How many orbitals can have the following set of quantum numbers, `n=3,l=1,m=0?`

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

Which orbital represents the following set of quantum numbers n =3, l=0, m =0 s = + 1//2

An electron in an atom can be completely designated with the help of four quantum numbers. Out of these, the first three i.e., principal (n), azimuthal (l) and magnetic (m) quantum number are obtained from the solution of Shrodinger wave equation while the spin(s) quantum number arises from the spin of the electron around its axis clockwise or antiaclockwise. Ot of these principal quantum number tells about the size, azimuthal quantum number about the shape and magnetic quantum signifies the orientation of the electron orbital. How many electrons in a given atom have the following set of quantium numbers? n = 3, l =2, m = +2, s = -1//2

In how many elements the last electron will have the following set of quantum numbers, n = 3 and l = 1?

what is the maximum number of electrons that can be associated with the following set of quantum numbers ? n=3 , l=1 and m=-1

An orbital made of four lobes can have the following quantum numbers n=2,l = 2, m=0; n=3,l = 1. m = -2; n=3,l = 2,m=-1; n=3,l = 3,m =-3;

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

An electron in an atom has the following set of quantum numbers: n=3,l=2,m_(l)=+1,m_(s)=+1//2 In which subshel can the electron be found?

An electron in an atom has the following set of quantum numbers: n=3,l=2,m_(l)=+1,m_(s)=+1//2 According to the quantum mechanical picture of the atom, which quantum number(s) could be different for electons in this same atom that have exactly the same energy?