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

C10-12 ELECTROLYSIS METALS , REVERSIBLE REACTIONS Flashcards

(66 cards)

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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
forming cations
the more relative metals more easily lose electrons to form cations
26
forming cations
the more reactive metals more easily lose electrons to from cations
27
reaction with cold water H20 l
metal + water - metal hydroxide + hydrogen potassium - violently sodium - very quickly calcium - slowly
28
reaction only with steam
metal + water - metal oxide + hydrogen | magnesium , zinc , iron
29
no reaction with water or steam
copper , sliver , gold
30
reaction with acid
metal + acid -nsalt + hydrogen sodium, potassium - violent calcium magnesium , zinc , iron - steady coper , sliver , gold - no reaction
31
displacement acid
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
redox reactions
reactions in which an oxidation and reduction happen at the same time , such as displacement reactions
33
redox during displacement
the more reactive metal gets oxidised e.g. Zn - Zn2+ + 2e- the less reactive metal gets reduced e.g. cu2+ +2e- -> cu
34
spectator ion
an ion that does not change during a chemical reaction
35
native state
when metals are found naturally in their pure from such as silver and gold
36
ore
rock containing enough of a metal compound to extract for profit . normally oxides or sulphides of the metal
37
extracting metals by heating with carbon
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
extracting metals by electrolysis
done with metals more reactive than carbon such as potassium, sodium, calcium , magnesium, aluminium, e.g: aluminium oxide - aluminium + oxygen
39
bioextraction
using living organisms to extract metals
40
bleaching
growing bacteria on poor quality copper ore. the bacteria produce a solution of copper sulphate from which copper can be extracted by electrolysis
41
phyoextraction
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
oxidation
gaining oxygen
43
reduction
losing oxygen
44
redox
when reduction and oxidation reactions happen together
45
reduction of iron
iron produced from iron oxide by heating with carbon: iron oxide + carbon - carbon dioxide + iron iron is reduced, carbon is oxidised
46
reduction of aluminium ore
aluminium is produced from aluminium oxide by electrolysis: aluminium oxide - alluminium + oxygen aluminium is reduced , oxygen is oxidised
47
corrosion
when metals slowly react with oxygen , making them weaker
48
rates of corrosion
more reactive metals corrode more quickly
49
tarnish
a protective layer of oxide that stops the layers below from corroding
50
recycling
converting old waste metal into new metal that can be reused
51
advantages of recycling
``` natural reserves last longer less pollution from mining less pollution from processing less waste in landfill often less energy used ```
52
disadvantages of recycling
can be expensive | can use a lot of energy in transporting, collecting and sorting
53
life-cycle assessment LCA
looks at environmental impact of all stages of a products lifecycle, we should aim to reduce all damage
54
LCA stages
obtaining and processing raw materials making and packaging the product using the product disposal or recycling of the product
55
reversible reaction
reactions that can go forwards as well as backwards (with products turning back into reactants)
56
dynamic equilibrium
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
closed systems
nothing can escape, so dynamic equilibrium can be reached
58
open systems
gases can escape so dynamic equilibrium can't be reached
59
equation for making ammonia
nitrogen + hydrogen = ammonia N2 + 3H2 = 2NH3 exothermic
60
hater process
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
effect on equilibrium of increasing temperature
exothermic reaction equilibrium shifts left, yield decreases endothermic reaction equilibrium shifts right , yield increases
62
effect on equilibrium of decreasing temperature
exothermic reaction equilibrium shifts right, yield increase endothermic reaction equilibrium shifts left, yield decreases
63
effect on equilibrium of increasing gas pressure
equilibrium shifts to side with fewer gas molecules
64
effect on equilibrium of decreasing pressure
equilibrium sifts to side with more gas molecules
65
effect on equilibrium of increasing concentration
of products - equilibrium shifts left, yield decreases of reactants equilibrium shifts right , yield increases
66
effects on equilibrium of decreasing concentration
of products- equilibrium shifts right, yield increases of products - equilibrium shifts left , yield decreases

Chemistry GCSE (8 decks)

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