Bonding, structure and properties of matter- part 2 Flashcards
What are the main 3 examples of giant covalent structures?
1) diamond
2) graphite
3) silicon dioxide
What are allotropes of carbon?
1) diamond
2) graphite
3) graphene
4) fullerene
What are properties of diamond?
1) really hard
2) high boiling point
3) doesn’t conduct electricity
What are properties of graphite?
2) are not covalent bonds between layers so they slide over each other- makes graphite soft and slippery
3) high melting point
4) conducts electricity and thermal energy
Why does graphite conduct electricity?
Only three out the four of carbons electrons are used in bonds, so has a delocalised electron which can carry charge
What is graphene and what are its properties?
= one layer of graphite
2) very light
3) conducts electricity
What is fullerene and what is its properties?
= molecules of carbon shaped like closed tubes or hollow balls
1) used to deliver drugs in the body
2) huge surface area
3) good catalysts
What can fullerenes form?
Nanotubes, which can conduct electricity and thermal energy, they have high strength
What is metallic bonding?
Bonding between metals- involving delocalised electrons
Properties of metals (metallic bonding):
1) solid at rooms temperature
2) good conductors of electricity and heat
3) malleable- slide over each other
What is an alloy?
A mixture of two or more metals- they are harder and more powerful than pure metals
How does a gas condensent?
As gas cools, particles no longer have enough energy to overcome the forces of attraction so bonds form
