Chemistry
Chemistry
4th Edition
ISBN: 9780078021527
Author: Julia Burdge
Publisher: McGraw-Hill Education
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Chapter 7, Problem 58QP
Interpretation Introduction

Interpretation:

The ground-state electronic configuration of the given ions is to be written.

Concept introduction:

Elements that lose electrons are called cations. They have a lesser number of electrons than that of their neutral states.

Elements that gain electrons are called anions. They have a greater number of electrons than that of their neutral states.

Expert Solution & Answer
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Answer to Problem 58QP

Solution:

a) 1s2

b) 1s2

c) 1s22s22p6

d) 1s22s22p6

e) [Ne]3s23p6

f) [Ne]

g) [Ar]3d104s24p6

h) [Ar]3d104s24p6

i) [Kr]

j) [Kr]

k) [Kr]4d105s2

l) [Kr]4d105s25p6

m) [Xe]

n) [Xe]4f145d106s2

o) [Kr]5d10

p) [Xe]4f145d106s2

q) [Xe]4f145d10

Explanation of Solution

a)Ion Li+

The neutral state of lithium is Li3 withelectronic configuration 1s22s1. Li+ has oneelectronless

than its neutral state, and hence, electronic configuration of Li+ ion is 1s22s0.

So, its ground-state electronic configuration is 1s22s0.

b)Ion H

Hydrogen in its neutral state has only one electron (H1) in the sorbital. H has two electrons (H1), having theelectronic configuration as 1s2. Hydrogen has a general tendency of losing its electron forming a cation as; H+. In H form, it forms hydrides with electropositive elements.

Its ground-state electronic configuration is 1s2.

c)Ion N3

The neutral state electron-arrangement of nitrogen is N7 with the electronic configuration 1s22s22p3. N3 has ten electrons as threemore are added to its neutral state. The electronic configuration of N3 is 1s22s22p6.

So, its ground-state electronic configuration is 1s22s22p6.

d)Ion F

The neutral state electronic configuration of fluorine (F9) is 1s22s22p5. F has ten electrons as onemore is added to its neutral state. It is isoelectronic with N3 ion.

So, its ground-state electronic configuration is 1s22s22p6.

e)Ion S2

The neutral state electron-arrangement of sulphur is S16 with the electronic configuration [Ne]3s23p4. S2 has eighteen electrons astwomore are added to its neutral state. Electronic configuration of S2 is [Ne]3s23p6.

So, its ground-state electronic configuration is [Ne]3s23p6.

f)Ion Al3+

The neutral state of aluminium is Al13 withelectronic configuration [Ne]3s23p1.

Al3+ has ten electrons. The ground state electronic configuration of Al3+ is [Ne]3s03p0. It is isoelectronic with N3 and F ions.

So, its ground-state electronic configuration is [Ne]3s03p0.

g)Ion Se2

The ground state electron-arrangement of selenium is Se2 with the electronic configuration [Ar]3d104s24p4. Se2 has thirty-six electrons astwo more are added to its neutral state. Electronic configuration of S2 is [Ar]3d104s24p6. It is isoelectronic with Kr36.

So, its ground-state electronic configuration is [Ar]3d104s24p6.

h) Ion Br

The ground state electron-arrangement of bromine is Br35 with the electronic configuration of [Ar]3d104s24p5. Br has thirty-six electrons asone more added to its neutral state. Electronic configuration of Br is [Ar]3d104s24p6. It is isoelectronic with Kr36.

So, its ground-state electronic configuration is [Ar]3d104s24p6.

i) Ion Rb+

The neutral state of rubidium is Rb37 withelectronic configuration [Kr]5s1. Rb+ has one electron less than its neutral state, and hence, its electronic configurationis [Kr]5s0. It is isoelectronic with Kr36.

So, its ground-state electronic configuration is [Kr].

j)Ion Sr2+

The neutral state of strontium is Sr38 with the electronic configuration [Kr]5s2. Sr2+ ion has two electrons less than its neutral state with an electronic configuration [Kr]. It is isoelectronic with Kr36 and Rb+.

So, its ground-state electronic configuration is [Kr].

k) Ion Sn2+

The neutral state of stannous is Sn50 with the electronic configuration [Kr]4d105s25p2. Sn2+ ion hastwo electrons less than its neutral state with an electronic configuration [Kr]4d105s25p0.

So, its ground-state electronic configuration is [Kr]4d105s2.

l)Ion Te2

Te2 has two more electrons than its neutral state of Te52 with its ground state electronic configuration as [Kr]4d105s25p4. The electronic configuration of Te2 is [Kr]4d105s25p6. It is isoelectronic with the noble gas Xe54.

So, its ground-state electronic configuration is [Kr]4d105s25p6.

m)Ion Ba2+

The neutral state of barium is Ba56 with the electronic configuration [Xe]6s2. Ba2+ ion hastwo electrons less than its neutral state with theelectronic configuration [Xe]6s0. It is isoelectronic with Xe54 and Te2.

So, its ground-state electronic configuration is [Xe].

n)Ion Pb2+

The neutral state of lead is Pb82 with the electronic configuration [Xe]4f145d106s26p2. Pb2+ ion has two electrons less than its neutral state. Its electronic configurationis [Xe]4f145d106s26p0.

So, its ground-state electronic configuration is [Xe]4f145d106s2.

o)Ion In3+

The neutral state of indium is In49 with the electronic configuration [Kr]4d105s25p1. In3+ ion has three electrons less than its neutral state with an electronic configuration [Kr]5d105s05p0.

So, its ground-state electronic configuration is [Kr]5d10.

p)Ion Tl+

The neutral state of thallium is Tl81 having theelectronic configuration [Xe]4f145d106s26p1. Tl+ ion has one electron less than its neutral state with an electronic configuration [Xe]4f145d106s2 with a total of eighty electrons.

So, its ground-state electronic configuration is [Xe]4f145d106s2.

q)Ion Tl3+

The neutral state of thallium is Tl81 having the electronic configuration [Xe]4f145d106s26p1. Tl3+ ion has three electrons less than its neutral state with an electronic configuration [Xe]4f145d10, having a total of seventy-eight electrons.

So, its ground-state electronic configuration is [Xe]4f145d10.

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Chapter 7 Solutions

Chemistry

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