Quantum Mechanical Model of the Atom

The total number of atomic orbitals in the fourth energy level of an atom is :

Consider the following sets of quantum numbers :

which of the following sets of quantum number is not possible ?

The orientation of an atomic orbital is governed by

The number of orbitals possible for the following quantum numbers is/are

$\mathrm{n}=3,\hspace{0.17em}\hspace{0.17em}\mathrm{l}=2, \mathrm{m}=+2$

The number of spherical nodes in 3p orbitals are

The electron was shown experimentally to have wave properties by

Draw the diagram of different $\mathrm{d}$-orbitals. 

Describe the shape of different $\mathrm{p}$-orbitals. 

How many nodes are present in $3\mathrm{s},3\mathrm{p}$ and $3\mathrm{d}$ orbitals? 

What is azimuthal quantum number? 

"The larger the value of '$\mathrm{l}$' belonging to the same main energy, higher is the energy associated with it." Comment on this statement.

Are the magnetic quantum number and angular momentum of an electron related to each other? Explain.

The principal and azimuthal quantum numbers associated with a subshell are a and $\mathrm{a}-4$, respectively. Predict the shape of that subshell if the shape of another subshell having azimuthal quantum number $\mathrm{a}-5$ is spherical. If that subshell is half-filled, predict the atomic number of the element.

In how many $\mathrm{d}$-orbitals do the lobes lie in between coordinate axes? What are those? 

In the pictorial representation of an orbital, what is the role of different intensity of shading? 

How many nodal surface(s) can $5\mathrm{s}$ orbital have? 

Why does $\mathrm{L}$ shell does not have $\mathrm{d}$-orbitals? 

What is the shape of a '$\mathrm{s}$' orbital? Draw the diagram.