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AQA GCSE Chemistry > Metals and Redox > Flashcards

Metals and Redox Flashcards

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1
Q

What makes a metal more or most reactive?

A

If it can easily give away it’s outer shell elctrons

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2
Q

What method of extraction is used for all metals more reactive than zinc?

A

Electrolysis

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3
Q

How is zinc and iron extracted?

A

By reducing them with carbon (carbon is more reactive)

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4
Q

How is copper extracted?

A

By being reduced with either of the more reactive non-metals hydrogen and carbon

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5
Q

What is the term used to define metals which are found naturally in the ground as they are unreactive?

A

Native

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6
Q

What are the two native metals in the reactivity series?

A

Silver and gold

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7
Q

How are metals which aren’t native found as?

A

Compounds which are called ores

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8
Q

What is an ore?

A

A metal compound dug out of the ground which is economically worth extracting

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9
Q

What is the colour and name of copper carbonate ore?

A

Green compound called Malachite

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10
Q

What is the first stage of extracting copper from copper carbonate?

A

Thermal decomposition

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11
Q

What are the products and reactants of thermal decomposition of copper carbonate?

A

Reactants: Copper carbonate (CuCO3)
Products: Copper oxide (CuO) and carbon dioxide(CO2)

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12
Q

What is the second stage of extracting copper from copper carbonate?

A

Reacting the copper oxide with carbon to get copper and carbon dioxide

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13
Q

What is reduction?

A

The loss of oxygen from one reactant or the gain of electrons

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14
Q

What is oxidation?

A

The gain of oxygen or the loss of electrons

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15
Q

What is the name of the ore and chemical symbol of Aluminium Oxide?

A
  • Bauxite

- Al2O3

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16
Q

How is aluminium extracted from bauxite?

A

Using electrolysis

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17
Q

How is aluminium oxide made into an electrolyte for electrolysis?

A

It is melted until it is molten and is dissolved in cryolyte to lower it’s melting point in the first place

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18
Q

During the electrolysis of aluminium oxide, what product is made at the cathode?

A

Pure aluminum

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19
Q

During the electrolysis of aluminium oxide, what product is made at the anode? Why?

A

Carbon dioxide because oxygen reacts with the carbon anode to make carbon dioxide

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20
Q

What kind of structure does a metal have?

A

A giant metallic structure

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21
Q

What kind of bonding does a metal have?

A

Metallic bonding

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22
Q

Define metallic bonding:

A

The electrostatic attraction between positive ions and delocalised electrons in a layered structure

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23
Q

What are the general physical properties of metals?

A
  • High metling point
  • Ductile (can be drawn into wires)
  • Malleable (can be shaped)
  • Good conductor of electricity
  • Good conductor of heat
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24
Q

Why do metals (transition) generally have a high melting point?

A

Because there are strong metallic bonds which take a lot of energy to break

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25
Q

Why are metals generally ductile?

A

The layers of positive ions can slide past eachother when a force is applied

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26
Q

Why are metals generally malleable?

A

The layers of positive ions can slide past eachother when a force is applied

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27
Q

Why are metals generally good conductors of heat?

A

The delocalised electrons in the metal can transfer the heat effectively

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28
Q

Why are metals generally good conductors of electricity?

A

The delocalised electrons can carry the electric charge through the metal

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29
Q

What are the similar physical properties of alkali metals and transition metals?

A
  • Good conductors of heat and electricity
  • Malleable and Ductile
  • Shiny
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30
Q

What are the different physical properties of alkali metals and transition metals?

A
  • Alkali metals have lower density (float on water)
  • Alkali metals are softer (cut easily)
  • Alkali metals aren’t as strong as transition metals
  • Alkalis have lower melting and boiling points
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31
Q

What are the products when a metal and oxygen react?

A

A metal oxide

32
Q

What are the products when a metal and acid react?

A

A metal salt and hydrogen

33
Q

What are the products when a metal and water react?

A

A metal hydroxide and hydrogen

34
Q

What kind of compounds do alkali metals form?

A

White compounds

35
Q

What is the only oxidation number for any alkali metal?

A

+1

36
Q

Can alkali metals be used as catalysts?

A

No

37
Q

How do alkalis react in water typically?

A

Violently

38
Q

What kind of compounds do transition metals form?

A

Coloured compounds

39
Q

How do transition metals react with water?

A

Fairly unreactive ie. Copper does not react with water

40
Q

Can transition metals be used as catalysts>

A

Yes ie. Fe used to make ammonia and Nickel used to harden margarine

41
Q

How do potassium, sodium, lithium and calcium react with O2?

