The Reactivity Series Of Metals

Question 1

Combustion

Answer 1

Burning

Question 2

General equation for a metal burning in oxygen.

Answer 2

Metal + oxygen —-> metal oxide

Question 3

Na + water

Answer 3

It fizzes, flotes, moves, melts and forms a ball, disappears, and a colourless solution forms.

Question 4

K + water

Answer 4

As for sodium +
burns with a lilac flam.
Popping sound at the end

Question 5

Why are these metals stored in oil.

Answer 5

To prevent a reaction with moisture and oxygen in the air.

Question 6

Na and K

Answer 6

Na and K are easily cut and are shiny when freshly cut but they fornish rapidly in air.

Question 7

Reaction of Calcuim with COLD water observations.

Answer 7

Ca sinks and rises
Fizzes
Ca disappears
Test tube warms up
filtrate is a colourless solution

Question 8

Method of magnesium and steam

Answer 8

Heat the mg until it is red hot and the heat the damp mineral wool to convert water into steam.

Question 9

Results of magnesium and steam

Answer 9

Mg burns with a bright white light.
white Ash forms.
Gas burns with a pop

Question 10

General equation for metal and water

Answer 10

Metal + water ——-> metal oxide + hydrogen

Question 11

Whqt happens when u add copper to water

Answer 11

Nothing, copper does not react with water or steam

Question 12

Can u add sodium and potassium to acid?

Answer 12

No, they are too reactive to add to acids.

Question 13

How to tell is hydrogen is present

Answer 13

If u collect the gas and it burns with a pop there is hydrogen.

Question 14

General equation for metal and acid

Answer 14

Metal + acid ——> salt + hydrogen

Question 15

What is salt

Answer 15

Salt is the name of the product of a specific acid and metal.
The name of the salt depends on the acid used.

Question 16

Displacement

Answer 16

Displacement reaction is one which a more reactive metal will displace a less reactive metal from a compound.

A metal can’t displace the same metal compound.

Question 17

Magnesium

Answer 17

Magnesium is more reactive so it displaces the less reactive copper.

Question 18

A more reactive metal will displace a less reactive metal from its compound.

Answer 18

Word equation:
Magnesium + copper (sulfate) —> copper+ Magnesium supfate

Question 19

Observation on mg + copper sulfate

Answer 19

Red brown solid forms.
Grey solid diapers.
Blue solution turns colourless.
Test tube warms up.

Question 20

Poor scientists can make a zoo in China

Answer 20

Potassium
Sodium
Calcium
Magnesium
Aluminium
Zinc
Iron
Copper

Question 21

The reactivity series

Answer 21

Potassium- burn in air to form metal oxide. Reacted with (cold) water to form metal hydroxide (solution) + hydrogen. Reacts dangerously fast with acid.
Sodium- same as potassium.

Calcium- same as potassium.

Magnesium- burns in airbto form metal oxides. Reacts slowly woth water but reacts with steam. Reacts with acids to form a salt + hydrogen.

Aluminium- burns in air to form metal oxides. Reacts with steam to form metal oxide (solid) + hydrogen. Reacts with acids to form salt + hydrogen.

Zinc- metal oxides form slowly. Reacts with steam to form metal oxide (solid) + hydrogen. Reacts with acids to form a salt + hydrogen.
Iron- same ad zinc.

Copper- metal oxids form slowly. Does not react with water or steam. Does not react woth acid

This tells us that potassium is the most reactive and copper is the lest reactive.

Sometimes aluminium is less reactive during our experiments as it is permanently coated in a protective layer of aluminium oxide

Question 22

Word equation for k, Na, & Ca with cold water.

Answer 22

Metal + water —–> metal hydroxide + hydrogen

Question 23

Word equation for Mg, Al, Zn, & Fe with steam

Answer 23

Metal + steam —> metal oxide + hydrogen

Question 24

Most metals, except Cu, rwact with dilute acids to give a salt & hydrogen ( Na K wr don’t do to dangerous)

Answer 24

Metal + acid —-> salt + hydrogen