Chapter 14, Problem 14.125P

(a)

Interpretation Introduction

Interpretation:

The Lewis structure for carbon monoxide has to be drawn.

Concept Introduction:

Lewis structure: This is the only way to show the sharing of electrons between atom in polar covalent bonds or covalent bond. This is often called as Lewis structure. This structure denotes valence electrons of an atom by dots and also it shows the way of valence electron distributed within a molecule.

(b)

Interpretation Introduction

Interpretation:

The formal charge of atoms in carbon monoxide has to be calculated.

Concept introduction:

Formal charge: The formal charge is defined as the charge carried by an atom in a molecule assuming that, irrespective of the relative electronegativity of the shared atoms, all the chemical bonds are shared equally between the two atoms.

Formal Charge: The formal charge on atoms in the Lewis structure is calculated by the equation below.

$\text{FC}\text{=}\text{valence electrons}\text{-}\text{number of non-bonding valence electrons }\text{-}\frac{\text{number}\text{of}\text{shared}\text{electrons}}{\text{2}}$

(c)

Interpretation Introduction

Interpretation:

The reason for small dipole moment of carbon monoxide based on a and b sub-parts have to be given.

Concept Introduction:

The polar molecules possess charge separation in them. The charge separation arises due to the difference in the electronegativity between the atoms in a molecule. So, polar molecules possess a permanent dipole moment in them. There won’t be electronegativity difference between the atoms in non-polar molecules. Hence charge separation does not arise in the non-polar molecules. So, non-polar molecules do not possess dipole moment in them.