Structure and Bonding

Question 1

What general properties do metals have

Answer 1

Conduct electricity
Shiny
Malleable

Question 2

What general properties do most non-metals have

Answer 2

Don’t conduct heat + electricity (insulators)
Weak (brittle)
Dull colour

Question 3

What type of elements are involved in Ionic bonding

Answer 3

Metal + non-metal

Question 4

What type of elements are involved in covalent bonding

Answer 4

Non-metal + non-metal

Question 5

What type of elements are involved in metallic bonding

Answer 5

Metal + Metal

Question 6

Covalent bonds =……….

Answer 6

Strong

Question 7

Describe simple molecular bonds

Answer 7

Non metal + non metal
Strong covalent bonds within molecules
Weak intermolecular forces that requires little energy to break

Question 8

What is a covalent bond

Answer 8

The electrostatic attraction between the positive nuclei and the shared pair of electrons

Question 9

Are covalent binds weak or strong

Answer 9

They’re strong because of the strong electrostatic attraction

Question 10

Do simple molecular structures conduct electricity

Answer 10

No - they don’t have a sea of delocalised electrons

It’s an insulator

Question 11

Why does the melting points of a substance with simple molecular bonds increase

Answer 11

As the molecules get bigger, there are more intermolecular forces, so more energy required to overcome them

Question 12

Describe giant covalent structures

Answer 12

Strong covalent bonds

Question 13

Do giant covalent structures conduct electricity

Answer 13

No, they don’t have a sea of delocalised electrons, except GRAPHITE!

Question 14

Why does diamond have a high melting point

Answer 14

Because of it’s giant covalent structure
With many strong covalent bonds
Which require a lot of energy to overcome

Question 15

Describe a Giant Ionic structure

Answer 15

Strong ionic bonds
Positive cations
Negative anions
Giant 3D lattice

Question 16

How and why do ions form

Answer 16

Metal atoms loose electrons to become positive ions with full outer shells

Non-metal atoms gain electrons to become negative ions with full outer shells

Question 17

Describe the structure of ionic materials

Answer 17

Giant 3D lattice

Question 18

Why do solid ionic substances not conduct electricity

Answer 18

No delocalised electrons and the ions can’t move

Question 19

When do ionic substances conduct electricity

Answer 19

When in a liquid state - ions can move

Question 20

Why do ionic compounds have high melting points

Answer 20

Strong electrostatic forces between oppositely charged ions that require a lot of energy to break

Question 21

Why does MgO have a higher melting point than NaCl

Answer 21

Magnesium oxide is 2+ 1- and NaCl is 1+ 1-. So MgO has a higher attraction so more energy is needed to overcome this

Question 22

Describe giant metallic structures

Answer 22

Strong electrostatic attraction between ions
Sea of delocalised electrons
Layers of atoms which can slide over each other
Malleable
Ductile

Question 23

Describe the structure of metals

Answer 23

Layers of positive cations surrounded by a sea of delocalised electrons

Question 24

What is metallic bonding

Answer 24

The strong electrostatic attraction between positive metal ions and a sea of delocalised electrons

Question 25

Why do metallic structures have high melting points

Answer 25

Lots of strong metallic bonds that require a lot of energy to overcome

Question 26

Why are alloys not as malleable as pure metals

Answer 26

It districts the layers, they can no longer slide over each other

Question 27

What is diamond used for

Answer 27

Drilling

Question 28

Whats an allotrope

Answer 28

Atoms of the same element arranged in different ways

Question 29

Due to the sliding layers, what can graphite be used for

Answer 29

A lubricant

Question 30

In graphite, there are delocalised electrons between the layers, what does this do

Answer 30

Conducts electricity

Not a metal