Covalent and Ionic Bonding
Chemical bonding involves the electrons in the outer shells. Whatever type of bonding holds the structure together it is only the outer electrons that are used.
Covalent Bonding:
Non-metallic elements are held together by covalent bonding (elements to the right side of the periodic table).
Covalent bonding can result in simple molecules or giant molecular lattices.
Covalent bonding is driven by the atom wanting to have a full outer electron shell.
The atoms share electrons, the orbital’s overlap, so that both achieve a full outer electron shell and stability.
The bond is formed by the sharing of a pair of electrons between two atoms.
Molecules are formed by atoms joining together by covalent bonds.
Example:Only outer electron shell shown
Ionic Bonding:
A non-metal and a metal are held together by ionic bonding.
In ionic bonding electrons are transferred from one atom to another.
The transfer of electrons results in the formation of positive and negative ions.
The ions are then attracted to each other by electrostatic forces.
Metal atoms lose their outer electrons to become positive ions (cation).
Non-metals gain electrons in their outer shells to become negative ions (anion).
Example:
