The ratio of the number of neutrons to a number of proton for 144 Sm 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 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, Total number of neutrons ( N ) = [ Mass number ( A ) − Total number of protons ( Z ) ] (1) The expression to calculate the ratio of ( N Z ) is as follows: N Z = Total number of neutrons Total number of proton (2)

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Answer 1

Question

Chapter 2, Problem 2.140P

(a)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $144Sm$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(a)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $144Sm$ is $1.3$ .

Explanation of Solution

In $S62144m$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $144Sm$ an atom is $62$ . Thus, the number of protons in $S62144m$ is $62$ .

Substitute $144$ for the mass number and $62$ for the total number of protons in equation (1) to calculate the number of neutrons in $S62144m$ .

$Total number of neutrons=144−62=82$

Substitute $82$ for a total number of neutrons and $62$ for the total number of protons in the equation (2).

$NZ=8262=1.3.$

Conclusion

The value of $(NZ)$ for $144Sm$ is $1.3$ .

(b)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $56Fe$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(b)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $56Fe$ is $1.2$ .

Explanation of Solution

In $F2656e$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $F2656e$ is $26$ . Thus, the number of protons is 26.

Substitute $56$ for the mass number and 26 for the total number of protons in equation (1).

$Total number of neutrons=56−26=30$

Substitute $30$ for a total number of neutrons and $26$ for a total number of protons in the equation (2).

$NZ=3026=1.2.$

Conclusion

The value of $(NZ)$ for $56Fe$ is $1.2$ .

(c)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $20Ne$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(c)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $20Ne$ is $1.0$ .

Explanation of Solution

In $N1020e$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $N1020e$ is 10. Thus, the number of protons is 10.

Substitute $20$ for the mass number and 10 for the total number of protons in equation (1).

$Total number of neutrons=20−10=10$

Substitute $10$ for a total number of neutrons and $10$ for a total number of protons in the equation (2).

$NZ=1010=1.$

Conclusion

The value of $(NZ)$ for $20Ne$ is $1.0$ .

(d)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $107Ag$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(d)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $107Ag$ is $1.3$ .

Explanation of Solution

In $A47107g$ atoms, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $A47107g$ is 47. Thus, the number of protons is 47.

Substitute $107$ for the mass number and 47 for the total number of protons in equation (1).

$Total number of neutrons=107−47=60$

Substitute $60$ for a total number of neutrons and $47$ for the total number of protons in the equation (2).

$NZ=6047=1.3.$

Conclusion

The value of $(NZ)$ for $107Ag$ is $1.3$ .

(e)

Interpretation Introduction

Interpretation:

The number of neutrons, proton, and electron in $234U$ , $238U$ , $214Pb$ , $210Pb$ and $206Pb$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

(e)

Expert Solution

Answer to Problem 2.140P

The number of neutrons, protons, and electrons in $234U$ , $238U$ , $214Pb$ , $210Pb$ and $206Pb$ are as follows:

$IsotopeNeutronsProtonsElectrons234U1469292238U1429292214Pb1328282210Pb1288282206Pb1248282$

Explanation of Solution

In $U92238$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $U92238$ is $92$ . Thus, the number of protons is 92. In neutral atom number of electrons is equal to the number of protons, therefore, the number of electrons is 92.

Substitute $238$ for the mass number and 92 for the total number of protons in equation (1) to calculate the number of neutrons in $U92238$ .

$Total number of neutrons=238−92=146$

In $U92234$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $U92234$ is $92$ . Thus, the number of protons is 92 and the number of electrons is also 92.

Substitute 234 for the mass number and 92 for the total number of protons in equation (1) to calculate the number of neutrons in $U92234$ .

$Total number of neutrons=234−92=142$

In $P82214b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, the number of protons is 82 and the number of electrons is also 82.

Substitute $214$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82214b$ .

$Total number of neutrons=214−82=132$

In $P82210b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, the number of protons is 82 and the number of electrons is also 82.

Substitute $210$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82210b$ .

$Total number of neutrons=210−82=128$

In $P82206b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, a number of protons is 82 and the number of electrons is 82.

Substitute $206$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82206b$ .

$Total number of neutrons=206−82=124.$

Conclusion

Isotopes are the atoms of the same element with the same atomic number but different mass number. In a neutral atom, the number of electrons is equal to the number of protons.

