Covalent Bonding

Question 1

What is Covalent Bonding?

Answer 1

The electrostatic attraction between protons in two nuclei and a shared pair of electrons

Question 2

Intermolecular forces require less energy to break than…

Answer 2

Covalent bonds

Question 3

Properties of Fullerene

Answer 3

Simple molecule - 60 carbon atoms in a ball
Low BP/MP - Intermolecular forces are weaker than covalent bonds
Soft and Slippery solid - molecules roll over each other
Electrical insulator - molecules are neutral

Question 4

Properties of Diamond

Answer 4

Very Strong covalent bonds - each carbon atom is joined to 4 other carbon atoms
High MP/BP - Lots of energy needed to break bonds
Hard - Lots of strong bonds
Does not conduct electricity - electrons are stuck

Question 5

Uses of Diamond

Answer 5

Cutting

Question 6

Properties of Graphite

Answer 6

Giant covalent structure - each carbon atoms is joined to 3 other carbon atoms
Hexagonal arrangements of atoms = weak IMFs
High MP/BP - lots of energy needed
Soft and Slippery - consists of layers that can slide over each other
Conducts electricity - one delocalised electron per atom, delocalised electrons move to conduct electricity

Question 7

Uses of graphite

Answer 7

Pencils
Soft lubricant

Question 8

Properties of Silicon Dioxide

Answer 8

Giant covalent structure
High MP/BP - lots of energy needed to break bonds
Hard - network of oxygen atoms
Doesn’t conduct electricity no delocalised electrons
Similar properties to diamond - just less expensive