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Edexcel GCSE Chemistry Higher > Topic 6 - Groups of the Periodic Table > Flashcards

Topic 6 - Groups of the Periodic Table Flashcards

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1
Q

Name for the group 1 elements

A

Alkali metals

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2
Q

Name for the group 7 elements

A

Halogens

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3
Q

Ion, definiton

A

An atom, or group of atoms, that have gained or lost an electron

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4
Q

Molecule, definition

A

A group of atoms that are chemically joined

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5
Q

Name for the group 0 elements

A

Noble gases

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6
Q

A column on the periodic table

A

group

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7
Q

A row on the periodic table

A

period

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8
Q

The group number provides this information about an atom…

A

The number of electrons in the outer shell

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9
Q

The period number provides this information about an atom…

A

The number of electron shells

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10
Q

The electronic configuration of a sodium atom

A

2,8,1

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11
Q

The electronic configuration of a sodium ion

A

2,8

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12
Q

The electronic configuration of a lithium atom

A

2,1

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13
Q

The electronic configuration of a lithium ion

A

2

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14
Q

The electronic configuration of a chlorine atom

A

2,8,7

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15
Q

The electronic configuration of a chloride ion

A

2,8,8

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16
Q

Reasons for including hydrogen in group 1 of the periodic table

A
  1. It has one electron in its outer shell
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17
Q

Reasons for NOT including hydrogen in group 1 of the periodic table

A
  1. It is a non-metal
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18
Q

Group 1 elements form ions with a charge of..

A

1

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19
Q

Group 7 elements form ions with a charge of..

A

-1

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20
Q

Properties of the group 1 metals

A
  1. Soft - they can be cut with a scalpel
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21
Q

Colour of fluorine

A

yellow

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22
Q

Colour of chlorine

A

yellow-green

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23
Q

Colour of bromine

A

red-brown

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24
Q

Colour of iodine, in the solvent hexane

A

purple

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25
Q

Colour of iodine, in the solvent water

A

brown

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26
Q

Reason why the group 1 metals are stored under mineral oil

A

They would react with the water in the atmosphere

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27
Q

Reason why lithium turns black when exposed to air

A

It reacts with nitrogen in the air to make a layer of lithium nitride on the surface of the metal

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28
Q

Lithium reacts with water to make…

A

Lithium hydroxide and hydrogen gas

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29
Q

Sodium reacts with water to make…

A

Sodium hydroxide and hydrogen gas

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30
Q

Potassium reacts with water to make…

A

Potassium hydroxide and hydrogen gas

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31
Q

pH of potassium hydroxide solution

A

12 to 14

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32
Q

Colour of potassium hydroxide solution with universal indicator

A

Dark blue to purple

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33
Q

State symbol of hydrogen

A

(g)

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34
Q

State symbol of sodium

A

(s)

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35
Q

State symbol of water

A

(l)

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36
Q

State symbol of potassium hydroxide

A

(aq)

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37
Q

Atomic radius

A

Size of an atom, from the centre to the outermost electron

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38
Q

Ionic radius

A

Size of an ion, from the centre to the outermost electron

39
Q

Aqueous

A

Soluble in water, has the state symbol (aq)

40
Q

Describe the trend in reactivity of the group 1 elements

A

Reactivity increases as you descend the group

41
Q

Describe the trend in reactivity of the group 7 elements

A

Reactivity decreases as you descend the group

42
Q

Describe the trend in the melting points of the group 1 elements

A

Meting points decrease as you descend the group.

-

43
Q

Describe the trend in the melting points of the group 7 elements

A

Meting points increase as you descend the group

44
Q

State of fluorine at room temperature

A

gas

45
Q

State of chlorine at room temperature

A

gas

46
Q

State of bromine at room temperature

A

liquid

47
Q

State of iodine at room temperature

A

solid

48
Q

Explanation for the trend in melting points for the group 7 elements

A
  1. As you descend the group, the size of the diatomic molecules increases because the size of the atoms increases
49
Q

Displacement reaction

A

Reaction in which one element replaces a similar element in a compound

50
Q

Redox reaction

A

A reaction in which both reduction and oxidation take place.

51
Q

Oxidation, in terms of electrons

A

Loss of electrons

52
Q

Reduction, in terms of electrons

A

Gain of electrons

53
Q

Ionic equation

A

An equation that shows only those ions or atoms that change in a chemical reaction. It ignores the spectator ions that do not take part.

