Indicate which one of the two species in each of the following pairs is smaller: (a) Cl or Cl − ; (b) Na or Na + ; (c) O 2− or S 2− ; (d) Mg 2+ or Al 3+ ; (e) Au + or Au 3+ .

Question

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Answer 1

Textbook Question

Chapter 8, Problem 8.43QP

Indicate which one of the two species in each of the following pairs is smaller: (a) Cl or Cl⁻; (b) Na or Na⁺; (c) O²⁻ or S²⁻; (d) Mg²⁺ or Al³⁺; (e) Au⁺ or Au³⁺.

(a)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (a) Cl will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (a) is,

Species	Total number of Electrons	Total number of Protons
Cl	17	17
Cl-	18	17

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of protons in all the given species is same, but the total numbers of electrons are different.

Cl have smaller size than Cl- because,

By comparing the total number of protons and electrons in the table given in the previous step and as comparing to the size of atom size of anion is larger. And also here the proton number is lesser than the electron in Cl- so the size of the ion will be larger due to more shielding

(b)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (b) Na+ will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (b)

Species	Total number of Electrons	Total number of Protons
Na	11	11
Na+	10	11

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total numbers of protons in all the given species are same, but the total numbers of electrons are different.

Na+ have smaller size than Na, because

By comparing the total number of protons and electrons in the table given in the previous step it is clear that the number of proton is greater than the electron in Na+ so the size of ion will be smaller due to less shielding. Therefore Na+ have smaller size than Na.

(c)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (c) O2- will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (c)

Species	Total number of Electrons	Total number of Protons
O2-	8	10
S2-	16	18

The total number of electrons and protons present for the given species are found out and presented in the above table.

O2- Will be smaller compared to S2-

The given two species belong to group “6A” of periodic table. The oxygen atom comes before the sulphur atom when we move down the periodic table. As discussed above, when we move down the group the ionic radius increases because the electrons are added to a new subshell. Hence, O2- will be smaller compared to S2-

(d)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (d) Al3+ will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (d)

Species	Total number of Electrons	Total number of Protons
Mg2+	10	12
Al3+	10	13

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of electrons in all the given ions is same, but the total numbers of protons are different.

Al3+ have smaller size than Mg2+ because,

The number of proton in Al3+ is greater than the number of protons in the Mg2+. When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. Therefore Al3+ have small size than Mg2+.

(e)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (e) Au3+ will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (e)

Species	Total number of Electrons	Total number of Protons
Au	79	79
Au3+	76	79

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of protons in the given species is same, but the total numbers of electrons are different.

Au3+ have smaller size than Au because,

By comparing the total number of protons and electrons in the table given in the previous step it is clear that the number of proton is greater than the electron in Au3+ so the size of ion will be smaller due to less shielding. Therefore Au3+ have smaller size than Au.

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Students have asked these similar questions

b) For each pair indicate which Ion you would expect to have the largest Radius: (a) 02 and O; (b) N³ and Mg2+ (c) Al3* and Al

Boron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively. (a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Draw the orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons in boron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation for the reaction of solid boron with fluorine gas. (e) ΔHf° for BF3(g) is -1135.6 kj/mol. Calculate the standard enthalpy change in the reaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?

Identify each statement as true or false: (a) Cations are largerthan their corresponding neutral atoms. (b) Li+ is smallerthan Li. (c) Cl- is bigger than I-.

Answer 2

Textbook Question

Chapter 8, Problem 8.43QP

Indicate which one of the two species in each of the following pairs is smaller: (a) Cl or Cl⁻; (b) Na or Na⁺; (c) O²⁻ or S²⁻; (d) Mg²⁺ or Al³⁺; (e) Au⁺ or Au³⁺.

(a)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (a) Cl will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (a) is,

Species	Total number of Electrons	Total number of Protons
Cl	17	17
Cl-	18	17

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of protons in all the given species is same, but the total numbers of electrons are different.

Cl have smaller size than Cl- because,

By comparing the total number of protons and electrons in the table given in the previous step and as comparing to the size of atom size of anion is larger. And also here the proton number is lesser than the electron in Cl- so the size of the ion will be larger due to more shielding

(b)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (b) Na+ will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (b)

Species	Total number of Electrons	Total number of Protons
Na	11	11
Na+	10	11

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total numbers of protons in all the given species are same, but the total numbers of electrons are different.

Na+ have smaller size than Na, because

By comparing the total number of protons and electrons in the table given in the previous step it is clear that the number of proton is greater than the electron in Na+ so the size of ion will be smaller due to less shielding. Therefore Na+ have smaller size than Na.

(c)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (c) O2- will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (c)

Species	Total number of Electrons	Total number of Protons
O2-	8	10
S2-	16	18

The total number of electrons and protons present for the given species are found out and presented in the above table.

O2- Will be smaller compared to S2-

The given two species belong to group “6A” of periodic table. The oxygen atom comes before the sulphur atom when we move down the periodic table. As discussed above, when we move down the group the ionic radius increases because the electrons are added to a new subshell. Hence, O2- will be smaller compared to S2-

(d)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (d) Al3+ will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (d)

Species	Total number of Electrons	Total number of Protons
Mg2+	10	12
Al3+	10	13

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of electrons in all the given ions is same, but the total numbers of protons are different.

Al3+ have smaller size than Mg2+ because,

The number of proton in Al3+ is greater than the number of protons in the Mg2+. When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. Therefore Al3+ have small size than Mg2+.

(e)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (e) Au3+ will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (e)

Species	Total number of Electrons	Total number of Protons
Au	79	79
Au3+	76	79

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of protons in the given species is same, but the total numbers of electrons are different.

Au3+ have smaller size than Au because,

By comparing the total number of protons and electrons in the table given in the previous step it is clear that the number of proton is greater than the electron in Au3+ so the size of ion will be smaller due to less shielding. Therefore Au3+ have smaller size than Au.

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Answer 3

Textbook Question

Chapter 8, Problem 8.43QP

Indicate which one of the two species in each of the following pairs is smaller: (a) Cl or Cl⁻; (b) Na or Na⁺; (c) O²⁻ or S²⁻; (d) Mg²⁺ or Al³⁺; (e) Au⁺ or Au³⁺.

(a)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (a) Cl will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (a) is,

Species	Total number of Electrons	Total number of Protons
Cl	17	17
Cl-	18	17

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of protons in all the given species is same, but the total numbers of electrons are different.

Cl have smaller size than Cl- because,

By comparing the total number of protons and electrons in the table given in the previous step and as comparing to the size of atom size of anion is larger. And also here the proton number is lesser than the electron in Cl- so the size of the ion will be larger due to more shielding

(b)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (b) Na+ will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (b)

Species	Total number of Electrons	Total number of Protons
Na	11	11
Na+	10	11

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total numbers of protons in all the given species are same, but the total numbers of electrons are different.

Na+ have smaller size than Na, because

By comparing the total number of protons and electrons in the table given in the previous step it is clear that the number of proton is greater than the electron in Na+ so the size of ion will be smaller due to less shielding. Therefore Na+ have smaller size than Na.

(c)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (c) O2- will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (c)

Species	Total number of Electrons	Total number of Protons
O2-	8	10
S2-	16	18

The total number of electrons and protons present for the given species are found out and presented in the above table.

O2- Will be smaller compared to S2-

The given two species belong to group “6A” of periodic table. The oxygen atom comes before the sulphur atom when we move down the periodic table. As discussed above, when we move down the group the ionic radius increases because the electrons are added to a new subshell. Hence, O2- will be smaller compared to S2-

(d)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (d) Al3+ will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (d)

Species	Total number of Electrons	Total number of Protons
Mg2+	10	12
Al3+	10	13

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of electrons in all the given ions is same, but the total numbers of protons are different.

