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Dipole Moment

Posted: Sun Nov 10, 2019 11:06 pm
by Tracy Tolentino_2E
How do we know if a molecule has a dipole moment? And why does the arrow have to point to the lowercase delta positive?

Re: Dipole Moment

Posted: Sun Nov 10, 2019 11:08 pm
by Alex Tchekanov Dis 2k
You know a molecule has a dipole moment when there is an unequal sharing of the electron. The dipole moment is larger when the difference in electronegativity is greater. The reason why the arrow points towards the partially charged atom is because that is the direction that the electron is being pulled towards.

Re: Dipole Moment

Posted: Sun Nov 10, 2019 11:13 pm
by Eesha Sohail 1D
Aren't van der Waals interactions still technically dipoles, just not permanent ones? I've seen them referred to as instantaneous dipoles. Also just to clarify, would the C=O bond be able to produce a dipole moment?

Re: Dipole Moment

Posted: Mon Nov 11, 2019 10:43 am
by Trent Yamamoto 2J
I believe you can also recognize a dipole moment when there is a polar covalent bond, which by definition is when electrons in a covalent bond are not equally shared.

Re: Dipole Moment

Posted: Mon Nov 11, 2019 3:43 pm
by Kelsey Ash 1D
You know there is a dipole moment when there is an unequal sharing of electrons among atoms. The arrow always points in the direction in which the electron os being pulled.

Re: Dipole Moment

Posted: Mon Nov 11, 2019 5:48 pm
by Ashley Fang 2G
To add to that, the arrow always points to the lowercase delta negative sign, and a line strikes through the arrow at the lowercase delta positive sign (making a cross or a "+" to help you remember it)

Re: Dipole Moment

Posted: Tue Nov 12, 2019 3:58 pm
by EricZhao3G
A molecule has a dipole moment if there is an unequal sharing of electrons. The arrow points towards the delta negative not delta positive since that is where the electron is being pulled towards.