Covalent Bonds

It involves the sharing of electron pairs between two atoms.

It occurs when metals bond to each other.

It results from the transfer of electrons from one atom to another.

It only occurs in ionic compounds.

Nonpolar covalent

Polar covalent

Ionic

Metallic

Electrons are shared equally between atoms.

The negative charge is distributed evenly.

Examples include hexane and oil.

Poles of positive and negative charges form at each atom.

It increases to its highest value

It stays the same

It is at its lowest

It fluctuates randomly

Bond length is the distance at maximum potential energy between two atoms.

Bond energy is the energy released when a bond forms.

Atoms release energy as they change from individual atoms to a molecule.

Bond length is the distance between two bonded atoms at their minimum potential energy.

Lone pairs

Bonding pairs

Valence electrons

Core electrons

Add valence electrons, arrange atoms, add unshared pairs, count electrons

Arrange atoms, add unshared pairs, count electrons, add valence electrons

Add unshared pairs, add valence electrons, arrange atoms, count electrons

Count electrons, arrange atoms, add valence electrons, add unshared pairs

Double and triple bonds have higher bond energies than single bonds.

Single bonds have higher bond energies than double bonds.

Triple bonds have longer bond lengths than single bonds.

Double bonds are weaker than single bonds.

They result from the sharing of electron pairs between two atoms.

They occur when metals bond to nonmetals.

They involve the transfer of electrons from one atom to another.

They only occur in ionic compounds.