Al3+ have smaller size than Mg2+ because,

The number of proton in Al3+ is greater than the number of protons in the Mg2+. When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. Therefore Al3+ have small size than Mg2+.

(e)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (e) Au3+ will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (e)

Species	Total number of Electrons	Total number of Protons
Au	79	79
Au3+	76	79

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of protons in the given species is same, but the total numbers of electrons are different.

Au3+ have smaller size than Au because,

By comparing the total number of protons and electrons in the table given in the previous step it is clear that the number of proton is greater than the electron in Au3+ so the size of ion will be smaller due to less shielding. Therefore Au3+ have smaller size than Au.

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Answer 4

Textbook Question

Chapter 8, Problem 8.43QP

Indicate which one of the two species in each of the following pairs is smaller: (a) Cl or Cl⁻; (b) Na or Na⁺; (c) O²⁻ or S²⁻; (d) Mg²⁺ or Al³⁺; (e) Au⁺ or Au³⁺.

(a)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (a) Cl will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (a) is,

Species	Total number of Electrons	Total number of Protons
Cl	17	17
Cl-	18	17

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of protons in all the given species is same, but the total numbers of electrons are different.

Cl have smaller size than Cl- because,

By comparing the total number of protons and electrons in the table given in the previous step and as comparing to the size of atom size of anion is larger. And also here the proton number is lesser than the electron in Cl- so the size of the ion will be larger due to more shielding

(b)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (b) Na+ will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (b)

Species	Total number of Electrons	Total number of Protons
Na	11	11
Na+	10	11

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total numbers of protons in all the given species are same, but the total numbers of electrons are different.

Na+ have smaller size than Na, because

By comparing the total number of protons and electrons in the table given in the previous step it is clear that the number of proton is greater than the electron in Na+ so the size of ion will be smaller due to less shielding. Therefore Na+ have smaller size than Na.

(c)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (c) O2- will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (c)

Species	Total number of Electrons	Total number of Protons
O2-	8	10
S2-	16	18

The total number of electrons and protons present for the given species are found out and presented in the above table.

O2- Will be smaller compared to S2-

The given two species belong to group “6A” of periodic table. The oxygen atom comes before the sulphur atom when we move down the periodic table. As discussed above, when we move down the group the ionic radius increases because the electrons are added to a new subshell. Hence, O2- will be smaller compared to S2-

(d)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (d) Al3+ will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (d)

Species	Total number of Electrons	Total number of Protons
Mg2+	10	12
Al3+	10	13

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of electrons in all the given ions is same, but the total numbers of protons are different.

Al3+ have smaller size than Mg2+ because,

The number of proton in Al3+ is greater than the number of protons in the Mg2+. When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. Therefore Al3+ have small size than Mg2+.

(e)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (e) Au3+ will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (e)

Species	Total number of Electrons	Total number of Protons
Au	79	79
Au3+	76	79

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of protons in the given species is same, but the total numbers of electrons are different.

Au3+ have smaller size than Au because,

By comparing the total number of protons and electrons in the table given in the previous step it is clear that the number of proton is greater than the electron in Au3+ so the size of ion will be smaller due to less shielding. Therefore Au3+ have smaller size than Au.

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Answer 5

Textbook Question

Answer 6

Textbook Question

Answer 7

(a)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (a) Cl will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (a) is,

Species	Total number of Electrons	Total number of Protons
Cl	17	17
Cl-	18	17

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of protons in all the given species is same, but the total numbers of electrons are different.

Cl have smaller size than Cl- because,

By comparing the total number of protons and electrons in the table given in the previous step and as comparing to the size of atom size of anion is larger. And also here the proton number is lesser than the electron in Cl- so the size of the ion will be larger due to more shielding

(b)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (b) Na+ will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (b)

Species	Total number of Electrons	Total number of Protons
Na	11	11
Na+	10	11

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total numbers of protons in all the given species are same, but the total numbers of electrons are different.

Na+ have smaller size than Na, because

By comparing the total number of protons and electrons in the table given in the previous step it is clear that the number of proton is greater than the electron in Na+ so the size of ion will be smaller due to less shielding. Therefore Na+ have smaller size than Na.

(c)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (c) O2- will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (c)

Species	Total number of Electrons	Total number of Protons
O2-	8	10
S2-	16	18

The total number of electrons and protons present for the given species are found out and presented in the above table.

O2- Will be smaller compared to S2-

The given two species belong to group “6A” of periodic table. The oxygen atom comes before the sulphur atom when we move down the periodic table. As discussed above, when we move down the group the ionic radius increases because the electrons are added to a new subshell. Hence, O2- will be smaller compared to S2-

(d)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (d) Al3+ will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (d)

Species	Total number of Electrons	Total number of Protons
Mg2+	10	12
Al3+	10	13

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of electrons in all the given ions is same, but the total numbers of protons are different.

Al3+ have smaller size than Mg2+ because,

The number of proton in Al3+ is greater than the number of protons in the Mg2+. When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. Therefore Al3+ have small size than Mg2+.

(e)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (e) Au3+ will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (e)

Species	Total number of Electrons	Total number of Protons
Au	79	79
Au3+	76	79

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of protons in the given species is same, but the total numbers of electrons are different.

Au3+ have smaller size than Au because,

By comparing the total number of protons and electrons in the table given in the previous step it is clear that the number of proton is greater than the electron in Au3+ so the size of ion will be smaller due to less shielding. Therefore Au3+ have smaller size than Au.

Answer 8

(a)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (a) Cl will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (a) is,

Species	Total number of Electrons	Total number of Protons
Cl	17	17
Cl-	18	17

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of protons in all the given species is same, but the total numbers of electrons are different.

Cl have smaller size than Cl- because,

By comparing the total number of protons and electrons in the table given in the previous step and as comparing to the size of atom size of anion is larger. And also here the proton number is lesser than the electron in Cl- so the size of the ion will be larger due to more shielding

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer 13

Answer to Problem 8.43QP

In (a) Cl will be smaller in the given set of species

Answer 14

Explanation of Solution

The number of electrons and protons in the given set of species (a) is,

Species	Total number of Electrons	Total number of Protons
Cl	17	17
Cl-	18	17

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of protons in all the given species is same, but the total numbers of electrons are different.

Cl have smaller size than Cl- because,

By comparing the total number of protons and electrons in the table given in the previous step and as comparing to the size of atom size of anion is larger. And also here the proton number is lesser than the electron in Cl- so the size of the ion will be larger due to more shielding

Answer 15

(b)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (b) Na+ will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (b)

Species	Total number of Electrons	Total number of Protons
Na	11	11
Na+	10	11

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total numbers of protons in all the given species are same, but the total numbers of electrons are different.

Na+ have smaller size than Na, because

By comparing the total number of protons and electrons in the table given in the previous step it is clear that the number of proton is greater than the electron in Na+ so the size of ion will be smaller due to less shielding. Therefore Na+ have smaller size than Na.

Answer 16

(b)

Expert Solution

Answer 17

(b)

Expert Solution

Answer 18

Expert Solution

Answer 19

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer 20

Answer to Problem 8.43QP

In (b) Na+ will be smaller in the given set of species

Answer 21

Explanation of Solution

The number of electrons and protons in the given set of species (b)

Species	Total number of Electrons	Total number of Protons
Na	11	11
Na+	10	11

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total numbers of protons in all the given species are same, but the total numbers of electrons are different.

Na+ have smaller size than Na, because

By comparing the total number of protons and electrons in the table given in the previous step it is clear that the number of proton is greater than the electron in Na+ so the size of ion will be smaller due to less shielding. Therefore Na+ have smaller size than Na.

