Question
Net dipole moment of CH_(2)Cl_(2) No net polarity
Answer
4.3
(290 Votes)
Erin
Veteran · Tutor for 12 years
Answer
No net polarity.
Explanation
## Step1A molecule has a net dipole moment when there is a sufficient difference in electronegativity between two atoms binding in that molecule, creating a region of slightly negative charge (δ-) and another region of slightly positive charge (δ+). This results in a polar bond. However, a molecule composed of such polar bonds can be either polar or nonpolar. The determining factor for the overall polarity of the molecule is its shape or geometry.## Step2The test molecule here is CH2Cl2, often called dichloromethane. In dichloromethane, the molecule adopts a tetrahedral shape.## Step3The PolarPlot vector of H-C bonds cancelled each other and the dipole vectors of C-Cl bonds also cancelled each other out, leaving the net dipole moment of the molecule to be zero despite having polar bonds.