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Chemistry GCSE OCR Gateway B > C4 - The Periodic Table > Flashcards

C4 - The Periodic Table Flashcards

1
Q

C4 - The Periodic Table

What is a neutron?

A

Has 0 charge and a relative atomic mass of 1

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2
Q

C4 - The Periodic Table

What is an electron?

A

Has a charge of -1 and a relative atomic mass of 0.0005

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3
Q

C4 - The Periodic Table

What is a proton?

A

Has a charge of +1 and a relative atomic mass of 1

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4
Q

C4 - The Periodic Table

What is the atomic number?

A

(BOTTOM NUMBER) The number of protons (or number of electrons)

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5
Q

C4 - The Periodic Table

What is the mass number?

A

(TOP NUMBER) Number of neutrons plus number of protons

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6
Q

C4 - The Periodic Table

What is the order of reactivity for Group 1?

A

As they go down the group, the reactivity increases (get more reactive)

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7
Q

C4 - The Periodic Table

What is the order of reactivity for Group 7?

A

As they go down the group, the halogens become less reactive

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8
Q

C4 - The Periodic Table

What produces a white precipitate?

A

Chloride ions

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9
Q

C4 - The Periodic Table

What produces a cream precipitate?

A

Bromide ions

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10
Q

C4 - The Periodic Table

What produces a pale yellow precipitate?

A

Iodide ions

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11
Q

C4 - The Periodic Table

What are the processes in water purification?

A

Filtration, Sedimentation, Chlorination

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12
Q

C4 - The Periodic Table

What is filtration?

A

A layer of sand or gravel filters remaining small particles and sometimes removes microbes

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13
Q

C4 - The Periodic Table

What is sedimentation?

A

Chemicals are added to make solid particles and bacteria settle

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14
Q

C4 - The Periodic Table

What is chlorination?

A

Chlorine is added to kill remaining microbes

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15
Q

C4 - The Periodic Table

What pollutants are found in water?

A

Nitrates - from fertilisers via eutrophication Lead compounds - from water pipes to houses Pesticides - from spraying crops

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16
Q

C4 - The Periodic Table

What is a superconductor?

A

Materials which can conduct electricity with little or no resistance

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17
Q

C4 - The Periodic Table

What are the two types of superconductor?

A

Type I - metals Type 2 - alloys

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18
Q

C4 - The Periodic Table

What are the benefits of superconductors?

A

Loss free power transmission, superfast electronic circuits and powerful electromagnets

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19
Q

C4 - The Periodic Table

What are the difficulties with superconductors?

A

They only work at very low temperatures, limiting their use and superconductors that work at room temperature need to be developed.

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20
Q

C4 - The Periodic Table

What is the Period number?

A

(ROWS - ACROSS) Number of electron shells

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21
Q

C4 - The Periodic Table

What is the Group number?

A

(COLUMN - DOWN) Number of electrons in outer shell

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22
Q

C4 - The Periodic Table

What is an isotope?

A

An atom of the same element but with different mass numbers (different number of neutrons)

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23
Q

C4 - The Periodic Table

Give one example of an isotope…

A

Carbon-12 and Carbon-14

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24
Q

C4 - The Periodic Table

What did John Dalton do?

A

(1803) Said atoms where solid spheres and there was a different sphere for each element

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25
Q

C4 - The Periodic Table

What did J.J Thomson discover?

A

(1897) That atoms weren’t solid spheres and there were negatively charged particles - electrons. Theory was called the “Plum Pudding Model”.

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26
Q

C4 - The Periodic Table

How did Rutherford describe the atom?

A

(1911) Theory of the Nuclear Atom - Gold Foil experiment found that the positive nucleus was surrounded by negative electrons after positive particles passed through the gold, rather than be deflected.

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27
Q

C4 - The Periodic Table

What did Niels Bohr describe?

A

(1913) Electrons had fixed orbits and fixed energy which prevented the electrons being attracted to the positive nucleus. They orbited in shells.

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28
Q

C4 - The Periodic Table

What are the properties of ionic compounds?

A

Typically dissolve in water, conduct electricity when in a solution/molten, have very high melting points and their structures are described as giant ionic lattices.

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29
Q

C4 - The Periodic Table

What is a covalent bond?

