Chapter 10, Problem 10A.1ST

Interpretation Introduction

Interpretation:

The magnitude of the dipole moment and the atom lies at the negative end of the dipole in a $\text{C-H}$ bond has to be given.

Concept introduction:

Polar covalent bond involves an unequal sharing of electrons between two bonded atoms; it creates a partial separation of charge and a dipole moment.

Covalent bonds are polar, if there is a difference in electronegativity between the bonded atoms.

Direction of dipole moment in a molecule is can be represented as follows,

Explanation of Solution

The given bond is $\text{C-H}$.

The electronegativity of atoms in a bond will be the deciding factor to predict the dipole moment of the bond.

Electronegativities of the atoms in $\text{CO}$ are given below:

$\begin{array}{l}\text{Hydrogen}\text{-}\text{2}\text{.1}\\ \text{Carbon}\text{-}\text{2}\text{.5}\end{array}$

Electronegativity difference between atoms in the bond is given below:

$\text{C}-\text{H =}\text{2}\text{.5 - 2}\text{.1 = 0}\text{.4}$

Thus, the dipole moment is $\text{0}\text{.4}\text{D}$

Electronegativity of carbon is more than hydrogen. Therefore, the negative end of the dipole lies at more electronegative atom carbon.