Chapter 5.5, Problem 5.9E

(a)

Interpretation Introduction

Interpretation:

All four possible sets of quantum numbers for an electron in $\text{3s}$ atomic orbitalhas to begiven.

Concept Introduction:

Principal Quantum Number (n): In an atom, theelectron 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 different shapes of orbitals for given n.  For a given n, there are n different shapes of orbitals are present and are denoted as l.   Angular momentum quantum number is also known as Azimuthalquantum number.  The possible values ofangular momentum quantum number are 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 $\text{+}\frac{\text{1}}{\text{2}}\text{or}\text{-}\frac{\text{1}}{\text{2}}$.

(b)

Interpretation Introduction

Interpretation:

All four possible sets of quantum numbers for an electron in $\text{2p}$ atomic orbital has to be given.

Concept Introduction:

Refer to part (a)

(c)

Interpretation Introduction

Interpretation:

All four possible sets of quantum numbers for an electron in ${\text{4d}}_{\text{xy}}$ atomic orbital has to be given.

Concept Introduction:

Refer to part (a)