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 $m_l$.  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 $+1/2\text{or}-1/2$.