Chemistry in Society

Question 1

Where are most naturally-occurring metals found?

Answer 1

Inside rocks — called ores

Question 2

Where are newer metals made?

Answer 2

Inside reactors.

Question 3

Can Au make compounds and why?

Answer 3

No, because it is too unreactive.

Question 4

Give examples of naturally occurring metals.

Answer 4

Gold (Au)

Silver (Ag)

Magnesium (Mg)

Question 5

Give examples of metals that are not naturally occurring.

Answer 5

Copernicium (Cn)

Nihonium (Nh)

Flerovium (Fl)

Question 6

What is a metallic bond?

Answer 6

A metallic bond is an electrostatic force of attraction between positive nuclei (ions) and delocalised electrons.

Question 7

What is the structure of a metal?

Answer 7

A metallic lattice

Question 8

Why are the electrons in a metal, delocalised?

Answer 8

The atoms are so close that the electrons are attracted to many ions, allowing them to move freely through the lattice.

Question 9

Give some examples of metallic properties.

Answer 9

conductors of heat

conductors of electricity

malleable

high mpt/bpt

Question 10

Why can metals conduct electricity?

Answer 10

Because of delocalised electrons moving through the lattice

Question 11

What is the general equation of a metal reacting with oxygen?

Answer 11

metal + oxygen → metal oxide

Question 12

Give examples of metal reacting with oxygen.

Answer 12

eg 1: 2Mg + O₂ → 2MgO

eg 2: 4Al + 3O₂ → 2Al₂O₃

Question 13

What is the general equation of a metal reacting with water?

Answer 13

metal + water → metal hydroxide + hydrogen

Question 14

Give examples of metals reacting with water.

Answer 14

eg 1: 2Na + 2H₂O → 2NaOH + H₂

eg 2: Ca + 2H₂O → Ca²⁺(OH⁻⁻)₂ + H₂

Question 15

What is the general equation of a metal reacting with acid?

Answer 15

metal + acid → salt + hydrogen

Question 16

Give examples of a metal reacting with acid.

Answer 16

eg 1: Li + HCl → LiCl + H₂

eg 2: Zn + HNO₃ → Zn(NO₃)₂ + H₂

Question 17

State the reactivity series (school metals).

Answer 17

K, Na, Li, Ca

Mg, Al, Zn, Fe, Sn

Cu, Ag

Au

Question 18

What are the three ways to separate metals from their compounds?

Answer 18

• electrolysis: for most reactive metals
• heat + CO/C: for metals in the middle of reactivity series
• heat: metals of low reactivity

Question 19

Why does a DC supply need to be used for electrolysis?

Answer 19

Allows the products to be identified.

Question 20

Give the equation for CuCl₂ being separated using electrolysis.

Answer 20

Cu²⁺(Cl⁻⁻)₂ → Cu + Cl₂

Question 21

How do you know where to add electrons in an ion-electron equation?

Answer 21

To whichever side is more positive.

Question 22

If electrons are added to the left in an ion-electron equation, what is that called?

Answer 22

Reduction.

Question 23

If electrons are added to the right in an ion-electron equation, what is that called?

Answer 23

Oxidation.

Question 24

Give the ion-electron equation for Al.

Answer 24

Al³⁺ + 3e⁻⁻ → Al

Question 25

Give the ion-electron equation for O.

Answer 25

2O²⁻⁻ → O₂ + 4e⁻⁻

Question 26

Which metals need electrolysis to be separated?

Answer 26

K, Na, Li, Ca, Mg, Al.

Question 27

Which metals need heat + C(O) to be separated?

Answer 27

Zn, Fe, Sn, Pb, Cu.

Question 28

Give the equation for the separation of copper(II) oxide.

Answer 28

CuO + C → Cu + CO₂

Question 29

Give the ionic equation for the separation of mercury oxide.

Answer 29

Hg²⁻⁻O²⁻⁻ → Hg + O₂

Question 30

Which metals need heat alone to be separated?

Answer 30

Hg and Ag