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chemistry > reactivity series metals alloys rusting electrolyisis > Flashcards

reactivity series metals alloys rusting electrolyisis Flashcards

1
Q

reactivity series

A

K
Na
Li
Ca
Mg
Al
C
Zn
Fe
H
Cu
Ag
Au

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2
Q

react with water

A

K Na Li Ca
metal + water > metal hydroxide + hydrogen

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3
Q

potassium + water

A

> potassium hydroxide + hydrogen
- effervescence
- moves on surface of water
- melts into ball
- lilac flame

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4
Q

sodium + water

A

> sodium hydroxide + hydrogen
- effervescence
- moves on surface of water
- melts into ball

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5
Q

lithium + water

A

> lithium hydroxide + hydrogen
- effervescence
- moves on surface of water

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6
Q

calcium + water

A

> calcium hydroxide + hydrogen
- effervescence
- forms white precipitate

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7
Q

react with acids

A

Mg Zn Fe
metal + acid > salt + hydrogen

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8
Q

magnesium + hydrochloric acid

A

> magnesium chloride + hydrogen
- effervescence
- moves on surface
- disappears

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9
Q

zinc + hydrochloric acid

A

> zinc chloride + hydrogen
- effervescence

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10
Q

iron + hydrochloric acid

A

> iron chloride + hydrogen
- effervescence

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11
Q

copper + hydrochloric acid

A

no reaction

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12
Q

don’t react with acids or water

A

Cu Ag Au
(use displacement reactions to order them)

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13
Q

displacement reaction

A

use to see which metal is more reactive
- in terms of O2
oxidation - gain O2
reduction - loss O2
- in terms of e-
oxidation - loss e-
reduction - gain e-

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14
Q

magnesium + copper oxide
Mg + CuO
(displacement example - from metal oxide)

A

> magnesium oxide + copper
MgO + Cu
- bright white light
- exothermic
Cu displaced by Mg
Mg > oxidised (gain O2)
CuO > reduced (lost O2)
Mg is more reactive than Cu

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15
Q

magnesium + copper sulphate
Mg + CuSO4
(displacement example - from aq solution)

A

magnesium sulphate + copper
MgSO4 + Cu
- solution becomes paler
- pink brown solid disappears
Cu is displaced by Mg
Mg > oxidised (lost e-)
Cu2+ > reduced (gain e-)
Mg is more reactive than Cu

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16
Q

extracting metals

A

with carbon
electrolysis

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17
Q

metal ore

A

rocks that contain enough metal in a compound to be economical to extract
(metals can be extracted from their ore)

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18
Q

extracting with carbon

A
  • used for metals less reactive than carbon
  • heat with C/ CO - displaces metal from ore
    eg 2CuO + C > CO2 +2Cu
    C - oxidised - reducing agent
    CuO - reduced
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19
Q

extracting by electrolysis

A
  • used for metals more reactive than carbon
  • expensive so carbon is preferable if it can be used
  • uses lots of electricity
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20
Q

pure metals - bonding/properties

A
  • metallic bonding - EA between cations and sea of delocalised electrons
  • conducts elec- delocalised electrons free to move throughout structure
  • malleable - layers of ions can slide over each other
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21
Q

alloy

A

mixture of metals with another metal or carbon - harder than pure metal

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22
Q

why is allot harder than pure metal?

A
  • consists of diff. sized atoms
  • layers distorted
  • layers can no longer slide over each ither
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23
Q

alloy examples

A

sterling silver
bronze
brass
18k gold
steel

24
Q

steel

A

alloy of iron and carbon
4 types
- cast iron
- low carbon
- high carbon
- stainless steel

25
Q

cast iron

A
  • hard - brittle - can’t be compressed
  • stoves - drains - engines
26
Q

low carbon steels

A
  • easily shaped
  • car body panels - domestic goods
27
Q

high carbon steels

A
  • hard
  • cutting tools
28
Q

stainless steel

A
  • hard - strong - resistant to corrosion
  • cutlery - sink - tools
29
Q

iron uses

A
  • machinery
  • tools
  • bridges
  • car bodies
  • engines
  • cutlery
  • sink
30
Q

iron properties

A
  • hard+tough
  • can be rolled into sheets and cut
31
Q

aluminium uses

A
  • aircraft
  • trains
  • power cables
  • saucepans
  • cooking foil
32
Q

aluminiums properties

A
  • conducts heat
  • connects electrons
  • malleable
  • high mtp.
  • low density
  • resist corrosion
33
Q

copper uses

A
  • electrical cabling
  • plumbing pipes
34
Q

copper properties

A
  • conducts heat
  • conducts electricity
  • malleable
  • high mtp.
  • ductile
  • unreactive
35
Q

rust

A

corrosion of iron (+steel)

36
Q

conditions required for ruse

A
  • oxygen
  • water
    (salt - speeds up rusting)
37
Q

sacrificial protection

A

coat iron with a more reactive metal (reacts + looses electrons instead of iron so corrodes instead)
eg Mg
eg Zn - galvanisation

38
Q

anode

A

+ charged
anions moves to anode (opposite charges attract)

39
Q

cathode

A
  • charge
    cation moves to cathode (opposite charges attract)
40
Q

electrolyte

A

substance that under goes electrolysis (must conduct)
molten or aq - so ions are free to move

41
Q

electrolysis of molten lead bromide

A

heated to molten so ions can move
cathode - orange gas bubbles - oxidation
2Br- (l)>Br2 (g)+ 2e-
anode - dark grey liquid - reduction
Pb2+ (l) + 2e- > Pb(l)

42
Q

test of hydrogen

A

lit splint
squeaky pop

43
Q

test for oxygen

A

glowing splint
relight

44
Q

OILRIG

A

oxidation is loss reduction is gain

45
Q

PANIC

A

Positive anode negative is cathode

46
Q

corrosion

A

metals react with substances in air

47
Q

rust equation

A

iron + water + oxygen > hydrated iron oxide

48
Q

rust prevention

A

physical barriers
sacrificial protection (galvanisation)

49
Q

physical barriers

A

prevent iron coming into contact with water and oxygen in air
eg paint plastic oil

50
Q

galvanisation

A

iron is coated with zinc
Zn is more reactive so oxidised in preference to iron

51
Q

electrolysis

A

splitting of a compound into its elements using electricity

52
Q

electrodes

A

conduct electricity
high mtp.
unreactivity
usually platinum /graphite

53
Q

electrolysis of aqueous sodium chloride

A

cathode - H+, Na+ - colourless gas - 2H+ + 2e- > H2
anode - OH- Cl- - pale green gas - 2Cl- > Cl2 + 2e-

54
Q

electrolysis of water

A

H2O > H+ + OH-
- anode - 4OH- > 2H2O + O2 + 4e- bubbles of O2 - relights glowing splint
- cathode - 2H+ +2e- > H2 - bubbles of H2 - lit splint squeaky pop
- 2H2O > 2H2 + O2 (2H:O)

55
Q

aq - which ion will be discharged- cathode

A

least reactive is discharges (reduced)

56
Q

aq - which ion will be discharged anode

A

halides always discharged if not a halide then hydroxide will be discharged
(halide than hydroxide then anything else)

57
Q

mnemonic

A

Please
Send
Lions
Cats
Monkeys
And
Cool
Zebras
Into
Hot
Countries
Sincerely
Gordon

chemistry (17 decks)

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