Chapter 21, Problem 23E

(a)

Interpretation Introduction

Interpretation:

Electronic configuration of the following metals has to be written –

$\left(\text{a}\right){\text{ Ti, Ti}}^{\text{2+}}{\text{,Ti}}^{\text{4+}}\left(\text{b}\right){\text{ Re, Re}}^{\text{2+}}{\text{, Re}}^{\text{3+}}\left(\text{c}\right){\text{ Ir, Ir}}^{\text{2+}}{\text{, Ir}}^{\text{3+}}$

Concept Introduction:

Electronic configuration of an atom represents the arrangement of electrons in various energy levels.  The electrons are arranged in increasing order of energy levels according to Aufbau principle.  It is pictorially represented as –

Figure 1

The terms $1s,\text{ 2s, 3s }\mathrm{...}$ etc represent the energy levels inside an atom in which electrons are filled.

Answer to Problem 23E

Electronic configuration of Ti -   $\left[Ar\right]4s^{2}3d^2$

Electronic configuration of Ti²⁺ - $\left[Ar\right]3d^2$

Electronic configuration of Ti⁴⁺ - $\left[Ar\right]4s^{0}3d^0$

Explanation of Solution

Atomic number of Nickel is $22$.  Accordingly the electronic configuration is –

$1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{2}4s^2$

The above electronic configuration corresponds to that of Argon till $3p^6$ energy level.  Hence the electronic configuration can be simplified as – $\left[Ar\right]3d^{2}4s^2$

Ti²⁺ is formed when Titanium loses two electrons.  Accordingly the electronic configuration of Ti²⁺ is –

$1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^2$

The above electronic configuration corresponds to that of Argon till $3p^6$ energy level.  Hence the electronic configuration can be simplified as – $\left[Ar\right]3d^2$

Ti⁴⁺ is formed when Titanium loses four electrons.  Accordingly the electronic configuration of Ti⁴⁺ is –

$1s^{2}2s^{2}2p^{6}3s^{2}3p^6$

The above electronic configuration corresponds to that of Argon till $3p^6$ energy level.  Hence the electronic configuration can be simplified as – $\left[Ar\right]$

(b)

Interpretation Introduction

Interpretation:

Electronic configuration of the following metals has to be written –

$\left(\text{a}\right){\text{ Ti, Ti}}^{\text{2+}}{\text{,Ti}}^{\text{4+}}\left(\text{b}\right){\text{ Re, Re}}^{\text{2+}}{\text{, Re}}^{\text{3+}}\left(\text{c}\right){\text{ Ir, Ir}}^{\text{2+}}{\text{, Ir}}^{\text{3+}}$

Concept Introduction:

Electronic configuration of an atom represents the arrangement of electrons in various energy levels.  The electrons are arranged in increasing order of energy levels according to Aufbau principle.  It is pictorially represented as –

Figure 1

The terms $1s,\text{ 2s, 3s }\mathrm{...}$ etc represent the energy levels inside an atom in which electrons are filled.

Answer to Problem 23E

Electronic configuration of Re - $\left[Xe\right]6s^{2}4f^{14}5d^5$

Electronic configuration of Re²⁺ - $\left[Xe\right]4f^{14}5d^5$

Electronic configuration of Re³⁺ - $\left[Xe\right]4f^{14}5d^4$

Explanation of Solution

Atomic number of Rhenium is $75$. Accordingly the electronic configuration is –

$1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{10}4s^{2}4p^{6}4d^{10}5s^{2}5p^{6}4f^{14}6s^{2}5d^5$

The above electronic configuration corresponds to that of Xenon till $5p^6$ energy level.  Hence the electronic configuration can be simplified as – $\left[Xe\right]6s^{2}4f^{14}5d^5$

Re²⁺ is formed when Rhenium loses two electrons. Accordingly the electronic configuration of Re²⁺ is –

$1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{10}4s^{2}4p^{6}4d^{10}5s^{2}5p^{6}4f^{14}5d^5$

The above electronic configuration corresponds to that of Xenon till $5p^6$ energy level.  Hence the electronic configuration can be simplified as – $\left[Xe\right]4f^{14}5d^5$

Re³⁺ is formed when Rhenium loses three electrons. Accordingly the electronic configuration of Re²⁺ is –

$1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{10}4s^{2}4p^{6}4d^{10}5s^{2}5p^{6}4f^{14}5d^5$

The above electronic configuration corresponds to that of Xenon till $5p^6$ energy level.  Hence the electronic configuration can be simplified as – $\left[Xe\right]4f^{14}5d^4$

(c)

Interpretation Introduction

Interpretation:

Electronic configuration of the following metals has to be written –

$\left(\text{a}\right){\text{ Ti, Ti}}^{\text{2+}}{\text{,Ti}}^{\text{4+}}\left(\text{b}\right){\text{ Re, Re}}^{\text{2+}}{\text{, Re}}^{\text{3+}}\left(\text{c}\right){\text{ Ir, Ir}}^{\text{2+}}{\text{, Ir}}^{\text{3+}}$

Concept Introduction:

Electronic configuration of an atom represents the arrangement of electrons in various energy levels.  The electrons are arranged in increasing order of energy levels according to Aufbau principle.  It is pictorially represented as –

Figure 1

The terms $1s,\text{ 2s, 3s }\mathrm{...}$ etc represent the energy levels inside an atom in which electrons are filled.

Answer to Problem 23E

Electronic configuration of Ir -   $\left[Xe\right]6s^{2}4f^{14}5d^7$

Electronic configuration of Ir²⁺ - $\left[Xe\right]4f^{14}5d^7$

Electronic configuration of Ir³⁺ - $\left[Xe\right]4f^{14}5d^6$

Explanation of Solution

Atomic number of Iridium is $77$.  Accordingly the electronic configuration is –

$1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{10}4s^{2}4p^{6}4d^{10}5s^{2}5p^{6}4f^{14}6s^{2}5d^7$

The above electronic configuration corresponds to that of Xenon till $5p^6$ energy level.  Hence the electronic configuration can be simplified as – $\left[Xe\right]6s^{2}4f^{14}5d^7$

Ir²⁺ is formed when Iridium loses two electrons.  Accordingly the electronic configuration of Ir²⁺ is –

$1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{10}4s^{2}4p^{6}4d^{10}5s^{2}5p^{6}4f^{14}5d^7$

The above electronic configuration corresponds to that of Xenon till $5p^6$ energy level.  Hence the electronic configuration can be simplified as – $\left[Xe\right]4f^{14}5d^7$

Ir³⁺ is formed when Iridium loses three electrons. Accordingly the electronic configuration of Ir³⁺ is –

$1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{10}4s^{2}4p^{6}4d^{10}5s^{2}5p^{6}4f^{14}5d^6$

The above electronic configuration corresponds to that of Xenon till $5p^6$ energy level.  Hence the electronic configuration can be simplified as – $\left[Xe\right]4f^{14}5d^6$