GCSE > 3.5 METALS > Flashcards

3.5 METALS Flashcards

(52 cards)

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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

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A

Metal + Steam → Metal Oxide + Hydrogen

22
Q

How is a metal and steam reaction usually conducted

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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

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A

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

24
Q

Magnesium observation

25
Copper sulphate observation
Blue solution
26
Copper observation
Pink-orange solid
27
Magnesium sulphate observation
Colourless solution
28
Observations for displacement reaction
Solid colour change and solution colour change
29
Magnesium and copper sulfate reaction observations
* Solid turns from grey to pink * Solution turns from blue to colourless
30
Define an ore
A substance found in the Earth's crust as compounds bonded with oxygen and sulfur impurities
31
Define the term ‘native’
Substances that are found in their pure form as they are too chemically unreactive to react with oxygen and sulfur impurities
32
What are the only 2 native metals
Gold and SIlver
33
How do you separate metals more reactive than carbon
By electrolysis - Using electricity to break down their ore compounds
34
How do you separate ores less reactive than carbon
Carbon Displacement - The compound is heated and the carbon displaces the metal from it's compound
35
What is oxidation and reduction in terms of oxygen
Oxidised - Gains oxygen Reduced - Loses oxygen
36
Chemical name for rust
Hydrated iron(III) oxide
37
Properties of rust
Brown, dull, brittle
38
Iron observation
Grey, shiny, malleable solid
39
Stages of rusting
Iron become oxidized and then hydrated
40
What 2 conditions are needed for rusting to occur
Oxygen and water
41
How can rusting be prevented
* 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
Disadvantage to sacrificial protection
The block of metal (usually magnesium has to be replaced often)
43
Disadvantage to barriers
As soon as it breaks, rusting occurs
44
Define an alloy
A mixture of a metal with one or more other elements, usually other metals or carbon
45
Why are alloys harder than pure metals
* The different-sized atoms-ions prevent the layers of metal ions from sliding over each other * Meaning the alloy is less malleable
46
Use of iron
Making steel as it is more useful
47
Use of low-carbon steel
Ships, cars and bridges - very malleable
48
Use of high-carbon steel
Tools like knives and screwdrivers - less malleable than low-carbon so stiffer
49
Use of stainless steel
Cutlery, cooking utensils, kitchen sinks - Cr forms oxide layer that resists corrosion and so stays shiny and clean
50
Use of copper
Wires, cooking pans and water pipes - Excellect conductor of electricity and heat, unreactive and malleable
51
Uses of aluminium
Aircraft bodies, power cables - low-density, high strength and conducts
52
Composition of low-carbon, high-carbon and stainless steel
* 0.1% C * 1% C * 1%C + 10% Cr
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