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Chemistry gcse > 2.3 Metals and their extractions > Flashcards

2.3 Metals and their extractions Flashcards

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1
Q

Using a mnemonic, state the order of the reactivity series to platinum.

A

Please
Stop
Calling
Me
A
Careless
Zebra
I
Truly
Like
Him
Calling
Silly
Girl
(penis)

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2
Q

How do you get a metal from its ore?

A

Ore - Metal compound - Metal

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3
Q

What is the blast furnace used for?

A

extract iron from its ore

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4
Q

What are the three steps of the blast furnace?

A
  1. Hot air (oxygen) reacts with the coke (carbon) to produce carbon dioxide and heat energy to heat up the furnace.
  2. More coke is added to the furnace and reduces the carbon dioxide into carbon monoxide, a good reducing agent.
  3. iron(III) oxide is reduced. (either by carbon monoxide or js carbon)
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5
Q

What are the three stages in terms of symbol equations?

A
  1. C(s) + O2(g) → CO2(g)
  2. CO2(g) + C(s) → 2CO(g)
  3. 2Fe2O3(s) + 3C(s) → 4Fe(l) + 3CO2(g)
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6
Q

What is the overall equation for the blast furnace?

A

iron oxide + carbon -> iron + carbon dioxide

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7
Q

What is oxidation?

A

The gain of oxygen

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8
Q

What is reduction?

A

The loss of oxygen/adding electrons

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9
Q

What are the four raw materials used in a blast furnace and what are they?

A
  1. Iron ore (iron oxide mixed w sand)
  2. Limestone (calcium carbonate)
  3. Hot air (blasted at bottom of the furnace to provide heat and oxygen)
  4. Coke (coal and nearly pure carbon)
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10
Q

What is an alloy?

A

mixture of different metals

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11
Q

What does the carbon content tell you about the alloy?

A

The greater the carbon content, the harder the alloy (but brittle)
The lower the carbon content, the softer the alloy

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12
Q

Give examples of low carbon steel uses.

A

bridges, cars, building materials

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13
Q

Give examples of high carbon steel uses.

A

Drill bits

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14
Q

What is electrolysis?

A

The process of passing an electric current trough an ionic substance that is molten or in a solution broken down into its elements

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15
Q

What is the substance called that is broken down in electrolysis? Is it a molten compound or dissolved in water?

A

Electrolyte
Molten, not dissolved in water

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16
Q

Metals always lose electrons, what’s their charge? What electrode are they attracted to?

A

Positive charge, cathode

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17
Q

Non-metals always gain electrons, what’s their charge? What electrode are they attracted to?

A

Negative charge, anode

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18
Q

What is a positive electrode called? What ion is attracted to it?

A

A anode, cation

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19
Q

What is a negative electrode called? What ion is attracted to it?

A

An cathode, anion

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20
Q

What does OIL RIG stand for?

A

Oxidation is loss (of electrons)
Reduction is gain (of electrons)

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21
Q

Summarise what happens during electrolysis

A

During electrolysis, electricity is passed through a liquid containing positive and negative ions. As it is a liquid, ions are free to move around. The positively charged metal ions move to the negative electrode because opposite charges attract. Non-metal ions are negatively charged so they move to the positive electrode.

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22
Q

Do metal ions have a positive or negative charge? What about non-metals?

A

Positive
Negative

23
Q

What is the half equation for oxygen?

A

2O(2-) - 4e(-) -> O2

24
Q

What is the main reaction in the blast furnace? (word equation)

A

Iron (III) oxide + Carbon monoxide -> iron + carbon dioxide

25
Q

What is the symbol equation of the main reaction in the blast furnace?(carbon monoxide)

A

Fe2O3 + 3CO -> 2Fe + 3CO2

26
Q

What is oxidation in terms of oxygen?

A

Gain of oxygen

27
Q

What is reduction in terms of oxygen?

A

Loss of oxygen

28
Q

What does the carbon monoxide gain to become carbon dioxide?

A

Oxygen

29
Q

In the symbol equation Al(3+) + 3e- -> Al, what has happened to the aluminium in terms of electrons?

