Dipole Moment

(Polar molecules, Non-polar molecules, etc.)

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Chloe Orsini 1K
Posts: 32
Joined: Fri Sep 28, 2018 12:18 am

Dipole Moment

Postby Chloe Orsini 1K » Thu Nov 15, 2018 1:39 pm

Will someone please explain what this is and how to determine the size of it, thanks!

klarratt2
Posts: 60
Joined: Fri Sep 28, 2018 12:16 am

Re: Dipole Moment

Postby klarratt2 » Thu Nov 15, 2018 2:28 pm

Dipole moments arise from differences in electronegativity. The larger the difference in electronegativity, the larger the dipole moment. The distance between the charge separation is also a deciding factor into the size of the dipole moment. The dipole moment is a measure of the polarity of the molecule.

When atoms in a molecule share electrons unequally, they create what is called a dipole moment. This occurs when one atom is more electronegative than another, resulting in that atom pulling more tightly on the shared pair of electrons, or when one atom has a lone pair of electrons and the difference of electronegativity vector points in the same way. One of the most common examples is the water molecule, made up of one oxygen atom and two hydrogen atoms. The differences in electronegativity and lone electrons give oxygen a partial negative charge and each hydrogen a partial positive charge.

The equation for a dipole moment is: dipole moment = charge x distance. The dipole moment is measured in debye (D).


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