   Chapter 6, Problem 39PS

Chapter
Section
Textbook Problem

State which of the following orbitals cannot exist according to the quantum theory: 2s, 2d, 3p, 3f, 4f, and 5s. Briefly explain your answers.

Interpretation Introduction

Interpretation: According to quantum theory the orbitals that cannot exist should be identified from the given list of orbitals.

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.

When n=2, the values of l are, l=(n1)=0,1. Each l value indicates subshell where 0 and 1 represents s and p orbitals. Therefore according to quantum theory 2d cannot exist

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