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Dipole Moment

Posted: Tue Nov 14, 2017 3:19 pm
by Jessica Lutz 2E
I'm confused on how you can tell which direction the dipole moments of each atom in a molecule go. Can anyone clarify that concept?

Re: Dipole Moment

Posted: Tue Nov 14, 2017 3:40 pm
by Hyein Cha 2I
The element with higher electronegativity (higher pull for electrons) will have negative sign, and the element with lower electronegativity (less pull for electrons) will have positive sign. It makes sense, because if you want 'negative' more strongly, you will have partially negative sign. For example, in a water molecule, H2O, Oxygen has higher electronegativity, thus has a partial negative charge, whereas Hydrogen has partial positive charge.

Re: Dipole Moment

Posted: Wed Nov 15, 2017 11:46 am
by Jingyi Li 2C
The more electronegative atom will have a partial negative charge, and the less electronegative atom will have an equal but partial positive charge. When we draw an arrow to represent this, we draw it from the positive charge pointing to the negative charge (δ+ to δ-).

Re: Dipole Moment

Posted: Wed Nov 15, 2017 12:35 pm
by Amy Zheng 2l
Its from the less electronegative atom to the more electronegative atom. So arrow goes from + ---> -