Question

Only certain transitions are allowed from one energy level to another. In one-electron species, the change in l of an allowed transition is ±1. For example, a 3p electron can move to a 2s orbital but not to a 2p. Thus, in the UV series, where n_final =1 , allowed transitions can start in a p orbital (l = 1) of n = 2 or higher, not in an s (l = 0) or d (l = 2) orbital of n = 2 or higher. From what orbital do each of the allowed transitions start for the first four emission lines in the visible series ( n_final=2)?

Answer 1

In light of the orbital n = 2, (L) can be either 0 or 1.

Accordingly, the possible transitions from higher levels with n_final=2 will be n = 6 → n = 2, n = 5 → n= 2, n = 4 → n= 2, n= 3 → n= 2

Typically, both s(L = 0) and p(L = 1) orbitals are present in the second orbit.

This indicates that the allowed transition in the selection rule requires that the change in the quantum number (L) of an allowed transition be +1.

The permitted transitions in the second orbit are as follows:

between n = 3 and n = 2

The third orbit often contains three orbitals, which means that the three potential transitions for an electron from n = 3 to n = 2 are 3p to 2s, 3d to 2p, and 3s to 2p.

Additionally, the transitions 4p 2s, 4d 2p, and 4s 2p are achievable from n = 4 to n = 2.

This implies that four spectral lines—3p to 2s, 3d to 2p, 3s to 2p, and 4s to 2p—are obtained from these transitions.

What is determined by PQN?

• In general, the principal quantum number (PQN) determines the permitted sub shell (L) in a specific orbit (n).

• The angular quantum number L (i.e., the sub shells) can now only have the value of "0" for the first orbit.

Learn more about spectral lines here:

brainly.com/question/27494244

#SPJ4