   Chapter 6, Problem 33PS

Chapter
Section
Textbook Problem

Explain briefly why each of the following is not a possible set of quantum numbers for an electron in an atom.(a) n = 2, ℓ = 2, mℓ = 0(b) n = 3, ℓ = 0, mℓ = -2(c) n = 6, ℓ = 0, mℓ = 1

(a)

Interpretation Introduction

Interpretation: The reason for why the given set of quantum numbers is not possible for an electron has to be explained.

Concept introduction:

Quantum numbers are numbers, which explains the existence and the behavior of electron in an atom.

1. a) Principle quantum number is represented by n and this number describes the energy of the orbital and the size of an atom.
2. b) Angular momentum quantum number (or azimuthal quantum number) is represented by l and this number indicates the shape of the orbitals.
3. c) Magnetic quantum number is represented by ml and this number indicates the orientation of the orbital.
4. d) Spin quantum number is represented by ms and this number indicates the spin of the electron.

The principal quantum number and number of subshells are same in a shell.

The values of l when the principal quantum number is n are from 0 to (n1). Each l value indicates subshell.

The values of ml when the orbital angular quantum number is l are from l to +l.

Explanation

Given,

n=2,l=2,ml=0

The values of l when the principal quantum number is n are from 0 to (n1). Each l value indicates subshell

(b)

Interpretation Introduction

Interpretation: The reason for why the given set of quantum numbers is not possible for an electron has to be explained.

Concept introduction:

Quantum numbers are numbers, which explains the existence and the behavior of electron in an atom.

1. a) Principle quantum number is represented by n and this number describes the energy of the orbital and the size of an atom.
2. b) Angular momentum quantum number (or azimuthal quantum number) is represented by l and this number indicates the shape of the orbitals.
3. c) Magnetic quantum number is represented by ml and this number indicates the orientation of the orbital.
4. d) Spin quantum number is represented by ms and this number indicates the spin of the electron.

The principal quantum number and number of subshells are same in a shell.

The values of l when the principal quantum number is n are from 0 to (n1). Each l value indicates subshell.

The values of ml when the orbital angular quantum number is l are from l to +l.

(c)

Interpretation Introduction

Interpretation: The reason for why the given set of quantum numbers is not possible for an electron has to be explained.

Concept introduction:

Quantum numbers are numbers, which explains the existence and the behavior of electron in an atom.

1. a) Principle quantum number is represented by n and this number describes the energy of the orbital and the size of an atom.
2. b) Angular momentum quantum number (or azimuthal quantum number) is represented by l and this number indicates the shape of the orbitals.
3. c) Magnetic quantum number is represented by ml and this number indicates the orientation of the orbital.
4. d) Spin quantum number is represented by ms and this number indicates the spin of the electron.

The principal quantum number and number of subshells are same in a shell.

The values of l when the principal quantum number is n are from 0 to (n1). Each l value indicates subshell.

The values of ml when the orbital angular quantum number is l are from l to +l.

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