Chapter 7, Problem 7.60QP

Interpretation Introduction

Interpretation:

For the given principal quantum number, the probable subshells and orbitals have to be identified.

Concept introduction:

Principal Quantum Number (n): In an atom, the electron energy mainly depends on principal quantum number.  The energy of an electron becomes lower when the value of n is smaller.  The orbital size also depends on n.  The size of orbital increases with increase in value of principal quantum number (n)

Angular Momentum Quantum Number (l): It helps to differentiate the different shapes of orbitals for given n.  For a given n, there are different shapes of orbitals are present and are denoted as l.  Angular momentum quantum number is also known as Azimuthal quantum number.  The possible values of angular momentum quantum number is in between $\text{0}\text{and}\text{(n-1)}$.  If the n is $3$, then l value is $0,1,2$

Magnetic Quantum Number (${\text{m}}_{\text{l}}$): It helps to distinguish orbitals having various orientations in space.  Any integer between $\text{-l and +l}$ is the probable values of magnetic quantum number.  For s subshell the $\text{l}\text{=}\text{0}$, then ${\text{m}}_{\text{l}}$ is zero.  For p subshell the $\text{l}\text{=}1$, then ${\text{m}}_{\text{l}}=-1,0,+1$.

Spin Quantum Number(${\text{m}}_{\text{s}}$): It refers to direction of spin of an electron in an orbital.  The possible values are $\text{+}\frac{\text{1}}{\text{2}}\text{or}\text{-}\frac{\text{1}}{\text{2}}$.