Chapter 10, Problem 10.41QP

(a)

Interpretation Introduction

Interpretation:

The number of Sigma $\left(\text{σ}\right)$ and pi $\left(\text{π}\right)$ bonds have to be known in the given molecule.

Concept Introduction:

$\text{σ}$-bonds are covalent bonds formed by the end-to-end overlapping of two atomic orbitals. In the $\text{σ}$-bonding, the electronic concentration will be only within the bond and because of that the $\text{σ}$-bond is being a localized bond.

$\text{π}$-bonds are also covalent bonds formed by the sideways overlapping of two atomic orbitals. In the $\text{π}$-bonding, the electronic concentration will be above and below the plane of the $\text{σ}$-bond and because of that the $\text{π}$-bond is being a delocalized bond.

There will be one $\text{π}$-bond in a double bond and two $\text{π}$-bonds in a triple bond. However, there will be only one $\text{σ}$-bond in both double and triple bonds. $\text{σ}$-bonds always exist as single bonds.

(b)

Interpretation Introduction

Interpretation: The number of Sigma $\left(\text{σ}\right)$ and pi $\left(\text{π}\right)$ bonds have to be known in the given molecule.

Concept Introduction:

$\text{σ}$-bonds are covalent bonds formed by the end-to-end overlapping of two atomic orbitals. In the $\text{σ}$-bonding, the electronic concentration will be only within the bond and because of that the $\text{σ}$-bond is being a localized bond.

$\text{π}$-bonds are also covalent bonds formed by the sideways overlapping of two atomic orbitals. In the $\text{π}$-bonding, the electronic concentration will be above and below the plane of the $\text{σ}$-bond and because of that the $\text{π}$-bond is being a delocalized bond.

There will be one $\text{π}$-bond in a double bond and two $\text{π}$-bonds in a triple bond. However, there will be only one $\text{σ}$-bond in both double and triple bonds. $\text{σ}$-bonds always exist as single bonds.

(c)

Interpretation Introduction

Interpretation: The number of Sigma $\left(\text{σ}\right)$ and pi $\left(\text{π}\right)$ bonds have to be known in the given molecule.

Concept Introduction:

$\text{σ}$-bonds are covalent bonds formed by the end-to-end overlapping of two atomic orbitals. In the $\text{σ}$-bonding, the electronic concentration will be only within the bond and because of that the $\text{σ}$-bond is being a localized bond.

$\text{π}$-bonds are also covalent bonds formed by the sideways overlapping of two atomic orbitals. In the $\text{π}$-bonding, the electronic concentration will be above and below the plane of the $\text{σ}$-bond and because of that the $\text{π}$-bond is being a delocalized bond.

There will be one $\text{π}$-bond in a double bond and two $\text{π}$-bonds in a triple bond. However, there will be only one $\text{σ}$-bond in both double and triple bonds. $\text{σ}$-bonds always exist as single bonds.