Determine the hybridization of the central atom in PCl5.

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Question: Determine the hybridization of the central atom in PCl5.

Options:

Correct Answer: dsp3

Solution:

Phosphorus in PCl5 is dsp3 hybridized, allowing it to form five bonds.

Determine the hybridization of the central atom in PCl5.

Determine the hybridization of the central atom in PCl5.

Step 1: Identify the central atom in PCl5, which is phosphorus (P).
Step 2: Count the number of bonds phosphorus forms in PCl5. It forms five bonds with five chlorine (Cl) atoms.
Step 3: Determine the steric number, which is the number of bonds plus lone pairs on the central atom. Here, phosphorus has 5 bonds and 0 lone pairs, so the steric number is 5.
Step 4: Use the steric number to find the hybridization. A steric number of 5 corresponds to dsp3 hybridization.
Step 5: Conclude that the hybridization of phosphorus in PCl5 is dsp3, which allows it to form five bonds.

Hybridization – The concept of hybridization involves the mixing of atomic orbitals to form new hybrid orbitals suitable for the pairing of electrons to form chemical bonds.
Molecular Geometry – Understanding the molecular geometry helps in determining the hybridization state of the central atom based on the number of bonds and lone pairs.
Valence Shell Electron Pair Repulsion (VSEPR) Theory – VSEPR theory is used to predict the geometry of individual molecules based on the repulsion between electron pairs in the valence shell.