The molecule PCl5 is observed not to have a dipole moment. This is because: A. T

Question

The molecule PCl5 is observed not to have a dipole moment. This is because:

A. There are no lone pairs of electrons on the central atom

B. As a gas and liquid PCl5 is not a ionic, but rather the bonds are covalent

C. The polarity of the P-Cl bonds cancel out due to the geometry of the molecule.

D. There are two lone pairs of electrons on the central atom, but due to the repulsion, they are on opposite sides of the central atom and cancel out.

E. P and Cl are ciose in the periodic table, so they have very similar electronegatives, and as such, the P-Cl bonds are not polar.

Explanation / Answer

The polarity of the P-Cl bonds cancel out due to the geometry of the molecule.

PCl5 has a trigonal bipyramidal structure. Since the molecule is symmetric around the central phosphorus atom, there is no net dipole moment.

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