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IGCSE Chemistry > Metals > Flashcards

Metals Flashcards

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1
Q

Why do we use copper pipes

A

Copper doesn’t react with water

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2
Q

Why can a more reactive metal displace a less reactive metal from its salt

A

As it forms positive ions more easily, the higher up on the reactivity series the more reactive

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3
Q

What metal is used in sacrificial protection

A

Zinc

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4
Q

Why are carbon and hydrogen apart of the reactivity series

A

They are used to extract metal from their oxides

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5
Q

What is a measure of how reactive the metal is

A

The tendency of the metal to lose electrons to form a positive ion

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6
Q

When does a displacement reaction occur

A

When a more reactive metal can displace a less reactive metal ion from its salt

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7
Q

Physical properties of metals (3)

A

Good conductors of heat + electricity
Malleable+ductile
High melting and boiling point

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8
Q

Physical properties of metalloids

A

A mix between metals and non-metals

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9
Q

Physical properties of non metals(3)

A

Do not conduct heat or electricity
Low melting and boiling point
Brittle

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10
Q

4 reactions with metals

A

Cold water
Steam
Oxygen
Acid

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11
Q

Reaction of metal with acid

A

Metal + acid -> Metal salt + hydrogen
Forms metal salt and hydrogen gas

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12
Q

Reaction of metal and cold water

A

Metal + water -> metal hydroxide + hydrogen
Forms metal hydroxide and hydrogen gas

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13
Q

Reaction of metal and steam

A

Forms metal oxide and hydrogen gas
Metal + steam -> metal oxide + hydrogen

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14
Q

Reaction of metal and oxygen

A

Some reactive metals (alkali) react easily, unreactive metals don’t at all
Metal + oxygen -> metal oxide

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15
Q

Alloy and advantages of alloys

A

Mixture of a metal with other elements
Tend to be harder, stronger and more resistive to corrosion and high temperatures

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16
Q

Uses of aluminium and the properties most suitable for that use (5)

A

Aeroplane bodies - high strength to weight ratio and low density
Tin cans - non-toxic, resistant to corrosion and acidic food
Saucepans - good conductor of heat
Window frames - resistant to corrosion
Overhead power cables - good conductor of electricity and low density

17
Q

In what form/state will the salt be after a metal reacts with acid

A

Aqueous

18
Q

What are the uses of copper (3) and why

A

Electrical wires - good conductor of electricity, malleable and ductile
Water pipes - easy to work with and bend non-toxic and unreactive (does not react with water)
Cooking pans - malleable, unreactive to water and good conductor of heat

19
Q

Alloy

A

Mixture of a metal with other elements

20
Q

Advantages of alloys

A

Harder
Stronger
More resistive to corrosion/high temperatures

21
Q

3 commonly used alloys, and their mixture composition

A

Brass - copper and zinc
Stainless steel - Iron and other elements usually nickel/carbon/chromium
Aluminium alloy - aluminium + silicon +manganese

22
Q

What does it mean if theres a white shine in stainless steel

A

It is an alloy containing chromium

23
Q

Uses of 3 alloys and why

A

Brass - jewelery, musical instruments (corrosion resistant and has conductive properties)
Stainless steel - cutlery (hardness and resistance to rust)
Aluminium alloy - aircraft bodies (alloy is stronger but still has a low density)

24
Q

Why are alloys harder than most pure metals

A

Alloys contain atoms of different sizes which distorts the normally regular arrangement of atoms in metals making it more difficult for the layers to slide over each other. This means what alloys are harder than most pure metals

25
Q

How can we determine the reactivity of a metal

A

Reacting metals with water and acids.
The more vigorous the reaction the higher up on the reactivity series
The greater the change in temperature, the higher up on the series

26
Q

List the reactivity series

A

Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
Carbon
Zinc
Iron
Hydrogen
Copper
Silver
Gold

27
Q

Displacement reactions

A

When a more reactive metal can displace a less reactive metal ion from its salt
The higher up on the RS , the easier it is to lose electrons (forms cation)

28
Q

Reactivity of aluminium

A

Does not react with water, only slowly reacts with dilute acids. Reacts readily with oxygen forming a protective, thin layer of aluminium oxide. This prevents reaction with water and dilute acids allowing aluminium to behave as if it is an unreactive metal

29
Q

Thermal decomposition of metal compounds formulas (4)

A

Metal hydroxides -> mtetal oxide + water
Metal carbonates -> metal oxide +carbon dioxide
Metal nitrates -> metal oxide +nitrogen dioxide + oxygen
Group 1 metal nitrates -> metal nitrite + oxygen

30
Q

Colour of oxygen gas

A

Colourless

31
Q

Colour of nitrogn dioxide gas

A

Reddish-brownish

32
Q

Thermal stability of group 1 carbonates

A

Carbonates are more thermally stable than group 2, so the compounds must be heated to undergo decomposition (needs more heat to break down)

33
Q

Rust
(Statements and formula)

A

ONLY HAPPENS WITH IRON
Chemical reaction between iron, water and oxygen to form the compound hydrated iron (III) oxide
Oxygen and water must be present for reaction to occur
Iron is oxidised (loses some of its electrons)

34
Q

Methods of rust prevention (2)

A

Barriers
Galvanising

35
Q

Galvanising
Eg.

A

Process where iron is coated witgh a layer of zinc. As zinc is more reactive than iron it loses its electrons more easily/is more easily oxidised. It corrodes first and protects the less reactive metal from corrosion
Zinc bars on the side of ships

36
Q

Sacrificial protection

A

A more reactive metal can be attached to a less reactive metal, the more reactive metal will oxidise and corrode first and protect the less reactive metal from corrosion
Eg. Zinc bars on sides of steel ships

37
Q

Barrier - rust prevention
Common methods (4)

A

Cover iron with barriers that prevent it from coming into contact with water and oxygen
If coatings are scratched/washed away the iron is exposed again
Oil, paint, plastic, grease

38
Q

Describe the reaction of:
Potassium
Sodium
Calcium
With water

A

Potassium: vigourously (exothermic) to form a colourless, basic, KOH solution
Sodium: readily (exothermic) to form NaOH and H gas
Calcium: less strongly to form CaOH and H

39
Q

Reaction of magnesium with steam

A

Burns in steam to produce white magnesium oxide and hydrogen gas

IGCSE Chemistry (21 decks)

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