Chemical Bonding

1. Chemical Bonding • Is an electrostatic force of attraction between atoms that holds them together. • It is the exposed electrons in the outermost shell that are the ones most responsible for an atoms chemical properties, including its bonds with other atoms.

2. Covalent Bond • An electrical attraction in which atoms are held together by their mutual attraction for shared electrons.

3. Ions • Any atom having a net electric charge is an ion. • When an atom either loses or gains electrons it is called an ion. • If electrons are lost, protons outnumber electrons and the ion’s net charge is positive. • If electrons are gained, electrons outnumber protons and ion’s net charge is negative.

4. Metals • The outer electrons of most metals tend to be weakly held to the nucleus. • These electrons are easily dislodged, leaving behind positively charged metal ions (M+) • The electrons that are dislodged flow freely through the metal ions.

5. Metallic Bond • A “fluid” of electrons that hold the positively charged metal ions together. • The outer electrons(-) from the original metal atoms are free to move around between the positive metal ions formed (+).

6. Metallic Bond • These free electrons are the 'electronic glue’ holding the particles together. • There is a strong electrical force of attraction between these free and mobile electrons (-) and the 'immobile' positive metal ions (+) and this is the metallic bond. • The mobility of electrons in a metal accounts for the metals ability to conduct electricity and heat.