-Dipole moment:When a molecule has both a positive and negative charge.

-It measures the polarity of the chemical bonds in the mole.

-Occurs when charges are being unequally distributed (one side positive, one side negative).

-Depending on the electronegativity or the shape of the molecule, it can either be polar or nonpolar.

Ex: HCl

*Note: Just because a molecule has polar bonds doesn't necessary mean it results in a dipole moment for example CO₂ <—Since it has a symmetrical shape, the charges cancel out.

-The direction of a molecule goes from the positive side to the negative side

Ex: NaCl

      +—>

-H₂O is always polar.

-Diatomic atoms have no dipole moments because their charges cancel out.

Ex: Br₂, I₂, F₂, Cl₂, O₂, N₂ <— They don’t have dipole moments.

Bader, Dr. Richard F. W.. "Dipole Moments and Polar Bonds." An Introduction to the Electronic Structure of Atoms and Molecules. 1 Jun 2009 <http://www.chemistry.mcmaster.ca/esam/Chapter_7/section_3.html>.                                                                                                            

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