Bond energy: is the energy required to break 1 mole of a given bond.
Ionic bond: is an electrostatic force of attraction between oppositely charged ions.
Coulomb’s Law:
Bond length: is the distance between the nuclei of two atoms that are chemically bonded.
Chemical bond: is the energy that holds two atoms together in a compound.
Atoms bond together forming molecules because that decreases their total energy
Covalent bond: Electrostatic force of attraction between nuclei of atoms and shared electrons. The
two atoms may share 1, 2 or 3 pairs of electrons. Electrons are equally shared.
If electrons are not equally shared the bond is called polar covalent.
When the shared electrons are not equally shared the molecule develops a positive center and a
negative center. The molecule develops a dipole or is said to have a dipole moment.
Electronegativity: is a measure of the ability of an atom to attract shared electrons in a covalent bond.
Electronegativity increases across a period and decreases down a group.
Electronegativity difference can be used to identify bond types.
The greater the electronegativity difference, the more polar is the bond.
A molecule is said to be polar if it has dipoles AND the net dipole is not zero.
Isoelectronic ions: are ions that have the same number of electrons.