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Answer 2

Question

Chapter 2, Problem 2.140P

(a)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $144Sm$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(a)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $144Sm$ is $1.3$ .

Explanation of Solution

In $S62144m$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $144Sm$ an atom is $62$ . Thus, the number of protons in $S62144m$ is $62$ .

Substitute $144$ for the mass number and $62$ for the total number of protons in equation (1) to calculate the number of neutrons in $S62144m$ .

$Total number of neutrons=144−62=82$

Substitute $82$ for a total number of neutrons and $62$ for the total number of protons in the equation (2).

$NZ=8262=1.3.$

Conclusion

The value of $(NZ)$ for $144Sm$ is $1.3$ .

(b)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $56Fe$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(b)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $56Fe$ is $1.2$ .

Explanation of Solution

In $F2656e$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $F2656e$ is $26$ . Thus, the number of protons is 26.

Substitute $56$ for the mass number and 26 for the total number of protons in equation (1).

$Total number of neutrons=56−26=30$

Substitute $30$ for a total number of neutrons and $26$ for a total number of protons in the equation (2).

$NZ=3026=1.2.$

Conclusion

The value of $(NZ)$ for $56Fe$ is $1.2$ .

(c)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $20Ne$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(c)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $20Ne$ is $1.0$ .

Explanation of Solution

In $N1020e$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $N1020e$ is 10. Thus, the number of protons is 10.

Substitute $20$ for the mass number and 10 for the total number of protons in equation (1).

$Total number of neutrons=20−10=10$

Substitute $10$ for a total number of neutrons and $10$ for a total number of protons in the equation (2).

$NZ=1010=1.$

Conclusion

The value of $(NZ)$ for $20Ne$ is $1.0$ .

(d)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $107Ag$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(d)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $107Ag$ is $1.3$ .

Explanation of Solution

In $A47107g$ atoms, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $A47107g$ is 47. Thus, the number of protons is 47.

Substitute $107$ for the mass number and 47 for the total number of protons in equation (1).

$Total number of neutrons=107−47=60$

Substitute $60$ for a total number of neutrons and $47$ for the total number of protons in the equation (2).

$NZ=6047=1.3.$

Conclusion

The value of $(NZ)$ for $107Ag$ is $1.3$ .

(e)

Interpretation Introduction

Interpretation:

The number of neutrons, proton, and electron in $234U$ , $238U$ , $214Pb$ , $210Pb$ and $206Pb$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

(e)

Expert Solution

Answer to Problem 2.140P

The number of neutrons, protons, and electrons in $234U$ , $238U$ , $214Pb$ , $210Pb$ and $206Pb$ are as follows:

$IsotopeNeutronsProtonsElectrons234U1469292238U1429292214Pb1328282210Pb1288282206Pb1248282$

Explanation of Solution

In $U92238$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $U92238$ is $92$ . Thus, the number of protons is 92. In neutral atom number of electrons is equal to the number of protons, therefore, the number of electrons is 92.

Substitute $238$ for the mass number and 92 for the total number of protons in equation (1) to calculate the number of neutrons in $U92238$ .

$Total number of neutrons=238−92=146$

In $U92234$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $U92234$ is $92$ . Thus, the number of protons is 92 and the number of electrons is also 92.

Substitute 234 for the mass number and 92 for the total number of protons in equation (1) to calculate the number of neutrons in $U92234$ .

$Total number of neutrons=234−92=142$

In $P82214b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, the number of protons is 82 and the number of electrons is also 82.

Substitute $214$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82214b$ .

$Total number of neutrons=214−82=132$

In $P82210b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, the number of protons is 82 and the number of electrons is also 82.

Substitute $210$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82210b$ .

$Total number of neutrons=210−82=128$

In $P82206b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, a number of protons is 82 and the number of electrons is 82.

Substitute $206$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82206b$ .

$Total number of neutrons=206−82=124.$

Conclusion

Isotopes are the atoms of the same element with the same atomic number but different mass number. In a neutral atom, the number of electrons is equal to the number of protons.

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Answer 3

Question

Chapter 2, Problem 2.140P

(a)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $144Sm$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(a)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $144Sm$ is $1.3$ .

Explanation of Solution

In $S62144m$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $144Sm$ an atom is $62$ . Thus, the number of protons in $S62144m$ is $62$ .

Substitute $144$ for the mass number and $62$ for the total number of protons in equation (1) to calculate the number of neutrons in $S62144m$ .

$Total number of neutrons=144−62=82$

Substitute $82$ for a total number of neutrons and $62$ for the total number of protons in the equation (2).

$NZ=8262=1.3.$

Conclusion

The value of $(NZ)$ for $144Sm$ is $1.3$ .

(b)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $56Fe$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(b)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $56Fe$ is $1.2$ .

Explanation of Solution

In $F2656e$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $F2656e$ is $26$ . Thus, the number of protons is 26.

Substitute $56$ for the mass number and 26 for the total number of protons in equation (1).

$Total number of neutrons=56−26=30$

Substitute $30$ for a total number of neutrons and $26$ for a total number of protons in the equation (2).

$NZ=3026=1.2.$

Conclusion

The value of $(NZ)$ for $56Fe$ is $1.2$ .

(c)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $20Ne$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(c)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $20Ne$ is $1.0$ .

Explanation of Solution

In $N1020e$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $N1020e$ is 10. Thus, the number of protons is 10.

Substitute $20$ for the mass number and 10 for the total number of protons in equation (1).

$Total number of neutrons=20−10=10$

Substitute $10$ for a total number of neutrons and $10$ for a total number of protons in the equation (2).

$NZ=1010=1.$

Conclusion

The value of $(NZ)$ for $20Ne$ is $1.0$ .

(d)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $107Ag$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(d)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $107Ag$ is $1.3$ .

Explanation of Solution

In $A47107g$ atoms, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $A47107g$ is 47. Thus, the number of protons is 47.

Substitute $107$ for the mass number and 47 for the total number of protons in equation (1).

$Total number of neutrons=107−47=60$

Substitute $60$ for a total number of neutrons and $47$ for the total number of protons in the equation (2).

$NZ=6047=1.3.$

Conclusion

The value of $(NZ)$ for $107Ag$ is $1.3$ .

(e)

Interpretation Introduction

Interpretation:

The number of neutrons, proton, and electron in $234U$ , $238U$ , $214Pb$ , $210Pb$ and $206Pb$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

(e)

Expert Solution

Answer to Problem 2.140P

The number of neutrons, protons, and electrons in $234U$ , $238U$ , $214Pb$ , $210Pb$ and $206Pb$ are as follows:

$IsotopeNeutronsProtonsElectrons234U1469292238U1429292214Pb1328282210Pb1288282206Pb1248282$

Explanation of Solution

In $U92238$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $U92238$ is $92$ . Thus, the number of protons is 92. In neutral atom number of electrons is equal to the number of protons, therefore, the number of electrons is 92.

Substitute $238$ for the mass number and 92 for the total number of protons in equation (1) to calculate the number of neutrons in $U92238$ .

$Total number of neutrons=238−92=146$

In $U92234$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $U92234$ is $92$ . Thus, the number of protons is 92 and the number of electrons is also 92.

Substitute 234 for the mass number and 92 for the total number of protons in equation (1) to calculate the number of neutrons in $U92234$ .

$Total number of neutrons=234−92=142$

In $P82214b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, the number of protons is 82 and the number of electrons is also 82.

Substitute $214$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82214b$ .

$Total number of neutrons=214−82=132$

In $P82210b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, the number of protons is 82 and the number of electrons is also 82.

Substitute $210$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82210b$ .

$Total number of neutrons=210−82=128$

In $P82206b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, a number of protons is 82 and the number of electrons is 82.

Substitute $206$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82206b$ .

$Total number of neutrons=206−82=124.$

Conclusion

Isotopes are the atoms of the same element with the same atomic number but different mass number. In a neutral atom, the number of electrons is equal to the number of protons.

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Answer 4

Question

Chapter 2, Problem 2.140P

(a)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $144Sm$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(a)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $144Sm$ is $1.3$ .

Explanation of Solution

In $S62144m$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $144Sm$ an atom is $62$ . Thus, the number of protons in $S62144m$ is $62$ .

Substitute $144$ for the mass number and $62$ for the total number of protons in equation (1) to calculate the number of neutrons in $S62144m$ .

$Total number of neutrons=144−62=82$

Substitute $82$ for a total number of neutrons and $62$ for the total number of protons in the equation (2).

$NZ=8262=1.3.$

Conclusion

The value of $(NZ)$ for $144Sm$ is $1.3$ .

(b)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $56Fe$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(b)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $56Fe$ is $1.2$ .

Explanation of Solution

In $F2656e$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $F2656e$ is $26$ . Thus, the number of protons is 26.

Substitute $56$ for the mass number and 26 for the total number of protons in equation (1).

$Total number of neutrons=56−26=30$

Substitute $30$ for a total number of neutrons and $26$ for a total number of protons in the equation (2).

$NZ=3026=1.2.$

Conclusion

The value of $(NZ)$ for $56Fe$ is $1.2$ .

(c)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $20Ne$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(c)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $20Ne$ is $1.0$ .

Explanation of Solution

In $N1020e$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $N1020e$ is 10. Thus, the number of protons is 10.

Substitute $20$ for the mass number and 10 for the total number of protons in equation (1).

$Total number of neutrons=20−10=10$

Substitute $10$ for a total number of neutrons and $10$ for a total number of protons in the equation (2).

$NZ=1010=1.$

Conclusion

The value of $(NZ)$ for $20Ne$ is $1.0$ .

(d)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $107Ag$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(d)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $107Ag$ is $1.3$ .

Explanation of Solution

In $A47107g$ atoms, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $A47107g$ is 47. Thus, the number of protons is 47.

Substitute $107$ for the mass number and 47 for the total number of protons in equation (1).

$Total number of neutrons=107−47=60$

Substitute $60$ for a total number of neutrons and $47$ for the total number of protons in the equation (2).

$NZ=6047=1.3.$

Conclusion

The value of $(NZ)$ for $107Ag$ is $1.3$ .

(e)

Interpretation Introduction

Interpretation:

The number of neutrons, proton, and electron in $234U$ , $238U$ , $214Pb$ , $210Pb$ and $206Pb$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

(e)

Expert Solution

Answer to Problem 2.140P

The number of neutrons, protons, and electrons in $234U$ , $238U$ , $214Pb$ , $210Pb$ and $206Pb$ are as follows:

$IsotopeNeutronsProtonsElectrons234U1469292238U1429292214Pb1328282210Pb1288282206Pb1248282$

Explanation of Solution

In $U92238$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $U92238$ is $92$ . Thus, the number of protons is 92. In neutral atom number of electrons is equal to the number of protons, therefore, the number of electrons is 92.

Substitute $238$ for the mass number and 92 for the total number of protons in equation (1) to calculate the number of neutrons in $U92238$ .

$Total number of neutrons=238−92=146$

In $U92234$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $U92234$ is $92$ . Thus, the number of protons is 92 and the number of electrons is also 92.

Substitute 234 for the mass number and 92 for the total number of protons in equation (1) to calculate the number of neutrons in $U92234$ .

$Total number of neutrons=234−92=142$

In $P82214b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, the number of protons is 82 and the number of electrons is also 82.

Substitute $214$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82214b$ .

$Total number of neutrons=214−82=132$

In $P82210b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, the number of protons is 82 and the number of electrons is also 82.

Substitute $210$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82210b$ .

$Total number of neutrons=210−82=128$

In $P82206b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, a number of protons is 82 and the number of electrons is 82.

Substitute $206$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82206b$ .

$Total number of neutrons=206−82=124.$

Conclusion

Isotopes are the atoms of the same element with the same atomic number but different mass number. In a neutral atom, the number of electrons is equal to the number of protons.

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Answer 5

Chapter 2, Problem 2.140P

(a)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $144Sm$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(a)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $144Sm$ is $1.3$ .

Explanation of Solution

In $S62144m$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $144Sm$ an atom is $62$ . Thus, the number of protons in $S62144m$ is $62$ .

Substitute $144$ for the mass number and $62$ for the total number of protons in equation (1) to calculate the number of neutrons in $S62144m$ .

$Total number of neutrons=144−62=82$

Substitute $82$ for a total number of neutrons and $62$ for the total number of protons in the equation (2).

$NZ=8262=1.3.$

Conclusion

The value of $(NZ)$ for $144Sm$ is $1.3$ .

(b)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $56Fe$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(b)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $56Fe$ is $1.2$ .

Explanation of Solution

In $F2656e$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $F2656e$ is $26$ . Thus, the number of protons is 26.

Substitute $56$ for the mass number and 26 for the total number of protons in equation (1).

$Total number of neutrons=56−26=30$

Substitute $30$ for a total number of neutrons and $26$ for a total number of protons in the equation (2).

$NZ=3026=1.2.$

Conclusion

The value of $(NZ)$ for $56Fe$ is $1.2$ .

(c)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $20Ne$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(c)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $20Ne$ is $1.0$ .

Explanation of Solution

In $N1020e$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $N1020e$ is 10. Thus, the number of protons is 10.

Substitute $20$ for the mass number and 10 for the total number of protons in equation (1).

$Total number of neutrons=20−10=10$

Substitute $10$ for a total number of neutrons and $10$ for a total number of protons in the equation (2).

$NZ=1010=1.$

Conclusion

The value of $(NZ)$ for $20Ne$ is $1.0$ .

(d)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $107Ag$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(d)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $107Ag$ is $1.3$ .

Explanation of Solution

In $A47107g$ atoms, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $A47107g$ is 47. Thus, the number of protons is 47.

Substitute $107$ for the mass number and 47 for the total number of protons in equation (1).

$Total number of neutrons=107−47=60$

Substitute $60$ for a total number of neutrons and $47$ for the total number of protons in the equation (2).

$NZ=6047=1.3.$

Conclusion

The value of $(NZ)$ for $107Ag$ is $1.3$ .

(e)

Interpretation Introduction

Interpretation:

The number of neutrons, proton, and electron in $234U$ , $238U$ , $214Pb$ , $210Pb$ and $206Pb$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

(e)

Expert Solution

Answer to Problem 2.140P

The number of neutrons, protons, and electrons in $234U$ , $238U$ , $214Pb$ , $210Pb$ and $206Pb$ are as follows:

$IsotopeNeutronsProtonsElectrons234U1469292238U1429292214Pb1328282210Pb1288282206Pb1248282$

Explanation of Solution

In $U92238$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $U92238$ is $92$ . Thus, the number of protons is 92. In neutral atom number of electrons is equal to the number of protons, therefore, the number of electrons is 92.

Substitute $238$ for the mass number and 92 for the total number of protons in equation (1) to calculate the number of neutrons in $U92238$ .

$Total number of neutrons=238−92=146$

In $U92234$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $U92234$ is $92$ . Thus, the number of protons is 92 and the number of electrons is also 92.

Substitute 234 for the mass number and 92 for the total number of protons in equation (1) to calculate the number of neutrons in $U92234$ .

$Total number of neutrons=234−92=142$

In $P82214b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, the number of protons is 82 and the number of electrons is also 82.

Substitute $214$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82214b$ .

$Total number of neutrons=214−82=132$

In $P82210b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, the number of protons is 82 and the number of electrons is also 82.

Substitute $210$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82210b$ .

$Total number of neutrons=210−82=128$

In $P82206b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, a number of protons is 82 and the number of electrons is 82.

Substitute $206$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82206b$ .

$Total number of neutrons=206−82=124.$

Conclusion

Isotopes are the atoms of the same element with the same atomic number but different mass number. In a neutral atom, the number of electrons is equal to the number of protons.

Answer 6

Chapter 2, Problem 2.140P

(a)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $144Sm$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(a)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $144Sm$ is $1.3$ .

Explanation of Solution

In $S62144m$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $144Sm$ an atom is $62$ . Thus, the number of protons in $S62144m$ is $62$ .

Substitute $144$ for the mass number and $62$ for the total number of protons in equation (1) to calculate the number of neutrons in $S62144m$ .

$Total number of neutrons=144−62=82$

Substitute $82$ for a total number of neutrons and $62$ for the total number of protons in the equation (2).

$NZ=8262=1.3.$

Conclusion

The value of $(NZ)$ for $144Sm$ is $1.3$ .

Answer 7

Chapter 2, Problem 2.140P

(a)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $144Sm$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

Answer 8

(a)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $144Sm$ is $1.3$ .

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

In $S62144m$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $144Sm$ an atom is $62$ . Thus, the number of protons in $S62144m$ is $62$ .

