Chapter 22: Problem 97

Solid \(\mathrm{PCl}_{5}\) exists as \(\left[\mathrm{PCl}_{4}^{+}\right]\left[\mathrm{PCl}_{6}^{-}\right] .\) Draw Lewis structures for these ions. Describe the hybridization state of the \(\mathrm{P}\) atoms.

Short Answer

Expert verified

The Lewis structure of \(\left[\mathrm{PCl}_{4}^{+}\right]\) ion shows P atom at the center surrounded by 4 Cl atoms with single bonds, indicating a \(sp^{3}\) hybridization state. The Lewis structure of \(\left[\mathrm{PCl}_{6}^{-}\right]\) ion shows the P atom surrounded by 6 Cl atoms with single bonds, pointing to a \(sp^{3}d^{2}\) hybridization state.

Step by step solution

Draw the Lewis Structure for \(\left[\mathrm{PCl}_{4}^{+}\right]\)

A Lewis structure is the graphic representation of the electron distribution around atoms. In \(\left[\mathrm{PCl}_{4}^{+}\right]\), phosphorus (P) forms 4 bonds with Chlorine (Cl). The Lewis structure would show Phosphorus in the middle surrounded by the 4 Chlorine atoms, indicating the single bonds between them. Since it's a positively charged ion, we will be missing one electron from P’s usual five.

Draw the Lewis Structure for \(\left[\mathrm{PCl}_{6}^{-}\right]\)

For \(\left[\mathrm{PCl}_{6}^{-}\right]\), Phosphorus is bonded to 6 Chlorine atoms, also represented by single bonds between each P-Cl. The negative charge here indicates an additional electron added to the structure, making the total number of valence electrons for P to be 6 in this case.

Determine the Hybridization State

The hybridization of an atom in a molecule can be determined by the number of atomic orbitals that mix to form the hybrid orbitals. In \(\left[\mathrm{PCl}_{4}^{+}\right]\), the P atom forms four sigma bonds with four Cl atoms, so it is in a \(sp^{3}\) hybridization state. In \(\left[\mathrm{PCl}_{6}^{-}\right]\), the P atom forms six sigma bonds with six Cl atoms, so we need to have six hybrid orbitals formed implying a \(sp^{3}d^{2}\) hybridization state.

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Solid \(\mathrm{PCl}_{5}\) exists as \(\left[\mathrm{PCl}_{4}^{+}\right]\left[\mathrm{PCl}_{6}^{-}\right] .\) Draw Lewis structures for these ions. Describe the hybridization state of the \(\mathrm{P}\) atoms.

Short Answer

Step by step solution

Draw the Lewis Structure for \(\left[\mathrm{PCl}_{4}^{+}\right]\)

Draw the Lewis Structure for \(\left[\mathrm{PCl}_{6}^{-}\right]\)

Determine the Hybridization State

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