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

Bookmarks Profiles Tab Window Help Chemical Formula - Aktiv Che X + → C 11 a app.aktiv.com Google Chrome isn't your default browser Set as default Question 12 of 16 Q Fri Feb 2 Verify it's you New Chrome availabl- Write the balanced molecular chemical equation for the reaction in aqueous solution for mercury(I) nitrate and chromium(VI) sulfate. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction. 3 Hg(NO3)2(aq) + Cг2(SO4)3(aq) → 3 Hg₂SO (s) + 2 Cr(NO3), (aq) ean Ui mate co ence an climate bility inc ulnerabili women, main critic CLIMATE-INI ernational + 10 O 2 W FEB 1 + 4- 3- 2- 2 2 ( 3 4 NS 28 2 ty 56 + 2+ 3+ 4+ 7 8 9 0 5 (s) (1) Ch O 8 9 (g) (aq) Hg NR CI Cr x H₂O A 80 Q A DII A F2 F3 FA F5 F6 F7 F8 F9 #3 EA $ do 50 % 6 CO & 7 E R T Y U 8 ( 9 0 F10 34 F11 川 F12 Subr + delete 0 { P }

Deducing the reactants of a Diels-Alder reaction n the molecule on the right-hand side of this organic reaction be made in good yield from no more than two reactants, in one step, by moderately heating the reactants? ? Δ • If your answer is yes, then draw the reactant or reactants in the drawing area below. You can draw the reactants in any arrangement you like. • If your answer is no, check the box under the drawing area instead. Explanation Check Click and drag to start drawing a structure. >

Predict the major products of the following organic reaction: + Some important notes: A ? • Draw the major product, or products, of the reaction in the drawing area below. • If there aren't any products, because no reaction will take place, check the box below the drawing area instead. • Be sure to use wedge and dash bonds when necessary, for example to distinguish between major products that are enantiomers. Explanation Check Click and drag to start drawing a structure.

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