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Chapter 10: Problem 34

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

Short Answer

Expert verified
In this reaction, the hybridization of Boron (B) transitions from sp2 to sp3 while the hybridization of Nitrogen (N) remains sp3.

Step by step solution

01

Identify initial hybridization

Boron (B) in \(\mathrm{BF}_{3}\) is sp2 hybridized, which results in a trigonal planar arrangement of electron pairs. Nitrogen (N) in \(\mathrm{NH}_{3}\) is sp3 hybridized, which results in a tetrahedral arrangement of electron pairs.
02

Reaction formation

The lone pair on the Nitrogen in \(\mathrm{NH}_{3}\) forms a coordinate bond with the empty p-orbital on the Boron in \(\mathrm{BF}_{3}\), resulting in the formation of \(\mathrm{F}_{3} \mathrm{B}-\mathrm{NH}_{3}\).
03

Identify final hybridization

In \(\mathrm{F}_{3} \mathrm{B}-\mathrm{NH}_{3}\), the boron atom (B) changes from sp2 to sp3 hybridization due to the formation of an additional bond. Here the molecular geometry becomes tetrahedral. The nitrogen atom (N) remains sp3 hybridized as no change in its bonding occurs.

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Most popular questions from this chapter

Compare the relative stability of these species and indicate their magnetic properties (that is, diamagnetic or paramagnetic): \(\mathrm{O}_{2}, \mathrm{O}_{2}^{+}, \mathrm{O}_{2}^{-}\) (superoxide ion), \(\mathrm{O}_{2}^{2-}\) (peroxide ion).

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What is the relationship between the dipole moment and bond moment? How is it possible for a molecule to have bond moments and yet be nonpolar?
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