The number of electrons in an atom which has its quantum number n equal to 2 (n = 2) and ml equal to 2 (ml = 2) is equal to zero (0).
An electron can be defined as a subatomic particle that is negatively charged and it's found outside the nucleus of the atom of a chemical element. This ultimately implies that, an electron is the opposite of a subatomic particle called proton.
The Pauli exclusion principle can be defined as a principle which states that no two electrons (fermions) in a single atom can have the same numerical values for all four (4) of their electronic quantum numbers.
Furthermore, this principle states that the orbital of an atom can only contain a maximum of two (2) electrons, and they must have opposing spin orientations.
Based on Pauli exclusion principle, we can infer and logically deduce that the number of electrons in an atom which has its quantum number n equal to 2 (n = 2) and ml equal to 2 (ml = 2) would be equal to zero (0).
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