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Chemistry > 3.5 Metals > Flashcards

3.5 Metals Flashcards

1
Q

Metallic structure

A
  • A lattice of positive metals ions

- A ‘sea’ of delocalised electrons

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2
Q

Metallic bonding

A

The electrostatic attraction between positive metals ions and (negative) delocalised electrons.

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3
Q

Metallic bonding, strong

A

The strong electrostatic attraction between positive metals ions and (negative) delocalised electrons requires lots of energy to overcome

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4
Q

Properties of metals

A
  • High melting point
  • Malleable
  • Conducts electricity
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5
Q

High melting point explanation

A

Strong electrostatic attraction between positive metals ions and (negative) delocalised electrons requires lots of energy to overcome

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6
Q

Conducts electricity explanation

A

The delocalised electrons are free to move and can carry charge through the lattice

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7
Q

Malleable explination

A

The layers of positive metal ions can slide over each other and the delocalised electrons keep the attraction

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8
Q

Thermal decomposition

A

When heat energy is used to break down a substance

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9
Q

Metal carbonate thermal decomposition

A

Metal carbonate —> Metal Oxide + Carbon Dioxide

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10
Q

Thermal decomposition of copper carbonate

A

Copper Carbonate —> Copper Oxide + Carbon Dioxide

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11
Q

Thermal decomposition of copper carbonate: Colour change

A

Green —> black solid (+ colourless gas)

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12
Q

Downward delivery

A

Carbon dioxide is denser than air meaning it is collected by downward delivery. It sinks to the bottom until you want to use it.

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13
Q

Metal + Water reaction

A

Metal + Water —> Metal Hydroxide + Hydrogen

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14
Q

Metal + Water Reaction: Magnesium

A

Magnesium + Water —> Magnesium Hydroxide + Water

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15
Q

Metal + Water Reaction: Observations

A
  • Solid disappears as it is used up
  • Fizzing as gas is given off (hydrogen)
  • Metals that are less reactive react slower
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16
Q

What are the group one metals called?

A

The alkali metals

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17
Q

What do group 1 metals do?

A

They react violently with water to form metal hydroxides and hydrogen

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18
Q

Observations of Reaction of Lithium, Sodium and Potassium in water

A
  • Fizzing (hydrogen gas)
  • Solid floats
  • Solid moves
  • Solid disappears
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19
Q

What happens to the reactivity as you go down group 1?

A

The reactivity increases

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20
Q

What are all metal hydroxides?

A

Alkalis as they have donated OH-

21
Q

What colour is the universal indicator after reaction of a group 1 metal with water?

A

Turns dark blue as they are alkali

22
Q

Observations of potassium reaction with water?

A

Lilac Flame and melts fastest

23
Q

Trend going down group 1

A

As you go down group one, there are more shells on each atom meaning it is easier to lose the outer electron as it’s further away from the nucleus. Therefore less energy is needed to break the attraction.

24
Q

What happens if you react a metal with steam

A

Doesn’t produce a metal hydroxide, only a metal oxide. This is because steam has more energy so both bonds in the water molecule can break.

25
Q

How are most metals found?

A

In the earths crust as compound with oxygen and sulphur, these are called ores

26
Q

Why are gold and silver metals special?

A

They are too unreactive to combine with oxygen and sulphur, they are found ‘native’ which means chemically uncombined

27
Q

Metal more reactive than carbon

A

If a metal is more reactive than carbon it has to be extracted using electrolysis

28
Q

Electrolysis

A

In water, molecules that are positive go to one side, and negative to another, separating them

29
Q

Carbon Extraction

A

-Heat with carbon and the metal is displaced by the carbon, this only works because it is more reactive than carbon.

30
Q

Carbon Extraction Example

A

Carbon + Copper Oxide —> Carbon Dioxide + Copper

Redox reaction

31
Q

Reduction

A

Loss of oxygen, Gain of electron

32
Q

Reducing Agent

A

Takes oxygen away from something else

33
Q

Oxidation

A

Gain of oxygen, Loss of electrons

34
Q

Oxidising Agent

A

Gives oxygen to something else

35
Q

Redox

A

When both oxidation and reduction occurs

36
Q

Rusting

A

When iron is oxidised to form rust

37
Q

Rusting requires two substances

A

Water and Oxygen

38
Q

Barrier method

A

Coat iron in paint, oil, grease or plastic so the water and oxygen can’t get into the iron

But, the coat will wear away meaning it has to be replaced

39
Q

Sacrificial Protection

A

Attach a more reactive metal so it will displace the iron

But, you need to replace the more reactive metal often (usually magnesium)

40
Q

Galvanising Method

A

Barrier method & Sacrificial protection combined, you coat the iron in zinc, it’s more reactive and water and oxygen can’t get in.

But it is expensive and needs to be replaced.

41
Q

Alloy

A

Mixtures of a metal with one or more other elements (usually other metals or carbon)

42
Q

Alloy characteristics

A

Harder than pure metals because different sized atoms prevent the layers from sliding over each other (less malleable)

43
Q

Use of iron

A

Making steel as it’s more useful

44
Q

Low-Carbon steel use

A

Ships, Cars, Bridges, it’s strong but still can be hammered into shape

45
Q

High-Carbon steel use

A

Tools, less malleable and stiffer than low carbon steel

46
Q

Stainless steel use

A

Cooking pans, cutlery, kitchen sinks, (Cr forms oxide layer that resists corrosion meaning it’s shiny)

47
Q

Copper use

A

Wires, Water pipes (Conductor or heat and electricity, malleable)

48
Q

Aluminium use

A

Aircraft bodies, power cables (low density, high strength, conductors)

Chemistry (12 decks)

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