Covalent Structures

Question 1

Why is graphite a good conductor and slippy

Answer 1

Graphite is a good conductor because the carbon atoms only bond to three other carbons This allows for one delocalised electron which can move throughout the lattice causing charge and current. The electrons can move throughout the layers in between the graphite. Graphite is soft because it is arranged in layers the intermolecular forces between the layers are weak which makes it soft. These layers can slide over each other easily which is also why it is so slippery.

Question 2

What are giant covalent structures

Answer 2

Big covalent structures

Question 3

Why is amonia a gas at room temperature

Answer 3

This is beacuse of the weak intermolecular forces between molecules. it has a simple structure. The weak forces are easy to break with little energy.

Question 4

What is an allotrope

Answer 4

The same element in the same state in a different structure

Question 5

Structure

Diamond

Answer 5

Bonde to 4 carbons
Cant conduct electricity
Very strong
High melting point

Question 6

Structure

Graphite

Answer 6

bonded to 3 carbon atoms
Weak between layers as they slide over each other
High melting point
A single layer is graphene

Question 7

Differences between intermolecular and intramolecular forces

Answer 7

intermolecular forces are between molecules in simple covalent structures. They are quite weak.
Intramolecular forces are between ionic and covalent bonds

Question 8

How to calculate surface area of a cube

Answer 8

6 sides x side length squared