A

A shared pair of electrons

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30
Q

C4 - The Periodic Table

lithium + water

A

lithium hydroxide + hydrogen (2Li + 2H₂O → 2LiOH + H₂)

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31
Q

C4 - The Periodic Table

sodium + water

A

sodium hydroxide + hydrogen (2Na + 2H₂O → 2NaOH + H₂)

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32
Q

C4 - The Periodic Table

potassium + water

A

potassium hydroxide + hydrogen (2K + 2H₂O → 2KOH + H₂)

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33
Q

C4 - The Periodic Table

Why is potassium more reactive than lithium?

A

Because potassium is able to lose its outer electron easier than lithium because the larger radius means that the force of attraction from the nucleus is weaker.

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34
Q

C4 - The Periodic Table

What colour flame does lithium produce?

A

Red or crimson

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35
Q

C4 - The Periodic Table

What colour flame does sodium produce?

A

Orange

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36
Q

C4 - The Periodic Table

What colour flame does potassium produce?

A

Purple or lilac

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37
Q

C4 - The Periodic Table

What is the method for the flame test?

A

Wash the nichrome wire to clean and make compound stick. Dip into metal compound and hold in Bunsen Burner to produce coloured flame. Repeat with different metal compound.

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38
Q

C4 - The Periodic Table

What are halogens?

A

Salt formers’ - they (Group 7s) react with Group 1 to make salts

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39
Q

C4 - The Periodic Table

Potassium + chlorine

A

potassium chloride (2K + Cl₂ → 2KCl)

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40
Q

C4 - The Periodic Table

Sodium + chlorine

A

sodium chloride (2Na + Cl₂ → 2NaCl)

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41
Q

C4 - The Periodic Table

Potassium + bromine

A

potassium bromide (2K + Br₂ → 2KBr )

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42
Q

C4 - The Periodic Table

Complete and what is this an example of: Cl₂ + 2NaBr

A

2NaCl + Br₂ an example of a displacement reaction

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43
Q

C4 - The Periodic Table

What elements are bonded by covalent bonds?

A

Non metals. E.g. Hydrogen (H₂) or Carbon Dioxide (CO₂)

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44
Q

C4 - The Periodic Table

Which elements are bonded ionically?

A

A metal and a non metal. E.g. Magnesium and oxygen forms magnesium oxide.

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45
Q

C4 - The Periodic Table

What are the properties of Group 1 Metals?

A

Low melting point and boiling point. Low density (lithium, sodium and potassium float on water). Very soft - can be cut with a knife.

46
Q

C4 - The Periodic Table

Describe chlorine at room temperature…

A

Fairly reactuve, poisonous green gas (low boiling point)

47
Q

C4 - The Periodic Table

Describe bromine at room temperature…

A

A dense, poisonous orange liquid

48
Q

C4 - The Periodic Table

Describe iodine at room temperature…

A

A dark grey crystalline solid (high boiling point)

49
Q

C4 - The Periodic Table

Why are metals strong and able to bend into different shapes?

A

High tensile strength makes them hard to break. Can be hammered to different shapes because they are malleable.

50
Q

C4 - The Periodic Table

How are metals bonded?

A

With strong metallic bonds. Strong bond between delocalised electrons and positive ions. Outer electrons of each atom can move freely - delocalised and makes them good conductors of heat and electricity.

51
Q

C4 - The Periodic Table

What can transition metals be used for?

A

Catalysts - e.g. Iorn is used in Haber Process and nickel is used in hydrogenation of alkenes (making margarine).

52
Q

C4 - The Periodic Table

What colour are iron and copper compounds?

A

USUALLY: Iron (II) = light green Iron (III) = orange/brown Copper = blue

53
Q

C4 - The Periodic Table

What do transition metal carbonates usually thermally decompose into?

A

A metal oxide and carbon dioxide - usually results in a colour change

54
Q

C4 - The Periodic Table

What is a precipitate?

A

Where two solutions react and as solid forms in the solution

55
Q

C4 - The Periodic Table

What solution is used to test for sulphate ions?

A

Barium chloride - if a white precipitate forms then sulphate ions are present

56
Q

C4 - The Periodic Table

What solution is used to test halide ions?

