   Chapter 6, Problem 44PS

Chapter
Section
Textbook Problem

A given orbital has a magnetic quantum number of mℓ = −1. This could not be a(n) (a) f orbital (b) d orbital (c) p orbital (d) s orbital

Interpretation Introduction

Interpretation: The orbital which does not have ml=1 is to be identified from the given orbital.

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 (azimuthal quantum number) 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

Reason for correct option

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 s subshell, l=0 and hence the value of ml is zero since values of ml are from l to +l.

Therefore,

The orbital which does not have ml=1 is s subshell

Reason for correct option

In option (a), l=3 for f subshell and hence the value of ml is 3,2,1,0,1,2,3 since values of ml are from l to +l

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