Chapter 5, Problem 5.36P

(a)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of ${\text{O}}^{+}$ ion has to be written using Hund’s rule and also the neutral atom that is isoelectronic with ${\text{O}}^{\text{+}}$ has to be indicated.

Concept Introduction:

Each orbital has two electrons and they both are in opposite spin.  Electrons are filled up in the orbitals of a sub-shell by following Hund’s rule.  This rule tells that all the orbitals are singly filled in a sub-shell and then the pairing occurs.

Isoelectronic species are the ones that have different number of protons but same number of electrons.  No two neutral atom can be isoelectronic.  A neutral atom can be isoelectronic with an ion.

(b)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of ${\text{C}}^{-}$ ion has to be written using Hund’s rule and also the neutral atom that is isoelectronic with ${\text{C}}^{-}$ has to be indicated.

Concept Introduction:

Refer part (a).

(c)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of ${\text{F}}^{+}$ ion has to be written using Hund’s rule and also the neutral atom that is isoelectronic with ${\text{F}}^{\text{+}}$ has to be indicated.

Concept Introduction:

Refer part (a).

(d)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of ${\text{O}}^{2+}$ ion has to be written using Hund’s rule and also the neutral atom that is isoelectronic with ${\text{O}}^{\text{2+}}$ has to be indicated.

Concept Introduction:

Refer part (a).

Isoelectronic species are the ones that have different number of protons but same number of electrons.  No two neutral atom can be isoelectronic.  A neutral atom can be isoelectronic with an ion.