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Chemistry > Reactivity series and extraction of metals > Flashcards

Reactivity series and extraction of metals Flashcards

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1
Q

Why do some metals react with water?

A

They want to fill their outer electron shell and become a positive ion.

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2
Q

What is displacement

A

When a more reactive metal displaces a less reactive metal from a substance.

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3
Q

Recall the pneumonic fro remembering the order of reactivity

A 
Please
Sir
Can
Me
And
Collin
(the)
Zebra
Ignite
Lucky
Helen
Cruelly
(and)
Sneakily
Gandalf
Please
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4
Q

Using the pneumonic recall the order of reactivity including crabon and hydrogen

A 
Potassium
Sodium
Calcium
Magnesium
Aluminium
Carbon
Zinc
Iron
Lead
Hydrogen
Copper
Silver
Gold
Platinum
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5
Q

How are metals above Carbon extracted

A

Thropugh electrolysis

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6
Q

How are metals above Hydrogen but below Carbon extracted

A

Through reduction (using carbon coke or charcoal)

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7
Q

Why do metals that are below hydrogen not need extraction

A

Because they occur naturally and do not react with other metals

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8
Q

Define oxidation in the terms of electron

A

Substance loses electrons and becomes positive

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9
Q

Define oxidation in the terms of oxygen

A

Substance gains oxygen particles

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10
Q

Define reduction in terms of electrons

A

Substance gains electrons and becomes negative

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11
Q

Define reduction in the terms of oxygen

A

Substance loses oxygen particles

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12
Q

Outline the four steps of the extraction of iron

A
  1. Coke burns and release CO2
  2. C02 reduces to CO
  3. Iron ore is reduced by the CO
  4. Calcium oxide neutralises siliocon dioxide and forms a substance known as slag
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13
Q

What happens at the cathode during elctrolysis

A

The cathode is the negative electrode and reduction occurs here
(hydrogen or metals form here)

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14
Q

What happens at the cathode during elctrolysis

A

The Annode is the positive electrode and oxidation occurs here
(non-metals occur here)

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15
Q

Describe the electrolyssi of Lead Bromide

A 
At the negative electrode (cathode)
Pb2+ ions are attracted
Pb2+→Pb
Pb2+ + 2e- → Pb
At the positive electrode (annode)
Br- ions are attracted
Br- → Br2
2Br- →Br2 + e-
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16
Q

How does electrolysis work

A

Substances wish to have a full outer shell. By melting the substance youa re allowing the ions to move and therefore conduct a charge. When an ectrical charge is passed through the electrodes the ions move towards the one that will allow them to fill their outer shell. This involves either taking electrodes and sending them to the other substance or giving electrodes. Once full the gaseous substance is no longer bound to the solid and evaporates leaving behind the solid metal.

17
Q

Name the rule for ionic solutions and electrolysis at the positive elctrode (annode)

A

If the ion is a halogen (fluorine, chlorine, bromine and iodine) then the halogen is produced
If it is not a halogen then it is oxygen that is produced

18
Q

Name the rule for ionic solutions and electrolysis at the negative elctrode (cathode)

A

If the ion is more reactive than hydrogen then hydrogen is produced
If te ion is less reactive than hydrogen the metal is produced

19
Q

Extraction of aluminium ore (bauxite)

A

Bauxite (Al2O2 + Fe2O3)

20
Q

List the five steps of phytomining

A
  1. Plants absorb copper from the soil
  2. Plants are gathered and burnt
  3. Left with copper oxide
  4. Copper oxide mixed with sulfuric acid
  5. Copper sulphate is elctrolysed
21
Q

Name the benefits of phytomining

A
  1. Inexpensive
  2. Cleansd soil
  3. Cleans air
22
Q

Name the negatives of phytomining

A
  1. Takes along time

2. Poor quality copper produced

23
Q

List the four steps of bioleaching

A
  1. Bacteria breaks down waste copper
  2. Bacteria is mixed with chemicals
  3. Result is copper sulfate
  4. Copper sulphate undergoes electrolysis
24
Q

Name the benefits of bioleaching

A
  1. Cheap and economical
  2. Environmentally friendly
  3. Low emissions
25
Q

Name teh negatives of bioleaching

A
  1. Slow

2. Produces dangerous chemicals

26
Q

Why is water hard to electrolyse

A

Because it is a covalent liquid and has poor electrical conductivity

27
Q

Why is water still possible to elctrolyse

A

Because it does have some free H+ ions and some OH- ions

28
Q

How can the electrical conductivity of water be improved

A

By the addition of acid

29
Q

What happens at the positive elctrode during the electrolysis of water

A

4OH- → 2H2O + O2 + 4e-

oxidation

30
Q

What happens at the negative elctrode during the electrolysis of water

A

2H+ + 2e- → H2

reduction

31
Q

Recall the test for identifying aqeous Copper 2+, Iron 2+ and Iron 3+

A

Copper 2+ turns sodium hydroxide deep blue and cloudy
Iron 2+ turns sodium hydroxide olive green
Iron 3+ turns sodium hydroxide red

Chemistry (12 decks)

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