Substitute $144$ for the mass number and $62$ for the total number of protons in equation (1) to calculate the number of neutrons in $S62144m$ .

$Total number of neutrons=144−62=82$

Substitute $82$ for a total number of neutrons and $62$ for the total number of protons in the equation (2).

$NZ=8262=1.3.$

Answer 13

Conclusion

The value of $(NZ)$ for $144Sm$ is $1.3$ .

Answer 14

(b)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $56Fe$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(b)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $56Fe$ is $1.2$ .

Explanation of Solution

In $F2656e$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $F2656e$ is $26$ . Thus, the number of protons is 26.

Substitute $56$ for the mass number and 26 for the total number of protons in equation (1).

$Total number of neutrons=56−26=30$

Substitute $30$ for a total number of neutrons and $26$ for a total number of protons in the equation (2).

$NZ=3026=1.2.$

Conclusion

The value of $(NZ)$ for $56Fe$ is $1.2$ .

Answer 15

(b)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $56Fe$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

Answer 16

(b)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $56Fe$ is $1.2$ .

Answer 17

(b)

Expert Solution

Answer 18

(b)

Expert Solution

Answer 19

Expert Solution

Answer 20

Explanation of Solution

In $F2656e$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $F2656e$ is $26$ . Thus, the number of protons is 26.

Substitute $56$ for the mass number and 26 for the total number of protons in equation (1).

$Total number of neutrons=56−26=30$

Substitute $30$ for a total number of neutrons and $26$ for a total number of protons in the equation (2).

$NZ=3026=1.2.$

Answer 21

Conclusion

The value of $(NZ)$ for $56Fe$ is $1.2$ .

Answer 22

(c)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $20Ne$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(c)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $20Ne$ is $1.0$ .

Explanation of Solution

In $N1020e$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $N1020e$ is 10. Thus, the number of protons is 10.

Substitute $20$ for the mass number and 10 for the total number of protons in equation (1).

$Total number of neutrons=20−10=10$

Substitute $10$ for a total number of neutrons and $10$ for a total number of protons in the equation (2).

$NZ=1010=1.$

Conclusion

The value of $(NZ)$ for $20Ne$ is $1.0$ .

Answer 23

(c)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $20Ne$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

Answer 24

(c)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $20Ne$ is $1.0$ .

Answer 25

(c)

Expert Solution

Answer 26

(c)

Expert Solution

Answer 27

Expert Solution

Answer 28

Explanation of Solution

In $N1020e$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $N1020e$ is 10. Thus, the number of protons is 10.

Substitute $20$ for the mass number and 10 for the total number of protons in equation (1).

$Total number of neutrons=20−10=10$

Substitute $10$ for a total number of neutrons and $10$ for a total number of protons in the equation (2).

$NZ=1010=1.$

Answer 29

Conclusion

The value of $(NZ)$ for $20Ne$ is $1.0$ .

Answer 30

(d)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $107Ag$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

(d)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $107Ag$ is $1.3$ .

Explanation of Solution

In $A47107g$ atoms, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $A47107g$ is 47. Thus, the number of protons is 47.

Substitute $107$ for the mass number and 47 for the total number of protons in equation (1).

$Total number of neutrons=107−47=60$

Substitute $60$ for a total number of neutrons and $47$ for the total number of protons in the equation (2).

$NZ=6047=1.3.$

Conclusion

The value of $(NZ)$ for $107Ag$ is $1.3$ .

Answer 31

(d)

Interpretation Introduction

Interpretation:

The ratio of the number of neutrons to a number of proton for $107Ag$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

The expression to calculate the ratio of $(NZ)$ is as follows:

$NZ=Total number of neutronsTotal number of proton$ (2)

Answer 32

(d)

Expert Solution

Answer to Problem 2.140P

The ratio of the number of neutrons to a number of proton for $107Ag$ is $1.3$ .

Answer 33

(d)

Expert Solution

Answer 34

(d)

Expert Solution

Answer 35

Expert Solution

Answer 36

Explanation of Solution

In $A47107g$ atoms, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $A47107g$ is 47. Thus, the number of protons is 47.

Substitute $107$ for the mass number and 47 for the total number of protons in equation (1).

$Total number of neutrons=107−47=60$

Substitute $60$ for a total number of neutrons and $47$ for the total number of protons in the equation (2).

