Rules For Filling Electrons in Orbitals

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

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

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

Assertion : The ${19}^{\mathrm{th} }$electron in potassium atom enters into $4\mathrm{s}-$orbital and not the $3\mathrm{d}-$orbital.

Reason : $(\mathrm{n} + \mathrm{l})$ rule is followed for determining the orbital of the lowest energy state.

In any atom which sub-shell will have the highest energy in the following

If the principal quantum number $\text{n}=6,$ the correct sequence of filling of electrons will be:

When $4\mathrm{f}$ level is completely filled with electrons, the next electron will enter into the sub-shell whose $(\mathrm{n}+\mathrm{l})$ is equal to:

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

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

Which rule of filling of electrons states that every orbital in a sublevel is singly occupied before any orbital is doubly occupied, all the electrons in singly occupied orbitals have the same spin?

Four electrons, each of mass $m_e$ are in a one dimensional box of size $L$. Assume that, the electrons are non-interacting, obey the Pauli exclusion principle and are described by standing De Broglie waves confined within the box. Define $\alpha =\frac{h^2}{8m_e{L}^2}$ and $U_0$ to be the ground state energy. Then,

For a multi-electron atom, the highest energy level among the following is

Which of the following shell have maximum $32$ electrons?

The correct set of four quantum numbers for the valence electron of rubidium atom $(\mathrm{Z} = 37)$ is:

Hund's rule of maximum multiplicity is valid in :

Select correct electronic configuration following the Hund's Rule, if $6{\mathrm{e}}^{-}$ are present in $\mathrm{d}-$ sub shell

Arrangement of the following group of orbitals in which they fill with electrons:
$\left(5\mathrm{f},6\mathrm{p},4\mathrm{p},6\mathrm{s},4\mathrm{d},4\mathrm{f}\right)$

The orbital diagram in which the aufbau principle is violated is?