Question

the number of orbitals with the quantum numbers n=3, l=2 and ml=0 is _____

Answer 1

Explanation:

The total number of possible orbitals with the same value of l (a subshell) is 2l + 1. Thus, there is one s-orbital for ml = 0, there are three p-orbitals for ml = 1, five d-orbitals for ml = 2, seven f-orbitals for ml = 3, and so forth. The principal quantum number defines the general value of the electronic energy.

Answer 2

The number of orbitals with the quantum numbers n=3, l=2 and ml=0 is _five 3d orbitals. ____

• n is the principal quantum number. For n=3 the orbital will be third orbital.
• l is azimuthal quantum number. For l=0,1,2,3.... orbitals will be s, p, d, f.
• m is spin quantum number. For m equal to all five d orbitals will exist.