Chapter 3, Problem 3CTQ

(a)

Interpretation Introduction

Interpretation: Whether the proposed statement by the student about the bond shown below as triple bond should be explained with appropriate argument.

  

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy. This phenomenon is referred as hybridization.

A single bond has one $\text{σ}$ bond, double bond has one $\text{σ}$ bond along with one $\text{π}$ bond while triple bond has two $\text{π}$ bonds in addition to one $\text{σ}$ bond.

(b)

Interpretation Introduction

Interpretation: The number of electrons present in a triple bond and in one representation shown below should be indicated.

  

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy. This phenomenon is referred as hybridization.

A single bond has one $\text{σ}$ bond, double bond has one $\text{σ}$ bond along with one $\text{π}$ bond while triple bond has two $\text{π}$ bonds in addition to one $\text{σ}$ bond.

(c)

Interpretation Introduction

Interpretation: Misconception that might have led to bond identified as triple bond by the student should be known.

Concept introduction: The 2 types of overlapping are as follows:

1. Head-on overlapping (sigma bond)

  

2. Sideway overlapping (pi bond)

  

A single bond has one $\text{σ}$ bond, double bond has one $\text{σ}$ bond along with one $\text{π}$ bond while triple bond has two $\text{π}$ bonds in addition to one $\text{σ}$ bond.

(d)

Interpretation Introduction

Interpretation: The space that could be used to add another p bond so as to generate a triple bond should be determined.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy although they may differ in shape and orientation. This phenomenon is referred as hybridization.

The energy and orientation of the new hybrid orbital depend upon by the kind and number of orbitals used in the hybridization. The new hybrid orbitals are always equal in number to number of atomic orbitals that combine.