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Chapter 8: Q30E (page 449)

For each of the following structures, determine the hybridization requested and whether the electrons will be delocalized:

(a)Hybridization of each carbon

(b)Hybridization of sulphur


(c)

All atoms


Short Answer

Expert verified

(a) From left to right, the hybridization of each carbon atom is sp2, \({\rm{s}}{{\rm{p}}^{\rm{3}}}\), and sp2 . Delocalized electrons do not exist.

(b) Electrons are delocalized after sp2 hybridization of sulphur.

(c) All carbons and nitrogen have been sp2 hybridised, while hydrogen has been s hybridised

Step by step solution

01

Define hybridization

Hybridization is a concept in organic chemistry that is used to explain chemical bonding when the valence bond theory fails to provide adequate explanation. This hypothesis is particularly useful for explaining organic molecules' covalent bonding

02

Explanation

(a) There will be no delocalization of electrons.

Acetone

The hybridisation of saturated carbon is \(s{p^3}\) and double bonded carbon it is sp2.

03

Explanation

(b) Delocalization of electrons will occur.

Sulfur dioxide

The hybridisation of sulfur is sp2 .

04

Explanation

a. Delocalization of electrons will occur.

Benzene

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Most popular questions from this chapter

Use valence bond theory to explain the bonding in\({{\rm{O}}_{\rm{2}}}\). Sketch the overlap of the atomic orbitals involved in the bonds in \({{\rm{O}}_{\rm{2}}}\).

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).

Strike-anywhere matches contain a layer of \({\rm{KCl}}{{\rm{O}}_{\rm{3}}}\) and a layer of \({{\rm{P}}_{\rm{4}}}{{\rm{S}}_{\rm{3}}}\). The heat produced by the friction of striking the match causes these two compounds to react vigorously, which sets fire to the wooden stem of the match. \({\rm{KCl}}{{\rm{O}}_{\rm{3}}}\) contains the \({\rm{Cl}}{{\rm{O}}_{\rm{3}}}^{\rm{ - }}\) ion. \({{\rm{P}}_{\rm{4}}}{{\rm{S}}_{\rm{3}}}\) is an unusual molecule with the skeletal structure.

  1. Write Lewis structures for \({{\rm{P}}_{\rm{4}}}{{\rm{S}}_{\rm{3}}}\) and the \({\rm{Cl}}{{\rm{O}}_{\rm{3}}}^{\rm{ - }}\) ion.
  2. Describe the geometry about the \({\rm{P}}\) atoms, the \({\rm{S}}\) atom, and the \({\rm{Cl}}\) atom in these species.
  3. Assign a hybridization to the \({\rm{P}}\) atoms, the \({\rm{S}}\)atom, and the \({\rm{Cl}}\) atom in these species.
  4. Determine the oxidation states and formal charge of the atoms in \({{\rm{P}}_{\rm{4}}}{{\rm{S}}_{\rm{3}}}\) and the \({\rm{Cl}}{{\rm{O}}_{\rm{3}}}^{\rm{ - }}\) ion.

Explain how \({\rm{\sigma }}\) and \({\rm{\pi }}\) bonds are similar and how they are different.

Describe the molecular geometry and hybridization of the N, P, or S atoms in each of the following compounds. (a) \({{\rm{H}}_{\rm{3}}}{\rm{P}}{{\rm{O}}_{\rm{4}}}\), phosphoric acid, used in cola soft drinks (b) \({\rm{N}}{{\rm{H}}_{\rm{4}}}{\rm{N}}{{\rm{O}}_{\rm{3}}}\) , ammonium nitrate, a fertilizer and explosive (c) \({{\rm{S}}_{\rm{2}}}{\rm{C}}{{\rm{l}}_{\rm{2}}}\), disulfur dichloride, used in vulcanizing rubber (d) \({{\rm{K}}_{\rm{4}}}{\rm{[}}{{\rm{O}}_{\rm{3}}}{\rm{POP}}{{\rm{O}}_{\rm{3}}}{\rm{]}}\), potassium pyrophosphate, an ingredient in some toothpastes
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