A

Reduced as it has gained electrons so becomes less positive

30
Q

In the symbol equation 2O(2-) - 4E- -> O2, what has happened to the oxygen in terms of electrons?

A

Oxidised as it has lost electrons and becomes more positive

31
Q

In the symbol equation Fe(3+) + 2e- -> Fe(2+), has it reduced or oxidised?

A

Reduced as it has gained electrons and so becomes less positive

32
Q

What is the method of electroplating?

A

1.Measure 75cm3 of copper sulfate solution into a beaker
2.Measure and record mass of the negative electrode
3.Set up circuit, setting the power pack to 6V d.c
4.Turn on power supply for 3osecs then turn off
5.Remove carefully and dry negative electrode
6.Measure and record mass of negative elctrode
7.Put elecrode back on

33
Q

What is the IV of electroplating? DV? CV?

A

IV: Time electricity is on
DV: mass change in negative electrode
CV: conc and vol of copper sulfate, voltage

34
Q

What happens when the blue copper solution turns colourless?

A

Copper ions have been removed from solution

35
Q

Describe what happens during the extraction of aluminium?

A

1.Cryolite is used as it lowers the mp of Al2O3
2.When electricity is passed through, Al and O ions form
3.Al ions are positive and attracted to cathode where they gain electrons to form Al metal
4.Al ions are reduced, oxide ions are negative and ttracted to anode where they lose electrons to form Oxygen gas
5.Oxygen reacts w graphite electrodes to produce CO2 which burns the electrode and wears away

36
Q

What is the half equation for what is happening at the anode? (aluminium extraction)

A

2O(2-) - 4e- -> O2

37
Q

What is the half equation for what is happening at the cathode? (aluminium extraction)

A

Al(3+) + 3e- _> Al

38
Q

Why is this process expensive? (aluminium extraction)

A

Replacement of anode means lots of electricity is used

39
Q

What are the four factors influencing the placing of steel and electrolysis plants?

A
  1. Good transport links (im/export of goods, workers can get to work)
  2. Workforce (easily employed, some companies build houses for workers)
  3. Reliable energy source (cannot risk powercut)
  4. Safe disposal of waste (toxic waste produced)
40
Q

What are benefits of recycling metals?

A
  • better for environment
  • keeping natural resources
  • prices remain low
41
Q

What four ions are in brine?

A
  1. sodium
  2. chloride
  3. hydrogen
  4. hydroxide
42
Q

Why are Na+ and OH- ions left behind in the solution? What is the remaining compound? Is it an acid or alkali?

A
  • sodium is more reactive than hydrogen so reacts and stays in solution
  • hydroxide produced slower than Cl- so can’t get to electrode as fast
  • compound sodium hydroxide
  • remaining solution is an alkali
43
Q

State some uses of sodium hydroxide.

A

-food processing
-removing pollutants from water

44
Q

State some uses of chlorine

A

-disinfectant
-acid
-manufacture and making plastic

45
Q

Summarise what happens during electrolysis of brine.

A

Compounds are split using electricity, positive ions move to negative electrode, negative ions move to plastic electrode.

46
Q

During electrolysis of water, why is oxygen formed at the anode?

A

Oxide ions are negative

47
Q

What is the half equation for hydrogen?

A

2H(+) + 2e- -> H2

48
Q

Why are different volumes of oxygen and hydrogen produced?

A

There are two hydrogen atoms for every one oxygen atom

49
Q

Why doe the water levels fall during the electrolysis of water?

A

Water is being taken apart and gases are less dense so sit atop the water

50
Q

What is the method of purification of copper?

A
  1. Impure copper on the cathode, liquid has copper in it e.g CuCl2
  2. Cu2+ ions enter the electrolyte from the anode and CU2+ ions leave the solution at the cathode
  3. Solution remains blue as the CU2+ ions enter at the same rate they leave
51
Q

What do transition metals form?

A

Coloured compounds

52
Q

Are transition metals more or less reactive than alkalis, eg sodium?

A

Less reactive

53
Q

True or false, transition metals are usually hard and tough.
True or false they usually have low densities

A

True
False

54
Q

Can transition metals form ions with different charges? If so give an example

A

Yes, Cu+ looses two electrons to form Cu2+ ions

Chemistry gcse (7 decks)

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