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Chemistry Year 9 > Reactivity Series > Flashcards

Reactivity Series Flashcards

(61 cards)

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1
Q

What do atoms form when they get rid of electrons in their outer shell?

A

Positive ions

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2
Q

Metals that form ions most easily are …

A

The most reactive

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3
Q

Metal + acid —> …

A

Metal + acid —> salt + hydrogen gas

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4
Q

Potassium + acid —> …

A

Potassium + acid —> potassium chloride + hydrogen (lots)

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5
Q

How does potassium react with acid?

A

Explosively
Possibly catching fire
Whizzing around

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6
Q

What do the most reactive metals produce the most of?

A

Heat

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7
Q

How to make a fair test reacting metals with acid

A

Each metal has the same mass and surface area
Use the same type and concentration of acid each time

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8
Q

Magnesium and cold acid observations

A

Fast reaction
Lots of fizzing
Tube gets hot
Metal dissolves

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9
Q

Iron and cold acid observations

A

Bubbles form on surface
Slow fizzing when warmed

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10
Q

Iron and warm acid observations

A

Slow fizzing
Iron very slowly dissolves

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11
Q

Aluminium and cold acid observations

A

Initially no reaction (protected by layer of aluminium oxide)

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12
Q

Aluminium and warm acid observations

A

Fast reaction
Lots of bubbles
Aluminium dissolves
Tube heats up

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13
Q

Copper and cold acid observations

A

No change

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14
Q

Dipper and warm acid observations

A

No change

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15
Q

Zion and cold acid observations

A

Slow fizzing
Metal dissolves
Tube gets warm

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16
Q

Lead and cold acid observations

A

No change

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17
Q

Lead and warm acid observations

A

No change

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18
Q

Magnesium + hydrochloric acid —> …

A

Magnesium + hydrochloric acid —> magnesium chloride + hydrogen

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19
Q

Order of reactivity

A

Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
Zinc
Iron
Copper
Silver
Gold

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20
Q

What is a reactive metal?

A

Metals which like to combine with other elements to form compounds
Unreactive elements tend to remain as elements

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21
Q

Metal + water —> …

A

Metal + water —> metal hydroxides + hydrogen (gas)

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22
Q

Potassium reaction with water

A

Moves on the surface
Ignites and burns with a lilac flame
Fizzes and dissolves

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23
Q

Calcium reaction with water

A

Fizzes
Sinks then rises
Forms a cloudy solution

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24
Q

Magnesium reaction with water

A

Very slow reaction
May form bubbles over time

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25
Magnesium reaction with steam
Reacts rapidly
26
Aluminium, zinc, iron reaction with steam
React slowly
27
Copper, silver, gold reaction with cold water
No reaction
28
Sodium + water —> …
Sodium + water —> sodium hydroxide + hydrogen
29
Zinc + steam —> …
Zinc + steam —> zinc oxide + hydrogen
30
Sodium and water reaction
Floats Fizzes Moves May catch fire
31
If universal indicator is added to water and then sodium is added, what colour will the indicator turn?
Purple/violet
32
Lithium reaction with water
Floats Fizzes Moves Dissolves
33
How do we test for hydrogen gas?
Hold a burning splint near the test tube with the gas —> if hydrogen is present it will burn with a squeaky pop
34
Iron + copper oxide —>
Iron + copper oxide —> iron oxide + copper
35
Iron + copper oxide —> iron oxide + copper (explain)
Iron is the more reactive metal and it displaces the copper from its oxide Iron gains oxygen (oxidised) Copper loses oxygen (reduced) Iron = reducing agent (causes copper to be reduced) Copper = oxidising agent (causes iron to be oxidised)
36
What happens if you react magnesium with copper oxide?
A rapid and violent reaction —> a bronze coloured metal (copper) and white powder (magnesium oxide) were formed Magnesium + copper oxide —> magnesium oxide + copper Magnesium is the more reactive metal and it displaces the copper from its oxide Magnesium = oxidised, reducing agent Copper = reduced, oxidising agent
37
When is a metal oxidised?
When it combines with oxygen Or when it’s atoms lose electrons
38
When is a metal reduced?
When combined oxygen is removed Or when its atoms gain extra electrons
39
How to remember oxidising and reducing
O xidation I s L oss R eduction I s G ain
40
What is a redox reaction?
When one metal is oxidised and another is reduced —> displacement reactions are all redox reactions
41
What is an oxidising agent?
A substance which causes another substance to be oxidised E.g. by providing oxygen
42
What is a reducing agent?
A substance which causes another substance to be reduced E.g. by removing oxygen
43
What is a displacement reaction?
A more reactive metal displacing a less reactive metal from a compound
44
What do ionic equations only show?
The particles that take part in the reaction - and change in some way
45
In ionic equations what is the name for the particles that don’t change?
Spectator ions
46
What is the order of reactivity of metal sulfates?
It is opposite to the order of reactivity of the metal elements —> because a reactive metal does not easily let go of the elements it has combined with
47
Zinc + copper sulfate —>
Zinc + copper sulfate —> zinc sulfate + copper
48
What two substances are needed to make iron rust?
Water Oxygen
49
What is the chemical name for rust?
Hydrated iron (III) oxide
50
What makes iron rust more quickly?
If the water is salty
51
When does iron not rust?
If it is in electrical contact with a more reaction metal E.g. magnesium
52
What is corrosion?
Only the surface of a metal that dissolves —> only the surface is exposed to substances in the environment —> water, oxygen
53
Iron rusting:
The rust that forms at the surface gradually flakes off, revealing new metal underneath —> the next layer can also rust and also flake away
54
Aluminium corroding:
Only the surface atoms are affected because when the top layer of aluminium atoms are oxidised to form aluminium oxide they form a protective layer around the rest of the metal
55
What are examples of creating a barrier against air or oxygen to stop iron rusting?
Paint Oil or grease Plastic Electroplating
56
What is electroplating?
Using electrolysis to cover the iron in a thin layer of another metal
57
Why is creating a barrier only temporary to stop iron from rusting?
As soon as there is a hole in the coating, the iron will start to rust
58
What is sacrificial protection (stopping iron from rusting)?
Attaching a more reactive metal to the iron object —> doesn’t need to fully cover the iron, only needs to be attached If the object is exposed to oxygen and water the more reactive metal will be oxidised instead
59
What are examples of a sacrificial metal which could be attached to the underside of a ship to prevent it from rusting?
Zinc Magnesium
60
What is galvanising (stopping iron from rusting)?
Coating the iron object in a thin layer of zinc (barrier method) Even if the iron becomes exposed the zinc will react with the oxygen —> zinc is more reactive than iron (sacrificial method) - after time it will wear away and eventually iron underneath would start to rust —> protection would last longer if the galvanised iron is also painted —> provides an additional barrier protection
61
What is a halide?
A compound containing a halogen combined with a metal

Chemistry Year 9 (5 decks)

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