How many electron in an atom may have the following quantum number? `n = 4, l=0 , s=+1//2`

The set of quantum numbers, n = 3, l = 2, m_(l) = 0

What is the maximum number of electrons in a subshell that can have the quantum numbers n = 3 and l = 2 ?

How many electrons in an atom can have n = 4, l =2 ,m= -2 and s = +1/2 ?

Describe the orbital with quantum number n=5 and l=3

No two electrons in an atom will have all the four quantum numbers same. This statement is known as

STATEMENT-1: An orbital cannot have more then two electrons and they must have opposite spins. STATEMENT-2: No two electrojns in an atom can have same set of all the four quantum numbers as per Pauli's exclusion principle.

Describe the orbital with the quantum number : n = 1 l = 0

An orbital is occupied by an electrons with the quantum numbers n = 4, l = 1. How many orbitals of this type are found in a multi- electron atom ?

Calculate the minimum and maximum number of electrons which may have magnetic quantum number m=+1 and spin quantum number s=-(1)/(2) in chromium (Cr)

Using s, p, d notations, describe the orbital with the quantum number. n = 4 , l = 2