A

Very quickly (they tarnish) so they must be stored in oil

42
Q

How do potassium, sodium, lithium and calcium react with water?

A

All produce gas, potassium produces lilac flame, float and move on surface and eventually dissolve

43
Q

How do potassium, sodium, lithium and calcium react with acid?

A

explosive

44
Q

How does magnesium react with oxygen?

A

Very slowly if at all (tinges of tarnishing)

45
Q

How does magnesium react with water?

A

Very slowly

46
Q

How does magnesium react with acid?

A

Quickly and fairly violent. Lots of gas is produced

47
Q

How do iron and zinc and copper react with oxygen?

A

Very very slow (no visible observations really)

48
Q

How do iron and zinc and copper react with water?

A

Iron slowly rusts but the other two have no reaction

49
Q

How do iron and zinc and copper react with acid?

A

Slowly , bubbles form on the surface

50
Q

What gas is given off during the metal s reacting with water and acid?

A

Hydrogen

51
Q

What is the test for hydrogen?

A

Squeaky pop with a lighted splint

52
Q

What is a displacement reaction?

A

When a more reactive metal displaces a less reactive metal from its compound

53
Q

What are the ions in a redox reaction called if they don’t take part in the reaction?

A

Spectator ions

54
Q

What is an alloy?

A

A mixture of a metal and either a non-metal or an additional metal

55
Q

What makes a metal an element?

A

When there is only one type of ato making it up

56
Q

Why are alloys stronger than pure metals?

A

The atoms in them are different sizes so layers cannot easily slide past eachother

57
Q

What is low carbon steel composed of and used for due to its property?

A

Iron with 0.1%-0.3% of carbon

It is easily shaped so is ideal for car bodies

58
Q

What is high carbon steel composed of and used for due to its properties?

A

Iron with 0.22%-0.25% of carbon

Very strong, inflexible, brittle so used for blades for cutting tools and even bridges

59
Q

What is low stainless steel composed of and used for due to its properties?

A

Iron with added chromium and nickel

Corrosion resistant and hard so used for medical equipment, cutlery and corrosive substance containers

60
Q

What is brass composed of and used for due to its property?

A

70% Copper and 30% Zinc

Low friction so used for moving parts such as taps, door fittings and musical instruments

61
Q

What is bronze composed of and used for due to its property?

A

95% Copper and 5% Tin

Harder than copper so used for statues. church bells and medals

62
Q

What is gold composed of and used for due to its property?

A

Gold with copper, zinc or silver
24 carat is soft so used in jewellery
9 carat is used in dental fillings and electronic devices due to low resistance and high conductivity

63
Q

What is aluminium composed of and used for due to its property?

A

Aluminium with other metals such as magnesium

Low density and soft and conductive so alloyed to make stronger for aircrafts and electric pylon wores

64
Q

Why does aluminum not corrode?

A

It has a layer of aluminum oxide on it’s surface

65
Q

What is corrosion?

A

The destruction of materials by chemical reactions with substances in the environment

66
Q

Rust is a form of corrosion which only occurs with iron, what is its chemical name and symbol?

A

A hydrated iron oxide - Fe2O3.H2O

67
Q

Why does all pure iron with water eventually corrode away?

A

The rust gets on the surface of the iron but is soft and crumbly so flakes off leaving more of the surface of the iron to rust.

68
Q

What are the conditions which are required for iron to rust?

A

Water and air

69
Q

What are in the three test tubes used to set up the different conditions for iron to see under which ones it rusts?

A
  • Test tube with iron and anhydrous calcium oxide which absorbs moisture
  • Test tube with boiled water (removes oxygen) and oil (prevents re-entry of oxygen) with iron
  • Test tube with half air and water for nail
70
Q

How coukd you tell rust is present on the iron in the test tube with water and air?

A

Because the mass of the nail increases as the iron atoms chemically bond to the oxygen and water molecules creating a new compound

71
Q

What are the methods to prevent corrosion?

A
  • Coating to create a barrier (e.g. greasing, painting)
  • Cover in plastic
  • Electroplating
  • Sacrificial protection
  • Galvanising
72
Q

How does sacrificial protection prevent the desired metal from corroding?

A

The more reactive metal attached to the desired metal corrodes in its place

73
Q

How does galvanising prevent the desired metal from corroding?

A

The desired metal’s surface is covered so there is a barrier but it is covered with a meterial which if scratched, will corrode in place of the desired metal as sacrifical protection (used in “tin cans”)

74
Q

Why do electrons become delocalised in metals?

A

Because the electron orbitals in metal atoms overlap.

75
Q

What is a pure compound?

A

A coumpound made of one substance without any mixtures

AQA GCSE Chemistry (10 decks)

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