Answer 22

(c)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (c) O2- will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (c)

Species	Total number of Electrons	Total number of Protons
O2-	8	10
S2-	16	18

The total number of electrons and protons present for the given species are found out and presented in the above table.

O2- Will be smaller compared to S2-

The given two species belong to group “6A” of periodic table. The oxygen atom comes before the sulphur atom when we move down the periodic table. As discussed above, when we move down the group the ionic radius increases because the electrons are added to a new subshell. Hence, O2- will be smaller compared to S2-

Answer 23

(c)

Expert Solution

Answer 24

(c)

Expert Solution

Answer 25

Expert Solution

Answer 26

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer 27

Answer to Problem 8.43QP

In (c) O2- will be smaller in the given set of species

Answer 28

Explanation of Solution

The number of electrons and protons in the given set of species (c)

Species	Total number of Electrons	Total number of Protons
O2-	8	10
S2-	16	18

The total number of electrons and protons present for the given species are found out and presented in the above table.

O2- Will be smaller compared to S2-

The given two species belong to group “6A” of periodic table. The oxygen atom comes before the sulphur atom when we move down the periodic table. As discussed above, when we move down the group the ionic radius increases because the electrons are added to a new subshell. Hence, O2- will be smaller compared to S2-

Answer 29

(d)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (d) Al3+ will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (d)

Species	Total number of Electrons	Total number of Protons
Mg2+	10	12
Al3+	10	13

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of electrons in all the given ions is same, but the total numbers of protons are different.

Al3+ have smaller size than Mg2+ because,

The number of proton in Al3+ is greater than the number of protons in the Mg2+. When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. Therefore Al3+ have small size than Mg2+.

Answer 30

(d)

Expert Solution

Answer 31

(d)

Expert Solution

Answer 32

Expert Solution

Answer 33

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer 34

Answer to Problem 8.43QP

In (d) Al3+ will be smaller in the given set of species

Answer 35

Explanation of Solution

The number of electrons and protons in the given set of species (d)

Species	Total number of Electrons	Total number of Protons
Mg2+	10	12
Al3+	10	13

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of electrons in all the given ions is same, but the total numbers of protons are different.

Al3+ have smaller size than Mg2+ because,

The number of proton in Al3+ is greater than the number of protons in the Mg2+. When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. Therefore Al3+ have small size than Mg2+.

Answer 36

(e)

Expert Solution

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer to Problem 8.43QP

In (e) Au3+ will be smaller in the given set of species

Explanation of Solution

The number of electrons and protons in the given set of species (e)

Species	Total number of Electrons	Total number of Protons
Au	79	79
Au3+	76	79

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of protons in the given species is same, but the total numbers of electrons are different.

Au3+ have smaller size than Au because,

By comparing the total number of protons and electrons in the table given in the previous step it is clear that the number of proton is greater than the electron in Au3+ so the size of ion will be smaller due to less shielding. Therefore Au3+ have smaller size than Au.

Answer 37

(e)

Expert Solution

Answer 38

(e)

Expert Solution

Answer 39

Expert Solution

Answer 40

Interpretation Introduction

Interpretation:

In the given set of species which will be smaller in size has to be identified.

Concept Introduction:

The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
Anions will have larger size compared to cations.
The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.

Answer 41

Answer to Problem 8.43QP

In (e) Au3+ will be smaller in the given set of species

Answer 42

Explanation of Solution

The number of electrons and protons in the given set of species (e)

Species	Total number of Electrons	Total number of Protons
Au	79	79
Au3+	76	79

The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of protons in the given species is same, but the total numbers of electrons are different.

Au3+ have smaller size than Au because,

By comparing the total number of protons and electrons in the table given in the previous step it is clear that the number of proton is greater than the electron in Au3+ so the size of ion will be smaller due to less shielding. Therefore Au3+ have smaller size than Au.