Chemistry: Atoms First
Chemistry: Atoms First
3rd Edition
ISBN: 9781259638138
Author: Julia Burdge, Jason Overby Professor
Publisher: McGraw-Hill Education
bartleby

Videos

Question
Book Icon
Chapter 4, Problem 4.73QP

(a)

Interpretation Introduction

Interpretation: Ground-state electronic configuration of the given set of metal ions has to be written.

Concept Introduction:

  • Electronic configuration is the arrangement of the electrons of atoms in the orbital.  For atoms and ions the electronic configuration are written by using Pauli Exclusion Principle and Hund’s rule.
  • According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
  • According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled.  When the orbitals are singly filled, all the electrons have same spin.  In a doubly filled orbital, there are two electrons with opposite spin.
  • Half-filled orbitals are comparatively stable as completely filled orbitals.  Therefore if there is a possibility of forming half filled orbital then the electron will be moved to the respective orbitals giving rise to more stability.
  • When cation is formed it means the electrons are removed from the outermost orbital of atom.  If anion is formed means then the electrons are added to the atom in its outermost orbital.

(a)

Expert Solution
Check Mark

Answer to Problem 4.73QP

Answer

The ground-state electronic configuration of (a) is 1s22s22p63s23p63d8

To write: Ground-state electronic configuration of Ni2+ .

Explanation of Solution

Electronic configuration of Ni is,

1s22s22p63s23p64s23d8

The electronic configuration of Ni is found using the total number of electrons present in the atom.  The total number of electrons present in Ni is 28.  According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of Ni is found as 1s22s22p63s23p64s23d8.

Electronic configuration of Ni2+ is,

1s22s22p63s23p63d8

The electronic configuration of Ni2+ is found from the electronic configuration of Ni.  Ni2+ is formed from Ni when two valence electrons are removed from the outermost orbitals.  According to Pauli Exclusion Principle and Hund’s rule, the ground state electronic configuration of Ni2+ is found as 1s22s22p63s23p63d8.

(b)

Interpretation Introduction

Interpretation: Ground-state electronic configuration of the given set of metal ions has to be written.

Concept Introduction:

  • Electronic configuration is the arrangement of the electrons of atoms in the orbital.  For atoms and ions the electronic configuration are written by using Pauli Exclusion Principle and Hund’s rule.
  • According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
  • According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled.  When the orbitals are singly filled, all the electrons have same spin.  In a doubly filled orbital, there are two electrons with opposite spin.
  • Half-filled orbitals are comparatively stable as completely filled orbitals.  Therefore if there is a possibility of forming half filled orbital then the electron will be moved to the respective orbitals giving rise to more stability.
  • When cation is formed it means the electrons are removed from the outermost orbital of atom.  If anion is formed means then the electrons are added to the atom in its outermost orbital.

To write: Ground-state electronic configuration of Cu+ .

(b)

Expert Solution
Check Mark

Answer to Problem 4.73QP

Answer

The ground-state electronic configuration of (b) is 1s22s22p63s23p63d10

Explanation of Solution

Electronic configuration of Cu is,

1s22s22p63s23p64s13d10

The electronic configuration of Cu is found using the total number of electrons present in the atom.  The total number of electrons present in Cu is 29.  According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of Cu is found as 1s22s22p63s23p64s13d10.

Electronic configuration of Cu+ is,

1s22s22p63s23p63d10

The electronic configuration of Cu+ is found from the electronic configuration of CuCu+ is formed from Cu when one electron is removed from the outermost orbital.  According to Pauli Exclusion Principle and Hund’s rule, the ground state electronic configuration of Cu+ is found as 1s22s22p63s23p63d10.

(c)

Interpretation Introduction

Interpretation: Ground-state electronic configuration of the given set of metal ions has to be written.

Concept Introduction:

  • Electronic configuration is the arrangement of the electrons of atoms in the orbital.  For atoms and ions the electronic configuration are written by using Pauli Exclusion Principle and Hund’s rule.
  • According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
  • According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled.  When the orbitals are singly filled, all the electrons have same spin.  In a doubly filled orbital, there are two electrons with opposite spin.
  • Half-filled orbitals are comparatively stable as completely filled orbitals.  Therefore if there is a possibility of forming half filled orbital then the electron will be moved to the respective orbitals giving rise to more stability.
  • When cation is formed it means the electrons are removed from the outermost orbital of atom.  If anion is formed means then the electrons are added to the atom in its outermost orbital

To write: Ground-state electronic configuration of Ag+ .

(c)

Expert Solution
Check Mark

Answer to Problem 4.73QP

Answer

The ground-state electronic configuration of (c) is 1s22s22p63s23p64s23d104p64d10

Explanation of Solution

Electronic configuration of Ag

1s22s22p63s23p64s23d104p65s14d10

The electronic configuration of Ag is found using the total number of electrons present in the atom.  The total number of electrons present in Ag is 47.  According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of Ag is found as 1s22s22p63s23p64s23d104p65s14d10.

Electronic configuration of Ag+ is,

1s22s22p63s23p64s23d104p64d10

The electronic configuration of Ag+ is found from the electronic configuration of AgAg+ is formed from Ag when one electron is removed from the outermost orbital.  According to Pauli Exclusion Principle and Hund’s rule, the ground state electronic configuration of Ag+ is found as 1s22s22p63s23p64s23d104p64d10.

(d)

Interpretation Introduction

Interpretation: Ground-state electronic configuration of the given set of metal ions has to be written.

Concept Introduction:

  • Electronic configuration is the arrangement of the electrons of atoms in the orbital.  For atoms and ions the electronic configuration are written by using Pauli Exclusion Principle and Hund’s rule.
  • According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
  • According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled.  When the orbitals are singly filled, all the electrons have same spin.  In a doubly filled orbital, there are two electrons with opposite spin.
  • Half-filled orbitals are comparatively stable as completely filled orbitals.  Therefore if there is a possibility of forming half filled orbital then the electron will be moved to the respective orbitals giving rise to more stability.
  • When cation is formed it means the electrons are removed from the outermost orbital of atom.  If anion is formed means then the electrons are added to the atom in its outermost orbital.

To write: Ground-state electronic configuration of Au+ .

(d)

Expert Solution
Check Mark

Answer to Problem 4.73QP

Answer

The ground-state electronic configuration of (d) is 1s22s22p63s23p64s23d104p65s24d105p64f145d10

Explanation of Solution

Electronic configuration of Au is,

1s22s22p63s23p64s23d104p65s24d105p66s14f145d10

The electronic configuration of Au is found using the total number of electrons present in the atom.  The total number of electrons present in Au is 24.  According to Pauli Exclusion Principle, the electronic configuration of Au is found as 1s22s22p63s23p64s23d104p65s24d105p66s14f145d10.

Electronic configuration of Au+ is,

1s22s22p63s23p64s23d104p65s24d105p64f145d10

The electronic configuration of Au+ is found from the electronic configuration of AuAu+ Is formed from Au when three electrons are removed from the outermost orbital.  According to Pauli Exclusion Principle and Hund’s rule, the ground state electronic configuration of Au+ is found as 1s22s22p63s23p64s23d104p65s24d105p64f145d10.

(e)

Interpretation Introduction

Interpretation: Ground-state electronic configuration of the given set of metal ions has to be written.

Concept Introduction:

  • Electronic configuration is the arrangement of the electrons of atoms in the orbital.  For atoms and ions the electronic configuration are written by using Pauli Exclusion Principle and Hund’s rule.
  • According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
  • According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled.  When the orbitals are singly filled, all the electrons have same spin.  In a doubly filled orbital, there are two electrons with opposite spin.
  • Half-filled orbitals are comparatively stable as completely filled orbitals.  Therefore if there is a possibility of forming half filled orbital then the electron will be moved to the respective orbitals giving rise to more stability.
  • When cation is formed it means the electrons are removed from the outermost orbital of atom.  If anion is formed means then the electrons are added to the atom in its outermost orbital.

