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Chemistry > 2. d - Reactivity series > Flashcards

2. d - Reactivity series Flashcards

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1
Q

definition of OIL RIG

A

Oxidation
Is
Loss of electrons

Reduction
Is
Gain of electrons

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2
Q

definition of oxidation reaction ( simplistic terms)

A

addition of oxygen

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3
Q

definition of reduction reaction ( simplistic terms)

A

removal of oxygen

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4
Q

acid + metal = ???

A

salt + hydrogen

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5
Q

how can you tell how reactive metals are from reacting with HCl or sulphuric acid

( pg. 41 )

A
  1. ( boiling tube with same amounts of acid and place metal in it )
  2. fast reaction the more reactive the metal
  3. speed of reaction indicated by rate at which hydrogen bubbles given off
  4. test for hydrogen with burning splint = metal with loudest squeaky pop = given off most hydrogen = most reactive
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6
Q

metal + water =???

A

metal hydroxide + hydrogen

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7
Q

less reactive metal + steam = ???

A

metal oxide + hydrogen

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8
Q

what metals react very vigorously with water

A

potassium
sodium
lithium
calcium

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9
Q

what metals are considered less reactive and only react with steam

A

magnesium
zinc
iron

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10
Q

what metal won’t react with water or steam

A

copper

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11
Q

definition of displacement reaction in terms of metal and metals and metal oxides

A

a more reactive metal will displace a less reactive metal from its oxide because it will bond more strongly to the oxygen

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12
Q 
displacement reaction ( metal + metal oxide)
- iron oxide + aluminium = aluminium oxide + iron

explain what has happened
and what kind of reaction this is

A

iron is displaced from iron oxide by the more reactive aluminium

redox reaction = metal ( aluminium ) is oxidised + displaced metal ion ( iron ) is reduced

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13
Q

give some examples of metal salts

A

copper sulphate
zinc chloride
sodium chloride

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14
Q

what happens if you put a reactive metal into a solution of a less reactive metal salt

A

reactive metal will replace the less reactive metal in the salt

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15
Q

displacement reaction ( metal + aqueous solution of metal salt )

eg. iron nail in solution of copper sulphate
iron + copper sulphate = iron sulphate + copper

what happens and what kind of reaction is this

A

more reactive iron displaces less reactive copper

redox reaction = iron is oxidised + copper is reduced

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16
Q

what happens if a piece of silver metal is put into a solution of copper sulphate

A

Nothing

-more reactive metal ( copper ) is already the salt

17
Q

when a reaction occurs how can you tell which metal is more reactive by temperature

A

change in temperature

more reactive metal will give a greater change in temperature than a less reactive metal

18
Q

what is rhyme for reactivity series

A

Please Send Lions Cats Monkeys And (Cool) Zebras Into ( Hot ) Countries Signed General Penguin

19
Q

what is the order of the reactivity series - metals ( remember the rhyme ) from most reactive to least reactive

A 
Potassium 
Sodium
Lithium
Calcium 
Magnesium
Aluminium 
CARBON
Zinc 
Iron
HYDROGEN
Copper
Silver 
Gold
20
Q

what are the conditions needed for iron to rust ( corrode )

A

oxygen ( from air ) + water

21
Q

what is the word equation for the rusting if iron

A

iron + oxygen + water = hydrated iron ( III ) oxide ( rust)

22
Q

what are the 3 main ways to prevent rusting of iron

A

barrier methods
sacrificial protection
galvanising

23
Q

how does a barrier method work ( prevent iron rusting )

A

coat the iron with a barrier to keep out the water and oxygen

24
Q

examples of barrier methods

A

painting / coating with plastic ( big + small structures )

oil / greasing ( when moving parts involved eg. bike chains )

25
Q

how does a sacrificial method work ( prevent iron rusting )

A

placing a more reactive metal with the iron = water + oxygen react with sacrificial metal instead of with the iron

26
Q

example of sacrificial method

A

zinc ( galvanising )

27
Q

how does galvanising work ( prevent iron rusting )

A

coating of zinc spayed onto object or big blocks of zinc can be bolted to the iron ( ships / underground iron pipes )

zinc is more reactive than iron = zinc will be oxidised instead of the iron

28
Q

definition oxidising agent

A

substance that oxidises the metal

is reduced itself

29
Q

definition of reducing agent

A

substance that reduces the metal

is oxidised itself

30
Q

definition of redox reaction

A

where reduction and oxidation happen at the same time

Chemistry (23 decks)

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