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Chemistry 1 > 3 - Metals > Flashcards

3 - Metals Flashcards

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1
Q

What does ‘reducing an ore’ mean?

A

Removing the oxygen

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2
Q

What are 3 properties of aluminium?

A
  • high tensile strength
  • good conductor of heat
  • low density

(Non toxic)

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3
Q

What are 3 uses of aluminium?

A
  • overhead power cables
  • saucepans and aluminium cooking foil
  • drinks cans and saucepans
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4
Q

What are 3 uses of copper?

A
  • copper wire in electrical circuits
  • bottoms of saucepans
  • copper piping in plumbing wires
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5
Q

What are 3 properties of copper?

A
  • excellent conductor of electricity
  • malleable and ductile
  • excellent conductor of heat
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6
Q

What are 3 properties of titanium?

A
  • high tensile strength
  • high melting point
  • high resistance to corrosion and low density
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7
Q

What are 2 uses of titanium?

A
  • rotor blades for helicopters and golf clubs

- artificial hip joints, surgical pins and plates for bone fractures

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8
Q

8 properties of metals

A
  1. Good conductors of electricity
  2. Good conductors of heat
  3. Shiny
  4. Sonorous
  5. Ductile
  6. Malleable
  7. High melting point
  8. Dense
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9
Q

What observations occur when magnesium reacts with copper sulphate?

A

-magnesium is more reactive so it displaces the copper from the solution so the blue colour disappears

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10
Q

What happens when an iron nail reacts with copper sulphate?

A

-displacement reaction
-orange brown coating on the silver grey iron nail
-copper sulphate solution gets paler or goes colourless
CUSO4 + FE = CU + FESO4

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11
Q

What is a mineral?

A

Any element or compound found naturally in the Earth’s crust

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12
Q

What is an ore?

A

A rock that contains enough metal to make it economically viable to extract

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13
Q

What is reduction?

A

When a substance loses oxygen (gains electrons)

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14
Q

What is oxidation?

A

When a substance gains oxygen

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15
Q

What happens in the THERMIT REACTION of aluminium + iron oxide = aluminium oxide + iron

A

The iron is reduced as it is less reactive than the aluminium and the aluminium has been oxidised

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16
Q

Why are Gold, Silver and Copper known as ‘native’?

A

Because they are found in the Earth’s crust as pure substances
-don’t need to be extracted

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17
Q

What is iron extracted from?

A

Haematite

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18
Q

What are four things that are put into the blast furnace?

A
  • hot air
  • coke
  • limestone
  • iron
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19
Q

What are the 3 raw materials in the iron blast furnace?

A
  • iron ore
  • coke (pure carbon)
  • limestone
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20
Q

Why is hot air put into the blast furnace?

A

So it makes the coke burn faster than normal and it enables combustion

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21
Q

Why is coke put into the blast furnace?

A

-to reduce the iron oxide to iron metal

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22
Q

Why is limestone put into the blast furnace?

A

So it takes away the impurities in the form of slag

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23
Q

How is iron produced in the blast furnace?

A
  • the coke, limestone and iron ore are fed at the top of the blast furnace.
  • the coke burns to produce carbon dioxide which reacts which the unburnt coke to form carbon monoxide
  • the carbon monoxide then reduces the iron ore to iron
  • the iron is molten and dense so runs to the bottom of the surface where it is tapped off
  • the limestone decomposes to calcium oxide which reacts with the impurities (sand) to give molten slag
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24
Q

What state is the cooled slag?

A

Solid

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25
Q

What can cooled slag be used for?

A
  • fertiliser

- road building

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26
Q

What is the equation for the coke burning to produce carbon dioxide?

A

Carbon + oxygen = carbon dioxide

C + O2 = CO2

27
Q

What is the balanced and word equation for the coke burning to produce carbon monoxide?

A

CO2 + C = 2CO

carbon dioxide + carbon = carbon monoxide

28
Q

What is the equation to reduce the iron ore to iron?

A

3CO + FE2O3 = 3CO2 + 2FE

carbon monoxide + iron oxide = carbon dioxide + iron

29
Q

What is the formation equation for slag from the impurity silicon dioxide?

A

Ca0 + SiO2 = CaSiO3

Calcium oxide + silicon dioxide = molten slag

30
Q

What is electrolysis?

A

The breaking down of ionic substances into simpler substances using electricity

31
Q

In electrolysis, why do the substances have to be melted or dissolved in water?

