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Chemistry > Metals > Flashcards

Metals Flashcards

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1
Q

2 components of the structure of a metal

A

Lattice of positive metal ions

A sea of delocalised electrons

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2
Q

Metallic bonding definition

A

Electrostatic attraction between positive metal ions and negative delocalised electrons

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3
Q

3 metallic properties

A

HIGH MELTING POINT - metallic bonding is very strong so lots of energy is required to break it
CONDUCT ELECTRICITY- delocalised electrons are free to move the rough the lattice
MALLEABLE- layers of metal can slide over eachother

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4
Q

Metal reactivity least to most

A 
Gold
Silver
Copper
HYDROGEN 
lead
Iron 
Zinc 
CARBON
Aluminium
Magnesium 
Calcium
Lithium 
Sodium
Potassium
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5
Q

What are ores

A

Most metals are found in the Earth’s crust as compounds with oxygen and sulphur
The rocks containing specific metal compounds are called ores
(Copper- Potassium)

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6
Q

What are natives

A

Gold and silver are too unreactive to have combined with oxygen and sulphur. They are found native which means that they are chemically uncombined

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7
Q

extraction from ores

ELECTRICITY

A

Metals more reactive than carbon cannot be displaced by carbon
Instead, electricity is used to break down their compounds

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8
Q

extraction from ores

CARBON

A

Metals less reactive than carbon can be displaced by carbon

Eg copper can be displaced from its ore (copper oxide) by heating with carbon

Carbon + copper oxide —> carbon dioxide + copper

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9
Q

Reduction definition

A

Loss of oxygen

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10
Q

Oxidation definition

A

Gain of oxygen

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11
Q

Reducing agent definition

A

Takes oxygen away from something else

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12
Q

Oxidising agent definition

A

Gives oxygen to something else

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13
Q

Redox reaction definition

A

Reduction and oxidation in the same reaction

Eg carbon is used to extract zinc from zinc oxide

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14
Q

Chemical name for rust

A

Hydrated iron (III) oxide

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15
Q

Rusting definition

A

Chemical process by which iron is oxidised from rust

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16
Q

2 stages of rusting

A
  1. Iron is oxidised by oxygen to form iron (III) oxide:
    4Fe(s) + 3O2(g) —> 2Fe2O3(s)
    Fe has gained oxygen and lost electrons to form Fe3+ ions
  2. Iron (III) oxide is hydrated by water
    Fe2O3(s) + xH2O (l) —> Fe2O3 . xH2O (s)

The amount of water gained by the iron (III) oxide varies alot

17
Q

Preventing rusting

USING BARRIERS

A

Coating the iron in paint, oil, grease or plastic prevents the iron from coming into contact with oxygen or water

This only works when coating is intact, as soon as it breaks rusting happens

18
Q

Preventing rusting

SACRIFICIAL PROTECTION

A

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

The downside of this is the block of magnesium has to be replaced often

Equation: Magnesium + Iron (III) oxide —> magnesium oxide + iron
3Mg (s) + Fe2O3 (s) —> 3MgO(s) + 2Fe(s)

19
Q

Preventing rusting

GALVINISING

A

Involves coating iron in zinc
Coating protects O2 and H2O from coming into contact with the iron
Even if a crack appears the zinc is more reactive than the iron so acts as sacrificial protectin

20
Q

What is an alloy

A

Mixture of a metal with one or more other elements or carbon

Alloys are harder than pure metals because the different sized atoms/ ions prevent the layers of metal ions from sliding over each other- less malleable

21
Q

Iron use

A

Making steel- more useful than iron

22
Q

Low carbon steel use

A

Ships cars bridges, sting but can be hammered into different shaped

23
Q

High carbon steel

A

Tools knives

24
Q

Stainless steel

A

Cutlery, kitchen sinks

25
Q

Copper

A

Wires, water pipes, good conductor and unreacgive

26
Q

Aluminium

A

Aircraft bodies, power cables

Low density high strength

Chemistry (6 decks)

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