   Chapter 6, Problem 59GQ

Chapter
Section
Textbook Problem

If sufficient energy is absorbed by an atom, an electron can be lost by the atom and a positive ion formed. The amount of energy required is called the ionization energy. In the H atom, the ionization energy is that required to change the electron from n = 1 to n = infinity. Calculate the ionization energy for the He+ ion. Is the ionization energy of the He+ more or less than that of H? (Bohr′s theory applies to He+ because it, like the H atom, has a single electron. The electron energy, however, is now given by E = −Z2Rhc/n2, where Z is the atomic number of helium.)

Interpretation Introduction

Interpretation: The ionization energy of He+ has to be calculated. The ionization energy of He+ is whether more or less than that of hydrogen atom has to be determined.

Concept introduction:

Ionization energy is the quantity of energy which is needed to remove an electron which is not tightly bound to it forming a cation.

IonizationEnergy=Z2Rhc(1nfinal21ninitial2)

Where,

R is Rydberg constant

h is Planck’s constant

c is speed of light

Z is atomic number

Explanation

Given,

Ionization energy of He+ is calculated,

IonizationEnergy=Z2Rhc(1nfinal21ninitial2)

Substituting the values

E=22×(1.097×107m1)×(6.626×1034J.s)×(2.998×108m/s)(12112)=8

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