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GCSE > 3.5 METALS > Flashcards

3.5 METALS Flashcards

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1
Q

Describe metallic structure

A
  • Lattice of positive metal ions
  • Sea of delocalised electrons
  • Metal ions have their usual charges and electrons are labelled e-
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2
Q

Define metallic bonding

A

The strong electrostatic force of attraction between a lattice of positive metal ions, and a seas of delocalised electrons

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3
Q

Explain why metals have high melting points

A
  • The metallic bonds are very strong
  • There are lots of metallic bonds in the structure
  • A lot of energy is required to break the strong metallic bonds
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4
Q

Explains why metals conduct electricity

A

The sea of delocalised electrons are free to move through the positive metal ion lattice, allowing current to flow

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5
Q

Explain why metals are malleable

A

The layers of metal ions are able to slide over each other

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6
Q

Define a thermal decomposition

A

A reaction where heat (thermal) energy is used to break down a substance

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7
Q

Metal carbonate thermal decomposition reaction

A

Metal Carbonate → Metal Oxide + Carbon Dioxide

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8
Q

Colour of copper carbonate

A

Green

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9
Q

Colour of copper oxide

A

Black

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10
Q

What is downward delivery

A

As CO2 is denser than air, carbon dioxide sinks to the bottom of a tube and stays there until it is needed

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11
Q

Reactivity series

A
  • Potassium
  • Sodium
  • Lithium
  • Calcium
  • Magnesium
  • Aluminium
  • Carbon
  • Zinc
  • Iron
  • Lead
  • Hydrogen
  • Copper
  • Silver
  • Gold
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12
Q

First 6 metals of reactivity series

A
  • Potassium
  • Sodium
  • Lithium
  • Calcium
  • Magnesium
  • Aluminium
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13
Q

Middle of reactivity series

A
  • Carbon
  • Zinc
  • Iron
  • Lead
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14
Q

Bottom or reactivity series reactivity series

A
  • Hydrogen
  • Copper
  • Silver
  • Gold
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15
Q

Metal and water reaction

A

Metal + Water → Metal hydroxide + Hydrogen

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16
Q

Observations to a metal and water reaction

A
  • Effervescence - due to hydrogen gas being produced
  • Solid disappears - Used up in the reaction
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17
Q

Observations to Alkali Metals reacting with water

A
  • Solid floats - Less dense than water
  • Effervescence - Hydrogen gas is produced
  • Solid Moves - The effervescence propels it around the surface of the water
  • Solid disappears - It is used up in the reaction
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18
Q

Unique reaction to potassium reacting with water

A

The potassium melts and produces a lilac flame

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19
Q

Unique reaction to sodium reacting with water

A

Sodium melts

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20
Q

Why do the alkali metals get more reactive down the group

A
  • Reacts by losing its outer shell electron to gain a full shell
  • The atoms get bigger and have more shells down the group
  • The outer-electron is further from the attraction of the nucleus
  • The attraction between the nucleus and outer-electron is weaker
  • So less energy is needed to break the attraction
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21
Q

Metal and steam reaction

A

Metal + Steam → Metal Oxide + Hydrogen

22
Q

How is a metal and steam reaction usually conducted

A
  • In a horizontal tube
  • Wet wool is heated to generate steam for the metal further down the tube to react with
  • The hydrogen produced is ignited to safely destroy it
23
Q

Why do metals react different with hot steam and cold water

A

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

24
Q

Magnesium observation

A

Grey solid

25
Q

Copper sulphate observation

A

Blue solution

26
Q

Copper observation

A

Pink-orange solid

27
Q

Magnesium sulphate observation

A

Colourless solution

28
Q

Observations for displacement reaction

A

Solid colour change and solution colour change

29
Q

Magnesium and copper sulfate reaction observations

A
  • Solid turns from grey to pink
  • Solution turns from blue to colourless
30
Q

Define an ore

A

A substance found in the Earth’s crust as compounds bonded with oxygen and sulfur impurities

31
Q

Define the term ‘native’

A

Substances that are found in their pure form as they are too chemically unreactive to react with oxygen and sulfur impurities

32
Q

What are the only 2 native metals

A

Gold and SIlver

33
Q

How do you separate metals more reactive than carbon

A

By electrolysis - Using electricity to break down their ore compounds

34
Q

How do you separate ores less reactive than carbon

A

Carbon Displacement - The compound is heated and the carbon displaces the metal from it’s compound

35
Q

What is oxidation and reduction in terms of oxygen

A

Oxidised - Gains oxygen

Reduced - Loses oxygen

36
Q

Chemical name for rust

A

Hydrated iron(III) oxide

37
Q

Properties of rust

A

Brown, dull, brittle

38
Q

Iron observation

A

Grey, shiny, malleable solid

39
Q

Stages of rusting

A

Iron become oxidized and then hydrated

40
Q

What 2 conditions are needed for rusting to occur

A

Oxygen and water

41
Q

How can rusting be prevented

A
  • Coating the iron in paint, oil, grease or plastic prevents it coming into contact with oxygen or water (use of barriers)
  • Sacrificial protection - by attaching a block of more reactive metal (usually magnesium) to the iron (displaces the iron from the rust as soon as it forms)
  • Galvanising - Coating the iron in zinc that coats the iron preventing it coming into contact with water and oxygen, as well as acting as sacrificial protection
42
Q

Disadvantage to sacrificial protection

A

The block of metal (usually magnesium has to be replaced often)

43
Q

Disadvantage to barriers

A

As soon as it breaks, rusting occurs

44
Q

Define an alloy

A

A mixture of a metal with one or more other elements, usually other metals or carbon

45
Q

Why are alloys harder than pure metals

A
  • The different-sized atoms-ions prevent the layers of metal ions from sliding over each other
  • Meaning the alloy is less malleable
46
Q

Use of iron

A

Making steel as it is more useful

47
Q

Use of low-carbon steel

A

Ships, cars and bridges - very malleable

48
Q

Use of high-carbon steel

A

Tools like knives and screwdrivers - less malleable than low-carbon so stiffer

49
Q

Use of stainless steel

A

Cutlery, cooking utensils, kitchen sinks - Cr forms oxide layer that resists corrosion and so stays shiny and clean

50
Q

Use of copper

A

Wires, cooking pans and water pipes - Excellect conductor of electricity and heat, unreactive and malleable

51
Q

Uses of aluminium

A

Aircraft bodies, power cables - low-density, high strength and conducts

52
Q

Composition of low-carbon, high-carbon and stainless steel

A
  • 0.1% C
  • 1% C
  • 1%C + 10% Cr

GCSE (71 decks)

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