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Metals Flashcards

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1
Q

What are the two components in the structure of a metal?

A

A lattice of positive metal ions and a ‘sea’ of delocalised electrons.

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2
Q

Define metallic bonding:

A

Metallic bonding is the electrostatic attraction between the positive metal ions and the negative delocalised electrons.

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3
Q

Is metallic bonding a usually strong or weak attraction?

A

Usually a very strong reaction.

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4
Q

What are the 3 properties of metals?

A

-High melting points

-Conduct electricity

-Malleable

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5
Q

Why do metals have high boiling points?

A

Because the metallic bonding is usually very strong, so lots of energy is needed to break it.

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6
Q

Why do metals conducts electricity?

A

Because the delocalised electrons are free to move through the lattice.

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7
Q

Why are metals malleable?

A

Because the layers of metal ions can slide over each other.

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8
Q

What is thermal decomposition?

A

When heat energy is used to break down a substance.

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9
Q

What do metal carbonates decompose into?

Metal Carbonate ->

A

Metal Carbonate -> Metal Oxide + Carbon Dioxide

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10
Q

What does the thermal decomposition of copper carbonate look like?

A

Copper carbonate (green solid) -> Copper Oxide (black solid) + Carbon Dioxide (colourless gas)

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11
Q

Carbon dioxide is often collected by downward delivery, what does this mean?

A

As carbon dioxide is denser than air, it sinks to the bottom of a tube and can stay there until you want to use it.

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12
Q

Metal + Water ->

A

Metal + Water -> Metal Hydroxide + Hydrogen

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13
Q

What are the two observations (in the metal + water reaction) between magnesium and water?

A

-Effervescence as hydrogen is produced

-Solid disappears due to being used up in the reaction

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14
Q

What is another name for the metals in group 1 of the periodic table?

A

Alkali metals.

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15
Q

What is one word to describe the reaction between group 1 metals and water?

A

Violent.

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16
Q

What are the four similar observations in the reactions between Li, K and Na with water?

A

-Solid floats
-Effervescence
-Solid Moves
-Solid disappears

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17
Q

Why does the solid float in a group 1 metal + water reaction?

A

It is less dense than water.

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18
Q

Why does the solid move in a group 1 metal + water reaction?

A

The effervescence propels it around the surface of the water.

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19
Q

Why does the solid disappear in a group 1 metal + water reaction?

A

It is used up in the reaction.

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20
Q

What colour does a universal indicator turn in water after a group 1 metal and water reaction?

Why?

A

Dark blue because the metal hydroxides are alkalis because they donate OH-.

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21
Q

What is the reaction between Li and water like?

A

Fast.

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22
Q

What is the reaction between Na and water like?

A

Faster than lithium and Na melts

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23
Q

What is the reaction between K and water like?

A

The fastest, K melts and there is a lilac flame.

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24
Q

What is the group 1 metal reactivity trend?

A

The group 1 metals get more reactive as you go down the group.

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25
Q

What do group 1 metals have to do to their electrons when they react?

A

They have to lose 1 electron to get an outer shell

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26
Q

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

A

It’s easier for them to lose an electron when you go down because:

  1. The atoms get bigger and have more shells
  2. the outer-electron is further from the nucleus
  3. The attraction between the nucleus and outer-electron is weaker
  4. Less energy is needed to break the attraction
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27
Q

Metal + Steam -> ?

A

Metal + Steam -> Metal oxide + Hydrogen

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28
Q

Describe the reaction between magnesium and steam:

A

-Usually conducted in a horizontal tube
-Wet wool is heated at the end of the tube to generate steam for the Mg to react with
-The H2 gas is ignited to safely destroy it

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29
Q

Why do metals react with cold water and hot steam to produce different products?

A

Steam has more energy, so both bonds in the water molecule can break.

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30
Q

Acid + Metal ->

A

Acid + Metal -> Salt + Hydrogen

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31
Q

A salt is a compound formed when…

A

A salt is a compound formed when H is displaced from an acid.

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32
Q

What are the 2 important observations in an acid + metal reaction?

A

-The metal disappears because it is used up in the reaction
-There is fizzing because hydrogen is produced

33
Q

What elements are not possible to react with an acid and why?

A

-Au, Ag and Cu
-Because they are less reactive than H, so cannot replace it.

34
Q

What elements are not allowed to react with an acid and why?

A

-Li, Na and K
-Because their reaction with acids is too violent

35
Q

What is a metal displacement reaction?

A

More reactive metals can displace less reactive metals from their compounds.

36
Q

Give an example of a metal displacement reaction:

A

Magnesium can displace copper from copper sulphate

Mg(s) + CuSO4(aq) ->
grey solid blue solution

Cu(s) + MgSO4(aq)
Pink- colourless solution
orange solid

37
Q

What are 2 observations in a metal displacement reaction?

