covalent bonds and structures
covalent bonds
non metal and non metal combine by sharing electrons
Gain full outer shell
Strong electrostatic attraction
simple molecular structures with very strong covalent bonds
melting and boiling point is low
giant covalent structures
no charge ions unlike giant ionic latice.
Atoms bonded by strong covalent bonds
Don't conduct electristy
Carbon can form lots of different types of molecules because carbon atoms form up to 4 covalent bonds and easily bond to other carbons to make chains.
Diamond
lustrous and colourless. good for jewllery.
each carbon forms 4 covalent bonds in a very rigid
strong covalent bonds take a lot of energy to break and give diamond a very high melting point
Doesn't conduct electricity
Graphite
black and opaque, but kind of shiny
each carbon forms 3 covalent bonds, creating a sheeth of carbon atoms
Carbon atoms free to slide over eachother. can be rubbed off
High melting point - can conduct electrisity
Graphene - single sheet of graphene. strong covalent bonds. thin sheet.
Fullerenes
different fullerenes contain different numbers of carbon atoms.
Atoms arranged in rings, they have delocalised electrons so conduct electricity
ionic - non metal and metal
non metal - gais electrons to become negative and is anion
metal - loses electrons to become positive and is cation
form regular lattice with strong force of attraction