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.

Question

Want to see more full solutions like this?

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

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Students have asked these similar questions

For this question, if the product is racemic, input both enantiomers in the same Marvin editor. A) Input the number that corresponds to the reagent which when added to (E)-but-2-ene will result in a racemic product. Input 1 for Cl, in the cold and dark Input 2 for Oy followed by H₂O, Zn Input 3 for D₂ with metal catalyst Input 4 for H₂ with metal catalyst B) Draw the skeletal structure of the major organic product made from the reagent in part A Marvin JS Help Edit drawing C) Draw the skeletal structure of the major organic product formed when (2)-but-2-ene is treated with peroxyacetic acid. Marvin 35 Help

Michael Reactions 19.52 Draw the products from the following Michael addition reactions. 1. H&C CH (a) i 2. H₂O* (b) OEt (c) EtO H₂NEt (d) ΕΙΟ + 1. NaOEt 2. H₂O' H H 1. NaOEt 2. H₂O*

Rank the labeled protons (Ha-Hd) in order of increasing acidity, starting with the least acidic. НОН НЬ OHd Онс

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

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

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

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

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

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

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