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Ch.9 - Molecular Geometry and Bonding Theories
All textbooksBrown 14th EditionCh.9 - Molecular Geometry and Bonding TheoriesProblem 49c
Chapter 9, Problem 49c

Consider the molecule BF3. (c) What hybrid orbitals should be constructed on the B atom to make the B–F bonds in BF3?

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Step 1: Identify the central atom in the molecule. In this case, the central atom is Boron (B).
Step 2: Determine the number of electron domains around the central atom. An electron domain is any area where electrons are most likely to be found, such as a single bond, double bond, triple bond, or a lone pair of electrons. In BF3, Boron forms single bonds with three Fluorine atoms, so there are three electron domains.
Step 3: Use the number of electron domains to determine the hybridization of the central atom. In this case, three electron domains correspond to sp2 hybridization.
Step 4: The sp2 hybridization means that one s orbital and two p orbitals on Boron are mixed to form three new sp2 hybrid orbitals.
Step 5: These sp2 hybrid orbitals are then used to form bonds with the Fluorine atoms in BF3.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Hybridization

Hybridization is the process of combining atomic orbitals to form new hybrid orbitals that can accommodate bonding. In BF3, the boron atom undergoes sp2 hybridization, which involves mixing one s orbital and two p orbitals to create three equivalent sp2 hybrid orbitals. This allows boron to form three sigma bonds with fluorine atoms.
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Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. In the case of BF3, the sp2 hybridization leads to a trigonal planar geometry, where the three B–F bonds are arranged at 120-degree angles around the boron atom. Understanding molecular geometry is crucial for predicting the shape and reactivity of molecules.
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Bonding and Lone Pairs

In covalent bonding, atoms share electrons to achieve stability. In BF3, boron forms three bonds with fluorine atoms, utilizing its sp2 hybrid orbitals. Importantly, boron has an incomplete octet, as it does not have any lone pairs of electrons, which influences its reactivity and the overall electron deficiency of the molecule.
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Related Practice
Textbook Question

For each statement, indicate whether it is true or false. (d) Nonbonding electron pairs cannot occupy a hybrid orbital.

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How would you expect the extent of overlap of the bondingatomic orbitals to vary in the series IF, ICl, IBr, and I2?Explain your answer.
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Textbook Question

Consider the molecule BF3. (a) What is the electron configuration of an isolated B atom? (b) What is the electron configuration of an isolated F atom?

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Consider the SCl2 molecule. (c) What hybrid orbitals should be constructed on the S atom to make the S-Cl bonds in SCl2?

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Consider the SCl2 molecule.(d) What valence orbitals, if any, remain unhybridized on the S atom in SCl2?

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Indicate the hybridization of the central atom in (a) H2S (b) SeF6