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A Level Chemistry > Chapter 8 - Reactivity trends > Flashcards

Chapter 8 - Reactivity trends Flashcards

1
Q

What is common about all elements in group 2?

A

They are all reactive metals which form 2+ ions

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2
Q

Why are group 2 elements called reducing agents?

A

In a redox reaction, they lose electrons (oxidation) which is donated to the other reactant, reducing it

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3
Q

What is the most common type of reaction for group 2 elements?

A

Redox

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4
Q

What happens when a group 2 metal reacts with oxygen?

A

It forms a metal oxide with the general formula MO

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5
Q

What is produced when a group 2 metal burns in oxygen?

A

A solid, white oxide

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6
Q

What is produced when group 2 metals react with water?

A

An alkaline metal hydroxide and hydrogen gas

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7
Q

What is the general formula for group 2 metal hydroxides?

A

M(OH)2

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8
Q

What is produced when group 2 metals react with dilute acid?

A

Metal + Acid -> Salt + Hydrogen

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9
Q

Why does reactivity increase down group 2?

A

Group 2 metals wish to lose 2 electrons from their outer shell, to gain a full outer shell. Ionisation energy decreases down the group, because of an increase in atomic radius and there are more electrons to shield

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10
Q

Why do the first and second ionisation energies decrease down group 2?

A

Increasing atomic radius and the shielding effect of other electrons means less energy is needed to overcome the force

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11
Q

What happens when an oxide of a group 2 metal reacts with water?

A

Metal hydroxides are formed which dissolve to form hydroxide ions (OH-) and alkaline solutions of the metal hydroxide (ions)

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12
Q

Why is slaked lime (Ca(OH)2) often spread onto fields?

A

It is a base and neutralises acidic soils so crops can grow

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13
Q

Why are group 2 bases, like Mg(OH)2 and CaCO3 used as antacids?

A

The bases neutralise the hydrochloric acid in your stomach which is causing the discomfort

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14
Q

Ionic equation for neutralisation

A

H+ (aq) + OH- (aq) -> H2) (l)

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15
Q

What happens when a solution of group 2 hydroxides becomes saturated?

A

Any metal and hydroxide ions will form a solid precipitate

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16
Q

Because the solubility of group 2 hydroxides increases down the group, what happens to the resulting solution?

A

They contain more OH- ions and are more alkaline

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17
Q

How to show the increasing alkalinity of group 2 hydroxides?

A

Add a spatula of metal oxide to some water and shake

Measure the pH. This will increase down the group

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18
Q

Why do the group 7 elements not occur in their elemental forms in nature?

A

They are highly reactive

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19
Q

At RTP, what will all halogens exist as?

A

Diatomic molecules (two atoms joined by a single covalent bond)

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20
Q

In their solid states, what will the halogens form lattices with?

