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Chemistry GCSE > C10-12 ELECTROLYSIS METALS , REVERSIBLE REACTIONS > Flashcards

C10-12 ELECTROLYSIS METALS , REVERSIBLE REACTIONS Flashcards

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1
Q

electrolysis

A

using direct current to break compounds down their elements

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2
Q

electrolyte

A

liquid used for electrolysis because ions can move - either molten or dissolved ionic compounds

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3
Q

electroylsis of solids

A

does not work as ions can’t move

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4
Q

electrodes

A

conducting rods placed in electrolyte , connect to power supply

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5
Q

cathode

A

negative electrode where cations + are discharged

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6
Q

anode

A

positive electrode where anions - are discharged

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7
Q

oxidation HT

A

loss of electrons OIL

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8
Q

reduction HT

A

gain of electrons RIG

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9
Q

anOx

A

Anode is for Oxidation

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10
Q

caRe

A

CAthode is for Reduction

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11
Q

half equations

A

an equation that shows what happens to just one of the ions during chemical reaction. Two half - equations combine to give the overall ionic equation

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12
Q

half equations in electrolysis

A

show electron transfer
cathode (reduction):
m+ + e - m

anode (oxidation):
x - X + e-

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13
Q

electrons in half equations

A

cations will gain the same number of electrons as their charge. anions will lose the same number of electrons as their charge

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14
Q

non-metals in half equations

A

most non-metals will form molecules : O2 , F2 , CL2, BR2 , L2 etc
so you will need two of them in the half equation

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15
Q

discharged

A

when an ion loses its charge to become an atom

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16
Q

electrolysis of molten salts

A

cathode: metal
anode: non-metal

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17
Q

ions in salt solutions

A

metal, non-metal and H+ and OH- because water partially ionises

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18
Q

hydrogen half equation

A

2H+g + 2e- -> H2g

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19
Q

electrolysis of salt solutions cathode

A

metal unless reactive metal such as K, Na ,Li , Ca in which case hydrogen

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20
Q

electrolysis of salt solutions anode

A

non metal unless sulphate salt in which case oxygen

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21
Q

electroylsis of sulfuric acid

A

cathode: hydrogen
anode: oxygen

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22
Q

purifying copper set up

A

anode: impure copper
cathode: pure copper
electrolyte: coppe sulphate solution

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23
Q

purifying copper explanation

A

copper atoms leave the anode
(cu - cu2 + 2e-) travel through solution and go to cathode (cu2 + 2e- -> cu)
impure atoms on the anode fall to the bottom as sludge

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24
Q

reactivity series (most to least)

A

potassium , sodium , calcium , magnesium , aluminum , zic , iron , copper , silver , gold

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25
Q

forming cations

A

the more relative metals more easily lose electrons to form cations

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26
Q

forming cations

A

the more reactive metals more easily lose electrons to from cations

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27
Q

reaction with cold water H20 l

A

metal + water - metal hydroxide + hydrogen

potassium - violently
sodium - very quickly
calcium - slowly

28
Q

reaction only with steam

A

metal + water - metal oxide + hydrogen

magnesium , zinc , iron

29
Q

no reaction with water or steam

A

copper , sliver , gold

30
Q

reaction with acid

A

metal + acid -nsalt + hydrogen

sodium, potassium - violent
calcium magnesium , zinc , iron - steady

coper , sliver , gold - no reaction

31
Q

displacement acid

A

reactions in which a more reactive metal displaces a less reactive metal from a salt e.g.
copper sulfate + zinc -> zinc sulfate + copper
does not work backwards as copper is less reactive than zinc

32
Q

redox reactions

A

reactions in which an oxidation and reduction happen at the same time , such as displacement reactions

33
Q

redox during displacement

A

the more reactive metal gets oxidised e.g.
Zn - Zn2+ + 2e-
the less reactive metal gets reduced e.g.
cu2+ +2e- -> cu

