Problem: The molecules BF3, CF4, CO2, PF5, and SF6 are all nonpolar, even though they all contain polar bonds. Why?

FREE Expert Solution

A nonpolar molecule does not have a permanent dipole moment. For a molecule to not have  a permanent dipole moment, the individual dipole moments of its bonds must cancel out.

(a) BF3 : Boron (EN = 2.04) goes in the center since boron is less electronegative than fluorine (EN = 3.98). The Lewis structure for BF3 is:

90% (235 ratings)
View Complete Written Solution
Problem Details

The molecules BF3, CF4, CO2, PF5, and SF6 are all nonpolar, even though they all contain polar bonds. Why?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Molecular Polarity concept. You can view video lessons to learn Molecular Polarity. Or if you need more Molecular Polarity practice, you can also practice Molecular Polarity practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Dixon's class at UCF.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.