2. Bonding, Structure and the Properties of matter (Ions, Ionic and Metallic Bonding)

Question 1

What are ions?

Answer 1

Ions are charged particles due to the loss or gain of electrons

Question 2

What are positive ions called?

Answer 2

Cations

Question 3

What are negative ions called?

Answer 3

Anions

Question 4

How are positive ions formed?

Answer 4

When an atom loses electrons, which are negatively charged, the overall charge becomes positive

Question 5

How are negative ions formed?

Answer 5

When an atom gains electrons, which are negatively charged, so the overall charge becomes negative

Question 6

What ions do Group 1 atoms form?

Answer 6

+1 ions

Question 7

What ions do Group 7 atoms form?

Answer 7

1-

Question 8

What ions do Group 2 atoms form?

Answer 8

2+

Question 9

What ions do Group 6 atoms form?

Answer 9

2-

Question 10

What are group 7 ions called?

Answer 10

Halide ions

Question 11

What is an ionic bond?

Answer 11

The strong electrostatic force of attraction between a positively charged ion and a negatively charged ion between a metal and non-metal

Question 12

What is ionic bonding between?

Answer 12

A metal and a non-metal

Question 13

What does ionic bonding involve?

Answer 13

The transferring of electrons

Question 14

Explain how an Ionic bond works?

Answer 14

1. In order to gain a full outer shell, the metal will transfer electrons to the non-metal
2. The metal now has a full outer shell and a positive charge, the non-metal has gained electrons and will also have a full outer shell but now has a negative charge
3. Now as the ions are oppositiely charged, they are attracted to one another, hence an ionic bond

Question 15

What does the dot and cross model show?

Answer 15

The transferring of electrons

Question 16

What structure will ionic bonds form?

Answer 16

A lattice structure

Question 17

What is a lattice structure?

Answer 17

A regular repeating pattern

Question 18

What is an electrostatic force of attraction?

Answer 18

The force between unlike charges

Question 19

What ions are bigger than the other in a lattice structure?

Answer 19

The negative ions are bigger than positive ions

Question 20

What are the properties of ionic compounds?

Answer 20

• They have high melting and boiling points
• They cannot conduct electricity in solid form, they must be in molten or aqueous form

Question 21

Why do ionic bonds have high melting and boiling points?

Answer 21

Due to the strong electrostatic force of attraction between the positive and negative ions, which requires a lot of energy to overcome

Question 22

Why can’t ionic bonds conduct electricity in solid form and only molten/aqueous?

Answer 22

• the ions are not free to move in a solid form
• so must be in a molten or aqueous form so that the ions are free to move
• and are able to carry an electrical charge

Question 23

What does molten mean?

Answer 23

Liquid (has been melted)

Question 24

What does aqueous mean?

Answer 24

dissolved in water

Question 25

Why can't solid ionic compounds conduct electricty?

Answer 25

- The strong electrostatic forces of attraction between oppositely charged ions arranged in a regular lattice structure - means that they are in fixed positions so are unable to move - so they can't carry a charge - so cannot conduct electricty

Question 26

Why can molten/aqueous ionic compounds conduct electricty?

Answer 26

- an aqueous ionic compound means the ionic compound has been dissolved into a solution - Molten means that heat has been applied to melt the ionic compound and overcome the electrostatic forces of attraction - so the ions are free to move - so can carry an electrical charge - so can conduct electricty

Question 27

What is metallic bonding?

Answer 27

The electrostatic attraction between positively charged metal ions and negatively charged electrons in a lattice structure

Question 28

Why are metallic bonds arranged in a lattice structure?

Answer 28

Due to the strong electrostatic force of attraction between the positive metal ions and the sea of delocalised electrons

Question 29

What are the properties of metals? (4)

Answer 29

- High melting and boiling points - Good conductors of electricty - Malleable - Ductile

Question 30

Why do metals have high melting and boiling points?

Answer 30

Because a lot of energy is required to overcome the strong electrostatic force of attraction

Question 31

Why are metals good conductors of electricity?

Answer 31

- As the delocalised electrons are free to move - so can carry an electrical charge - through the metal structure

Question 32

What does malleable mean?

Answer 32

Able to be moulded / bent into shape

Question 33

Why are metals malleable?

Answer 33

Because the regular layers means the layers can slide over each other easily when force is applied

Question 34

What does ductile mean?

Answer 34

Able to be drawn into wires

Question 35

What are alloys?

Answer 35

A mixture of 2 or more metals

Question 36

Why are alloys harder than regular metals?

Answer 36

- Because they are a mix of different metals, which have different shapes and sizes, so distort the regular layers of the pure metal - So is harder for the layers to slide over each other, so are less malleable, therefore harder