34
Q

spectator ion

A

an ion that does not change during a chemical reaction

35
Q

native state

A

when metals are found naturally in their pure from such as silver and gold

36
Q

ore

A

rock containing enough of a metal compound to extract for profit . normally oxides or sulphides of the metal

37
Q

extracting metals by heating with carbon

A

for extracting less reactive metals such as zinc , iron, copper. works because carbon is more reactive, e.g.. iron oxide + carbon - carbon dioxide + iron

38
Q

extracting metals by electrolysis

A

done with metals more reactive than carbon such as potassium, sodium, calcium , magnesium, aluminium, e.g:
aluminium oxide - aluminium + oxygen

39
Q

bioextraction

A

using living organisms to extract metals

40
Q

bleaching

A

growing bacteria on poor quality copper ore. the bacteria produce a solution of copper sulphate from which copper can be extracted by electrolysis

41
Q

phyoextraction

A

plants are grown that absorb metal compounds as they grow. the plants are then burnt to produce ash that is rich in metal compounds

42
Q

oxidation

A

gaining oxygen

43
Q

reduction

A

losing oxygen

44
Q

redox

A

when reduction and oxidation reactions happen together

45
Q

reduction of iron

A

iron produced from iron oxide by heating with carbon:
iron oxide + carbon - carbon dioxide + iron
iron is reduced, carbon is oxidised

46
Q

reduction of aluminium ore

A

aluminium is produced from aluminium oxide by electrolysis:
aluminium oxide - alluminium + oxygen
aluminium is reduced , oxygen is oxidised

47
Q

corrosion

A

when metals slowly react with oxygen , making them weaker

48
Q

rates of corrosion

A

more reactive metals corrode more quickly

49
Q

tarnish

A

a protective layer of oxide that stops the layers below from corroding

50
Q

recycling

A

converting old waste metal into new metal that can be reused

51
Q

advantages of recycling

A 
natural reserves last longer 
less pollution from mining 
less pollution from processing 
less waste in landfill 
often less energy used
52
Q

disadvantages of recycling

A

can be expensive

can use a lot of energy in transporting, collecting and sorting

53
Q

life-cycle assessment LCA

A

looks at environmental impact of all stages of a products lifecycle, we should aim to reduce all damage

54
Q

LCA stages

A

obtaining and processing raw materials
making and packaging the product
using the product
disposal or recycling of the product

55
Q

reversible reaction

A

reactions that can go forwards as well as backwards (with products turning back into reactants)

56
Q

dynamic equilibrium

A

the point at which the rate of the forwards reaction and backwards reaction are equal, so the concentrations of reactants and products stops changing

57
Q

closed systems

A

nothing can escape, so dynamic equilibrium can be reached

58
Q

open systems

A

gases can escape so dynamic equilibrium can’t be reached

59
Q

equation for making ammonia

A

nitrogen + hydrogen = ammonia
N2 + 3H2 = 2NH3
exothermic

60
Q

hater process

A

for making ammonia in factories:
-200 atm pressure - equilibrium shifts right, yield increases - 450 - equilibrium shifts lefts, lower yield but MUCH faster reaction
catalyst - increases reaction rate

61
Q

effect on equilibrium of increasing temperature

A

exothermic reaction
equilibrium shifts left, yield decreases
endothermic reaction
equilibrium shifts right , yield increases

62
Q

effect on equilibrium of decreasing temperature

A

exothermic reaction
equilibrium shifts right, yield increase
endothermic reaction
equilibrium shifts left, yield decreases

63
Q

effect on equilibrium of increasing gas pressure

A

equilibrium shifts to side with fewer gas molecules

64
Q

effect on equilibrium of decreasing pressure

A

equilibrium sifts to side with more gas molecules

65
Q

effect on equilibrium of increasing concentration

A

of products - equilibrium shifts left, yield decreases of reactants equilibrium shifts right , yield increases

66
Q

effects on equilibrium of decreasing concentration

A

of products- equilibrium shifts right, yield increases of products - equilibrium shifts left , yield decreases

Chemistry GCSE (8 decks)

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