The element with quantum numbers $n = 2, l = 1, m = 1, s = -1/2$ has the following position in the periodic table:

Arrange the electrons represented by the following sets of quantum numbers in the decreasing order of energy.
$(i) \ n = 4, l = 0, m_l = 0, m_s = +\frac{1}{2}$
$(ii) \ n = 3, l = 1, m_l = 1, m_s = -\frac{1}{2}$
$(iii) \ n = 3, l = 2, m_l = 0, m_s = +\frac{1}{2}$
$(iv) \ n = 3, l = 0, m_l = 0, m_s = -\frac{1}{2}$

For $n = 3$ energy level,the number of possible orbitals (all kinds) are

Which one of the following sets of quantum numbers is incorrect?

Principal quantum number $(n)$	Azimuthal quantum number $(l)$	Magnetic quantum number $(m)$

What is the maximum number of electrons that can be associated with the following set of quantum numbers?
$n = 3, l = 1$ and $m = -1$

The outer electronic structure $3s^23p^5$ is possessed by