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GCSE Chemistry > Unit 2 Topic 1 Reactivity Series > Flashcards

Unit 2 Topic 1 Reactivity Series Flashcards

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1
Q

Why do metals reacting with air gain mass?

A

Because they form an oxide

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2
Q

When heated in air, metals react with the (?) in the air

A

oxygen

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3
Q

When heated in air, potassium

A

burns with a lilac flame, forming a white solid

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4
Q

When heated in air, sodium

A

burns with a golden yellow flame, forming a white solid

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5
Q

When heated in air, calcium

A

burns with a brick red flame, forming a white solid

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6
Q

When heated in air, magnesium

A

burns with a bright white light, forming a white solid/ash

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7
Q

Aluminium only burns in air when (?)

A

finely powdered

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8
Q

When heated in air, aluminium powder

A

burns with white sparks, forming a white solid

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9
Q

When heated in air, zinc

A

burns steadily forming a yellow solid, which becomes white on cooling

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10
Q

Which forms of iron burn/do not burn easily?

A

Sheets of iron do not burn easily, but iron filings do

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11
Q

When heated in air, iron

A

burns with yellow/orange sparks when in the form of filings, forming a black solid

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12
Q

When heated in air, copper

A

does not burn, but forms a black solid

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13
Q

After iron and copper are left in air, the oxide layer formed is easily (?)

A

rubbed off

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14
Q

To heat potassium and sodium in air you would use a (?)

A

deflagrating spoon

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15
Q

When potassium and sodium are freshly cut,

A

a shiny surface is exposed, which quickly tarnishes (goes dull)

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16
Q

When calcium, magnesium, aluminium, zinc, iron and copper are left in air, they react ….

A

slowly with the air, forming an oxide layer on the surface

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17
Q

Metal + oxygen —>

A

metal oxide

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18
Q

Fe3O4 is a (?)

A

mixed oxide

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19
Q

Why must sodium, potassium, and calcium be heated in air under very careful supervision and strict safety procedures?

A

The reactions can be extremely dangerous, because these metals are high up in the reactivity series.

20
Q

Metals other than sodium, potassium and calcium are heated in air in a (?)

A

crucible

21
Q

Which form of the metal is usually heated in air?

A

Powder form

22
Q

Why is the crucible lid lifted occasionally when heating a metal in air?

A

To allow more air into the crucible

23
Q

Draw the diagram for heating metals in air (with the exception of sodium, potassium and calcium)

A

Labels:

  • crucible containing metal
  • crucible lid
  • pipeclay triangle
  • tripod
  • heat/Bunsen burner
  • heatproof mat
24
Q

Describe the safety procedures when reacting sodium or potassium with water. [3]

A

A small piece of the metal is placed in a trough half-full of water.

The reaction is carried out behind a safety screen.

Tongs/tweezers are used to handle the metal.

25
Q

Describe the reaction of potassium with water.

A 
Potassium:
Floats on the surface
Moves around the surface
Burns with a lilac flame
Fizzes, giving off a gas
Heat is released
Small explosion/crackles
Eventually disappears
Forms a colourless solution
26
Q

Describe the reaction of sodium with water.

A 
Sodium:
Floats on the surface
Melts and forms a silvery ball
Fizzes, giving off a gas
Heat is released
Eventually disappears
Forms a colourless solution
27
Q

Describe a further test to prove potassium/sodium has fully reacted with the water.

A

Solution changes universal indicator from green to blue.

28
Q

Describe the reaction of calcium with water.

A 
Calcium:
Fizzes, giving off a gas
Sinks, then rises
Heat is released
Eventually disappears
Forms a colourless solution
29
Q

Aluminium, zinc, iron and copper have (?) with water, however iron will (?) after a few days

A

no reaction, rust

30
Q

Describe the reaction of magnesium with water.

A

Magnesium:
Undergoes a very slow reaction
Gives off a few bubbles of gas

31
Q

Why are potassium and sodium stored under oil?

A

To prevent reaction with oxygen and moisture in the air

32
Q

Metal + water –>

A

metal hydroxide + hydrogen

33
Q

Describe how you would react calcium and magnesium with water. [2]

A

The metal is placed in water inside a beaker and an inverted filter funnel is placed over the metal.

A boiling tube filled with water is used to collect the hydrogen produced.

34
Q

Draw a diagram of the apparatus used to react non-group 1 metals with cold water

A

Labels:

  • beaker
  • water
  • filter funnel
  • boiling tube
  • hydrogen
  • calcium/metal
35
Q

How do you test that hydrogen is produced?

A

Hydrogen burns with a squeaky pop, when in contact with a glowing splint

36
Q

Describe the production of bubbles of gas if magnesium is reacted with water.

A

Only a few bubbles of gas are produced over a period of several days.

37
Q

Describe the reaction of magnesium with steam.

A

The heated magnesium ribbon burns with a bright white light, forming a white solid, and heat is released

38
Q

Describe the reaction of aluminium with steam.

A

Powdered aluminium burns to form a white solid and heat is released

39
Q

Which form does aluminium not react in, and why?

A

Foil form, because the protective layer of aluminium oxide has to be removed by washing with mercury (II) chloride solution

40
Q

Describe the reaction of zinc with steam.

A

Powdered zinc glows to form a yellow solid, which changes to white on cooling, and heat is released.

41
Q

Describe the reaction of iron with steam.

A

Powdered iron glows at red heat forming a black solid

42
Q

Which metals in the reactivity series do not react with water or steam?

A

Copper and metals below it in the reactivity series.

43
Q

Metal + steam –>

A

metal oxide + hydrogen

44
Q

What is the colour of copper, if it is formed as a product in a displacement reaction?

A

Salmon pink

45
Q

What is the colour of copper (II) nitrate solution?

A

Blue

GCSE Chemistry (9 decks)

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