Chapter 2, Problem 2.136P

(a)

Interpretation Introduction

Interpretation:

The different molecular masses that are possible for the compound ${\text{N}}_2\text{O}$ are to be determined.

Concept introduction:

Isotopes are atoms with the same atomic number but a different mass number. The difference in the mass numbers of isotopes arises due to the difference in the number of neutrons in them. The mass number of an atom is the sum of the protons and neutrons in them. The number of protons of isotopes is the same but the neutron number varies. Due to the same number of protons in the isotopes, they occupy the same position in the periodic table.

The formula to calculate the molecular mass of a compound is,

$\text{Molecular mass}=\left[\begin{array}{l}\sum \left(\text{numer of atoms of the element}\right)\\ \left(\text{atomic mass of the element}\right)\end{array}\right]$ (1)

(b)

Interpretation Introduction

Interpretation:

The least and the most common molecular masses of ${\text{N}}_2\text{O}$ are to be determined.

Concept introduction:

Isotopes are atoms with the same atomic number but a different mass number. The difference in the mass numbers of isotopes arises due to the difference in the number of neutrons in them. The mass number of an atom is the sum of the protons and neutrons in them. The number of protons of isotopes is the same but the neutron number varies. Due to the same number of protons in the isotopes, they occupy the same position in the periodic table.