Multielectron vs H-atom

[JTieu_1L]

Which of the following increase when an electron in a lithium atom undergoes a transition from the 1s-orbital to a 2p-orbital? (a) Energy of the electron. (b) Value of n. (c) Value of l. (d) Radius of the atom. Which answers would be different for a hydrogen atom and in what way would they be different?

Does anyone know the answer to the second question? It does not say in the textbook solutions. Would c be the only one that is different?

[Kareena Patel 1G]

So actually these are all the same as the hydrogen atom. All of these would increase so there is no difference to the hydrogen atom.

[Shrey Pawar 2A]

As Kareena said above I would think that these would all be the same for hydrogen as everything would increase for both the lithium and hydrogen. The energy would increase because it is going to a higher energy level. N would increase for the same reason. l would increase due to a change from s to p orbital and the radius would be larger because there would be more electron-electron repulsion. Hope this helps!

[MHarrold_1E]

I believe that they all increase even for a H atom because when the energy level increases, so does the possible values for the quantum numbers.

[Yun Su Choi 3G]

So does that mean that even though the electron configuration for hydrogen is 1s1 (n=1, l=0, ml=0, ms=+1/2), the electron is not restricted to those quantum numbers and can potentially occupy n=2,3,4 shells and other sublevels?
Is the electron configuration for hydrogen 1s1 simply because that is its lowest energy state and therefore the most stable state?