Dipole Moment

[philipraj_1F]

What difference in electronegativity values is needed for a dipole moment and how do you calculate this difference if we are not given an electronegativity chart?

[Sophia Shaka 3L]

You know electronegativity trends from the periodic table, so unless you want the exact numerical value, you can just follow the trend. The larger the difference in electronegativity, the larger the dipole moment. Polar molecules have permanent dipole moments, and nonpolar molecules can have induced dipole moments.

[Jielena_Bragasin2G]

You can find the polarity of a molecule using the lewis structures and VSEPR models.

[Natalie Benitez 1E]

How do we tell there is a major difference in electronegativity to cause dipole-moments? Is there a specific range or even an electronegativity chart being given?

[Katherine Brenner 3H]

Can an individual molecule be dipole- dipole. Or would we just say that this is a dipole moment within 1 molecule?

[Sion Hwang 4D]

Can an individual molecule be dipole- dipole. Or would we just say that this is a dipole moment within 1 molecule?

An individual molecule will only have a dipole moment. Dipole-dipole interaction can only occur between two molecules. This is because dipole-dipole is an intermolecular force, not an intermolecular force.

[Daniel Yu 1E]

Dipole-Dipole is a describing two molecules, each with an individual dipole, interacting. Thus it is an intermolecular force. A dipole itself is a separation of charge in a molecule, resulting from an uneven distribution of electrons.

[April Pazos 3D]

The difference in electronegativities dictates the size of the dipole moment.

[Merin Padayatty 3G]

The periodic table provides a general trend of electronegativity, and you can determine whether a molecule has a dipole moment and is polar from the shape using the VSEPR model.

[Katherine Brenner 3H]

Does Dipole Moments indicate polarity also?

[Emily_4B]

Does Dipole Moments indicate polarity also?

Yes if dipole moments do not cancel out then the molecule is polar