A

-Solid colour change
-Solution colour change

38
Q

Where are most metals found and as what?

A

In the earth’s crust as compounds with oxygen and sulphur.

39
Q

Why are most metals found as compounds with oxygen and sulphur?

A

Because over a long time those metals have reacted with oxygen and sulphur.

40
Q

What are the rocks containing specific metal compounds called?

A

Ores.

41
Q

What metals aren’t found with oxygen and sulphur and why?

A

Gold (Au) and silver (Ag) as they are too un-reactive to have combines with sulphur or oxygen.

42
Q

How are gold and silver found naturally?

A

They are found ‘native’, which means chemically uncombined

43
Q

What process separates metals from their compound?

A

Chemical extraction.

44
Q

What 2 ways are metals chemically extracted from their compounds?

A
  1. Using electricity
  2. Carbon extraction
45
Q

When is electricity used to extract metals from their compounds?

A

When the metal is more reactive than carbon so cannot be displaced by carbon.

46
Q

When is carbon used to extract metals from their compounds?

A

When metals are less reactive than carbon so can be displaced by carbon.

47
Q

Define a redox reaction:

A

Using carbon to displace a metal from its oxide is a redox reaction.

48
Q

Define reduction in terms of oxygen:

A

Loss of oxygen

49
Q

Define reducing agent in terms of oxygen:

A

What takes oxygen away from something else

50
Q

Define oxidation in terms of oxygen:

A

Gain of oxygen

51
Q

Define oxidising agent in terms of oxygen:

A

Gives oxygen to something else

52
Q

Define redox in terms of oxygen:

A

Reduction and oxidation in the same reaction

53
Q

What is rusting?

A

Rusting is a chemical process by which iron is oxidized to form rust.

54
Q

What is the chemical name for rust:

A

Hydrated iron (III) oxide

55
Q

Rusting requires what 2 substances?

A

Oxygen and water.

56
Q

What 3 methods prevent rusting?

A
  1. Using barriers
  2. Sacrificial protection
  3. Galvanising
57
Q

List 3 barriers that can be used to prevent rusting:

A

Paint, plastic or oil.

58
Q

What happens as soon as the barrier on iron breaks?

A

Rusting happens

59
Q

How do you choose the coating material when using barriers to prevent rusting?

A

It depends on the use of the iron. For example oil/grease for moving parts (eg bike chains), paint/plastic for larger, stationary objects (eg buckets)

60
Q

What is sacrificial protection and how does it work?

A

Attaching a block of more reactive metal (eg magnesium) to the iron. This works by displacing the iron from rust as soon as the rust forms.

61
Q

What is the disadvantage of sacrificial protection?

A

The block of magnesium has to be replaced often.

62
Q

What is galvanising?

A

Coating the iron in zinc.

63
Q

How does galvanising work in 2 different ways?

A

-Coating prevents oxygen and water coming into contact with the iron
-Even if the coating cracks, zinc is more reactive than iron so acts as sacrificial protection too

64
Q

What are alloys?

A

Alloys are mixtures of metal with one or more other elements, usually other metals or carbon.

65
Q

What are 3 commonly known alloys:

A

-Steel
-Brass
-Bronze

66
Q

What is steel made up of?

A

Iron + carbon

67
Q

What is brass made up of?

A

Copper + zinc

68
Q

What is bronze made up of?

A

Copper + tin

69
Q

Are alloys harder or softer than pure metals? Why?

A

They are harder than pure metals because the different sized atoms/ions prevent the layers of metal ions from sliding over eachother.

70
Q

Are allows more or less malleable than pure metals?

A

Less malleable.

71
Q

What do the different types of steel depend on?

A

The amount of carbon.

72
Q

What is the use of iron and why?

A

Used to make steel because steel is more useful than iron.

73
Q

What is the use of low-carbon steel and why?

How much carbon is in this?

A

Used to make ships, cars, bridges etc because its strong, but low-carbon so can be hammered into various shapes.

0.1%C

74
Q

What is the use of high-carbon steel and why?

How much carbon is in this?

A

Used to make tools like knives and screwdrivers because it’s high carbon so less malleable and stiffer than low-carbon.

1%C

75
Q

What elements is stainless steel made up of?

A

Iron, carbon and chromium
1% C 10% Cr

76
Q

What is the use of stainless steel and why?

A

Used for cutlery, cooking utensils and kitchen sinks because the Cr forms an oxide layer that resists corrosion, so stays shiny and clean.

77
Q

What is the use of copper and why?

A

Used for wires, cooking pans and water pipes because it’s an excellent conductor of electricity, an excellent conductor of heat, un-reactive and malleable

78
Q

What is the use of aluminium and why?

A

Used for aircraft bodies and power cables because it’s low-density, high strength and conducts.

Chemistry (28 decks)

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