Filling of Electrons in Orbitals

In a given atom no two electrons can have the same values for all the four quantum numbers. This is called

An ion has $18$ electrons in the outermost shell is:

If n = 6, the correct sequence for filling of electrons will be :

Number of unpaired electrons in ${\mathrm{N}}^{2+}$ is

The orientation of an atomic orbital is governed by

If the energy of a photon is given as, $\text{E}=3.03\times {10}^{-19} \mathrm{J}$, then, the wavelength $\mathrm{(\lambda )}$ of the photon is

The Bohr orbit radius for the hydrogen atom (n = 1) is approximately  $0.530\AA .$  The radius for the first excited state (n = 2) orbit is  $(in\AA )$

For which one of the following sets of four quantum numbers, an electron will have the highest energy?

Incorrect among the following is/are

(a) The number of electrons having $\mathrm{m}=0$ in sodium metal is $7$

(b) Energy of $4\mathrm{s}$ orbital is more than $3\mathrm{d}$ orbital in $\mathrm{H}-$atom

(c) Energy of $2\mathrm{s}$ orbital in oxygen is more than in carbon atom

The total number of electrons present in all the $\mathrm{p}-$orbitals in the ground state of ${}_{34}\mathrm{Se}$ are

What is the total number of unpaired electrons in one mole of ${}_{29}\mathrm{Cu}$?

Maximum number of electrons in a subshell of an atom is determined by $4\mathrm{l}+2$.

The orbital diagram in which both the Pauli's exclusion principle and Hund's rule are violated is

Which is the correct order of increasing energy of the listed orbitals in the atom of titanium?

'The orbitals of equal energy (degenerate) are occupied with one electron each before the pairing of electron starts.' This is according to the: