Chapter 2, Problem 39P

Interpretation Introduction

(a)

Interpretation:

The atomic number in ${}^{\text{58}}{\text{Ni and }}^{60}\text{Ni}$ should be determined.

Concept Introduction:

An element consists of same type of atoms. An atom is composed of certain sub-atomic particles; electrons, protons and neutrons. Here the sum of number of protons and neutrons is called as mass number whereas number of protons is called as atomic number. The elements with same atomic number and different mass number are called as isotopes. Each isotope is found at certain percentage in nature that is called as isotopic abundance. The isotopic abundance and mass of isotope can be used to calculate the average atomic mass of element.

  $\text{Average atomic weight = }\frac{{\text{(Mass × isotopic abundance)}}_{\text{isotope 1}}+{\text{(Mass × isotopic abundance)}}_{\text{isotope 2}}+\mathrm{....}}{100}$

Interpretation Introduction

(b)

Interpretation:

The mass number in ${}^{\text{58}}{\text{Ni and }}^{60}\text{Ni}$ should be determined.

Concept Introduction:

An element consists of same type of atoms. An atom is composed of certain sub-atomic particles; electrons, protons and neutrons. Here the sum of number of protons and neutrons is called as mass number whereas number of protons is called as atomic number. The elements with same atomic number and different mass number are called as isotopes. Each isotope is found at certain percentage in nature that is called as isotopic abundance. The isotopic abundance and mass of isotope can be used to calculate the average atomic mass of element.

  $\text{Average atomic weight = }\frac{{\text{(Mass × isotopic abundance)}}_{\text{isotope 1}}+{\text{(Mass × isotopic abundance)}}_{\text{isotope 2}}+\mathrm{....}}{100}$

Interpretation Introduction

(c)

Interpretation:

The number of protons in ${}^{\text{58}}{\text{Ni and }}^{60}\text{Ni}$ should be determined.

Concept Introduction:

An element consists of same type of atoms. An atom is composed of certain sub-atomic particles; electrons, protons and neutrons. Here the sum of number of protons and neutrons is called as mass number whereas number of protons is called as atomic number. The elements with same atomic number and different mass number are called as isotopes. Each isotope is found at certain percentage in nature that is called as isotopic abundance. The isotopic abundance and mass of isotope can be used to calculate the average atomic mass of element.

  $\text{Average atomic weight = }\frac{{\text{(Mass × isotopic abundance)}}_{\text{isotope 1}}+{\text{(Mass × isotopic abundance)}}_{\text{isotope 2}}+\mathrm{....}}{100}$

Interpretation Introduction

(d)

Interpretation:

The number of neutrons in ${}^{\text{58}}{\text{Ni and }}^{60}\text{Ni}$ should be determined.

Concept Introduction:

An element consists of same type of atoms. An atom is composed of certain sub-atomic particles; electrons, protons and neutrons. Here the sum of number of protons and neutrons is called as mass number whereas number of protons is called as atomic number. The elements with same atomic number and different mass number are called as isotopes. Each isotope is found at certain percentage in nature that is called as isotopic abundance. The isotopic abundance and mass of isotope can be used to calculate the average atomic mass of element.

  $\text{Average atomic weight = }\frac{{\text{(Mass × isotopic abundance)}}_{\text{isotope 1}}+{\text{(Mass × isotopic abundance)}}_{\text{isotope 2}}+\mathrm{....}}{100}$