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Chapter 10: Problem 40

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

Understand Atomic Orbitals

Before we can derive the correct hybridization, we must understand the atomic orbitals of phosphorus. The electron configuration of phosphorus (\(P\)) is \([Ne] 3s^2 3p^3\). Phosphorus has five valence electrons.
02

Define Bonding in PF5

In \(\mathrm{PF}_5\), each of the five Fluorine (F) atoms will share a pair of electrons with the Phosphorus (P) atom. Therefore, P needs to have 5 orbitals available for bonding. This exceeds the number of orbitals available in the ground state, therefore, P atom has to excite one of its 3s electrons to the 3d orbital. After exciting one electron, the electron configuration will be: \([Ne] 3s^1 3p^3 3d^1\). Now there are five unpaired electrons, so five hybrid orbitals can be formed.
03

Determine Hybridization

The hybridization which allows for the formation of five molecular orbitals for bonding is sp3d. This hybridization combines one s orbital, three p orbitals, and one d orbital to form five new sp3d orbitals, each of which can form a bond with one of the 5 fluorine atoms. Hence, the hybridization of phosphorus in \(\mathrm{PF}_5\) is sp3d.

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Most popular questions from this chapter

The geometry of \(\mathrm{CH}_{4}\) could be square planar, with the four \(\mathrm{H}\) atoms at the corners of a square and the \(\mathrm{C}\) atom at the center of the square. Sketch this geometry and compare its stability with that of a tetrahedral \(\mathrm{CH}_{4}\) molecule.

Discuss the basic features of the VSEPR model. Explain why the magnitude of repulsion decreases in this order: lone pair-lone pair \(>\) lone pair-bonding pair \(>\) bonding pair-bonding pair.

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Consider the reaction $$ \mathrm{BF}_{3}+\mathrm{NH}_{3} \longrightarrow \mathrm{F}_{3} \mathrm{~B}-\mathrm{NH}_{3} $$ Describe the changes in hybridization (if any) of the \(B\) and \(N\) atoms as a result of this reaction

Explain why an atom cannot have a permanent dipole moment.
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