Chapter 10, Problem 10.62QE

(a)

Interpretation Introduction

Interpretation:

The hybrid orbitals on the central atom that form $\text{σ}$ bond in ${\text{C}}_{\text{2}}{\text{H}}_{\text{6}}$ have to be given.

Concept Introduction:

Sigma and Pi bonds:

Sigma and pi bonds are chemical covalent bonds. Sigma and pi bonds are formed by the overlap of atomic orbitals. $\text{σ}$ bonds are formed by end-to-end overlapping and $\text{π}$ bonds are formed when the lobe of one atomic orbital overlaps another.  Generally sigma bonds are stronger than pi bonds. Both are used extensively to predict the behavior of molecules in molecular orbital theory.

Figure 1: Sigma bond formation;

(b)

Interpretation Introduction

Interpretation:

The hybrid orbitals on the central atom that form bond $\text{σ}$ in ${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}$ have to be given.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The hybrid orbitals on the central atom that form $\text{σ}$ bond in ${\text{CBr}}_{\text{4}}$ have to be given.

Concept Introduction:

Refer to part (a).