   # State which of the following orbitals cannot exist according to the quantum theory: 3 p , 4 s , 2 f , and 1 p . Briefly explain your answers. ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 6, Problem 40PS
Textbook Problem
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## State which of the following orbitals cannot exist according to the quantum theory: 3p, 4s, 2f, and 1p. 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 of Solution

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

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