Solution:
Principal Quantum Number (n): This number tells us the principal energy shell. In the notation of an orbital (like 3d or 4s), the number at the beginning is the value of n.
Azimuthal Quantum Number (l): This number defines the subshell and the shape of the orbital. We use specific letters to denote the value of l:
If l=0, the subshell is 's'.
If l=1, the subshell is 'p'.
If l=2, the subshell is 'd'.
If l=3, the subshell is 'f'.
The designation for an orbital is given by writing the value of n followed by the letter for the subshell (determined by l).
Now, let's look at each item from List I.
A. For n=2 and l=1:
The principal quantum number n is 2.
The azimuthal quantum number l is 1, which corresponds to the 'p' subshell.
Therefore, the orbital is designated as 2p.
This matches with II in List II.
B. For n=4 and l=0:
The principal quantum number n is 4.
The azimuthal quantum number l is 0, which corresponds to the 's' subshell.
Therefore, the orbital is designated as 4s.
This matches with III in List II.
C. For n=5 and l=3:
The principal quantum number n is 5.
The azimuthal quantum number l is 3, which corresponds to the 'f' subshell.
Therefore, the orbital is designated as 5f.
This matches with IV in List II.
D. For n=3 and l=2:
The principal quantum number n is 3.
The azimuthal quantum number l is 2, which corresponds to the 'd' subshell.
Therefore, the orbital is designated as 3d.
This matches with I in List II.
So, the correct matches are:
A → II
B → III
C → IV
D → I
Looking at the options, we can see that this combination corresponds to Option C.
The correct answer is Option C: A-II, B-III, C-IV, D-I.
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