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Dipole moments

Posted: Sun Nov 03, 2019 1:45 pm
by Matt Sanruk 2H
So the dipole moments translate whether or not the molecule is covalent, ionic, or polar?

Re: Dipole moments

Posted: Sun Nov 03, 2019 2:00 pm
by John Arambulo 1I
A molecule will always be covalent because it is covalently bonded. The dipole moment determines whether the covalent bond has ionic or covalent character because of the charge difference. If there is a dipole moment, it is a polar covalent bond, and as a result of the partial positive and partial negative regions, it has ionic character.

Re: Dipole moments

Posted: Sun Nov 03, 2019 2:03 pm
by Anokhi Patel 2B
How do we determine whether to place a positive or negative dipole moment in the Lewis structure and where to place them?

Re: Dipole moments

Posted: Sun Nov 03, 2019 2:13 pm
by Matt Sanruk 2H
John Arambulo 1I wrote:A molecule will always be covalent because it is covalently bonded. The dipole moment determines whether the covalent bond has ionic or covalent character because of the charge difference. If there is a dipole moment, it is a polar covalent bond, and as a result of the partial positive and partial negative regions, it has ionic character.


Ah I see that makes more sense, its just less covalent

Re: Dipole moments

Posted: Sun Nov 03, 2019 2:30 pm
by TimVintsDis4L
The dipole moment also tells us about the charge. The bigger the difference in electronegativity, the larger the charge and vice versa.

Re: Dipole moments

Posted: Sun Nov 03, 2019 2:45 pm
by Sally Qiu 2E
a dipole moment occurs when atoms in a molecule share electrons unequally. this means there's a difference in electronegativity, and this creates partially negative and positive regions which gives the molecule ionic character