Chemistry, 19.10.2021 20:40 allieeastridge

What is the hybridization of the central atom in the phosphorus tetrachloryl PCl+4 cation?

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Answer from: Ramann03

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Explanation:

In order to determine the hybridization of the central phosphorus atom in phosphorus pentafluoride,

, you must first draw the compound's Lewis structure.

The molecule will have a total of

valence electrons,

from the phosphorus atom, and

from each of the five fluorine atoms.

The phosphorus atom will be the molecule's central atom. It will form single bonds with the five fluorine atoms.

These will account for

of the

valence electrons the molecule has. Each fluorine atom will have three lone pairs of electrons, which will account for the rest of the valence electrons.

The molecule's Lewis structure will look like this

http://2012books.lardbucket.org/books/principles-of-general-chemistry-v1.0/s13-molecular-geometry-and-covalen.html

Now you need to focus on the central atom, more specifically on how many regions of electron density surround the central atom - this is known as the steric number

A region of electron density can be a covalent bond - single, double, and triple bonds all count as one region of electron density - or a lone pair of electrons.

Notice that phosphorus is bonded to five fluorine atoms and has no lone pairs of electrons attached, which means that it is surrounded by a total of five regions of electron density, which is equivalent to saying that it has a steric number equal to

The steric number gives you the number of hybrid orbitals. In this case, a steric number of

means that the phosphorus atom will have

hybrid orbitals

one s-orbital

three p-orbitals

one d-orbital

As a result, the central atom will be

hybridized.

http://chemwiki.ucdavis.edu/Theoretical_Chemistry/Chemical_Bonding/Valence_Bond_Theory/Overview_of_Valence_Bond_Theory

Answer from: Quest

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Answer from: Quest

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