hw problem 1D.21

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Joanna Mendoza 3J
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hw problem 1D.21

Postby Joanna Mendoza 3J » Thu Oct 17, 2019 6:49 pm

problem: Write the subshell notation (3d, for instance) and the number of orbitals having the following quantum numbers: (a) n=5, l=2; (b) n=1, l=0; (c) n=6, l=3; (d) n=2, l=1.

I know that to get the number of orbitals you use 2(l)+1 but can someone explain to me how to get/write the subshell notation?

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Re: hw problem 1D.21

Postby Chem_Mod » Thu Oct 17, 2019 7:38 pm

Subshell notation is written as the shell number, followed by the type of orbital it belongs (Ex: 3p, 4s, 5d)

Angular momentum numbers correlate as follows:
l=0 --> s
l=1 --> p
l=2 --> d

For part a, since n=5 and l=2 (ie d), then the subshell is 5d.

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Re: hw problem 1D.21

Postby AniP_2D » Fri Oct 18, 2019 11:26 am

The subshell notation is basically the n-value and and the subshell that corresponds to l.
If l=0, s is the subshell, l=1 then p, l=2 then d, and l=3 f
So for (a) the subshell notation would be 5d and for (b) it would be 1s

For orbitals you would just look and see how many possible ml values the certain of quantum numbers would have, so for (a) since l=2, the possible ml values are -2, -1, 0, 1, 2, so there would be 5 orbitals. For (b) since l=0, the possible ml values are 0, so there would be only one orbital.

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