Question

Consider the following set of quantum numbers and place them in order of increasing energy
I. n = 4, l = 0, ml = 0, ms = -1/2
II. n = 4, l = 2, ml = -1, ms = -1/2
III. n = 5, l = 0, ml = 0, ms = +1/2

I < II < III

III < II < I

I < III < II

II < III < I

III < I < II

Answer 1

If o can be predicted d) for each erbital n= Principal quantum numer la angular quantum number The relative energies of the orbitals can be pl by (n+1) rule. The sum of Chris for each on according to the following rules? a Orbitals are filled in order of increasing ( n l) which represents the relative energy, b) If two orbitals have the same value of (ned), they are filled in order of increasing n. 1. n=4, 120, me zo, my 2-2 - nel 24 11.0=4, 122, me aul, m, 2-1/2 url a 6 u n=5, 120, m, zo, mga +1/2 ntle 5 Order of increasing energy → 1 <11 ( 11