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Chapter 11: Problem 99

Explain why the molecular structure of \(\mathrm{BF}_{3}\) cannot be adequately described through overlaps involving pure \(s\) and \(p\) orbitals.

Short Answer

Expert verified
The molecular structure of \( BF_{3} \) cannot be adequately described through overlaps involving pure s and p orbitals because Boron doesn't have enough unpaired electrons to form bonds with three Fluorine atoms. Hybridization (sp2) in Boron results in the correct unpaired electron alignment for bond formation.

Step by step solution

01

Electron Configuration

Consider the electron configuration of Boron and Fluorine. Boron with an atomic number of 5 has a configuration of '2s2 2p1' whereas Fluorine with an atomic number of 9 has a configuration of '2s2 2p5'. This configuration explains the number of available electrons for bond formation.
02

Pure s and p Orbital Overlap

An attempt to describe the molecule structure using pure s and p orbitals would result in a molecule structure that doesn't agree with experimental facts. For the Boron atom to form bonds with the three Fluorine atoms, it would need to have a total of three unpaired electrons but it's observed from its electron configuration that it has only one unpaired electron available in the 2p orbital. The 2s orbital of Boron is completely filled with two paired electrons.
03

The Requirement of Hybridization

In order to form the three bonds to the fluorine atoms, Boron needs to have three unpaired electrons. This can be arranged by a process called 'hybridization', specifically sp2 hybridization. During sp2 hybridization, one of the 2s orbital electrons is promoted to the 2p orbital, resulting in 3 unpaired electrons which can form bonds. These hybridized orbitals can overlap with the singly occupied 2p orbitals of the Fluorine atoms. This results in aplanar molecule with bond angles of 120° which matches the observed structure of BF3.

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Most popular questions from this chapter

The hybridization scheme for the central atom includes a \(d\) orbital contribution in (a) \(\mathrm{I}_{3}^{-} ;\) (b) \(\mathrm{PCl}_{3}\) (c) \(\mathrm{NO}_{3}^{-} ;\) (d) \(\mathrm{H}_{2}\) Se.

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