Find the number of orbitals and maximum electrons respectively present in $M$-shell?

Explain,giving reasons,which of the following sets of quantum numbers are not possible.
$(a)$ $n=0, l=0, m_{l}=0, m_{s}=+\frac{1}{2}$
$(b)$ $n=1, l=0, m_{l}=0, m_{s}=-\frac{1}{2}$
$(c)$ $n=1, l=1, m_{l}=0, m_{s}=+\frac{1}{2}$
$(d)$ $n=2, l=1, m_{l}=0, m_{s}=-\frac{1}{2}$
$(e)$ $n=3, l=3, m_{l}=-3, m_{s}=+\frac{1}{2}$
$(f)$ $n=3, l=1, m_{l}=0, m_{s}=+\frac{1}{2}$

For hydrogen-like atoms,the average distance of an electron from the nucleus for the orbitals belonging to the $4^{th}$ orbit is minimum for:

How many electrons in an atom may have the following quantum numbers?
$(a)$ $n=4, m_{s}=-\frac{1}{2}$
$(b)$ $n=3, l=0$

Using $s$,$p$,$d$,and $f$ notations,describe the orbital with the following quantum numbers:
$(a)$ $n=1$,$l=0$
$(b)$ $n=3$,$l=1$
$(c)$ $n=4$,$l=2$
$(d)$ $n=4$,$l=3$

The maximum number of electrons that can have principal quantum number,$n=3$,and spin quantum number,$m_s=-1/2$,is