54
Q

Symbol equation

A

An equation that includes the spectator ions that do not take part in the reaction

55
Q

In general, metal atoms are oxidised / reduced

A

Oxidised

56
Q

In general, non-metal atoms are oxidised / reduced

A

Reduced

57
Q

Halide ion

A

A negative ion formed when a halogen atom gains an electron

58
Q

An element that is more reactive than iodine but less reactive than chlorine

A

Bromine

59
Q

An element that is more reactive than bromine but less reactive than fluorine

A

Chlorine

60
Q

An element that is more reactive than lithium but less reactive than potassium

A

Sodium

61
Q

An element that is more reactive than sodium but less reactive than rubidium

A

Potassium

62
Q

Chloride ions have a yellow-green colour

A

False. They are colourless.

63
Q

In this reaction what is reduced? Explain your answer.

The equation: F2 + 2Br- > 2F- + Br2

A
  • The fluorine atoms in the fluorine molecule are reduced because they gain electrons
64
Q

In this reaction what is oxidised? Explain your answer.

The equation:
F2 + 2I- > 2F- + I2

A

The iodide ion is reduced because it loses electrons

65
Q

Suggest 3 spectator ions that may have been excluded from this equation. Explain why they are not included.

The equation: Cl2 + 2Br > 2Cl + Br2

A
  • Ions of lithium, sodium or potassium.
  • They are not included because they do not take part in the reaction.
  • They are neither oxidised nor reduced. They remain unchanged at the end of the reaction.
66
Q

A colour change from yellow-green to brown

A

Suggest what would be observed in this reaction. Assume that the solvent is water.

67
Q

Explanation for the trend in reactivity of the group 1 elements

A
  1. As you descend the group the atomic radius increases
68
Q

Explanation for the trend in reactivity of the group 7 elements

A

1) - As you go up the group the atomic radius decreases (less electron shells).

2) - Therefore, the positively charged nucleus is closer to the outer electron of a neighbouring atom.

3) - Therefore, an electron is gained more easily.

4) - And the atom is more easily reduced.

69
Q

The colour of a potassium flame

A

Lilac

70
Q

State one similarity in the reactions between lithium, sodium and potassium with water

A

They are all exothermic and all involve fizzing

71
Q

State one similarity in the reactions between lithium and potassium with water. Explain your answer.

A
  • Potassium produces a lilac flame whereas lithium produces no flame.
  • This is because the reaction between potassium and water is more exothermic and sufficient heat energy is produced to ignite the hydrogen gas.
72
Q

Colour of potassium bromide solution

A

Colourless

73
Q

What is observed when chlorine is bubbled through potassium bromide solution

A

The solution changes colour from colourless to orange

74
Q

What is observed when chlorine is bubbled through potassium iodide solution

A

The solution changes colour from colourless to brown

75
Q

Formula of lithium hydroxide

A

LiOH

76
Q

Formula of sodium hydroxide

A

NaOH

77
Q

Formula of potassium hydroxide

A

KOH

78
Q

Formula of rubidium hydroxide

A

RbOH

79
Q

Group 1 hydroxides are acidic / alkaline / neutral

A

alkaline

80
Q

What can you observe when lithium reacts with water?

A

Fierce bubbling on surface of water

81
Q

What can you observe when sodium reacts with water?

A

Melts into a ball and fizzes on the surface

82
Q

What can you observe when potassium reacts with water

A

Bursts into flames and flies around surface

83
Q

Properties of group 7 elements (3)

A
  • do not conduct electricity
  • Brittle and crumbly solids
  • Poisonous with a strong odour
84
Q

Halogens react with metals to form…

A

metal halides (salts)

85
Q

Halogens react with hydrogen to form…

A

Hydrogen halides

86
Q

Test for chlorine gas

A

Turns damp litmus paper red and then bleaches white

87
Q

What happens in a displacement reaction?

A

A more reactive metal will displace a less reactive metal from a solution of its salt

88
Q

Properties of noble gases (7)

A
  • colourless
  • very low melting and boiling points
  • Poor conductors of heat and electricity
  • Inert
  • Monatomic
  • Low densities
  • Not flammable
89
Q

Give a use of helium and why

A

Zeppelins because of its low density and it isn’t flammable

90
Q

Give a use of neon and why

A

Used in signs because it glows red-orange when electricity is passed through it

91
Q

Give a use of argon and why

A

Used in filament lamps because it is inert and not flammable

92
Q

Why does melting point increase down group 7?

A

More shells, more electrons, more IMFs, more energy needed to allow a change of state to occur

93
Q

How can you improve the sodium thiosulfate practical?

A

Use a light spectrometer rather than judging when cross disappears

Edexcel GCSE Chemistry Higher (12 decks)

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