A

Silver nitrate solution - a coloured precipitate will form if chloride, bromide, or iodide ions are present.

57
Q

C4 - The Periodic Table

Has 0 charge and a relative atomic mass of 1

A

What is a neutron?

58
Q

C4 - The Periodic Table

Has a charge of -1 and a relative atomic mass of 0.0005

A

What is an electron?

59
Q

C4 - The Periodic Table

Has a charge of +1 and a relative atomic mass of 1

A

What is a proton?

60
Q

C4 - The Periodic Table

(BOTTOM NUMBER) The number of protons (or number of electrons)

A

What is the atomic number?

61
Q

C4 - The Periodic Table

(TOP NUMBER) Number of neutrons plus number of protons

A

What is the mass number?

62
Q

C4 - The Periodic Table

As they go down the group, the reactivity increases (get more reactive)

A

What is the order of reactivity for Group 1?

63
Q

C4 - The Periodic Table

As they go down the group, the halogens become less reactive

A

What is the order of reactivity for Group 7?

64
Q

C4 - The Periodic Table

Chloride ions

A

What produces a white precipitate?

65
Q

C4 - The Periodic Table

Bromide ions

A

What produces a cream precipitate?

66
Q

C4 - The Periodic Table

Iodide ions

A

What produces a pale yellow precipitate?

67
Q

C4 - The Periodic Table

Filtration, Sedimentation, Chlorination

A

What are the processes in water purification?

68
Q

C4 - The Periodic Table

A layer of sand or gravel filters remaining small particles and sometimes removes microbes

A

What is filtration?

69
Q

C4 - The Periodic Table

Chemicals are added to make solid particles and bacteria settle

A

What is sedimentation?

70
Q

C4 - The Periodic Table

Chlorine is added to kill remaining microbes

A

What is chlorination?

71
Q

C4 - The Periodic Table

Nitrates - from fertilisers via eutrophication Lead compounds - from water pipes to houses Pesticides - from spraying crops

A

What pollutants are found in water?

72
Q

C4 - The Periodic Table

Materials which can conduct electricity with little or no resistance

A

What is a superconductor?

73
Q

C4 - The Periodic Table

Type I - metals Type 2 - alloys

A

What are the two types of superconductor?

74
Q

C4 - The Periodic Table

Loss free power transmission, superfast electronic circuits and powerful electromagnets

A

What are the benefits of superconductors?

75
Q

C4 - The Periodic Table

They only work at very low temperatures, limiting their use and superconductors that work at room temperature need to be developed.

A

What are the difficulties with superconductors?

76
Q

C4 - The Periodic Table

(ROWS - ACROSS) Number of electron shells

A

What is the Period number?

77
Q

C4 - The Periodic Table

(COLUMN - DOWN) Number of electrons in outer shell

A

What is the Group number?

78
Q

C4 - The Periodic Table

An atom of the same element but with different mass numbers (different number of neutrons)

A

What is an isotope?

79
Q

C4 - The Periodic Table

Carbon-12 and Carbon-14

A

Give one example of an isotope…

80
Q

C4 - The Periodic Table

(1803) Said atoms where solid spheres and there was a different sphere for each element

A

What did John Dalton do?

81
Q

C4 - The Periodic Table

(1897) That atoms weren’t solid spheres and there were negatively charged particles - electrons. Theory was called the “Plum Pudding Model”.

A

What did J.J Thomson discover?

82
Q

C4 - The Periodic Table

(1911) Theory of the Nuclear Atom - Gold Foil experiment found that the positive nucleus was surrounded by negative electrons after positive particles passed through the gold, rather than be deflected.

A

How did Rutherford describe the atom?

83
Q

C4 - The Periodic Table

(1913) Electrons had fixed orbits and fixed energy which prevented the electrons being attracted to the positive nucleus. They orbited in shells.

A

What did Niels Bohr describe?

84
Q

C4 - The Periodic Table

Typically dissolve in water, conduct electricity when in a solution/molten, have very high melting points and their structures are described as giant ionic lattices.

A

What are the properties of ionic compounds?

85
Q

C4 - The Periodic Table

A shared pair of electrons

A

What is a covalent bond?

