<Dl> <Dd> E B = − R h c n 2 (\ displaystyle E_ (\ text (B)) = - (\ dfrac (Rhc) (n ^ (2)))), </Dd> </Dl> <Dd> E B = − R h c n 2 (\ displaystyle E_ (\ text (B)) = - (\ dfrac (Rhc) (n ^ (2)))), </Dd> <P> where R is the Rydberg constant, h is Planck's constant, c is the speed of light and n is the principal quantum number . </P> <P> For multi-electron atoms in Rydberg states with a low value of the orbital angular momentum, there is a high probability of finding the excited electron near the nucleus where it can polarize or even penetrate the ion core, modifying the potential . The resulting shift of the energy levels is represented mathematically as an angular momentum dependent quantum defect, δ: </P>

Why does quantum defect depend on n and l