To write: Ground-state electronic configuration of Au3+ .

(e)

Expert Solution
Check Mark

Answer to Problem 4.73QP

Answer

The ground-state electronic configuration of (e) is 1s22s22p63s23p64s23d104p65s24d105p64f145d8

Explanation of Solution

Electronic configuration of Au is,

                    1s22s22p63s23p64s23d104p65s24d105p66s14f145d10

The electronic configuration of Au is found using the total number of electrons present in the atom.  The total number of electrons present in Au is 79.  According to Pauli Exclusion Principle, the electronic configuration of Au is found as 1s22s22p63s23p64s23d104p65s24d105p66s14f145d10.

Electronic configuration of Au3+ is,

        1s22s22p63s23p64s23d104p65s24d105p64f145d8

The electronic configuration of Au3+ is found from the electronic configuration of AuAu3+ is formed from Au when two electrons are removed from the outermost orbital.  According to Pauli Exclusion Principle and Hund’s rule, the ground state electronic configuration of Au3+ is found as 1s22s22p63s23p64s23d104p65s24d105p64f145d8.

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
Write the electron configuration and orbital diagram for each ion and predict whether each will be paramagnetic or diamagnetic.(a) Co2+ (b) N3- (c) Ca2+
Write the electron configurations for (a) Ca2+, (b) Co3+, and (c) S2-.
Write the electron configuration and orbital diagram for each ion and determine whether each is diamagnetic or paramagnetic.(a) Al3 + (b) S2 - (c) Fe3 +

Chapter 4 Solutions

Chemistry: Atoms First

Ch. 4.2 - Prob. 2PPCCh. 4.2 - Prob. 4.2.1SRCh. 4.2 - Prob. 4.2.2SRCh. 4.4 - Referring only to a periodic table, arrange the...Ch. 4.4 - Prob. 3PPACh. 4.4 - Prob. 3PPBCh. 4.4 - Prob. 3PPCCh. 4.4 - Prob. 4.4WECh. 4.4 - Which element. Mg or Al, will have the higher...Ch. 4.4 - Explain why Rb has a lower IE1 than Sr, but Sr has...Ch. 4.4 - Imagine an arrangement of atomic orbitals in an...Ch. 4.4 - For each pair of elements, indicate which one you...Ch. 4.4 - Prob. 5PPACh. 4.4 - Explain why the EA1 for Ge is greater than the EA1...Ch. 4.4 - In the same hypothetical arrangement described in...Ch. 4.4 - For carbon and nitrogen, use the effective nuclear...Ch. 4.4 - Between which two charges is the attractive force...Ch. 4.4 - What must the distance be between charges of +2.25...Ch. 4.4 - Rank these pairs of charged objects in order of...Ch. 4.4 - Arrange the elements Ca, Sr, and Ba in order of...Ch. 4.4 - Prob. 4.4.2SRCh. 4.4 - For each of the following pairs of elements,...Ch. 4.4 - Prob. 4.4.4SRCh. 4.4 - Which pair of opposite charges has the greatest...Ch. 4.4 - What must the separation between charges of +2 and...Ch. 4.5 - Write electron configurations for the following...Ch. 4.5 - Write electron configurations for (a) O2, (b)...Ch. 4.5 - Prob. 7PPBCh. 4.5 - Prob. 7PPCCh. 4.5 - Prob. 4.8WECh. 4.5 - Prob. 8PPACh. 4.5 - Prob. 8PPBCh. 4.5 - Select the correct valence orbital diagram for the...Ch. 4.5 - What is the charge on a titanium ion that is...Ch. 4.5 - Prob. 4.5.2SRCh. 4.5 - Select the correct ground-state electron...Ch. 4.5 - Prob. 4.5.4SRCh. 4.5 - Which of the following ions is diamagnetic? (a)...Ch. 4.6 - Identify the isoelectronic series in the following...Ch. 4.6 - Arrange the following isoelectronic series in...Ch. 4.6 - List all the common ions that are isoelectronic...Ch. 4.6 - Prob. 9PPCCh. 4.6 - Prob. 4.6.1SRCh. 4.6 - Prob. 4.6.2SRCh. 4 - Prob. 4.1KSPCh. 4 - Prob. 4.2KSPCh. 4 - Prob. 4.3KSPCh. 4 - Prob. 4.4KSPCh. 4 - Briefly describe the significance of Mendeleevs...Ch. 4 - What is Moseleys contribution to the modem...Ch. 4 - Describe the general layout of a modern periodic...Ch. 4 - What is the most important relationship among...Ch. 4 - Prob. 4.5QPCh. 4 - Prob. 4.6QPCh. 4 - Prob. 4.7QPCh. 4 - Prob. 4.8QPCh. 4 - Without referring to a periodic table, write the...Ch. 4 - Prob. 4.10QPCh. 4 - Prob. 4.11QPCh. 4 - Prob. 4.12QPCh. 4 - For centuries, arsenic has been the poison of...Ch. 4 - In the periodic table, the element hydrogen is...Ch. 4 - An atom of a certain clement has 16 electrons....Ch. 4 - Prob. 4.16QPCh. 4 - Prob. 4.17QPCh. 4 - Prob. 4.18QPCh. 4 - Prob. 4.19QPCh. 4 - For each of the following ground-state electron...Ch. 4 - Determine what element is designated by each of...Ch. 4 - Prob. 4.22QPCh. 4 - Explain why there is a greater increase in...Ch. 4 - The election configuration of B is1s22s22p1. (a)...Ch. 4 - The election configuration of C is1s22s22p1. (a)...Ch. 4 - Prob. 4.26QPCh. 4 - Prob. 4.27QPCh. 4 - Equation 4.2 is used to calculate the force...Ch. 4 - Use the second period of the periodic table as an...Ch. 4 - Prob. 4.30QPCh. 4 - Prob. 4.31QPCh. 4 - Prob. 4.32QPCh. 4 - Prob. 4.33QPCh. 4 - Prob. 4.34QPCh. 4 - Prob. 4.35QPCh. 4 - Prob. 4.36QPCh. 4 - Prob. 4.37QPCh. 4 - Prob. 4.38QPCh. 4 - Prob. 4.39QPCh. 4 - Consider two ions with opposite charges separated...Ch. 