86
Q

C4 - The Periodic Table

lithium hydroxide + hydrogen (2Li + 2H₂O → 2LiOH + H₂)

A

lithium + water

87
Q

C4 - The Periodic Table

sodium hydroxide + hydrogen (2Na + 2H₂O → 2NaOH + H₂)

A

sodium + water

88
Q

C4 - The Periodic Table

potassium hydroxide + hydrogen (2K + 2H₂O → 2KOH + H₂)

A

potassium + water

89
Q

C4 - The Periodic Table

Because potassium is able to lose its outer electron easier than lithium because the larger radius means that the force of attraction from the nucleus is weaker.

A

Why is potassium more reactive than lithium?

90
Q

C4 - The Periodic Table

Red or crimson

A

What colour flame does lithium produce?

91
Q

C4 - The Periodic Table

Orange

A

What colour flame does sodium produce?

92
Q

C4 - The Periodic Table

Purple or lilac

A

What colour flame does potassium produce?

93
Q

C4 - The Periodic Table

Wash the nichrome wire to clean and make compound stick. Dip into metal compound and hold in Bunsen Burner to produce coloured flame. Repeat with different metal compound.

A

What is the method for the flame test?

94
Q

C4 - The Periodic Table

Salt formers’ - they (Group 7s) react with Group 1 to make salts

A

What are halogens?

95
Q

C4 - The Periodic Table

potassium chloride (2K + Cl₂ → 2KCl)

A

Potassium + chlorine

96
Q

C4 - The Periodic Table

sodium chloride (2Na + Cl₂ → 2NaCl)

A

Sodium + chlorine

97
Q

C4 - The Periodic Table

potassium bromide (2K + Br₂ → 2KBr )

A

Potassium + bromine

98
Q

C4 - The Periodic Table

2NaCl + Br₂ an example of a displacement reaction

A

Complete and what is this an example of: Cl₂ + 2NaBr

99
Q

C4 - The Periodic Table

Non metals. E.g. Hydrogen (H₂) or Carbon Dioxide (CO₂)

A

What elements are bonded by covalent bonds?

100
Q

C4 - The Periodic Table

A metal and a non metal. E.g. Magnesium and oxygen forms magnesium oxide.

A

Which elements are bonded ionically?

101
Q

C4 - The Periodic Table

Low melting point and boiling point. Low density (lithium, sodium and potassium float on water). Very soft - can be cut with a knife.

A

What are the properties of Group 1 Metals?

102
Q

C4 - The Periodic Table

Fairly reactuve, poisonous green gas (low boiling point)

A

Describe chlorine at room temperature…

103
Q

C4 - The Periodic Table

A dense, poisonous orange liquid

A

Describe bromine at room temperature…

104
Q

C4 - The Periodic Table

A dark grey crystalline solid (high boiling point)

A

Describe iodine at room temperature…

105
Q

C4 - The Periodic Table

High tensile strength makes them hard to break. Can be hammered to different shapes because they are malleable.

A

Why are metals strong and able to bend into different shapes?

106
Q

C4 - The Periodic Table

With strong metallic bonds. Strong bond between delocalised electrons and positive ions. Outer electrons of each atom can move freely - delocalised and makes them good conductors of heat and electricity.

A

How are metals bonded?

107
Q

C4 - The Periodic Table

Catalysts - e.g. Iorn is used in Haber Process and nickel is used in hydrogenation of alkenes (making margarine).

A

What can transition metals be used for?

108
Q

C4 - The Periodic Table

USUALLY: Iron (II) = light green Iron (III) = orange/brown Copper = blue

A

What colour are iron and copper compounds?

109
Q

C4 - The Periodic Table

A metal oxide and carbon dioxide - usually results in a colour change

A

What do transition metal carbonates usually thermally decompose into?

110
Q

C4 - The Periodic Table

Where two solutions react and as solid forms in the solution

A

What is a precipitate?

111
Q

C4 - The Periodic Table

Barium chloride - if a white precipitate forms then sulphate ions are present

A

What solution is used to test for sulphate ions?

112
Q

C4 - The Periodic Table

Silver nitrate solution - a coloured precipitate will form if chloride, bromide, or iodide ions are present.

A

What solution is used to test halide ions?

Chemistry GCSE OCR Gateway B (6 decks)

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