World of Chemistry, 3rd edition
World of Chemistry, 3rd edition
3rd Edition
ISBN: 9781133109655
Author: Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher: Brooks / Cole / Cengage Learning
bartleby

Videos

Question
Book Icon
Chapter 11, Problem 48A

(a)

Interpretation Introduction

Interpretation:

Short hand valence electron configuration of samarium with Z=62 should be determined.

Concept introduction:

Electronic configuration can be assigned to any elements in ground when they follow certain rules like Hund rule, Pauli Exclusion Principle and Aufbau rule. If atomic number of an element is Z then Z numbers of electrons are filled into the orbitals which are arranged in increasing order of energy.

No two electrons in an atom can have same group of four quantum numbers and this is Pauli Exclusion Principle.

While filling of orbital’s, electron first enters to each energy level with degenerate energy before paring of electron begins and this is Hund’s rules.

(a)

Expert Solution
Check Mark

Answer to Problem 48A

Short hand valence electron configuration of samarium with Z=62 is as follows:

  [Xe]4f66s2

Explanation of Solution

As per Aufbau rule electrons are filled in lower energy orbitals that are closer to the nucleus before they are filled in higher energy ones. The order of orbital arranged in their increasing energies is as follows:

  1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p< 6s<4f<5d<6p<7s<5f<6d<7p .

So complete electronic configuration of samarium with Z=62 is as follows:

  1s22s22p63s23p64s23d104p65s24d105p66s24f6

Hence the short hand valence electron configuration of samarium with Z=62 is

  [Xe]4f66s2

(b)

Interpretation Introduction

Interpretation:

Short hand valence electron configuration of osmium with Z=76 should be determined.

Concept introduction:

Electronic configuration can be assigned to any elements in ground when they follow certain rules like Hund rule, Pauli Exclusion Principle and Aufbau rule. If atomic number of an element is Z then Z numbers of electrons are filled into the orbitals which are arranged in increasing order of energy.

No two electrons in an atom can have same group of four quantum numbers and this is Pauli Exclusion Principle.

While filling of orbital’s, electron first enters to each energy level with degenerate energy before paring of electron begins and this is Hund’s rules.

(b)

Expert Solution
Check Mark

Answer to Problem 48A

Short hand valence electron configuration of osmium with Z=76 is as follows:

  [Xe]4f145d66s2

Explanation of Solution

As per Aufbau rule electrons are filled in lower energy orbitals that are closer to the nucleus before they are filled in higher energy ones. The order of orbital arranged in their increasing energies is as follows:

  1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p< 6s<4f<5d<6p<7s<5f<6d<7p .

So complete electronic configuration of osmium with Z=76 is as follows:

  1s22s22p63s23p64s23d104p65s24d105p66s24f145d6

Hence the short hand valence electron configuration of osmium with Z=76 is

  [Xe]4f145d66s2

(c)

Interpretation Introduction

Interpretation:

Short hand valence electron configuration of Iron with Z=26 should be determined.

Concept introduction:

Electronic configuration can be assigned to any elements in ground when they follow certain rules like Hund rule, Pauli Exclusion Principle and Aufbau rule. If atomic number of an element is Z then Z numbers of electrons are filled into the orbitals which are arranged in increasing order of energy.

No two electrons in an atom can have same group of four quantum numbers and this is Pauli Exclusion Principle.

While filling of orbital’s, electron first enters to each energy level with degenerate energy before paring of electron begins and this is Hund’s rules.

(c)

Expert Solution
Check Mark

Answer to Problem 48A

Short hand valence electron configuration of Iron with Z=26 is as follows:

  [Ar]3d64s2

Explanation of Solution

As per Aufbau rule electrons are filled in lower energy orbitals that are closer to the nucleus before they are filled in higher energy ones. The order of orbital arranged in their increasing energies is as follows:

  1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p< 6s<4f<5d<6p<7s<5f<6d<7p .

So complete electronic configuration of Iron with Z=26 is as follows:

  1s22s22p63s23p64s23d6

Hence the short hand valence electron configuration of Iron with Z=26 is

  [Ar]3d64s2

(d)

Interpretation Introduction

Interpretation:

Short hand valence electron configuration of Pb with Z=82 should be determined.

Concept introduction:

Electronic configuration can be assigned to any elements in ground when they follow certain rules like Hund rule, Pauli Exclusion Principle and Aufbau rule. If atomic number of an element is Z then Z numbers of electrons are filled into the orbitals which are arranged in increasing order of energy.

No two electrons in an atom can have same group of four quantum numbers and this is Pauli Exclusion Principle.

While filling of orbital’s, electron first enters to each energy level with degenerate energy before paring of electron begins and this is Hund’s rules.

