Which of the following sets of quantum numbers is impossible for an electron?

Assertion : An orbital designated by $n = 3, l = 1$ has double dumb-bell shape.
Reason : It belongs to $p-$subshell.

The quantum numbers of six electrons are given below. Arrange them in order of increasing energies. If any of these combination$(s)$ has/have the same energy,list them:
$(1).$ $n=4, l=2, m_l=-2, m_s=-1/2$
$(2).$ $n=3, l=2, m_l=1, m_s=+1/2$
$(3).$ $n=4, l=1, m_l=0, m_s=+1/2$
$(4).$ $n=3, l=2, m_l=-2, m_s=-1/2$
$(5).$ $n=3, l=1, m_l=-1, m_s=+1/2$
$(6).$ $n=4, l=1, m_l=0, m_s=+1/2$

How many nodal planes are present in a $d$-orbital?

An electron is in one of the $3d$ orbitals. Give the possible values of $n, l,$ and $m_l$ for this electron.

Which statement is not correct for $n = 5$,$m = +3$?