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Grace Chemistry IGCSE > Topic 7 - Metals > Flashcards

Topic 7 - Metals Flashcards

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1
Q

Describe the structure of metals

A

Positively charged metal ions touching in regular lattice

Delocalised elections floating between

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2
Q

What are delocalised electrons?

A

The electrons that a metal has lost to become an ion. They just float around

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3
Q

Define metallic bonding

A

The electrostatic attraction between the positive metal ions and the delocalised electrons

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4
Q

Explain why metals conduct electricity

A

Because to conduct you need
• charged particles
• that are free to move
The delocalised electrons fit both of these criteria

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5
Q

Explain why metals are malleable

A

When force is applied to metals, the top layer of ions slide across the one underneath it, causing it to bend

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6
Q

Define alloy

A

A mixture of a base metal and alloying agents

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7
Q

Describe the two methods with which alloys can be made

A

1) swapping out some of the base metal atoms and replacing them with alloying agent atoms
2) jamming some alloying agent atoms between some of the base metal atoms

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8
Q

Explain why alloys tend to be harder than base metals

A

The alloying agent atoms in an alloy tend to be a different size to those of the base metals atoms, distorting the layers of metal atoms and so the layers slide less easily.

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9
Q

Name the reactivity series

A 
K
Na
Li
Ca
Mg
Al
C
Zn
Fe
Pb
H
Cu
Ag
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10
Q

Describe the reactivity series

A

Potassium -> calcium: very reactive

Magnesium -> zinc: fairly reactive

Iron to silver -> not very reactive

Gold: not at all reactive

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11
Q

Describe metal + cold water reactions

A

There is only enough energy for one of the bonds to be broken

Metal + cold water -> metal hydroxide + hydrogen

Magnesium, zinc and iron won’t react much
Copper won’t react

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12
Q

Describe metal + steam reactions

A

There is enough energy to break both bonds

Element + steam -> element oxide + hydrogen

Copper won’t react

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12
Q

How to carry out metal + water reactions

A

Place the metal into a beaker of water and hold a burning splint close to the metal to test the gas given off

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14
Q

Which group are the alkali metals

A

Group 1

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15
Q

How to carry out metal + steam reactions

A

1) place some mineral wool soaked in water at the base of a test tube held horizontally
2) place a strip of metal half-way up the test tube
3) plug the test tube using a bung with a hole through the centre where u place a small plastic cylinder
4) beat the mineral wool and metal with Bunsen burners
5) the steam will react with the metal, producing hydrogen gas
6) test the hydrogen gas with a burning splint

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16
Q

Describe the alkali metals

A
  • they have low melting and boiling points
  • they are very soft and can be cut easily with a knife
  • they have low densities
  • they react quickly with water, producing hydroxides and hydrogen gas
  • their hydroxides and oxides dissolve in water to form alkaline solutions
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17
Q

Describe the reaction between Lithium and water

A

Li (s) + H2O (l) -> LiOH (aq) + 0.5H2 (g)

  • fizzing
  • solid disappears
  • moves on surface of water
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18
Q

Describe the reaction between Sodium and water

A

Na (s) + H2O (l) -> NAOH (aq) + 0.5H2 (g)

  • faster
  • fizzing
  • solid disappears
  • moves on the surface of the water
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19
Q

Describe the reaction between potassium and water

A

K (s) + H20 (l) -> KOH (aq) + 0.5H2 (g)

  • fizzing
  • solid disappears
  • moves on surface of water
  • lilac flame
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20
Q

Describe the reactivity trend of alkali metals

A

They get more reactive as the group descends, because as the group descends, the outermost electron is further away from the nucleus, meaning it’s attraction is weaker, and it is more easily lost.

This can be seen through their reactions with water and oxygen

21
Q

What happens to metal carbonated thermally decompose when heated

A

They thermally decompose

22
Q

Describe the general formula for thermal decomposition

A

heat

metal carbonate ——> metal oxide + CO2

23
Q

What is a displacement reaction

A

When a metal and a dissolved compound react, they displace each other (but only if the metal is more reactive)

24
Q

What are the reactions of displacement reaction

A

1) what is happening to the elements

2) what is happening to the compounds

25
Q

What are metal ores

A

Metal compounds found in the earths crust

26
Q

What do we use to displace metals from their ores?

