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Chapter 10: Problem 36

Describe the hybridization of phosphorus in \(\mathrm{PF}_{5}\).

Short Answer

Expert verified
The hybridization of phosphorus in \(\mathrm{PF}_5\) is sp3d.

Step by step solution

01

Evaluate the valence electron

Determine the number of valence electrons for phosphorus. Phosphorus is in group 15 of the Periodic Table, so it has 5 valence electrons.
02

Count bond pairs and lone pairs

\(\mathrm{PF}_5\) contains 5 bonded fluorine atoms, hence there are 5 bond pairs and no lone pairs around central Phosphorus atom.
03

Determine the hybridization

By using the formula of hybridization which is Hybridization = No. of Bond pairs + No. of Lone pairs, the hybridization will be \( 5 + 0 = 5 \). Hence, phosphorus is sp3d hybridized.

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Most popular questions from this chapter

How is the geometry of a molecule defined and why is the study of molecular geometry important?

Aluminum trichloride \(\left(\mathrm{AlCl}_{3}\right)\) is an electrondeficient molecule. It has a tendency to form a dimer (a molecule made of two \(\mathrm{AlCl}_{3}\) units): $$ \mathrm{AlCl}_{3}+\mathrm{AlCl}_{3} \longrightarrow \mathrm{Al}_{2} \mathrm{Cl}_{6} $$ (a) Draw a Lewis structure for the dimer. (b) Describe the hybridization state of \(\mathrm{Al}\) in \(\mathrm{AlCl}_{3}\) and \(\mathrm{Al}_{2} \mathrm{Cl}_{6}\). (c) Sketch the geometry of the dimer. (d) Do these molecules possess a dipole moment?

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