Chapter 2, Problem 34E

Interpretation Introduction

(a)

Interpretation:

Among the following species, the species with equal numbers of neutrons and protons should be identified.

${}^{24}{\text{Mg}}^{2+}{\text{, }}^{47}{\text{Cr, }}^{60}{\text{Co}}^{3+}{\text{, }}^{35}{\text{Cl}}^{-}{\text{, }}^{124}{\text{Sn}}^{2+}{\text{, }}^{226}{\text{Th, }}^{\text{90}}\text{Sr}$

Concept introduction:

The atomic number is equal to the number of protons of an element whereas sum of number of protons and number of neutrons is equal to mass number.

A form of chemical element having same atomic number but differ by mass number is known as isotopes. In nuclide notation of isotope, the mass number of the isotope is present in superscript in front of the symbol of given element and atomic number is present in subscript in front of the symbol of the element.

The expression is given by: $\text{E}$

where, A = mass number and Z = atomic number

Interpretation Introduction

(b)

Interpretation:

Among the following species, the species in which protons contributing 50% of the mass.

${}^{24}{\text{Mg}}^{2+}{\text{, }}^{47}{\text{Cr, }}^{60}{\text{Co}}^{3+}{\text{, }}^{35}{\text{Cl}}^{-}{\text{, }}^{124}{\text{Sn}}^{2+}{\text{, }}^{226}{\text{Th, }}^{\text{90}}\text{Sr}$

Concept introduction:

The atomic number is equal to the number of protons of an element whereas sum of number of protons and number of neutrons is equal to mass number.

A form of chemical element having same atomic number but differ by mass number is known as isotopes. In nuclide notation of isotope, the mass number of the isotope is present in superscript in front of the symbol of given element and atomic number is present in subscript in front of the symbol of the element.

The expression is given by: $\text{X}$

where, A = mass number and Z = atomic number

Interpretation Introduction

(c)

Interpretation:

Among the following species, the species which has about 50% more neutrons than protons should be identified.

${}^{24}{\text{Mg}}^{2+}{\text{, }}^{47}{\text{Cr, }}^{60}{\text{Co}}^{3+}{\text{, }}^{35}{\text{Cl}}^{-}{\text{, }}^{124}{\text{Sn}}^{2+}{\text{, }}^{226}{\text{Th, }}^{\text{90}}\text{Sr}$

Concept introduction:

The atomic number is equal to the number of protons of an element whereas sum of number of protons and number of neutrons is equal to mass number.

A form of chemical element having same atomic number but differ by mass number is known as isotopes. In nuclide notation of isotope, the mass number of the isotope is present in superscript in front of the symbol of given element and atomic number is present in subscript in front of the symbol of the element.

The expression is given by: $\text{X}$

where, A = mass number and Z = atomic number