4 - Prob. 4.41QPCh. 4 - Prob. 4.42QPCh. 4 - Prob. 4.43QPCh. 4 - On the basis of their positions in the periodic...Ch. 4 - Prob. 4.45QPCh. 4 - Prob. 4.46QPCh. 4 - Prob. 4.47QPCh. 4 - Prob. 4.48QPCh. 4 - Prob. 4.49QPCh. 4 - Prob. 4.50QPCh. 4 - Prob. 4.51QPCh. 4 - Prob. 4.52QPCh. 4 - In general, the first ionization energy increases...Ch. 4 - Prob. 4.54QPCh. 4 - Prob. 4.55QPCh. 4 - Prob. 4.56QPCh. 4 - Prob. 4.57QPCh. 4 - Prob. 4.58QPCh. 4 - Specify which of the following elements you would...Ch. 4 - Considering their electron affinities, do you...Ch. 4 - Prob. 4.61QPCh. 4 - Prob. 4.62QPCh. 4 - Prob. 4.63QPCh. 4 - Prob. 4.64QPCh. 4 - Prob. 4.65QPCh. 4 - Prob. 4.66QPCh. 4 - Prob. 4.67QPCh. 4 - Prob. 4.68QPCh. 4 - Prob. 4.69QPCh. 4 - Write the ground-state electron configurations of...Ch. 4 - Write the ground-state electron configurations of...Ch. 4 - Prob. 4.72QPCh. 4 - Prob. 4.73QPCh. 4 - Identify the ions, each with a net charge of +1,...Ch. 4 - Prob. 4.75QPCh. 4 - Prob. 4.76QPCh. 4 - Group the species that are isoelectronic: Be2+, F,...Ch. 4 - For each pair of ions, determine which will have...Ch. 4 - Rank the following ions in order of increasing...Ch. 4 - Prob. 4.80QPCh. 4 - Prob. 4.81QPCh. 4 - Prob. 4.82QPCh. 4 - A metal ion with a net +3 charge has five...Ch. 4 - Identify the atomic ground-state electron...Ch. 4 - Each of the following ground-state electron...Ch. 4 - Prob. 4.86QPCh. 4 - Prob. 4.87QPCh. 4 - Prob. 4.88QPCh. 4 - Indicate which one of the two species in each of...Ch. 4 - Prob. 4.90QPCh. 4 - Prob. 4.91QPCh. 4 - Prob. 4.92QPCh. 4 - Prob. 4.93QPCh. 4 - Prob. 4.94QPCh. 4 - Prob. 4.95QPCh. 4 - Prob. 4.96QPCh. 4 - Prob. 4.97QPCh. 4 - Prob. 4.98QPCh. 4 - Prob. 4.99QPCh. 4 - Prob. 4.100QPCh. 4 - Arrange the following species in isoelectronic...Ch. 4 - Prob. 4.102QPCh. 4 - Prob. 4.103QPCh. 4 - Prob. 4.104QPCh. 4 - Prob. 4.105QPCh. 4 - Prob. 4.106QPCh. 4 - Prob. 4.107QPCh. 4 - Prob. 4.108QPCh. 4 - Contrary to the generalized trend that atomic...Ch. 4 - Prob. 4.110QPCh. 4 - Prob. 4.111QPCh. 4 - Prob. 4.112QPCh. 4 - Prob. 4.113QPCh. 4 - Prob. 4.114QPCh. 4 - Prob. 4.115QPCh. 4 - Prob. 4.116QPCh. 4 - Prob. 4.117QPCh. 4 - Prob. 4.118QPCh. 4 - Prob. 4.119QPCh. 4 - The energy needed for the following process is...Ch. 4 - Using your knowledge of the periodic trends with...Ch. 4 - Prob. 4.122QPCh. 4 - Prob. 4.123QPCh. 4 - Prob. 4.124QPCh. 4 - Explain, in terms of their electron...Ch. 4 - Prob. 4.126QPCh. 4 - Prob. 4.127QPCh. 4 - This graph charts the first six ionization...Ch. 4 - Prob. 4.129QPCh. 4 - Prob. 4.130QPCh. 4 - Prob. 4.131QPCh. 4 - Prob. 4.132QPCh. 4 - Predict the atomic number and ground-state...Ch. 4 - Prob. 4.134QPCh. 4 - Prob. 4.135QPCh. 4 - Prob. 4.136QPCh. 4 - The first six ionizations of a gaseous atom can be...Ch. 4 - Prob. 4.138QPCh. 4 - Prob. 4.139QP
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.
Similar questions
SEE MORE QUESTIONS
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
Introduction to Coordination ComplexesWave Function for Hydrogen atom # All Vital Topics # Quantum Mechanics part -21; Author: Priyanka Jain;https://www.youtube.com/watch?v=GKgNV9dmUHo;License: Standard YouTube License, CC-BY
CBSE Class 12 Chemistry || The d & f Block Elements Part 1 || Full Chapter || By Shiksha House; Author: Best for NEET;https://www.youtube.com/watch?v=LzZWHSdYaxw;License: Standard Youtube License