Consider the following sets of quantum numbers (n, l, m, s): (i) 3, 0, 0, +1/2 (ii) 2, 2, 1, +1/2 (iii) 4, 3, -2, -1/2 (iv) 1, 0, -1, -1/2 (v) 3, 2, 3, +1/2

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

In hydrogen atom, what is the de Broglie wavelength of an electron in the second Bohr orbit? [Given that Bohr radius, $a_0 = 52.9$ pm]

Maximum number of electrons in a subshell with l = 3 and n = 4 is:

If the principal quantum number n=6, the correct sequence of filling of electrons will be:

The measurement of the electron position is associated with an uncertainty in momentum which is equal to $1 \times 10^{-18} \text{ g cm s}^{-1}$. The uncertainty in velocity of the electron will be: (mass of an electron is $9 \times 10^{-28} \text{ g}$)

What is the maximum number of orbitals that can be identified with the following quantum numbers? n = 3, l = 1, m = 0

The relation between $n_m$ ($n_m$ = number of permissible values of magnetic quantum number, $m_l$) for a given value of azimuthal quantum number ($l$) is:

Which one of the following ions has electronic configuration [Ar]3d⁶? (At. no: Mn = 25, Fe = 26, Co = 27, Ni = 28)

How many electrons can fit in the subshell for which n = 3 and l = 1?