorine give with Silver Nitrate?

A

White

78
Q

What colour precipitate does Bromine give with Silver Nitrate?

A

Cream

79
Q

What colour precipitate does Iodine give with Silver Nitrate?

A

Yellow

80
Q

How does AgCl behave with ammonia?

A

The precipitate dissolves to give a colourless solution

81
Q

How does AgBr behave with ammonia?

A

The precipitate remains unchanged in dilute, but will dissolve in conc ammonia

82
Q

How does AgI behave with ammonia?

A

The precipitate will not dissolve, even in conc ammonia

83
Q

What is the test for carbonates?

A

Add dilute hydrochloric acid and use lime water to test for any CO2 given off

84
Q

What is the test for Sulfates?

A

Add dilute HCl and BaCl2. If a white precipitate forms, a sulfate is present

The hydrochloric acid is needed to react with carbonate impurities that are often found in salts which would form a white Barium carbonate precipitate and so give a false result.
You could not used sulphuric acid because it contains sulphate ions and so would give a false positive result.

85
Q

How is ammonia tested for?

A

It is alkaline, so damp red litmus paper can be used. If ammonia gas is present, the paper will turn blue

86
Q

How are ammonium ions tested for?

A

Add sodium hydroxide and gently heat the mixture. If ammonia is given off, ammonium ions were present

Paper 1 CHEM MMS EXAM (12 decks)

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