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A-Level Edexcel Chemistry Flashcards > 4: Inorganic Chemistry and The Periodic Table > Flashcards

4: Inorganic Chemistry and The Periodic Table Flashcards

(75 cards)

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1
Q

What are the physical properties of group 2 elements?

A

They are bright silvery solids.
-> appear dull when exposed to oxygen

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2
Q

What is the trend in ionisation energy in Group 2 elements?

A

As you go down the group ionisation energy decreases.

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3
Q

Why does ionisation energy decreases as you go down group 2?

A

Greater atomic radius, so increased shielding effect. Making it easier to remove valence electron.

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4
Q

What is the trend in reactivity in Group 2 elements?

A

As you go down the group, reactivity increases.

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5
Q

Why does reactivity increase as you go down group 2?

A

Greater atomic radius, increases shielding affect. Easier to lose valence electrons

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6
Q

What elements of group 2 do you need to know the reactions of?

A

Mg to Ba

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7
Q

What is the reaction between group 2 metal and water?

A

Redox reaction to produce metal hydroxide + H2

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8
Q

What can be said about the reaction with water and magnesium?

A

Magnesium reacts slows with liquid water, reacts much faster with steam (due to extra energy).
- Produces Magnesium Oxide instead

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9
Q

What are the physical observations of magnesium oxide?

A

It’s a white powder

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10
Q

What is the reaction between group 2 metals and chlorine?

A

Reacts with chlorine gas to produce metal chlorides.

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11
Q

What colour are the group 2 metal chlorides?

A

All white precipitates

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12
Q

How do group 2 metals react with oxygen?

A

Form metal oxides
Strontium and barium react to form metal peroxides

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13
Q

Which group 2 oxides doesn’t react with water?

A

Beryllium oxide

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14
Q

What does the reaction between group 2 oxides with water produce?

A

Group 2 hydroxide + H2

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15
Q

What are the observation in a reaction between group 2 metals and water?

A

Fizzles and water vapour is released.

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16
Q

What is the reaction between group 2 oxides and HCl acid?

A

Forms chloride salt + water

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17
Q

What is the reaction between group 2 oxides and HNO3 acid?

A

Form nitrate salt + water

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18
Q

What is the reaction between group 2 hydroxides and HCl or HNO3?

A

Produce nitrate/chloirde salt + water

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19
Q

What happens to group 2 sulphate solubility as you go down the group?

A

Decreases.

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20
Q

What happens to group 2 hydroxide solubility as you go down the group?

A

Increases

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21
Q

What are the two factors that determine solubility?

A

1) Lattice dissociation enthalpy
2) Hydration enthalpy

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22
Q

What is lattice dissociation enthalpy?

A

Energy needed to break up a crystal structure.

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23
Q

What is hydration enthalpy?

A

Energy released when ions are hydrated

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24
Q

What affects the two solubility determining factors?

A

Ionic size

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25
Why does group 2 sulphate solubility decrease as you go down the group?
The lattice dissociation enthalpy and hydration enthalpy both decrease as you go down the group. - > hydration enthalpy decreases more than the lattice dissociation enthalpy
26
Why does group 2 hydroxide solubility increase as you go down the group?
There is a decrease in lattice dissociation enthalpy -> this outweighs the change in enthalpy of hydration
27
What is the trend in thermal stability of nitrates?
Thermal stability increases as you go down the group
28
What do group 1 nitrates (except Lithium) decompose to form?
Nitrites + Oxygen
29
Why does the thermal stability increase as you go down a group?
The metal ions have a smaller ionic radius, so higher charge density. This means that less heat energy is required to separate the two ions.
30
What do group 2 nitrates and Lithium decompose to form?
Metal oxide + nitrogen dioxide + oxygen
31
What can be said about the thermal stability of group 1 carbonates?
They are all stable, besides lithium. -> decomposed to give lithium oxide + carbon dioixde
32
What do group 2 carbonates decompose to?
Metal oxide + carbon dioxide
33
What colour are group 2 metal oxides?
White powder
34
In the flame test, what colour is lithium?
Red
35
In the flame test, what colour is sodium?
Yellow
36
In the flame test, what colour is potassium?
Lilac
37
In the flame test, what colour is magnesium?
No colour
38
In the flame test, what colour is calcium?
Brick red
39
In the flame test, what colour is strontium?
Crimson Red
40
41
In the flame test, what colour is Barium?
Pale green
42
What causes different colours in the flame tests?
When electrons drop back down to their original orbital, it releases a particular wavelength of energy
43
What is the trend in melting/boiling points in Group 7?
Increases as you go down the group.
44
Why does the melting/boiling point of group 7 increase as you go down the group?j
The strength of the London forces
45
What determines the strength of the London forces?
Number of electrons Size of electron cloud (molecule size)
46
What are the trends in electronegativity in group 7?
Electronegativity decreases as you go down the group
47
What are the trends in reactivity in group 7?
Decreases as you go down the group
48
Why does reactivity decrease as you go down group 7?
Electronegativity decreases as you go down, the more electronegative the more reactive.
49
What is the colour of potassium chloride KCl?
Colourless
50
What happens when you react potassium chloride (KCl) with either chlorine, bromine or iodine?
No reaction
51
What is the colour of potassium bromide (KBr)?
Colourless
52
What happens when you react potassium bromide (KBr) with either chlorine, bromine or iodine?
No reaction
53
What is the colour of potassium iodide (KI)?
Colourless
54
What happens when you react potassium iodide (KI) with either chlorine, bromine or iodine?
Chlorine - brown solution Bromine - brown solution Iodine - no reactioj
55
What colour is chlorine water?
Colourless
56
What colours is bromine water?
Orange
57
What colour is iodine water?
Brown
58
What happens to the oxidising power of halogens as you go down the group?
Decreases
59
What happens to the reducing power of halide ions as you go down the group?
Increases
60
What is the observation when you mix sulphuric acid with either fluoride or chloride?
Misty fumes
61
62
What is the observation when you mix sulphuric acid with bromide?
First reaction - misty fumes Second reaction - orange fumes (from Br2) and choking fumes (from SO2)
63
What is the observation when you mix sulphuric acid with iodide?
First reaction - misty fumes Second reaction - solid iodide and choking fumes Third reaction - toxic gas
64
What can be seen when silver nitrate is mixed with chloride ions?
White precipitate is formed
65
What can be seen when silver nitrate is mixed with bromide ions?
Cream precipitate is formed
66
What can be seen when silver nitrate is mixed with iodide ions?
Yellow precipitate is formed
67
Are chloride ions soluble in dilute aqueous ammonia?
Soluble
68
Are chloride ions soluble in concentrated aqueous ammonia
Soluble
69
Are bromide ions soluble in dilute aqueous ammonia?
Insoluble
70
Are bromide ions soluble in concentrated aqueous ammonia?
Soluble
71
Are iodide ions soluble in dilute aqueous ammonia?
Insoluble
72
Are iodide ions soluble in concentrated aqueous ammonia?
Insoluble
73
How are sulphate ions tested for?
Using acidified BaCl2. -> reacts to form barium sulphate (white precipitate)
74
How are carbonate and hydrocarbonate ions tested for?
HCl is added, fizz and CO2 gas is given off
75
What is the test for ammonium ions?
Damp red litmus paper would turn blue

A-Level Edexcel Chemistry Flashcards (10 decks)

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