C2.3 Flashcards
Why can carbon form many compounds?
Is in group 4 so 4 electrons in the outer shell and can form four covalent bonds
What is an allotrope?
Different forms of an element in the same state but with different atomic arrangements
What is diamond like?
Transparent
Very hard as covalent bonds are very strong
High melting point
Doesn’t conduct electricity (no delocalised electrons)
Giant covalent structure, each carbon atom is covalently bonded to 4 other carbon atoms
What is graphite like?
Grey-black
Soft
Giant covalent structure, each carbon atoms is covalently bonded to 3 other carbon atoms so one electron is not involved in bonding and becomes delocalised instead
Conducts electricity
What is the structure of graphite?
Layered structure
Many covalent bonds so high melting point, but forces between each layer are weak so layers slide over each other
Is slippery
What is graphene like?
Resembles a single layer of graphite
Almost transparent
Extremely strong
Conducts electricity
What is fullerene like?
Group of carbon allotropes that consist of molecules that form hollow tubes
Usually made up of carbon atoms arranged in hexagons
Huge SA
Useful catalysts
What is buckminsterfullerene?
First fullerene to be discovered
What happens when substances change state?
Forces of attraction are overcome
Bonds either form or break
What makes a metal malleable?
Even though their metallic forces are strong, the layers of metal ions slide over one another
Why are covalent structures and ionic compounds brittle?
They have strong forces of attraction ionic/covalent so the when a force is exerted the bonds break
Why do ionic compounds only conduct electricity in molten form?
As the ions in a solid aren’t feee to move around but when dissolved or molten they are
What is a nanoparticles
A particle between 1nm - 100nm
Risks of nanoparticles?
So small they may be breathed or absorbed by the skin or pass into cells
Take a long time to break down
Toxic substances may stick to their surface
