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17 Nov 2019

Part A

The PH3 molecule is polar. Does this offer experimental proof that the molecule cannot be planar? Explain.

The molecule is nonplanar. Thus, the P−H bond dipoles do not cancel making the molecule polar.
The molecule is nonplanar. Thus, the P−H bond dipoles cancel making the molecule polar.
The molecule is planar. Thus, the P−H bond dipoles cancel making the molecule polar.
The molecule is planar. Thus, the P−H bond dipoles do not cancel making the molecule polar.

Part B

It turns out that ozone, O3, has a small dipole moment. How is this possible, given that all the atoms are the same?

The trigonal planar e− domain geometry of the central O atom is the reason for the dipole moment in O3.
The sp2 hybridization of the central O atom is the reason for the dipole moment in O3.
The lone pair of electrons of the central O atom is the source of the dipole moment in O3.
The bent molecular geometry of the central O atom is the reason for the dipole moment in O3.

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Elin Hessel
Elin HesselLv2
5 Jul 2019
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