$A$ subshell with $n=3$ and $l=2$ can accommodate a maximum of:

Which of the following sets of quantum numbers is not possible?

Which of the following orbitals is represented by $n=3$ and $l=2$?

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:
$(1).$ $n=4, l=2, m_l=-2, m_s=-1/2$
$(2).$ $n=3, l=2, m_l=1, m_s=+1/2$
$(3).$ $n=4, l=1, m_l=0, m_s=+1/2$
$(4).$ $n=3, l=2, m_l=-2, m_s=-1/2$
$(5).$ $n=3, l=1, m_l=-1, m_s=+1/2$
$(6).$ $n=4, l=1, m_l=0, m_s=+1/2$

The number of radial and angular nodes in $4d$ orbital are,respectively $........$ .

Which of the following electronic configurations is closer to the nucleus: $4s^2 3d^{10}$ or $4s^0 3d^{10}$?