Bonding Theories

Molecular shape and overlapping of orbitals

This interaction of atomic orbitals, which gives rise to the molecular orbitals, may also be represented in the form of an orbital (electron) energy diagram

the strongest type of covalent chemical bond. They are formed by head-on overlapping between atomic orbital

 two lobes of an orbital on one atom overlap two lobes of an orbital on another atom and this overlap occurs laterally

 predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms

atomic orbitals fuse to form newly hybridized orbitals, which in turn, influences molecular geometry and bonding properties

non polar molecules share electrons equally

polar molecules share electrons unequally

differ in electronegativity

 atoms in a molecule have substantially different electronegativity: One atom attracts electrons more than another, becoming more negative, while the other atom becomes more positive

Can determine state of matter at a given temperature

Viscosity

Surface tension

The motion of the electron creates a momentary polarization (in both polar and nonpolar covalent bonds)

The strongest of the intramolecular forces