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Chapter 8: Q48 E (page 451)

Predict whether the MO diagram for S2 would show s-p mixing or not.

Short Answer

Expert verified

The molecular orbital diagram for S2 would not show s-p mixing.

Step by step solution

01

Molecular orbitals

The molecular orbitals are formed from the overlapping of atomic orbitals. The number of molecular orbitals formed is equal to the total number of atomic orbitals intermixed.

02

Explanation

In S, the energy gap between the 3s and 3p orbitals is substantial, preventing s-p mixing in S2. As a result, s-p mixing will not be seen in the molecular orbital diagram forS2.

Molecular orbital diagram of S2

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Most popular questions from this chapter

The bond energy of a C鈥揅 single bond averages \({\rm{347 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}\); that of a

C 鈮� C triple bond averages \({\rm{839 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}\). Explain why the triple bond is not three times as strong as a single bond.

Using the MO diagrams, predict the bond order for the stronger bond in each pair:

B2or B2+

F2orF2+

O2 or O22+

C2+or C2-

Identify the hybridization of the central atom in each of the following molecules and ions that contain multiple bonds: (a) \({\rm{ClNO}}\) (\({\rm{N}}\) is the central atom) (b) \({\rm{C}}{{\rm{S}}_{\rm{2}}}\) (c) \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{CO}}\) (\({\rm{C}}\) is the central atom) (d) \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{SO}}\) (\({\rm{S}}\) is the central atom) (e) \({\rm{S}}{{\rm{O}}_{\rm{2}}}{{\rm{F}}_{\rm{2}}}\) (\({\rm{S}}\) is the central atom) (f) \({\rm{Xe}}{{\rm{O}}_{\rm{2}}}{{\rm{F}}_{\rm{2}}}\) (\({\rm{Xe}}\) is the central atom) (g) \({\rm{ClO}}{{\rm{F}}_{\rm{2}}}^{\rm{ + }}\) (\({\rm{Cl}}\) is the central atom).

Methionine, \({\rm{C}}{{\rm{H}}_{\rm{3}}}{\rm{SC}}{{\rm{H}}_{\rm{2}}}{\rm{C}}{{\rm{H}}_{\rm{2}}}{\rm{CH}}\left( {{\rm{N}}{{\rm{H}}_{\rm{2}}}} \right){\rm{C}}{{\rm{O}}_{\rm{2}}}{\rm{H}}\), is an amino acid found in proteins. Draw a Lewis structure of this compound. What is the hybridization type of each carbon, oxygen, the nitrogen, and the sulfur?

Write Lewis structures for \({\rm{N}}{{\rm{F}}_{\rm{3}}}\) and \({\rm{P}}{{\rm{F}}_{\rm{5}}}\). On the basis of hybrid orbitals, explain the fact that \({\rm{N}}{{\rm{F}}_{\rm{3}}}\), \({\rm{P}}{{\rm{F}}_{\rm{3}}}\), and \({\rm{P}}{{\rm{F}}_{\rm{5}}}\) are stable molecules, but \({\rm{N}}{{\rm{F}}_{\rm{5}}}\) does not exist.
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