Structure And Bonding

Question 1

What forms ionic bonds?

Answer 1

Metals and non metals

Question 2

What forms simple molecular bonds?

Answer 2

Most nonmetals with other nonmetals

Question 3

3 examples giant covalent structures?

Answer 3

Graphite, diamond and SiO2

Question 4

What forms metalling bonds?

Answer 4

Metals on their own

Question 5

Properties of ionic bonds?

Answer 5

• High MP + BP

- Conducts electricity as liquid/solution but not as solid

Question 6

Properties of simple covalent bonds?

Answer 6

• Low MP + BP

- Does not conduct electricity

Question 7

Properties of giant covalent structures?

Answer 7

• High MP + BP
• Does not conduct electricity
• Graphite is soft/malleable

Question 8

Properties of metallic structures?

Answer 8

• High MP + BP
• Conducts electricity
• Malleable

Question 9

How do ionic bonds form?

Answer 9

Atoms gain or lose electrons to form charged ions with noble gas structures

Question 10

Why do ionic structures conduct electricity as a liquid/solution but not as a solid?

Answer 10

Because as a solid neither electrons nor ions are free to move about.
When dissolved in water ions are free to move around

Question 11

What particles carry electric charge?

Answer 11

Electrons or ions

Question 12

How to simple molecular bonds form?

Answer 12

Atoms share electrons in covalent bonds to get the noble gas electronic structure

Question 13

Why do simple molecular structure not conduct electricity?

Answer 13

There are no free electrons

Molecules are not charged

Question 14

What is present between molecules in a simple molecular structure?

Answer 14

A weak inter molecular force

Question 15

In an ionic bond what attracts the ions together?

Answer 15

Strong electrostatic attraction

Question 16

What holds atoms together in a giant covalent structure?

Answer 16

Very strong covalent bonds between atoms

Question 17

How does a giant covalent structure form?

Answer 17

Atoms share electrons in covalent bonds to form a giant covalent lattice

Question 18

How is graphite an exception of giant covalent structures?

Explain it’s properties

Answer 18

It conducts electricity because it only forms 3 covalent bonds there is an extra electron that is delocalised and can conduct electricity.

It is malleable because there is a weak bonding between layers, allowing them to slide

Question 19

How do metallic bonds form?

Answer 19

Metal atoms achieve a full outer shell of electrons by losing their outer electrons to a ‘sea’ of delocalised electrons.

Question 20

Why can metals conduct electricity?

Answer 20

Because delocalised electrons are free to move and carry electricity

Question 21

How are things in metals held together?

Answer 21

There is a strong electrostatic attraction between the positive ion and the sea of negative electrons

Question 22

Why is metal soft?

Answer 22

Layers are able to slide over each other

Question 23

What is an allotrope?

Answer 23

When an element exists in several different forms of the same state.

Question 24

Practice drawing a diamond and graphite structure

Answer 24

K

Question 25

What is the loss of electrons called?

What is the gain of electrons called?

Answer 25

Loss of electrons = oxidisation

Gain of electrons = reduction

Question 26

What’s the relationship between ionic charge and the MP and BP of an ionic compound ?

Answer 26

The higher the charge the higher the MP and BP

Because there is a stronger electrostatic attraction

Question 27

What is the attraction between the atoms in a simple molecular structure?

Answer 27

An attraction between the positive nuclei and the negative electrons

Question 28

What is an electrical current?

Answer 28

The flow of charges through a conducting substance

Question 29

What is the relative mass of a proton, neutron and electron?

Answer 29

Proton - 1
Neutron - 1
Electron - 1/2000

Question 30

What is the charge of a proton, neutron and electron?

Answer 30

Proton +1
Neutron 0
Electron -1