   Chapter 6, Problem 41PS

Chapter
Section
Textbook Problem

Write a complete set of quantum numbers (n, ℓ, mℓ) that quantum theory allows for each of the following orbitals: (a) 2p, (b) 3d, and (c) 4f.

(a)

Interpretation Introduction

Interpretation: The possible set of quantum number for the 2p orbital is to be identified.

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.

Principle quantum number is represented by n and this number describes the energy of the orbital and the size of an atom.

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

Principle quantum number is represented by n and this number describes the energy of the orbital and the size of an atom. 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.

For the orbital 2p, the principal quantum number,n=2 . For p subshell, l=1

(b)

Interpretation Introduction

Interpretation: The possible set of quantum number for the 3d orbital is to be identified.

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.

Principle quantum number is represented by n and this number describes the energy of the orbital and the size of an atom.

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 possible set of quantum number for the 4f orbital is to be identified.

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.

Principle quantum number is represented by n and this number describes the energy of the orbital and the size of an atom.

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

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

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