$NZ=6047=1.3.$

Answer 37

Conclusion

The value of $(NZ)$ for $107Ag$ is $1.3$ .

Answer 38

(e)

Interpretation Introduction

Interpretation:

The number of neutrons, proton, and electron in $234U$ , $238U$ , $214Pb$ , $210Pb$ and $206Pb$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

(e)

Expert Solution

Answer to Problem 2.140P

The number of neutrons, protons, and electrons in $234U$ , $238U$ , $214Pb$ , $210Pb$ and $206Pb$ are as follows:

$IsotopeNeutronsProtonsElectrons234U1469292238U1429292214Pb1328282210Pb1288282206Pb1248282$

Explanation of Solution

In $U92238$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $U92238$ is $92$ . Thus, the number of protons is 92. In neutral atom number of electrons is equal to the number of protons, therefore, the number of electrons is 92.

Substitute $238$ for the mass number and 92 for the total number of protons in equation (1) to calculate the number of neutrons in $U92238$ .

$Total number of neutrons=238−92=146$

In $U92234$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $U92234$ is $92$ . Thus, the number of protons is 92 and the number of electrons is also 92.

Substitute 234 for the mass number and 92 for the total number of protons in equation (1) to calculate the number of neutrons in $U92234$ .

$Total number of neutrons=234−92=142$

In $P82214b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, the number of protons is 82 and the number of electrons is also 82.

Substitute $214$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82214b$ .

$Total number of neutrons=214−82=132$

In $P82210b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, the number of protons is 82 and the number of electrons is also 82.

Substitute $210$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82210b$ .

$Total number of neutrons=210−82=128$

In $P82206b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, a number of protons is 82 and the number of electrons is 82.

Substitute $206$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82206b$ .

$Total number of neutrons=206−82=124.$

Conclusion

Isotopes are the atoms of the same element with the same atomic number but different mass number. In a neutral atom, the number of electrons is equal to the number of protons.

Answer 39

(e)

Interpretation Introduction

Interpretation:

The number of neutrons, proton, and electron in $234U$ , $238U$ , $214Pb$ , $210Pb$ and $206Pb$ 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 $ZAX$ . 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,

$Total number of neutrons(N)=[Mass number(A)−Total number of protons(Z)]$ (1)

Answer 40

(e)

Expert Solution

Answer to Problem 2.140P

The number of neutrons, protons, and electrons in $234U$ , $238U$ , $214Pb$ , $210Pb$ and $206Pb$ are as follows:

$IsotopeNeutronsProtonsElectrons234U1469292238U1429292214Pb1328282210Pb1288282206Pb1248282$

Answer 41

(e)

Expert Solution

Answer 42

(e)

Expert Solution

Answer 43

Expert Solution

Answer 44

Explanation of Solution

In $U92238$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $U92238$ is $92$ . Thus, the number of protons is 92. In neutral atom number of electrons is equal to the number of protons, therefore, the number of electrons is 92.

Substitute $238$ for the mass number and 92 for the total number of protons in equation (1) to calculate the number of neutrons in $U92238$ .

$Total number of neutrons=238−92=146$

In $U92234$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of $U92234$ is $92$ . Thus, the number of protons is 92 and the number of electrons is also 92.

Substitute 234 for the mass number and 92 for the total number of protons in equation (1) to calculate the number of neutrons in $U92234$ .

$Total number of neutrons=234−92=142$

In $P82214b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, the number of protons is 82 and the number of electrons is also 82.

Substitute $214$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82214b$ .

$Total number of neutrons=214−82=132$

In $P82210b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, the number of protons is 82 and the number of electrons is also 82.

Substitute $210$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82210b$ .

$Total number of neutrons=210−82=128$

In $P82206b$ atom, the number of protons and electrons is the same since the atom is a neutral species. The atomic number is equal to the number of protons. The atomic number of this atom is 82. Thus, a number of protons is 82 and the number of electrons is 82.

Substitute $206$ for the mass number and 82 for the total number of protons in equation (1) to calculate the number of neutrons in $P82206b$ .

$Total number of neutrons=206−82=124.$

Answer 45

Conclusion

Isotopes are the atoms of the same element with the same atomic number but different mass number. In a neutral atom, the number of electrons is equal to the number of protons.