A

So the ions are free to move

32
Q

What is an electrolyte?

A

The substance that the current passes through and splits up (contains pos and neg ions)

33
Q

What happens to the negative ions (anions) during electrolysis?

A

They move to the positive electrode (anode) and lose electrons
-oxidation

34
Q

What happens to the positive ions (cations) during electrolysis?

A 
Positive ions (canions) move to the negative electrode (cathode) and gain electrons
-reduction
35
Q

What are ionic equations?

A

-the equations occurring at the anode or the cathode
1/2 bc it shows half the whole process
-they only show the ions that are oxidised or reduced

36
Q

OIL RIG

A

oxidation is loss

Reduction is gain

37
Q

OIL

A

eg.
2Cl - 2e = Cl2
2Br - 2e = Br2

38
Q

RIG

A

e.g

Cu2+2e=Cu
Na+e=na

39
Q

What is the overall equation of aluminium oxide?

A

Aluminium oxide = aluminium + oxygen

2Al2O3 = 4Al + 3O2

40
Q

What is the basic ore for extracting aluminium

A

Bauxite

41
Q

Why is aluminium oxide dissolved in molten cryolite?

A
  • bc aluminium has a high melting point of over 2000C, and so a molten state is required which would be expensive
  • cryolite brings down the temperature so it is easier and cheaper
42
Q

Why do the aluminium electrodes need replacing often?

A

Because it keeps reacting with the oxygen to form CO2

43
Q

Why does the aluminium oxide need to be molten?

A

To release the ions so they’re free to move

44
Q

What is the ionic equation at the cathode? (Aluminium)

A

Al 3+ + 3e = Al

45
Q

What is the ionic equation at the anode? (Aluminium)

A

2O 2- - 4e = O2

46
Q

Why doesn’t aluminium corrode?

A

The outer aluminium atoms react with the oxygen in the atmosphere to form a thin layer of aluminium oxide on the metal’s surface which protects it from corroding

47
Q

What are 3 negative impacts of extracting aluminium?

A
  • destruction of habitats
  • waste material
  • makes a lot of noise
48
Q

What are 3 positive impacts of extracting aluminium?

A
  • creates jobs
  • local businesses gain custom
  • money for local businesses
49
Q

What are 4 reasons why we need to recycle?

A
  • use less resources
  • use less energy
  • use less money
  • make less rubbish
50
Q

What is an alloy?

A

A mixture of metals that is made by melting different metals and mixing them together

51
Q

How is the structure of an alloy different to a pure metal?

A

In an alloy the different metal atoms are different sizes which disrupts the layers
-they can’t slide over eachother easily so alloys are stronger and harder

52
Q

Why do we make metals into alloys?

A

-to improve the properties

E.g make them stronger and harder

53
Q

What is the size of a nanoparticle?

A

1-100nm

54
Q

Uses and explanation of silver? (Nanoparticle)

A

Uses:

  • antiseptic sprays
  • linings of refridgerators

Explanation:
-antibacterial

55
Q

Uses and explanation for titanium dioxide/zinc oxide (nanoparticles)

A

Uses
-sunscreens
Explanation:
-reflects UV light

56
Q

Why can nanoparticles be breathed in or absorbed through skin?

A

Because they are so small

57
Q

Why are people concerned about nanoparticles?

A

Because their long term health effects are unknown

58
Q

What is a nanoparticle?

A

They are very small particles

59
Q

What can molten slag be used for?

A
  • cement

- road building

60
Q

Anion
Cation
Anode
Cathode

A

Anion - negative ion
Cation- positive ion
Anode - positive electrode
Cathode - negative electrode

61
Q

What happens if the electrolysis process runs a long time?

A

-no more current flows as run out of ions

62
Q

What is the equation for the decomposition of limestone?

A 
CaCO3 = Ca0 + Co2
Limestone = carbon oxide + carbon dioxide
63
Q

Why can metals below carbon be extracted by carbon?

A

Because the carbon can displace them

64
Q

Describe the full process of extracting iron in the furnace

A

The raw materials are iron ore, coke, limestone and air. Hot air that oxidises coke is blasted into the furnace making coke burn much faster which increases the temperature and carbon dioxide is produced. The carbon dioxide reacts with the unburnt coke to form carbon monoxide which then reduces the iron oxide to iron. The limestone decomposes to calcium oxide which reacts with the impurities (mainly sand) to give molten slag. The molten slag floats on top of the iron and is tapped off

Chemistry 1 (7 decks)

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