Structure and Bonding

- Were atoms give or receive electrons to complete outer shells- This results in them having an overall charge, thus they become ions.- They then become attracted to one another as they have opposite charges.- Forming Ionic Bonds.

- Were atoms share electrons to complete outer shells.- Then all the atoms are happy as they have full outer shells.

- Closely packed regular lattice arrangement-Very strong Chemical bonds between all the ions.- Don't melt easily (high melting/boiling points.)- Dissolve in solution to conduct electricity- Conduct electricity when molten.

- Very strong Covalent bond molecules- Forces of attraction between molecules is weak.- Low melting/boiling points- Don't conduct electricity

- No charge ions-Strong Covalent bonds between all atoms- High melting/boiling points- Don't conduct electricity (usually.)- Insoluble in water

- Each carbon atom has four Covalent bonds- Rigid giant Covalent structure- Hardest natural substance

- Each carbon has three Covalent bonds.- Layers of atoms that slide over one another- Can easily be slid of one another (pencil)- Free electrons = conduct electricity.

-Giant structure of Silicon and Oxygen- What sand is made of-Melted down to make glass.

- Giant Structure- Metallic bonds = free electrons from outer shells of all the metal atoms- Free to move = conduct heat and electricity- Electrons hold atoms together in regular structure- Make metals malleable.