Atomic orbital designations has to be given for the quantum numbers. Concept Introduction: Principal quantum number is the one that specifies the extent or the effective size of an orbital. This is denoted by n . Shape of the orbital is denoted by the azimuthal quantum number. This is denoted by l and the values of azimuthal quantum number will be from zero to n − 1 . The subshell s , p , d , and f is denoted by the value of azimuthal quantum number as 0 , 1 , 2 , and 3 respectively. Magnetic quantum number has a value of + l to − l . This determines the spatial orientation of orbital and it is designated as m l . Spin state of an electron is designated by the spin quantum number. It is denoted by m s and it can have only two possible values. They are + 1 / 2 or − 1 / 2 .

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Chapter 5, Problem 5.7P

Interpretation Introduction

Interpretation:

Atomic orbital designations has to be given for the quantum numbers.

Concept Introduction:

Principal quantum number is the one that specifies the extent or the effective size of an orbital. This is denoted by n. Shape of the orbital is denoted by the azimuthal quantum number. This is denoted by l and the values of azimuthal quantum number will be from zero to n−1. The subshell s, p, d, and f is denoted by the value of azimuthal quantum number as 0, 1, 2, and 3 respectively.

Magnetic quantum number has a value of +l to −l. This determines the spatial orientation of orbital and it is designated as ml. Spin state of an electron is designated by the spin quantum number. It is denoted by ms and it can have only two possible values. They are +1/2 or−1/2.

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