covalent bonding 4.2

when non-metal atoms bond, they share pairs of electrons to get a full outer shell

covalent bonding is the electrostatic attraction between protons in two nuclei and a shared pair of electrons between them

very strong attraction

a small group of atoms held together by covalent bonds

simple molecules contain very strong covent bonds but also weak intermolecular forces between the molecules when simple molecular substances boil it’s the weak IMFs which break

as molecular mass increases, so does the strength of the weak IMFs increasing the boiling point

no as they don’t have charged particles that can move freely molecules are neutral

C60 fullerene composed of sixty carbon atoms low boiling point, but not as low as others as it has a high molecular mass soft and slippery solid as molecules can roll over each other electrical insulator as the molecules are neutral

a pure carbon arranged into a giant lattice every carbon makes 4 covalent bonds tetrahedral shape strong sublimes at a very high temperature

covalent bonds are very strong lots of bonds in the giant lattice lots of energy required to break all the bonds

cutting as it is a hard substance

it cannot conduct electricity as there are no moving particles all the atoms are neutral and the electrons are stuck inside a bond

pure carbon giant lattice layers of hexagons of carbon atoms every carbon makes 3 covalent bonds weak intermolecular forces between layers delocalised electrons inside each layer soft and slippery as layers can slide easy, used as a solid lubricant

• covalent bonds are strong • lots of bonds in the giant lattice • lots of energy is needed to break the bonds

yes as the delocalised electrons can move freely inside the layers

giant covalent structure every Si makes up 4 covalent bonds every O makes up 2 covalent bonds tetrahedral shape strong