metals and their extractions Flashcards

1
Q

what is metal extraction

A

metals are extracted from ores which are rocks containing metal compounds found in the earths crust

these metals can be extracted using chemical reactions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

what is the relationship between metal reactivity and extraction

A

the more reactive the metal is the more stable its metal compound so the harder it is ti extract the pure metal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

what are the extraction processes depending in the reactivity series

A

electrolysis - for metals more reactive than carbon

reduction with carbon - for metals less reactive than carbon (cheap process and is favoured over electrolysis)

metals less reactive than hydrogen are found pure in their native form

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

what is a displacement reaction and how is it useful

A

when a more reactive metal displaces a less reactive metal from a compound

they can be used to investigate the relative reactivities of metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

what is oxidation

A

gain of oxygen

loss of electrons

loss of hydrogen

the species oxidised is known as the reducing agent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

what is reduction

A

loss of oxygen

gain of electrons

gain of hydrogen

the species reduced is known as the oxidising agent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

what are the reactions involved in the extraction of iron in a blast furnace

A

the process is a reduction process

coke reacts with oxygen in the air to form carbon dioxide (exothermic combustion reaction)

C + O2 —> CO2

the carbon dioxide reacts with more coke to form carbon monoxide (the carbon is reduced)

CO2 + C —>2CO

the iron oxide reacts with the coke or carbon monoxide and is reduced to form molten iron

3CO + FE2O3 —>3CO2 +2FE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

how are impurities remove from the iron ore in a blast furnace

A

The main impurity in the mixture is silicon dioxide (sand)

Limestone and those thermal decomposition in calcium oxide

The calcium oxide reacts to silicon dioxide to from solid calcium silicate which can be removed from the furnace

this is a neutralisation reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

how does electrolysis work

A

When metallic compounds is melted or dissolved ions are free to move within the liquid or solution

passing a current through the molten liquid or solution means that their solution can be broken down into elements

during electrolysis the substance being broken down is the electrolyte

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

what are the properties and uses of iron

A

malleable

an alloy, steel, can be forged from iron and carbon

steel is harder and stronger than iron and is less likely to rust

used to build cars and used in the construction industry

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

what are the properties and uses of aluminium

A

low density

light weight for its size

resists corrosion due to very thin layer of oxides on the surface

used in aircraft, trains, overhead power cables, saucepans and cooking foil

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

what are the properties and uses of copper

A

good conductor of electricity and heat

soft, easily bent and shaped (malleable)

resistant to corrosion (very unreactive)

used in electrical wiring, gas and water pipes, and plumbing in houses as copper does not react with water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

what are the properties and uses of titanium

A

low density

light weight for its size

resists corrosion

used in fighter aircraft, artificial hip joints and pipes in nuclear power

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

what are the general properties of transition metals

A

high melting points

form coloured compounds

have the ability to form ions with different charges

most are malleable and ductile

good conductors of both heat and electricity due to their delocalised electrons

hard

less reactive than alkali metals ( group 1 metals )

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

what is the test for metal ions

A

when sodium hydroxide (NaOH) is added:

copper (II) ions give a blue precipitate

iron (II) ions give a green precipitate

iron (III) ions give a brown precipitate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

what is an alloy

A

a substance made of a mixture of 2 or more elements, of which at least one is metal

they are made by mixing molten metals

the composition of alloys can be changed to produce alloys with desired properties

16
Q

explain what happens during the electrolysis of water

A

Electrolysis can be used to separate water into hydrogen gas and oxygen gas

positively charged hydrogen ions move to the negative electrode and gain electrons in a reduction reaction

negatively charged hydroxide ions move to the positive electrode and lose electrons to form water and oxygen in oxidation reaction

17
Q

what are the half equation in the electrolysis of water

A

at the cathode the equation is 2H+ + 2e- –> H2

at the anode the equation is
2OH- –> O2 + 2H+ + 4E-

18
Q

Explain what happens during the electrolysis of aqueous solutions

A

An ionic solution contains the irons that make up the ionic compound and the ions in water (OH- and H+)

at the cathode hydrogen is produced unless the positively charged ions in the ionic compound are from a metal less reactive than hydrogen than this metal will be produced it instead

at the anode, oxygen will be produced unless the ionic compound contains halide ions (Cl-, Br-, I-) in this case the halogen will be produced

19
Q

what are the electrode equations in the electrolysis of copper (II) chloride

A

At the cathode cup is less reactive than hydrogen copper ions are reduced to solid copper:
Cu2+ + 2e- –> Cu

At the aloe chloride ions are oxidised:

2Cl- –> Cl2 + 2e-

20
Q

What are the electrode equation in the electrolysis of sodium chloride

A

At the cathode hydrogen ions are reduced as sodium is more reactive than hydrogen
2H+ + 2e- —> H2

at the anode chloride ions are oxidised:
2Cl- –> Cl2 + 2e-

21
Q

what are the uses of electrolysis

A

Electroplating – covering the surface of one met up with another matter

Example: jewellery coated in silver to make it silver plated

manufacture of copper

Manufacture of sodium hydroxide, are you on gas and chlorine gas

22
Q

what factors must be considered when extracting metals

A

Site of extraction plants:
Good infrastructure, close to power station, near a city as a source for workers, away from built-up areas due to noise and pollution

The method used – reduction with carbon can be used where possible to lower energy and cost needed

Recycling – Using recycling plant to recycle and reuse material as opposed to extract new raw materials

23
Q

why is aluminium oxide dissolved in molten cryolite

A

Alumina (aluminium oxide) dissolves in molten cryolite at a
temperature much lower than its melting point, therefore
saving energy