Chemistry: Atoms First
Chemistry: Atoms First
3rd Edition
ISBN: 9781259638138
Author: Julia Burdge, Jason Overby Professor
Publisher: McGraw-Hill Education
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Chapter 4, Problem 4.72QP

(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 ions are formed from the atoms the electrons are added or removed from the outermost orbital.

To write: Ground-state electronic configuration of Sc3+ .

(a)

Expert Solution
Check Mark

Answer to Problem 4.72QP

Answer

The ground-state electronic configuration of (a) is 1s22s22p63s23p6

Explanation of Solution

Electronic configuration of Sc is,

1s22s22p63s23p64s23d1

The electronic configuration of Sc is found using the total number of electrons present in the atom.  The total number of electrons present in Sc is 21.  According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of Sc is found as 1s22s22p63s23p64s23d1.

Electronic configuration of Sc3+ is,

1s22s22p63s23p6

The electronic configuration of Sc3+ is found from the electronic configuration of Sc.  Sc3+ is formed from Sc when three valence electrons are removed from the outermost orbitals.  According to Pauli Exclusion Principle and Hund’s rule, the ground state electronic configuration of Sc3+ is found as 1s22s22p63s23p6.

(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 ions are formed from the atoms the electrons are added or removed from the outermost orbital.

To write: Ground-state electronic configuration of Ti4+ .

(b)

Expert Solution
Check Mark

Answer to Problem 4.72QP

Answer

The ground-state electronic configuration of (b) is 1s22s22p63s23p6

Explanation of Solution

Electronic configuration of Ti

1s22s22p63s23p64s23d2

The electronic configuration of Ti is found using the total number of electrons present in the atom.  The total number of electrons present in Ti is 22.  According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of Ti is found as 1s22s22p63s23p64s23d2.

Electronic configuration of Ti4+

1s22s22p63s23p6

The electronic configuration of Ti4+ is found from the electronic configuration of TiTi4+ is formed from Ti when four electrons are removed from the outermost orbital.  According to Pauli Exclusion Principle and Hund’s rule, the ground state electronic configuration of Ti4+ is found as 1s22s22p63s23p6.

(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 ions are formed from the atoms the electrons are added or removed from the outermost orbital.

To write: Ground-state electronic configuration of V5+ .

(c)

Expert Solution
Check Mark

Answer to Problem 4.72QP

Answer

The ground-state electronic configuration of (c) is 1s22s22p63s23p6

Explanation of Solution

Electronic configuration of V is,

1s22s22p63s23p64s23d3

The electronic configuration of V is found using the total number of electrons present in the atom.  The total number of electrons present in V is 23.  According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of V is found as 1s22s22p63s23p64s23d3.

Electronic configuration of V5+ is,

1s22s22p63s23p6

The electronic configuration of V5+ is found from the electronic configuration of VV5+ is formed from V when five electrons are removed from the outermost orbital.  According to Pauli Exclusion Principle and Hund’s rule, the ground state electronic configuration of V5+ is found as 1s22s22p63s23p6.

(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 ions are formed from the atoms the electrons are added or removed from the outermost orbital.

To write: Ground-state electronic configuration of Cr3+ .

(d)

Expert Solution
Check Mark

Answer to Problem 4.72QP

Answer

The ground-state electronic configuration of (d) is 1s22s22p63s23p63d3

Explanation of Solution

Electronic configuration of Cr is,

1s22s22p63s23p64s13d5

The electronic configuration of Cr is found using the total number of electrons present in the atom.  The total number of electrons present in Cr is 24.  According to Pauli Exclusion Principle, the electronic configuration of Cr is found as 1s22s22p63s23p64s13d5.

Electronic configuration of Cr3+

1s22s22p63s23p63d3

The electronic configuration of Cr3+ is found from the electronic configuration of CrCr3+ is formed from Cr when three electrons are removed from the outermost orbital.  According to Pauli Exclusion Principle and Hund’s rule, the ground state electronic configuration of Cr3+ is found as 1s22s22p63s23p63d3.

(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 ions are formed from the atoms the electrons are added or removed from the outermost orbital.

To write: Ground-state electronic configuration of Mn3+ .

(e)

Expert Solution
Check Mark

Answer to Problem 4.72QP

Answer

The ground-state electronic configuration of (e) is 1s22s22p63s23p63d4

Explanation of Solution

Electronic configuration of Mn is,

1s22s22p63s23p64s23d5

The electronic configuration of Mn is found using the total number of electrons present in the atom.  The total number of electrons present in Mn is 25.  According to Pauli Exclusion Principle, the electronic configuration of Mn is found as 1s22s22p63s23p64s23d5.

Electronic configuration of Mn3+ is,

1s22s22p63s23p63d4

The electronic configuration of Mn3+ is found from the electronic configuration of MnMn3+ is formed from Mn when three electrons are removed from the outermost orbital.  According to Pauli Exclusion Principle and Hund’s rule, the ground state electronic configuration of Mn3+ is found as 1s22s22p63s23p63d4.

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Chapter 4 Solutions

Chemistry: Atoms First

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