Chem Topic 2: Bonding

Question 1

What are the three types of bonding in chemistry

Answer 1

Ionic
Covalent
Metallic

Question 2

What is ionic bonding

Answer 2

Non metal + metal

e.g. Sodium + chlorine

Question 3

Ionic bonding involves what happening to electrons

Answer 3

Metal donates electron(s) to the non metal

Question 4

Covalent bonding involves

Answer 4

Two or more non metals

Share electrons

Question 5

What is Metallic bonding

Answer 5

Bonding seen in metals
Layer of metal ions (positive)
Delocalised electrons
Electrostatic forces keep these together

Question 6

Why are metals solid at room temperature

Answer 6

• Strong electrostatic forces of attraction between positive metal ion + negative electron
• Require high amount of heat energy to overcome these strong bonds

Question 7

Describe the ionic bonding between Sodium (Na) + Chlorine (Cl) (3 marks)

Answer 7

1. Sodium donates 1 electron to chlorine
2. Sodium becomes +ve and chlorine becomes -ve
3. This creates a strong electrostatic force between the positive metal ion and negative non-metal ion

Question 8

Why are ionic compounds solid at room temperature (3 marks)

Answer 8

1. Due to strong electrostatic forces of attraction
2. Positive metal ion and the negative non-metal
3. Therefore a large amount of heat energy is required to overcome these strong forces

Question 9

What is the force called that can be seen between two oppositely charged particles

Answer 9

Electrostatic forces of attraction

Question 10

Electrostatic forces of attraction can only be found in two types of bonding

Answer 10

1. Ionic

2. Metallic

Question 11

What is an alloy

Answer 11

Mixture of metals

Question 12

Why can alloys not be bent into different shapes as easily as pure metals

Answer 12

Because the different atoms disrupt the regular layers

This means that the atoms cannot slide over each other as easily

Question 13

What are some properties of diamond

Answer 13

Solid at room temp - strong covalent bonds
High melting + boiling- strong covalent bonds
Poor conductors of electricity

Question 14

What are the properties of graphite

Answer 14

High melting + high boiling point (solid at room) - strong covalent bonds

Good conductor of electricity- free electrons

Question 15

What are the properties of silicon dioxide (sand)

Answer 15

Solid at room temp - strong covalent bonds
High melting + boiling- strong covalent bonds
Poor conductors of electricity

Question 16

Why are silicon dioxide, graphite and diamond solid at room temp/have a high melting and boiling point

Answer 16

Strong covalent bonds