Chapter 2, Problem 2.42P

(a)

Interpretation Introduction

Interpretation:

Whether ${}_1^3\text{H}$ and ${}_2^3\text{He}$ have the same number of protons, electrons or neutrons is to be determined.

Concept introduction:

Atoms are neutral in nature. They consist of even smaller particles namely, protons, electrons, and neutrons. Protons have a positive charge on them. Electrons have a negative charge. Neutrons have no charge in them. Protons and neutrons make up the nucleus in the atoms whereas the electrons revolve around the nucleus.

The general representation for an atom is given as ${}_Z^A\text{X}$. Here, $A$ is a mass number and $Z$ is the atomic number of an atom.

The superscript in the formula of elements or atoms is the mass number. The mass number is the sum of protons and neutrons in the atom. The subscript in the formula represents the atomic number. The atomic number of an element or atom is the number of protons in that element or atom. The difference between the mass number and the number of protons gives the number of neutrons.

The formula to calculate the number of neutrons is,

$\text{Total number of neutrons}\left(N\right)=\left[\begin{array}{l}\text{Mass number}\left(A\right)-\\ \text{Total number of protons}\left(Z\right)\end{array}\right]$ (1)

(b)

Interpretation Introduction

Interpretation:

Whether ${}_6^{14}\text{C}$ and ${}_7^{15}\text{N}$ have the same number of protons, electrons or neutrons is to be determined.

Concept introduction:

Atoms are neutral in nature. They consist of even smaller particles namely, protons, electrons, and neutrons. Protons have a positive charge on them. Electrons have a negative charge. Neutrons have no charge in them. Protons and neutrons make up the nucleus in the atoms whereas the electrons revolve around the nucleus.

The general representation for an atom is given as ${}_Z^A\text{X}$. Here, $A$ is a mass number and $Z$ is the atomic number of an atom.

The superscript in the formula of elements or atoms is the mass number. The mass number is the sum of protons and neutrons in the atom. The subscript in the formula represents the atomic number. The atomic number of an element or atom is the number of protons in that element or atom. The difference between the mass number and the number of protons gives the number of neutrons.

The formula to calculate the number of neutrons is,

$\text{Total number of neutrons}\left(N\right)=\left[\begin{array}{l}\text{Mass number}\left(A\right)-\\ \text{Total number of protons}\left(Z\right)\end{array}\right]$ (1)

(c)

Interpretation Introduction

Interpretation:

Whether ${}_9^{19}\text{F}$ and ${}_9^{18}\text{F}$ have the same number of protons, electrons or neutrons is to be determined.

Concept introduction:

Atoms are neutral in nature. They consist of even smaller particles namely, protons, electrons, and neutrons. Protons have a positive charge on them. Electrons have a negative charge. Neutrons have no charge in them. Protons and neutrons make up the nucleus in the atoms whereas the electrons revolve around the nucleus.

The general representation for an atom is given as ${}_Z^A\text{X}$. Here, $A$ is a mass number and $Z$ is the atomic number of an atom.

The superscript in the formula of elements or atoms is the mass number. The mass number is the sum of protons and neutrons in the atom. The subscript in the formula represents the atomic number. The atomic number of an element or atom is the number of protons in that element or atom. The difference between the mass number and the number of protons gives the number of neutrons.

The formula to calculate the number of neutrons is,

$\text{Total number of neutrons}\left(N\right)=\left[\begin{array}{l}\text{Mass number}\left(A\right)-\\ \text{Total number of protons}\left(Z\right)\end{array}\right]$ (1)