8.1: Covalent Bonds

Bond formed from atoms sharing electrons

Covalent compounds are called molecules

Ionic compounds are called formula units

Covalent bonds form so that atoms become stable (octet in their valence shell because of the shared electrons)

Covalent compounds form between nonmetals

Diatomic elements are elements in nature that are bonded to themselves

• H₂  N₂   O₂   F₂   Cl₂   Br₂   I₂

A single covalent bond is when one pair of electrons is shared

A double covalent bond is when two pairs of electrons are being shared

A triple covalent bond is when three pairs of electrons are being shared

The strength of covalent bonds depends on the length of a bond, the shorter the stronger

Atomic radius makes the bond length increase

Bond length decreases as the number of bonds increases

Strength increases as the number of bonds between the carbon atoms increase

Bond Dissociation Energy is the amount of energy required to break a specific covalent bond

Bond dissociation energy is always a positive value

Breaking bonds is endothermic

The shorter the bond length the greater the bond dissociation energy