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WorksheetsGiant covalent structures - Y9
Total questions: 16
Worksheet time: 12mins
What type of structure do diamond and graphite have?
Giant covalent structure
Ionic structure
Simple molecular structure
Metallic structure
How many covalent bonds does each carbon atom form in diamond?
Six
Four
Two
Three
What makes diamond very hard?
Hexagonal layers
Regular tetrahedral network structure
Delocalised electrons
Ionic bonding
Why does diamond not conduct electricity?
Because it is a liquid at room temperature
Because it has no free electrons
Because it has a high melting point
Because it has delocalised electrons
What is the shape of the carbon atoms' arrangement in graphite?
Linear
Cubic
Tetrahedral
Hexagonal rings
Why can graphite conduct electricity?
Because it has a high melting point
Because it has ionic bonds
Because it has delocalised electrons
Because it is a metal
What property makes graphite useful as a lubricant?
Its hardness
Its layers can slide over each other
Its ability to conduct electricity
Its high melting point
How many covalent bonds does each carbon atom form in graphite?
Two
Five
Four
Three
What is a common use for diamond due to its hardness?
In batteries
As a lubricant
For conducting electricity
For cutting tools
What is the main reason graphite is used in electrodes?
Its high melting point
Its hardness
Its ability to conduct electricity
Its slippery nature
What is the structure of Graphene?
Rolled Graphite
Several layers of Diamond
A single layer of Graphite
Graphite with the layers covalently bonded
What gives graphene a high melting point?
(a)
What property make nanotubes different to graphene?
(a)
How many covalent bonds does graphene make?
5
4
2
3
Does diamond conduct electricity?
Yes
No
Name one material with a giant covalent structure, explain how it is used and why its properties help it in this role
