The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations. Concept Introduction: An orbital is a region of space in which electrons are filled. It can hold up to two electrons. An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom. The orders in which orbitals are filled by the electrons are governed by three basic principles. 1. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons. 2. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins. 3. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin. The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written. To find: Count the total number of p-electrons in NGet the total number of electrons for N Nitrogen (N) is placed in VA group of the periodic table. Its atomic number is 7. Therefore, nitrogen has six electrons in its shells. Nitrogen (N) is a p-block element. So, its outermost electrons are located in a p-subshell.

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Answer 1

Question

Chapter 7, Problem 7.64QP

(a)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

1. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

2. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

3. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of p-electrons in NGet the total number of electrons for N

Nitrogen (N) is placed in VA group of the periodic table. Its atomic number is 7. Therefore, nitrogen has six electrons in its shells. Nitrogen (N) is a p-block element. So, its outermost electrons are located in a p-subshell.

(b)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

4. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

5. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

6. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of s-electrons in Si

Get the total number of electrons for Si

(c)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

7. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

8. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

9. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of 3d-electrons in S

Get the total number of electrons for S and S is placed in VIA group of the periodic table. Its atomic number is 16. Therefore, S has 16 electrons in its shells. S is a p-block element. So, its outermost electrons are located in a p-subshell.

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Answer 2

Question

Chapter 7, Problem 7.64QP

(a)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

1. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

2. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

3. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of p-electrons in NGet the total number of electrons for N

Nitrogen (N) is placed in VA group of the periodic table. Its atomic number is 7. Therefore, nitrogen has six electrons in its shells. Nitrogen (N) is a p-block element. So, its outermost electrons are located in a p-subshell.

(b)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

4. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

5. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

6. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of s-electrons in Si

Get the total number of electrons for Si

(c)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

7. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

8. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

9. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of 3d-electrons in S

Get the total number of electrons for S and S is placed in VIA group of the periodic table. Its atomic number is 16. Therefore, S has 16 electrons in its shells. S is a p-block element. So, its outermost electrons are located in a p-subshell.

Expert Solution & Answer

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Answer 3

Question

Chapter 7, Problem 7.64QP

(a)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

1. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

2. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

3. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of p-electrons in NGet the total number of electrons for N

Nitrogen (N) is placed in VA group of the periodic table. Its atomic number is 7. Therefore, nitrogen has six electrons in its shells. Nitrogen (N) is a p-block element. So, its outermost electrons are located in a p-subshell.

(b)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

4. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

5. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

6. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of s-electrons in Si

Get the total number of electrons for Si

(c)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

7. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

8. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

9. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of 3d-electrons in S

Get the total number of electrons for S and S is placed in VIA group of the periodic table. Its atomic number is 16. Therefore, S has 16 electrons in its shells. S is a p-block element. So, its outermost electrons are located in a p-subshell.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 7, Problem 7.64QP

(a)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

1. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

2. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

3. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of p-electrons in NGet the total number of electrons for N

Nitrogen (N) is placed in VA group of the periodic table. Its atomic number is 7. Therefore, nitrogen has six electrons in its shells. Nitrogen (N) is a p-block element. So, its outermost electrons are located in a p-subshell.

(b)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

4. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

5. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

6. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of s-electrons in Si

Get the total number of electrons for Si

(c)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

7. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

8. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

9. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of 3d-electrons in S

Get the total number of electrons for S and S is placed in VIA group of the periodic table. Its atomic number is 16. Therefore, S has 16 electrons in its shells. S is a p-block element. So, its outermost electrons are located in a p-subshell.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 5

Chapter 7, Problem 7.64QP

(a)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

1. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

2. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

3. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of p-electrons in NGet the total number of electrons for N

Nitrogen (N) is placed in VA group of the periodic table. Its atomic number is 7. Therefore, nitrogen has six electrons in its shells. Nitrogen (N) is a p-block element. So, its outermost electrons are located in a p-subshell.

(b)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

4. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

5. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

6. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of s-electrons in Si

Get the total number of electrons for Si

(c)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

7. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

8. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

9. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of 3d-electrons in S

Get the total number of electrons for S and S is placed in VIA group of the periodic table. Its atomic number is 16. Therefore, S has 16 electrons in its shells. S is a p-block element. So, its outermost electrons are located in a p-subshell.

Answer 6

Chapter 7, Problem 7.64QP

(a)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

1. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

2. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

3. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of p-electrons in NGet the total number of electrons for N

Nitrogen (N) is placed in VA group of the periodic table. Its atomic number is 7. Therefore, nitrogen has six electrons in its shells. Nitrogen (N) is a p-block element. So, its outermost electrons are located in a p-subshell.

Answer 7

Chapter 7, Problem 7.64QP

(a)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

1. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

2. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

3. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of p-electrons in NGet the total number of electrons for N

Nitrogen (N) is placed in VA group of the periodic table. Its atomic number is 7. Therefore, nitrogen has six electrons in its shells. Nitrogen (N) is a p-block element. So, its outermost electrons are located in a p-subshell.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

4. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

5. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

6. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of s-electrons in Si

Get the total number of electrons for Si

Answer 9

(b)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

4. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

5. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

6. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of s-electrons in Si

Get the total number of electrons for Si

Answer 10

(c)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

7. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

8. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

9. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of 3d-electrons in S

Get the total number of electrons for S and S is placed in VIA group of the periodic table. Its atomic number is 16. Therefore, S has 16 electrons in its shells. S is a p-block element. So, its outermost electrons are located in a p-subshell.

Answer 11

(c)

Interpretation Introduction

Interpretation:

The total number of the given shell electrons in the given atoms should be given by knowing their ground-state electron configurations.

Concept Introduction:

An orbital is a region of space in which electrons are filled. It can hold up to two electrons.

An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

The orders in which orbitals are filled by the electrons are governed by three basic principles.

7. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.

8. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

9. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.

The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.

To find: Count the total number of 3d-electrons in S

Get the total number of electrons for S and S is placed in VIA group of the periodic table. Its atomic number is 16. Therefore, S has 16 electrons in its shells. S is a p-block element. So, its outermost electrons are located in a p-subshell.

Answer 12

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Answer 13

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Answer 14

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Answer 15

Ch. 7.1 - Review of Concepts What of the waves shown here...Ch. 7.1 - Prob. 1PE Ch. 7.1 - Prob. 2RC Ch. 7.2 - Prob. 1PE Ch. 7.2 - Prob. 2PE Ch. 7.2 - Prob. 1RC Ch. 7.3 - Prob. 1PE Ch. 7.3 - Prob. 1RC Ch. 7.4 - Prob. 1PE Ch. 7.4 - Prob. 1RC

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