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

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.

Explain the Aufbau principle with copper and chromium.

Pauli exclusion principle states that the ground state of the atoms, the orbitals are filled in order of their increasing energies.

According to the Aufbau principle, valence electron in _____ must choose between 3d and 4s orbitals and as predicted by this sequence, it is found in 4s orbital.

Which formula is used for calculating effective nuclear charge?

What effective nuclear charge?

What do you mean by effective nuclear charge?

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: