The electronic configuration of Plutonium (Pu) has to be predicted using the noble gas and ( s, p, d, f ) orbital notation methods. Concept Introduction: Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals. The important there rules for electronic configuration given below: Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied. Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin. Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.

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Answer 1

Question

Chapter 7, Problem 10PS

a)

Interpretation Introduction

Interpretation:

The electronic configuration of Plutonium (Pu) has to be predicted using the noble gas and (s, p, d, f) orbital notation methods.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

The important there rules for electronic configuration given below:

Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.

a)

Expert Solution

Explanation of Solution

The electron configuration is,

Atomic number of Plutonium (Pu) =94Complete (spdf) notation of (Pu) = 1s22s22p63s23p63d104s24p64d10 5s25p64f145d106s26p65f66d07s2Orbital filling method =↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 1s2 2s2 2p6 3s2 3p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 3d10 4s2 4p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 4d10 5s2 5p6 ↑↓↑↓↑↓↑↓↑↓↑↓↑↓ ↑↓↑↓↑↓↑↓↑↓ ↑↓ 4f14 5d3 6s2 ↑↓↑↓↑↓ ↑↑↑↑↑↑ ↑↓ 6p6 5f6 7s2spdf with noble gas notation = [Rn]5f67s2 [∵ Atomic number of Radon=86]Orbital box notation = [Rn] ↑↑↑↑↑↑ ↑↓ 5f6 6d0 7s2

The electron configuration is, [Rn]5f67s2

b)

Interpretation Introduction

Interpretation:

The electronic configuration of Curium (Cm) has to be derived using the noble gas and (s, p, d, f) orbital notation methods.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

The important there rules for electronic configuration given below:

Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.

b)

Expert Solution

Explanation of Solution

The electron configuration is,

Atomic number of Curium (Cm) =96Complete (spdf) notation of (Cm) = 1s22s22p63s23p63d104s24p64d10 5s25p64f145d106s26p65f76d17s2Orbital filling method =↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 1s2 2s2 2p6 3s2 3p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 3d10 4s2 4p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 4d10 5s2 5p6 ↑↓↑↓↑↓↑↓↑↓↑↓↑↓ ↑↓↑↓↑↓↑↓↑↓ ↑↓ 4f14 5d10 6s2 ↑↓↑↓↑↓ ↑↑↑↑↑↑↑ ↑ ↑↓ 6p6 5f7 6d1 7s2spdf with noble gas notation = [Rn] 5f76d17s2 [∵ Atomic number of Radon=86]Orbital box notation = [Rn] ↑↑↑↑↑↑↑ ↑ ↑↓ 5f7 6d1 7s2

The electron configuration is,[Rn] 5f76d17s2

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Answer 2

Question

Chapter 7, Problem 10PS

a)

Interpretation Introduction

Interpretation:

The electronic configuration of Plutonium (Pu) has to be predicted using the noble gas and (s, p, d, f) orbital notation methods.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

The important there rules for electronic configuration given below:

Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.

a)

Expert Solution

Explanation of Solution

The electron configuration is,

Atomic number of Plutonium (Pu) =94Complete (spdf) notation of (Pu) = 1s22s22p63s23p63d104s24p64d10 5s25p64f145d106s26p65f66d07s2Orbital filling method =↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 1s2 2s2 2p6 3s2 3p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 3d10 4s2 4p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 4d10 5s2 5p6 ↑↓↑↓↑↓↑↓↑↓↑↓↑↓ ↑↓↑↓↑↓↑↓↑↓ ↑↓ 4f14 5d3 6s2 ↑↓↑↓↑↓ ↑↑↑↑↑↑ ↑↓ 6p6 5f6 7s2spdf with noble gas notation = [Rn]5f67s2 [∵ Atomic number of Radon=86]Orbital box notation = [Rn] ↑↑↑↑↑↑ ↑↓ 5f6 6d0 7s2

The electron configuration is, [Rn]5f67s2

b)

Interpretation Introduction

Interpretation:

The electronic configuration of Curium (Cm) has to be derived using the noble gas and (s, p, d, f) orbital notation methods.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

The important there rules for electronic configuration given below:

Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.

b)

Expert Solution

Explanation of Solution

The electron configuration is,

Atomic number of Curium (Cm) =96Complete (spdf) notation of (Cm) = 1s22s22p63s23p63d104s24p64d10 5s25p64f145d106s26p65f76d17s2Orbital filling method =↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 1s2 2s2 2p6 3s2 3p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 3d10 4s2 4p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 4d10 5s2 5p6 ↑↓↑↓↑↓↑↓↑↓↑↓↑↓ ↑↓↑↓↑↓↑↓↑↓ ↑↓ 4f14 5d10 6s2 ↑↓↑↓↑↓ ↑↑↑↑↑↑↑ ↑ ↑↓ 6p6 5f7 6d1 7s2spdf with noble gas notation = [Rn] 5f76d17s2 [∵ Atomic number of Radon=86]Orbital box notation = [Rn] ↑↑↑↑↑↑↑ ↑ ↑↓ 5f7 6d1 7s2

The electron configuration is,[Rn] 5f76d17s2

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Answer 3

Question

Chapter 7, Problem 10PS

a)

Interpretation Introduction

Interpretation:

The electronic configuration of Plutonium (Pu) has to be predicted using the noble gas and (s, p, d, f) orbital notation methods.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

The important there rules for electronic configuration given below:

Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.

a)

Expert Solution

Explanation of Solution

The electron configuration is,

Atomic number of Plutonium (Pu) =94Complete (spdf) notation of (Pu) = 1s22s22p63s23p63d104s24p64d10 5s25p64f145d106s26p65f66d07s2Orbital filling method =↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 1s2 2s2 2p6 3s2 3p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 3d10 4s2 4p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 4d10 5s2 5p6 ↑↓↑↓↑↓↑↓↑↓↑↓↑↓ ↑↓↑↓↑↓↑↓↑↓ ↑↓ 4f14 5d3 6s2 ↑↓↑↓↑↓ ↑↑↑↑↑↑ ↑↓ 6p6 5f6 7s2spdf with noble gas notation = [Rn]5f67s2 [∵ Atomic number of Radon=86]Orbital box notation = [Rn] ↑↑↑↑↑↑ ↑↓ 5f6 6d0 7s2

The electron configuration is, [Rn]5f67s2

b)

Interpretation Introduction

Interpretation:

The electronic configuration of Curium (Cm) has to be derived using the noble gas and (s, p, d, f) orbital notation methods.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

The important there rules for electronic configuration given below:

Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.

b)

Expert Solution

Explanation of Solution

The electron configuration is,

Atomic number of Curium (Cm) =96Complete (spdf) notation of (Cm) = 1s22s22p63s23p63d104s24p64d10 5s25p64f145d106s26p65f76d17s2Orbital filling method =↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 1s2 2s2 2p6 3s2 3p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 3d10 4s2 4p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 4d10 5s2 5p6 ↑↓↑↓↑↓↑↓↑↓↑↓↑↓ ↑↓↑↓↑↓↑↓↑↓ ↑↓ 4f14 5d10 6s2 ↑↓↑↓↑↓ ↑↑↑↑↑↑↑ ↑ ↑↓ 6p6 5f7 6d1 7s2spdf with noble gas notation = [Rn] 5f76d17s2 [∵ Atomic number of Radon=86]Orbital box notation = [Rn] ↑↑↑↑↑↑↑ ↑ ↑↓ 5f7 6d1 7s2

The electron configuration is,[Rn] 5f76d17s2

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Answer 4

Question

Chapter 7, Problem 10PS

a)

Interpretation Introduction

Interpretation:

The electronic configuration of Plutonium (Pu) has to be predicted using the noble gas and (s, p, d, f) orbital notation methods.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

The important there rules for electronic configuration given below:

Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.

a)

Expert Solution

Explanation of Solution

The electron configuration is,

Atomic number of Plutonium (Pu) =94Complete (spdf) notation of (Pu) = 1s22s22p63s23p63d104s24p64d10 5s25p64f145d106s26p65f66d07s2Orbital filling method =↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 1s2 2s2 2p6 3s2 3p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 3d10 4s2 4p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 4d10 5s2 5p6 ↑↓↑↓↑↓↑↓↑↓↑↓↑↓ ↑↓↑↓↑↓↑↓↑↓ ↑↓ 4f14 5d3 6s2 ↑↓↑↓↑↓ ↑↑↑↑↑↑ ↑↓ 6p6 5f6 7s2spdf with noble gas notation = [Rn]5f67s2 [∵ Atomic number of Radon=86]Orbital box notation = [Rn] ↑↑↑↑↑↑ ↑↓ 5f6 6d0 7s2

The electron configuration is, [Rn]5f67s2

b)

Interpretation Introduction

Interpretation:

The electronic configuration of Curium (Cm) has to be derived using the noble gas and (s, p, d, f) orbital notation methods.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

The important there rules for electronic configuration given below:

Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.

b)

Expert Solution

Explanation of Solution

The electron configuration is,

Atomic number of Curium (Cm) =96Complete (spdf) notation of (Cm) = 1s22s22p63s23p63d104s24p64d10 5s25p64f145d106s26p65f76d17s2Orbital filling method =↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 1s2 2s2 2p6 3s2 3p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 3d10 4s2 4p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 4d10 5s2 5p6 ↑↓↑↓↑↓↑↓↑↓↑↓↑↓ ↑↓↑↓↑↓↑↓↑↓ ↑↓ 4f14 5d10 6s2 ↑↓↑↓↑↓ ↑↑↑↑↑↑↑ ↑ ↑↓ 6p6 5f7 6d1 7s2spdf with noble gas notation = [Rn] 5f76d17s2 [∵ Atomic number of Radon=86]Orbital box notation = [Rn] ↑↑↑↑↑↑↑ ↑ ↑↓ 5f7 6d1 7s2

The electron configuration is,[Rn] 5f76d17s2

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Answer 5

Chapter 7, Problem 10PS

a)

Interpretation Introduction

Interpretation:

The electronic configuration of Plutonium (Pu) has to be predicted using the noble gas and (s, p, d, f) orbital notation methods.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

The important there rules for electronic configuration given below:

Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.

a)

Expert Solution

Explanation of Solution

The electron configuration is,

Atomic number of Plutonium (Pu) =94Complete (spdf) notation of (Pu) = 1s22s22p63s23p63d104s24p64d10 5s25p64f145d106s26p65f66d07s2Orbital filling method =↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 1s2 2s2 2p6 3s2 3p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 3d10 4s2 4p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 4d10 5s2 5p6 ↑↓↑↓↑↓↑↓↑↓↑↓↑↓ ↑↓↑↓↑↓↑↓↑↓ ↑↓ 4f14 5d3 6s2 ↑↓↑↓↑↓ ↑↑↑↑↑↑ ↑↓ 6p6 5f6 7s2spdf with noble gas notation = [Rn]5f67s2 [∵ Atomic number of Radon=86]Orbital box notation = [Rn] ↑↑↑↑↑↑ ↑↓ 5f6 6d0 7s2

The electron configuration is, [Rn]5f67s2

b)

Interpretation Introduction

Interpretation:

The electronic configuration of Curium (Cm) has to be derived using the noble gas and (s, p, d, f) orbital notation methods.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

The important there rules for electronic configuration given below:

Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.

b)

Expert Solution

Explanation of Solution

The electron configuration is,

Atomic number of Curium (Cm) =96Complete (spdf) notation of (Cm) = 1s22s22p63s23p63d104s24p64d10 5s25p64f145d106s26p65f76d17s2Orbital filling method =↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 1s2 2s2 2p6 3s2 3p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 3d10 4s2 4p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 4d10 5s2 5p6 ↑↓↑↓↑↓↑↓↑↓↑↓↑↓ ↑↓↑↓↑↓↑↓↑↓ ↑↓ 4f14 5d10 6s2 ↑↓↑↓↑↓ ↑↑↑↑↑↑↑ ↑ ↑↓ 6p6 5f7 6d1 7s2spdf with noble gas notation = [Rn] 5f76d17s2 [∵ Atomic number of Radon=86]Orbital box notation = [Rn] ↑↑↑↑↑↑↑ ↑ ↑↓ 5f7 6d1 7s2

The electron configuration is,[Rn] 5f76d17s2

Answer 6

Chapter 7, Problem 10PS

a)

Interpretation Introduction

Interpretation:

The electronic configuration of Plutonium (Pu) has to be predicted using the noble gas and (s, p, d, f) orbital notation methods.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

The important there rules for electronic configuration given below:

Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.

a)

Expert Solution

Explanation of Solution

The electron configuration is,

Atomic number of Plutonium (Pu) =94Complete (spdf) notation of (Pu) = 1s22s22p63s23p63d104s24p64d10 5s25p64f145d106s26p65f66d07s2Orbital filling method =↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 1s2 2s2 2p6 3s2 3p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 3d10 4s2 4p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 4d10 5s2 5p6 ↑↓↑↓↑↓↑↓↑↓↑↓↑↓ ↑↓↑↓↑↓↑↓↑↓ ↑↓ 4f14 5d3 6s2 ↑↓↑↓↑↓ ↑↑↑↑↑↑ ↑↓ 6p6 5f6 7s2spdf with noble gas notation = [Rn]5f67s2 [∵ Atomic number of Radon=86]Orbital box notation = [Rn] ↑↑↑↑↑↑ ↑↓ 5f6 6d0 7s2

The electron configuration is, [Rn]5f67s2

Answer 7

Chapter 7, Problem 10PS

a)

Interpretation Introduction

Interpretation:

The electronic configuration of Plutonium (Pu) has to be predicted using the noble gas and (s, p, d, f) orbital notation methods.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

The important there rules for electronic configuration given below:

Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.

Answer 8

a)

Expert Solution

Explanation of Solution

The electron configuration is,

Atomic number of Plutonium (Pu) =94Complete (spdf) notation of (Pu) = 1s22s22p63s23p63d104s24p64d10 5s25p64f145d106s26p65f66d07s2Orbital filling method =↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 1s2 2s2 2p6 3s2 3p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 3d10 4s2 4p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 4d10 5s2 5p6 ↑↓↑↓↑↓↑↓↑↓↑↓↑↓ ↑↓↑↓↑↓↑↓↑↓ ↑↓ 4f14 5d3 6s2 ↑↓↑↓↑↓ ↑↑↑↑↑↑ ↑↓ 6p6 5f6 7s2spdf with noble gas notation = [Rn]5f67s2 [∵ Atomic number of Radon=86]Orbital box notation = [Rn] ↑↑↑↑↑↑ ↑↓ 5f6 6d0 7s2

The electron configuration is, [Rn]5f67s2

Answer 9

a)

Expert Solution

Answer 10

a)

Expert Solution

Answer 11

Expert Solution

Answer 12

b)

Interpretation Introduction

Interpretation:

The electronic configuration of Curium (Cm) has to be derived using the noble gas and (s, p, d, f) orbital notation methods.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

The important there rules for electronic configuration given below:

Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.

b)

Expert Solution

Explanation of Solution

The electron configuration is,

Atomic number of Curium (Cm) =96Complete (spdf) notation of (Cm) = 1s22s22p63s23p63d104s24p64d10 5s25p64f145d106s26p65f76d17s2Orbital filling method =↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 1s2 2s2 2p6 3s2 3p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 3d10 4s2 4p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 4d10 5s2 5p6 ↑↓↑↓↑↓↑↓↑↓↑↓↑↓ ↑↓↑↓↑↓↑↓↑↓ ↑↓ 4f14 5d10 6s2 ↑↓↑↓↑↓ ↑↑↑↑↑↑↑ ↑ ↑↓ 6p6 5f7 6d1 7s2spdf with noble gas notation = [Rn] 5f76d17s2 [∵ Atomic number of Radon=86]Orbital box notation = [Rn] ↑↑↑↑↑↑↑ ↑ ↑↓ 5f7 6d1 7s2

The electron configuration is,[Rn] 5f76d17s2

Answer 13

b)

Interpretation Introduction

Interpretation:

The electronic configuration of Curium (Cm) has to be derived using the noble gas and (s, p, d, f) orbital notation methods.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

The important there rules for electronic configuration given below:

Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.

Answer 14

b)

Expert Solution

Explanation of Solution

The electron configuration is,

Atomic number of Curium (Cm) =96Complete (spdf) notation of (Cm) = 1s22s22p63s23p63d104s24p64d10 5s25p64f145d106s26p65f76d17s2Orbital filling method =↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 1s2 2s2 2p6 3s2 3p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 3d10 4s2 4p6 ↑↓↑↓↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ 4d10 5s2 5p6 ↑↓↑↓↑↓↑↓↑↓↑↓↑↓ ↑↓↑↓↑↓↑↓↑↓ ↑↓ 4f14 5d10 6s2 ↑↓↑↓↑↓ ↑↑↑↑↑↑↑ ↑ ↑↓ 6p6 5f7 6d1 7s2spdf with noble gas notation = [Rn] 5f76d17s2 [∵ Atomic number of Radon=86]Orbital box notation = [Rn] ↑↑↑↑↑↑↑ ↑ ↑↓ 5f7 6d1 7s2