   Chapter 6, Problem 27PS

Chapter
Section
Textbook Problem

(a) When n = 4, what are the possible values of ℓ?(b) When ℓ is 2, what are the possible values of mℓ(c) For a 4s orbital, what are the possible values of n, ℓ, and mℓ(d) For a 4f orbital, what are the possible values of n, ℓ, and mℓ?ss

(a)

Interpretation Introduction

Interpretation: The possible values of l, when n=4 has to be determined

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

Explanation

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 possible values of ml, when l=2 has to be determined

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

(c)

Interpretation Introduction

Interpretation: The possible values of n,l,ml for 4s orbital has to be determined

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.

For an orbital ns, the principal quantum number is n

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.

(d)

Interpretation Introduction

Interpretation: The possible values of n,l,ml for 4f orbital has to be determined

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.

For an orbital ns, the principal quantum number is n

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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