ASK ABOUT THIS

A

Carbon/ carbon monoxide

27
Q

Describe the general formula for carbon reduction

A

carbon + metal oxide -> metal + carbon dioxide

28
Q

What type of reaction is a carbon reduction and why?

A

REDOX

  • carbon is oxidised (gains oxygen)
  • metal oxide is reduced (loses oxygen)
29
Q

What is the reducing agent in carbon reduction?

A

Carbon

30
Q

What is a reducing agent?

A

The substance which takes oxygen away from another

31
Q

What is an oxidising agent?

A

The substance which gives away its oxygen

32
Q

Describe the extraction of iron from haematite in a blast furnace

A

1) coke (porous form of carbon) combusts
C + O2 -> CO2

2) CO2 reacts with coke
CO2 + C -> 2CO

3) CO reacts with haematite
3CO + Fe2O3 -> 2Fe + 3CO2

4) Limestone is thermally decomposed
CaCO3 -> CaO + CO2

5) CaO reacts with impurities in haematite
CaO + SiO2 -> CaSiO3 (slag)

33
Q

Describe the method for extracting aluminium from bauxite

A

Electrolysis

Positive aluminium is attracted to negative carbon electrode (cathode)

Negative oxygen is attracted to the positive carbon electrode (anode)

34
Q

Describe aluminium

A
  • light
  • strong
  • low density -> planes and bicycle frames
  • conducts electricity and heat well
  • resists corrosion -> drinks cans
  • reacts very quickly with oxygen in the air to form a protective layer of aluminium oxide to stop any further reactions taking place
35
Q

Describe copper

A
  • malleable
  • ductile
  • resistant to corrosion
  • conducts electricity and heat very well
  • used in wires because of low resistance
  • used to help construction
  • used in heating systems because of speedy transfer of heat
36
Q

Describe iron

A
  • soft, easily shaped
  • brittle
  • corrodes easily (rusts)
  • used for electromagnetic valves because it is magnetically soft, but most of it is turned into steel
  • dense
  • wrought iron is malleable -> used to make gates and railings
37
Q

Describe steel

A
  • low carbon steel is easily shaped and used for car body panels
  • high carbon steel is hard and used for cutting tools
  • stainless steel is resistant to corrosion and used for cutlery and sinks
38
Q

What is rust?

A 
Hydrated iron (iii) oxide
Fe2•O3

The water is loosely bonded to the iron(III) oxide

It is a soft, crumbly solid which flakes off to leave more iron available to rust again p

39
Q

What is the rust reaction

A

2Fe + 1.5O2 + H2O -> Fe2O3•H2O

40
Q

What are the methods of preventing rust

A

1) coating
2) sacrificial protection
3) galvanising

41
Q

Describe coating

A
  • using either paint, oil, grease (for moving parts), or plastic (for stationary parts)
  • the Fe3+ is separates from the O2 and the H2O
42
Q

Describe sacrificial protection

A
  • attach a block of more reactive metal (magnesium)
  • when oxygen reacts with iron, magnesium displaced it

3Mg + Fe2O3 -> 3MgO + Fe

43
Q

Describe galvanising

A

• coat (to protect Fe3+) with a thin layer of zinc (providing sacrificial protection if the coating is scratched)

44
Q

What happens when sodium reacts with oxygen?

A

Forms a mixture of sodium oxide (Na2O) and sodium peroxide (Na2O2)

45
Q

What happens when potassium reacts with oxygen?

A

Forms a mixture of potassium peroxide (K2O2) and potassium superoxide (KO2)

46
Q

Why do more reactive metals displace less reactive ones from their oxide

A

They bond more strongly to the oxygen

47
Q

Describe the relationship between temperature given off by displacement reactions and reactivity of metals

A

The more reactive the metal, the more temperature given off

48
Q

Name some alloys

A

Brass (copper + zinc)

Bronze (copper + tin)

Grace Chemistry IGCSE (21 decks)

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