Dipole moment

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philipraj_1F
Posts: 52
Joined: Fri Aug 30, 2019 12:16 am

Dipole moment

Postby philipraj_1F » Tue Nov 19, 2019 2:58 pm

How are you supposed to know the difference in electronegativity values in a molecule to tell that there is a dipole moment? And also, if a two atoms typically do not have a dipole moment but the arrangement is asymmetrical, does that cause a dipole moment and for them to be polar?

Hailey Kim 4G
Posts: 110
Joined: Sat Jul 20, 2019 12:16 am

Re: Dipole moment

Postby Hailey Kim 4G » Tue Nov 19, 2019 3:18 pm

The most electronegative elements are located in the upper right-hand corner of the periodic table. So as you move across a row from left to right, electronegativity increases. As you move down a group, electronegativity decreases. When drawing the lewis structure of a molecule, if it is symmetrical, then the molecule is non polar, which means there is no net dipole moment. If it is asymmetrical, then the molecule is polar, which means there is a dipole moment.


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