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Chemistry Part-I

Structure of Atom

How much energy is required to ionise H atom if the electron o

Chemistry Part-I

Class 11

NCERT

Chapter 1: Some Basic Concepts of Chemistry

44 questions

Chapter 2: Structure of Atom

85 questions

What is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from an energy level with n = 4 to an energy level with n = 2?

How much energy is required to ionise H atom if the electron occupies n = 5 orbits? Compare your answer with the ionization enthalpy of H atom

[ energy required to remove the electron from n =1 orbit].

What is the maximum number of emission lines when the excited electron of H atom in n = 6 drops to the ground state?

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Chapter 3: Classification of Elements and Periodicity in Properties

50 questions

Chapter 4: Chemical Bonding and Molecular Structure

44 questions

Chapter 5: States of Matter

28 questions

Chapter 6: Thermodynamics and Thermochemistry

36 questions

Chapter 7: Equilibrium

101 questions

Question

Medium

Solving time: 5 mins

How much energy is required to ionise H atom if the electron occupies n = 5 orbits? Compare your answer with the ionization enthalpy of H atom
[ energy required to remove the electron from n =1 orbit].

Views: 5,876 students

Updated on: Feb 21, 2024

Book:

Chemistry Part-I (NCERT)

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How much energy is required to ionise H atom if the electron occupies n = 5 orbits? Compare your answer with the ionization enthalpy of H atom

[ energy required to remove the electron from n =1 orbit].

9 mins ago

Discuss this question LIVE

9 mins ago

Text solutionVerified

The energy of an electron in nth orbit is

E = \frac{- 21.8 \times 1 0 ^{- 19}}{n ^{2}} J / a t o m

The ionization energy for the electron in the fifth orbit is:

Δ E = E_{2} - E_{1} = - 21.8 \times 1 0^{- 19} \frac{1}{n _{2}^{2}} = \frac{1}{n _{1}^{2}}

Δ E = E_{2} - E_{1} = - 21.8 \times 1 0^{- 19} \frac{1}{\infty} = \frac{1}{5 ^{2}} = 8.72 \times 1 0^{- 20}

J.

The ionization energy for the electron in the first orbit is:

Δ E^{'} = E_{2} - E_{1} = - 21.8 \times 1 0^{- 19} \frac{1}{n _{2}^{2}} = \frac{1}{n _{1}^{2}}

Δ E^{'} = E_{2} - E_{1} = - 21.8 \times 1 0^{- 19} \frac{1}{\infty} = \frac{1}{1 ^{2}} = 21.8 \times 1 0^{- 19}

.

The ratio of the ionization energy of electron in first orbit to the ionization energy of electron in fifth orbit is:

\frac{Δ E ^{'}}{Δ E} = \frac{21.8 \times 1 0 ^{- 19}}{8.72 \times 1 0 ^{- 20}} = 25

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Practice more questions from Chemistry Part-I (NCERT)

What is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from an energy level with n = 4 to an energy level with n = 2?

How much energy is required to ionise H atom if the electron occupies n = 5 orbits? Compare your answer with the ionization enthalpy of H atom

[ energy required to remove the electron from n =1 orbit].

What is the maximum number of emission lines when the excited electron of H atom in n = 6 drops to the ground state?

View all

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Question Text	How much energy is required to ionise H atom if the electron occupies n = 5 orbits? Compare your answer with the ionization enthalpy of H atom [ energy required to remove the electron from n =1 orbit].
Updated On	Feb 21, 2024
Topic	Structure of Atom
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1 Video solution: 11
Upvotes	1063
Avg. Video Duration	7 min

How much energy is required to ionise H atom if the electron occupies n = 5 orbits? Compare your answer with the ionization enthalpy of H atom
[ energy required to remove the electron from n =1 orbit].

Text solutionVerified

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