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Chemistry Revision > Chemistry Of The Elements (The Periodic Table. Reactivity Series, Tests) > Flashcards

Chemistry Of The Elements (The Periodic Table. Reactivity Series, Tests) Flashcards

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1
Q

Metal oxides are __________

Whereas non-metal oxides are __________

A

Basic

Acidic

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2
Q

Why do elements in the same group have similar chemical properties

A

Because they have the same number of electrons in their outer shell

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3
Q

Group 1 metal + water —>

A

Metal + Water –> Metal Hydroxide + Hydrogen

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4
Q

Group 1 elements become more reactive as you go _______ the group

A

Down

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5
Q

Why do group 1 elements become more reactive as you go down the group

A

Because the outermost electrons is in an shell which is further from a nucleus so the attraction between the outermost electron and the nucleus becomes less. So the bigger the group 1 atom, the weaker the attraction and the more easily the electron is lost. (So it wants to to react quicker and is more reactive)

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6
Q

Is metal hydroxide acidic or alkaline

A

Alkaline

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7
Q

As you go down group 7, the _________ the colour and the __________ the boiling point

A

Darker

Boiling

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8
Q

Colours of:
Chlorine
Bromine
Iodine

A

Chlorine - Green
Bromine -Red-brown
Iodine -Dark grey

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9
Q

Physical state at room temperature of:
Chlorine
Bromine
Iodine

A

Chlorine - Gas
Bromine - Liquid
Iodine - Solid

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10
Q

What is dissociation

A

When hydrogen splits up in water into H+ ions and cl- ions

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11
Q

Hydrogen chloride doesn’t dissociate in _____________

A

Methylbenzene

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12
Q

When hydrogen chloride dissociates in water, the H+ ions mean that the water is _________

A

Acidic

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13
Q

Chlorine water is colourless. What colour is bromine water

A

Orange

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14
Q

What colour is iodine water

A

Brown

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15
Q

Group 7 metals get _______ reactive as you go up the group

A

More

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16
Q

How to do a displacement reaction

A

Add potassium halide solution to halide water

See if the halide from the water displaces the halide from the potassium

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17
Q

Halogen displacement reactions are _______ reactions

A

Redox

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18
Q

What is a redox reaction

A

A reaction where oxidation and reduction occur

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19
Q

Acid + Metal –>

A

Acid + Metal –> Salt + Hydrogen

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20
Q

You can use the reactions of different metals with dilute acids to work out how _________ they are. The more reactive the metal, the faster the reaction, the _______ reactive the metal

A

Reactive

More

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21
Q

Acid + Metal –> Salt + Hydrogen
The speed of the reaction indicated by the rate at which the bubbles of __________ are given off. The ___________ is confirmed by the burning splint test

A

Hydrogen

Hydrogen

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22
Q

Magnesium gives a _____ squeaky pop whereas iron gives a ________ squeaky pop

A

Big

Small

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23
Q

Metal + Water –>

A

Metal + Water –> Metal Hydroxide + Hydrogen

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24
Q

Metal + Water –> Metal Hydroxide + Hydrogen

_______ reactive metals react vigorously with water

A

More/very

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25
Q

Metal + Water –> Metal Hydroxide + Hydrogen

_______ reactive metals won’t react vigorously with water but they will react with _______

A

Less

Steam

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26
Q

What is a reducing agent

A

A substance that brings about reduction by being oxidized and losing electrons.

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27
Q

What is an oxidising agent

A

A substance that brings about oxidation by being reduced and gaining electrons.

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28
Q

Rust equation:

A

Iron + Oxygen + Water –> Hydrated iron(|||) oxide (rust)

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29
Q

What are the two main ways to prevent rusting

A

Barrier method

Sacrificial method

30
Q

What is the barrier method

A

Painting/coating/oiling/greasing

31
Q

When should you paint and when should you use oil

A

Paint is good for immobile objects

Oil is good for objects with moving parts

32
Q

What is the sacrificial method

A

Putting a more reactive metal on top of the iron so that that metal reacts with the oxygen and water

33
Q

What is galvanising

A

When an object is coated with an element more reactive than iron

34
Q

Test for chlorine

A

Bleaches damp red litmus paper white

35
Q

Test for oxygen

A

Relights a glowing splint

36
Q

Test for co2

A

Turns limewater cloudy

37
Q

Test for hydrogen

A

Makes a squeaky pop with a lightedsplint

38
Q

Test for ammonia

A

Turns damp red litmus paper blue

39
Q

Wet copper sulfate is _______

Dry copper sulfate is ________

A

Blue

White

40
Q

How to make oxygen in the lab

A

By the decomposition of hydrogen peroxide

41
Q

What catalyst is used in the decomposition of hydrogen peroxide

A

Manganese oxide

42
Q

Magnesium oxide is slightly __________ when it’s dissolved in water

A

Alkaline

43
Q

Carbon dioxide is slightly __________ when it’s dissolved in water

A

Acidic

44
Q

Sulfur dioxide is slightly __________ when it’s dissolved in water

A

Acidic

45
Q

Flame tests: Lithium

A

Red flame

46
Q

Flame tests: Sodium

A

Yellow flame

47
Q

Flame tests: Potassium

A

Lilac flame

48
Q

Flame tests: Calcium

A

Brick-red

49
Q

Metal + NaOH: Copper

A

Blue

50
Q

Metal + NaOH: Iron (||)

A

Sludgy green

51
Q

Metal + NaOH: Iron (|||)

A

Reddish brown

52
Q

Ammonia + NaOH –>

A

Ammonia

53
Q

What should you use to test for carbonates

A

Hydrochloric acid

54
Q

What is formed if carbonates are present

A

CO2

55
Q

Carbonate + Acid –>

A

Carbonate + Acid –> Carbon dioxide + Water

56
Q

Test for sulfates:

A

Dilute HCl, followed by barium chloride solution

57
Q

What is formed if sulfates are present

A

White precipitate

58
Q

Test for halides:

A

Nitric acid followed by silver nitrate

59
Q

Test for halides: Nitric acid followed by silver nitrate solution:
Chloride

A

White precipitate of silver chloride

60
Q

Test for halides: Nitric acid followed by silver nitrate solution:
Bromide

A

Cream precipitate of silver bromide

61
Q

Test for halides: Nitric acid followed by silver nitrate solution:
Iodide

A

Yellow precipitate of silver iodide

62
Q

Test for metal ions

A

Flame tests

NaOH

63
Q

Test for carbonates

A

Hydrochloric acid

64
Q

Test for sulfates

A

HCl and Barium Chloride

65
Q

Test for halides

A

Nitric acid and silver nitrate

66
Q

Result for metal ions

A

Copper - Blue
Iron (||) - Sludgy green
Iron (|||) Reddish brown

67
Q

Result for carbonates

A

Carbon dioxide

68
Q

Result for sulfates

A

White precipitate

69
Q

Result for halides

A

Chloride - White
Bromide - Cream
Iodide - Yellow

70
Q

Uses of Carbon dioxide:

A

Fizzy drinks

Fire extinguishers

Chemistry Revision (9 decks)

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