   Chapter 6, Problem 43PS

Chapter
Section
Textbook Problem

A particular orbital has n = 4 and ℓ = 2. What must this orbital be: (a) 3p, (b) 4p, (c) 3d, or (d) 4d?

Interpretation Introduction

Interpretation: The particular orbital having n=4 and l=2 from the given 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.

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

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).

Here, the principal quantum number, n=4

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