S3 - Metals

Question 1

What structure do metals have?

Answer 1

A giant structure.

Question 2

What is metallic bonding?

Answer 2

The strong electrostatic attraction between positive metal ions and delocalised electrons.

Question 3

What are delocalised electrons?

Answer 3

Electrons from the outer shell of metal atoms that are free to move.

Question 4

Why are metals good conductors of electricity?

Answer 4

Because delocalised electrons can move and carry charge.

Question 5

What does the reactivity series show?

Answer 5

The order of how reactive different metals are.

Question 6

How do metals form ions?

Answer 6

By losing electrons to form positive ions.

Question 7

What does a more reactive metal do more easily?

Answer 7

Loses electrons to form positive ions.

Question 8

How can the reactivity series help you predict reactions?

Answer 8

It shows which metals react more easily with substances like water or acid.

Question 9

What determines a metal’s reactivity?

Answer 9

How easily it loses electrons.

Question 10

Name three very reactive metals from the reactivity series.

Answer 10

Potassium, sodium, calcium.

Question 11

Name two metals that are not very reactive.

Answer 11

Copper and silver.

Question 12

What happens when metals react with acids?

Answer 12

They form a salt and hydrogen gas.

Question 13

What does the rate of bubbling (hydrogen) in acid tell you?

Answer 13

How reactive the metal is — faster bubbling = more reactive.

Question 14

What test confirms hydrogen gas is produced?

Answer 14

The burning splint test — makes a squeaky pop.

Question 15

What is the word equation for a metal reacting with water?

Answer 15

Metal + Water → Metal Hydroxide + Hydrogen

Question 16

Which metals react with cold water?

Answer 16

Potassium, sodium, lithium, calcium.

Question 17

Which metals do not react with water?

Answer 17

Zinc, iron, copper.

Question 18

What happens when metals react with oxygen?

Answer 18

They form metal oxides.

Question 19

Do all metals react with oxygen at the same speed?

Answer 19

No — more reactive metals react faster.

Question 20

What is an ore?

Answer 20

A rock that contains enough metal to make extraction worthwhile.

Question 21

How can metals be extracted from their ores?

Answer 21

By reduction with carbon, carbon monoxide, or electrolysis.

Question 22

What does reduction mean in metal extraction?

Answer 22

The removal of oxygen from a metal oxide.

Question 23

What is the word equation for extracting iron using carbon?

Answer 23

Iron(III) oxide + carbon → iron + carbon dioxide

Question 24

What metals can be extracted using carbon?

Answer 24

Metals below carbon in the reactivity series (e.g. zinc, iron, lead).

Question 25

Why can't metals above carbon be extracted using it?

Answer 25

Carbon is not reactive enough to remove the oxygen.

Question 26

How are metals above carbon in the reactivity series extracted?

Answer 26

Using electrolysis.

Question 27

How are unreactive metals like gold found?

Answer 27

As uncombined elements in the Earth’s crust — no extraction needed.

Question 28

What is oxidation?

Answer 28

Loss of electrons (or gain of oxygen).

Question 29

What is reduction?

Answer 29

Gain of electrons (or loss of oxygen).

Question 30

: What is a redox reaction?

Answer 30

A reaction where oxidation and reduction happen at the same time.

Question 31

What does OIL RIG stand for?

Answer 31

Oxidation Is Loss, Reduction Is Gain (of electrons).

Question 32

What is an ion-electron equation?

Answer 32

An equation that shows electrons being lost or gained during a reaction.

Question 33

What is electrolysis?

Answer 33

The splitting up of a compound using electricity.

Question 34

What is an electrolyte?

Answer 34

A molten or dissolved ionic compound that conducts electricity.

Question 35

What happens at the positive electrode (anode)?

Answer 35

Negative ions (anions) are oxidised (lose electrons).

Question 36

What happens at the negative electrode (cathode)?

Answer 36

Positive ions (cations) are reduced (gain electrons).

Question 37

Why must the electrodes be inert?

Answer 37

So they don’t react with the electrolyte.

Question 38

Why should you use d.c. in electrolysis?

Answer 38

So the positive and negative terminals stay the same — clear ion movement.

Question 39

Name two inert electrodes.

Answer 39

Graphite and platinum.

Question 40

What do you use to connect the electrodes to the power supply?

Answer 40

Crocodile clips and wires.

Question 41

Why can’t ionic solids be electrolysed?

Answer 41

The ions are fixed in place and can’t move.

Question 42

Why can molten ionic compounds be electrolysed?

Answer 42

The ions are free to move and carry current.

Question 43

What happens to positive metal ions during electrolysis?

Answer 43

They go to the negative electrode and are reduced (gain electrons).

Question 44

What happens to negative non-metal ions during electrolysis?

Answer 44

They go to the positive electrode and are oxidised (lose electrons).

Question 45

Why is aluminium extracted by electrolysis, not carbon?

Answer 45

It’s too reactive to be reduced by carbon.

Question 46

What is cryolite used for in aluminium extraction?

Answer 46

It lowers the melting point of aluminium oxide.

Question 47

What happens at the negative electrode during aluminium extraction?

Answer 47

Al³⁺ ions gain 3 electrons to form aluminium metal.

Question 48

What happens at the positive electrode during aluminium extraction?

Answer 48

O²⁻ ions lose electrons to form oxygen gas.

Question 49

What is an electrochemical cell?

Answer 49

A device that creates electricity using a chemical reaction between two different metals in an electrolyte.

Question 50

What flows in the wires of an electrochemical cell?

Answer 50

Electrons

Question 51

What flows through the salt bridge?

Answer 51

Ions

Question 52

What is the function of a salt bridge in an electrochemical cell?

Answer 52

It completes the circuit and balances the charges.

Question 53

What type of solution is used in the beakers of an electrochemical cell?

Answer 53

An electrolyte — a solution containing ions of each metal.

Question 54

What should be connected to the electrodes to measure voltage?

Answer 54

A voltmeter.

Question 55

What are the electrodes usually made of in an electrochemical cell?

Answer 55

The metals being tested.

Question 56

What equipment connects the power supply in an experiment?

Answer 56

Crocodile clips and wires.

Question 57

What is the electrochemical series?

Answer 57

A list of metals in order of how easily they form ions.

Question 58

What is needed to produce a voltage in an electrochemical cell?

Answer 58

: A difference in reactivity between the two metals.

Question 59

Which metal is oxidised in an electrochemical cell?

Answer 59

The one higher in the electrochemical series.

Question 60

Which metal is reduced in an electrochemical cell?

Answer 60

The one lower in the electrochemical series.

Question 61

What makes the voltage in a cell greater?

Answer 61

A greater difference in reactivity between the two metals.

Question 62

In which direction do electrons flow in an electrochemical cell?

Answer 62

From the metal higher in the series to the one lower in the series.

Question 63

Why does the more reactive metal lose electrons?

Answer 63

It forms ions more easily — it is oxidised.

Question 64

What happens in the zinc/copper cell? A:

Answer 64

Zinc is oxidised: Zn → Zn²⁺ + 2e⁻ Copper is reduced: Cu²⁺ + 2e⁻ → Cu Overall: Zn + Cu²⁺ → Zn²⁺ + Cu