Dipole moments

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Manali Ghadiali 1E
Posts: 21
Joined: Sat Jul 09, 2016 3:00 am

Dipole moments

Postby Manali Ghadiali 1E » Fri Oct 28, 2016 9:42 pm

How can you identify a dipole moment and how do they relate to polarity?

Caitlin Dillon 3G
Posts: 26
Joined: Wed Sep 21, 2016 2:56 pm

Re: Dipole moments

Postby Caitlin Dillon 3G » Fri Oct 28, 2016 11:41 pm

This is a little difficult to explain through typing. The definition of a dipole moment can be simplified by the equation: the Greek letter mu= Q(magnitude of the charge) x d (distance between those charges). We most likely won't have to show any math for this. However, we must know how to ANALYZE a dipole moment in terms of the molecular structure. For example, draw the dot structure for HCL. so basically draw H-Cl (with 6 electrons surrounding L). Identify the more electronegative element between H and Cl. (Remember electronegativity decreases down a group and increases across a period.) Therefore, Cl is the more electronegative element, which means that the 2 electrons in the single bond will be pulled closer to the Cl. So, chlorine is going to get a little bit more electron density around it (can be represented by a lowercase delta with a partial negative charge) And since H is losing a little bit of electron density, it is partially positive. Since there is UNEQUAL sharing between the electrons, this would represent a POLAR covalent bond. If there was EQUAL sharing (or rather the elements were equal in electronegativity), this would be NONPOLAR!
I hope this helped!

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