A

Simple molecular structures

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21
Q

Colour and state of fluorine

A

Pale yellow, gas

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22
Q

Colour and state of chlorine

A

Green, gas

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23
Q

Colour and state of bromine

A

Red-brown, liquid

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24
Q

Colour and state of iodine

A

Grey, solid

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25
As you go down group 7, why do melting and boiling points increase?
As the size of the atom increases, there are more electrons, and so the strength of the induced dipole-dipole forces increases, meaning more energy is needed to overcome the intermolecular forces
26
What is the most common type of reaction for halogens?
Redox
27
Why are halogens known as oxidising agents?
In a reaction, they gain one electron from the other reactants, meaning the halogen is reduced and the other is oxidised
28
If the halogen added to the halide in a displacement reaction is more reactive, what happens?
The halogen will displace the halide from the solution and the reaction will change colour
29
What chemical is added to the solution during a displacement reaction and why?
Cyclohexane - the non-polar halogens dissolve more readily with this than water and so the colour change is clearer to see
30
What colour can be observed when bromide ions are added to chlorine?
Orange - Br2 is formed
31
What colour can be observed when iodide ions are added to chlorine?
Violet - I2 is formed
32
What colour can be observed when chloride ions are added to bromine?
No reaction
33
What colour can be observed when iodide ions are added to bromine?
Violet- I2 is formed
34
What colour can be observed when either chloride ions or bromide ions are added to iodine?
No colour change - iodine is the least reactive and won't be displaced
35
How reactive is fluorine?
Very - it reacts with almost any substance it comes into contact with
36
How reactive is astatine?
It is radioactive and decays rapidly so that is unknown, but it is predicted to be the least reactive
37
Why does reactivity decrease as you go down group 7?
Halogens want to gain another electron to achieve the full outer shell that is desirable As you down the group, the atomic radius increases and there more inner electrons, so shielding increases too There is, therefore, less nuclear attraction to attract the final electron needed for a full outer shell Reactivity decreases
38
What is a disproportionation reaction?
A chemical reaction in which an element is both oxidised and reduced
39
Two examples of disproportionation reactions
Chlorine with water | Chlorine with cold, dilute sodium hydroxide
40
Why is chlorine added to water?
It forms chloric acid which kills bacteria so the water is safe to drink
41
What is produced when chlorine is added to water?
Hydrochloric acid and chloric acid
42
What happens when chloric acid is ionised?
It forms chlorate (I) ions, which are what kills bacteria
43
What is produced when chlorine is added to sodium hydroxide?
Bleach
44
Why is chlorine important in water treatment? (3)
It kills bacteria Some chlorine remains in the water and prevents reinfection Prevents the growth of algae, which can cause discolouration and bad smells/tastes
45
Ethical issues with chlorinating water
We don't get a choice about having chlorine in our water
46
Problems with using chlorine in water (3)
It irritates the respiratory system if inhaled Liquid chlorine causes severe chemical burns Chlorine can react with organic hydrocarbons to form chlorinated hydrocarbons
47
What is bad about chlorinated hydrocarbons?
They are carcinogens
48
Alternatives to chlorinating the water
Use ozone, which is good at killing bacteria, but too expensive to produce Use UV light, which kills bacteria by damaging their DNA, but it isn't effective in cloudy water
49
What is formed when halogens are added to silver nitrate?
A coloured precipitate
50
How do you test for a carbonate?
Add dilute nitric acid to the solution If you see bubbles, these could be carbon dioxide To test for carbon dioxide, bubble the gas through limewater. It should turn cloudy. If carbon dioxide is produced, a carbonate is present
51
How to test for halides
Add aqueous silver nitrate to the solution Record the colour of the precipitate Add ammonia solution to the mixture Record the solubility
52
Colour of silver chloride
White
53
Colour of silver bromide
Cream
54
Colour of silver iodide
Yellow
55
When will silver chloride be soluble?
Dilute ammonia
56
When will silver bromide be soluble?
Concentrated ammonia
57
When will silver iodide be soluble?
It won't - it is insoluble in ammonia
58
How to test for ammonia compounds
Add sodium hydroxide to ammonia solution Warm the mixture and ammonia gas will be released Ammonia is alkaline so will turn red litmus paper blue
59
What is the correct order of testing for anions?
Carbonate test Sulfate test Halide test
60
Why should the carbonate test go first?
Neither sulfides nor halides produce bubbles with acid. Therefore, it can be carried out with the possibility of an incorrect answer
61
Why should the sulfate test go second?
Barium carbonate also produces the characteristic white precipitate, which could give you a false positive. Therefore, you have to carry out the carbonate test first to ensure it isn't a carbonate
62
Why should the halide test go last?
Silver carbonate and silver sulfate will also produce precipitates, so it is important to have carried out the other tests first to ensure there is no confusion
63
What should you when conducting the carbonate test on a mixture of ions?
Use nitric acid (sulfuric acid will interfere with the sulfate test and hydrochloric with the halide test) and continue adding until bubbling stops, so all the carbonate has been removed
64
What should you do when conducting the sulfate test on a mixture of ions?
Add an excess of barium nitrate | Any sulfate ions present will form a precipitate, which can then be removed
65
What should you do when conducting the halide test on a mixture of ions?
Add silver nitrate to the remaining solution Any sulfate or carbonate ions will have already been removed, so you know that if it forms a precipitate it will be a halide Add ammonia to discover which
66
How to test for a sulfate
Add barium nitrate to your solution (barium chloride introduces halide ions which can affect later tests) Barium sulfate forms a white precipitate - if this forms, sulfate ions are present
67
Equation for the formation of bleach
Cl2 + 2NaOH -> NaCl + NaClO + H2O
68
What conditions must be present for bleach to form?
The sodium hydroxide must be cold and dilute
69
What is periodicity?
A repeating pattern of properties shown across different periods
70
What colour does Cl2 go in cyclohexane?
Pale green
71
What colour does Br2 go in cyclohexane?
Orange
72
What colour does I2 go in cyclohexane?
Violet - it changes from brown
73
What happens to the pH of the solution formed when group 2 metals are added to water as you go down the group?
As you go down group 2, the solubility of the metal increases which increases the pH and alkalinity
74
Why is chlorine more reactive than bromine?
Gains an electron more easily Chlorine smaller Decreased shielding Greater nuclear attraction
75
How do you test for ammonia?
Add ammonia hydroxide Warm the mixture to produce gas Turns indicator blue

A Level Chemistry (29 decks)

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