(d)

Expert Solution
Check Mark

Answer to Problem 48A

Short hand valence electron configuration of Pb with Z=82 is as follows:

  [Xe]4f145d106s26p2

Explanation of Solution

As per Aufbau rule electrons are filled in lower energy orbitals that are closer to the nucleus before they are filled in higher energy ones. The order of orbital arranged in their increasing energies is as follows:

  1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p< 6s<4f<5d<6p<7s<5f<6d<7p .

So complete electronic configuration of Pb with Z=82 is as follows:

  1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p2

Hence the short hand valence electron configuration of Pb with Z=82 is

  [Xe]4f145d106s26p2

Chapter 11 Solutions

World of Chemistry, 3rd edition

Ch. 11.2 - Prob. 4RQCh. 11.2 - Prob. 5RQCh. 11.2 - Prob. 6RQCh. 11.3 - Prob. 1RQCh. 11.3 - Prob. 2RQCh. 11.3 - Prob. 3RQCh. 11.3 - Prob. 4RQCh. 11.3 - Prob. 5RQCh. 11.3 - Prob. 6RQCh. 11.4 - Prob. 1RQCh. 11.4 - Prob. 2RQCh. 11.4 - Prob. 3RQCh. 11.4 - Prob. 4RQCh. 11.4 - Prob. 5RQCh. 11.4 - Prob. 6RQCh. 11.4 - Prob. 7RQCh. 11 - Prob. 1ACh. 11 - Prob. 2ACh. 11 - Prob. 3ACh. 11 - Prob. 4ACh. 11 - Prob. 5ACh. 11 - Prob. 6ACh. 11 - Prob. 7ACh. 11 - Prob. 8ACh. 11 - Prob. 9ACh. 11 - Prob. 10ACh. 11 - Prob. 11ACh. 11 - Prob. 12ACh. 11 - Prob. 13ACh. 11 - Prob. 14ACh. 11 - Prob. 15ACh. 11 - Prob. 16ACh. 11 - Prob. 17ACh. 11 - Prob. 18ACh. 11 - Prob. 19ACh. 11 - Prob. 20ACh. 11 - Prob. 21ACh. 11 - Prob. 22ACh. 11 - Prob. 23ACh. 11 - Prob. 24ACh. 11 - Prob. 25ACh. 11 - Prob. 26ACh. 11 - Prob. 27ACh. 11 - Prob. 28ACh. 11 - Prob. 29ACh. 11 - Prob. 30ACh. 11 - Prob. 31ACh. 11 - Prob. 32ACh. 11 - Prob. 33ACh. 11 - Prob. 34ACh. 11 - Prob. 35ACh. 11 - Prob. 36ACh. 11 - Prob. 37ACh. 11 - Prob. 38ACh. 11 - Prob. 39ACh. 11 - Prob. 40ACh. 11 - Prob. 41ACh. 11 - Prob. 42ACh. 11 - Prob. 43ACh. 11 - Prob. 44ACh. 11 - Prob. 45ACh. 11 - Prob. 46ACh. 11 - Prob. 47ACh. 11 - Prob. 48ACh. 11 - Prob. 49ACh. 11 - Prob. 50ACh. 11 - Prob. 51ACh. 11 - Prob. 52ACh. 11 - Prob. 53ACh. 11 - Prob. 54ACh. 11 - Prob. 55ACh. 11 - Prob. 56ACh. 11 - Prob. 57ACh. 11 - Prob. 58ACh. 11 - Prob. 59ACh. 11 - Prob. 60ACh. 11 - Prob. 61ACh. 11 - Prob. 62ACh. 11 - Prob. 63ACh. 11 - Prob. 64ACh. 11 - Prob. 65ACh. 11 - Prob. 66ACh. 11 - Prob. 67ACh. 11 - Prob. 68ACh. 11 - Prob. 69ACh. 11 - Prob. 70ACh. 11 - Prob. 71ACh. 11 - Prob. 72ACh. 11 - Prob. 73ACh. 11 - Prob. 74ACh. 11 - Prob. 75ACh. 11 - Prob. 76ACh. 11 - Prob. 77ACh. 11 - Prob. 1STPCh. 11 - Prob. 2STPCh. 11 - Prob. 3STPCh. 11 - Prob. 4STPCh. 11 - Prob. 5STPCh. 11 - Prob. 6STPCh. 11 - Prob. 7STPCh. 11 - Prob. 8STPCh. 11 - Prob. 9STPCh. 11 - Prob. 10STPCh. 11 - Prob. 11STPCh. 11 - Prob. 12STP
Knowledge Booster
Background pattern image
Chemistry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Text book image
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Text book image
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Text book image
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Text book image
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Text book image
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
Quantum Numbers, Atomic Orbitals, and Electron Configurations; Author: Professor Dave Explains;https://www.youtube.com/watch?v=Aoi4j8es4gQ;License: Standard YouTube License, CC-BY
QUANTUM MECHANICAL MODEL/Atomic Structure-21E; Author: H to O Chemistry;https://www.youtube.com/watch?v=mYHNUy5hPQE;License: Standard YouTube License, CC-BY