I have done 5a, b and C. 5. Give the ground state electronic configuration of each of the following. You may abbreviatecomplete shells as a noble gas in brackets (e.g. [He], [Ar]).a) Cu*b) Fec) Au+d) Nd3+e) Mof) Os8.36. Identify the elements that have the ground-state electron configurations:a) [Ne]3s*3p*b) [Kr]5s?c) [Ar]4s*3dd) [Kr]5s²4d*e) [Kr]5s°4d105p!) [Xe]6s°4f

Answered: 5. Give the ground state electronic…

Introduction to Chemical Engineering Thermodynamics

8th Edition

ISBN:9781259696527

Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Chapter1: Introduction

Section: Chapter Questions

Problem 1.1P

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I have done 5a, b and C.

5. Give the ground state electronic configuration of each of the following. You may abbreviate
complete shells as a noble gas in brackets (e.g. [He], [Ar]).
a) Cu*
b) Fe
c) Au+
d) Nd3+
e) Mo
f) Os8.
3
6. Identify the elements that have the ground-state electron configurations:
a) [Ne]3s*3p*
b) [Kr]5s?
c) [Ar]4s*3d
d) [Kr]5s²4d*
e) [Kr]5s°4d105p!
) [Xe]6s°4f

Expert Solution

Step 1

(d)

Given ion is ${Nd}^{3 +}$ .

Atomic number of $Nd$ is $60$ .

There are 60 electrons in $Nd$ and 57 electrons in ${Nd}^{3 +}$ ion due to loss of 3 electrons..

Write the electron configuration of ${Nd}^{3 +}$ as follows:

$\begin{array}{rcl} [{Nd}^{3 +}] & = & 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{2} 4 p^{6} 4 d^{10} 5 s^{2} 5 p^{6} 4 f^{3} \\ = & [Xe] 4 f^{3} \end{array}$

Therefore, the required solution is $[Xe] 4 f^{3}$ .

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