Unit 2 Topic 1 Reactivity Series

Question 1

Why do metals reacting with air gain mass?

Answer 1

Because they form an oxide

Question 2

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

Answer 2

oxygen

Question 3

When heated in air, potassium

Answer 3

burns with a lilac flame, forming a white solid

Question 4

When heated in air, sodium

Answer 4

burns with a golden yellow flame, forming a white solid

Question 5

When heated in air, calcium

Answer 5

burns with a brick red flame, forming a white solid

Question 6

When heated in air, magnesium

Answer 6

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

Question 7

Aluminium only burns in air when (?)

Answer 7

finely powdered

Question 8

When heated in air, aluminium powder

Answer 8

burns with white sparks, forming a white solid

Question 9

When heated in air, zinc

Answer 9

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

Question 10

Which forms of iron burn/do not burn easily?

Answer 10

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

Question 11

When heated in air, iron

Answer 11

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

Question 12

When heated in air, copper

Answer 12

does not burn, but forms a black solid

Question 13

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

Answer 13

rubbed off

Question 14

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

Answer 14

deflagrating spoon

Question 15

When potassium and sodium are freshly cut,

Answer 15

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

Question 16

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

Answer 16

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

Question 17

Metal + oxygen —>

Answer 17

metal oxide

Question 18

Fe3O4 is a (?)

Answer 18

mixed oxide

Question 19

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

Answer 19

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

Question 20

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

Answer 20

crucible

Question 21

Which form of the metal is usually heated in air?

Answer 21

Powder form

Question 22

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

Answer 22

To allow more air into the crucible

Question 23

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

Answer 23

Labels:

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

Question 24

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

Answer 24

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.

Question 25

Describe the reaction of potassium with water.

Answer 25

``` 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 ```

Question 26

Describe the reaction of sodium with water.

Answer 26

``` 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 ```

Question 27

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

Answer 27

Solution changes universal indicator from green to blue.

Question 28

Describe the reaction of calcium with water.

Answer 28

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

Question 29

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

Answer 29

no reaction, rust

Question 30

Describe the reaction of magnesium with water.

Answer 30

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

Question 31

Why are potassium and sodium stored under oil?

Answer 31

To prevent reaction with oxygen and moisture in the air

Question 32

Metal + water -->

Answer 32

metal hydroxide + hydrogen

Question 33

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

Answer 33

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.

Question 34

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

Answer 34

Labels: - beaker - water - filter funnel - boiling tube - hydrogen - calcium/metal

Question 35

How do you test that hydrogen is produced?

Answer 35

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

Question 36

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

Answer 36

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

Question 37

Describe the reaction of magnesium with steam.

Answer 37

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

Question 38

Describe the reaction of aluminium with steam.

Answer 38

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

Question 39

Which form does aluminium not react in, and why?

Answer 39

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

Question 40

Describe the reaction of zinc with steam.

Answer 40

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

Question 41

Describe the reaction of iron with steam.

Answer 41

Powdered iron glows at red heat forming a black solid

Question 42

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

Answer 42

Copper and metals below it in the reactivity series.

Question 43

Metal + steam -->

Answer 43

metal oxide + hydrogen

Question 44

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

Answer 44

Salmon pink

Question 45

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

Answer 45

Blue