Types of Bonding
Ionic Bonding
occur between Metals and non-metals
They have an incomplete outer shell and are therefore unstable
electrons are transferred between from metal to non-metal
the positive and negative ions are attracted to each other
E.g. Sodium has 1 electron in its outer shell, it therefore loses one electron so its outer shell is full, and is now positive
When electrons are lost the ion becomes positive and when electrons are gained the ion becomes negative
- write down the elements symbols
- write down the charges for each element
- Swap and drop each elements charges
They cannot conduct electricity, They are hard but brittle
They form a lattice structure
When melted the ions can move freely
When dissolved it can carry energy
Metallic Bonding
Covalent Bonding
Metallic bonding is between metals only
The metal atoms lose their outer electrons to form metal ions
The electrons from all the metal atoms form a 'sea' of electrons that can flow around the metal
They conduct electricity
Generally high melting and boiling points
They are strong but not brittle
malleable, ductile, lustre and opaque
The bonds are very strong and takes a lot of energy to brake
It is only between two non-metal atoms
they usually only need 1 or 2 electrons to fill their outer shell
they cant from a bond by transferring and only sharing
They have low melting points and boiling points
the bonds in the molecule are strong but are weak between other molecules
They use the swap and drop method
They are liquids or gasses at room temperature
if it is solid it is quite brittle
cannot conduct electricity
they are written from left to right on the periodic table
Mono=1, Di=2, Tri=3, Tetra=4, Penta=5, Hexa=6, Hepta=7, Octa=8, Nona=9, Deca=10