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Dipole moments

Posted: Sun Nov 10, 2019 1:46 pm
by Ghadir Seder 1G
When a molecule has "dipole moments" is that referring to the fact that one atom is more electronegative than the other thus leading the electrons to attract to the more electronegative atom? When drawing these structures, do the arrows represent this idea? Or do they represent something else?

Re: Dipole moments

Posted: Sun Nov 10, 2019 1:50 pm
by Christine Honda 2I
Yes, dipole moments is referring to the fact that one atom is more electronegative. The larger the difference in electronegativity, the larger the dipole moment. It is conventional to draw a dipole moment arrow from positive to negative.

Re: Dipole moments

Posted: Sun Nov 10, 2019 1:52 pm
by Ada Chung 1C
Yes, you are correct think about it in terms of the electron cloud and the polarizability of the molecule.

Re: Dipole moments

Posted: Sun Nov 10, 2019 1:55 pm
by JohnWalkiewicz2J
Yes, typically a molecule will have dipole moments if the electronegativity diffence between the two atoms are between 0.4-1.7. The arrows illustrate the direction in which the dipole moments occur. For instance, in a H-O bond, the arrow will be pointing towards the oxygen atom as it is more electronegative and is partially negative. Hope this helps!