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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
cast iron
- hard - brittle - can’t be compressed - stoves - drains - engines
26
low carbon steels
- easily shaped - car body panels - domestic goods
27
high carbon steels
- hard - cutting tools
28
stainless steel
- hard - strong - resistant to corrosion - cutlery - sink - tools
29
iron uses
- machinery - tools - bridges - car bodies - engines - cutlery - sink
30
iron properties
- hard+tough - can be rolled into sheets and cut
31
aluminium uses
- aircraft - trains - power cables - saucepans - cooking foil
32
aluminiums properties
- conducts heat - connects electrons - malleable - high mtp. - low density - resist corrosion
33
copper uses
- electrical cabling - plumbing pipes
34
copper properties
- conducts heat - conducts electricity - malleable - high mtp. - ductile - unreactive
35
rust
corrosion of iron (+steel)
36
conditions required for ruse
- oxygen - water (salt - speeds up rusting)
37
sacrificial protection
coat iron with a more reactive metal (reacts + looses electrons instead of iron so corrodes instead) eg Mg eg Zn - galvanisation
38
anode
+ charged anions moves to anode (opposite charges attract)
39
cathode
- charge cation moves to cathode (opposite charges attract)
40
electrolyte
substance that under goes electrolysis (must conduct) molten or aq - so ions are free to move
41
electrolysis of molten lead bromide
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
test of hydrogen
lit splint squeaky pop
43
test for oxygen
glowing splint relight
44
OILRIG
oxidation is loss reduction is gain
45
PANIC
Positive anode negative is cathode
46
corrosion
metals react with substances in air
47
rust equation
iron + water + oxygen > hydrated iron oxide
48
rust prevention
physical barriers sacrificial protection (galvanisation)
49
physical barriers
prevent iron coming into contact with water and oxygen in air eg paint plastic oil
50
galvanisation
iron is coated with zinc Zn is more reactive so oxidised in preference to iron
51
electrolysis
splitting of a compound into its elements using electricity
52
electrodes
conduct electricity high mtp. unreactivity usually platinum /graphite
53
electrolysis of aqueous sodium chloride
cathode - H+, Na+ - colourless gas - 2H+ + 2e- > H2 anode - OH- Cl- - pale green gas - 2Cl- > Cl2 + 2e-
54
electrolysis of water
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
aq - which ion will be discharged- cathode
least reactive is discharges (reduced)
56
aq - which ion will be discharged anode
halides always discharged if not a halide then hydroxide will be discharged (halide than hydroxide then anything else)
57
mnemonic
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chemistry (17 decks)

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