Textbook 1D #21

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JaylinWangDis1L
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Textbook 1D #21

Postby JaylinWangDis1L » Sat Nov 07, 2020 7:46 pm

1D.21 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

IsaacLaw1E
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Re: Textbook 1D #21

Postby IsaacLaw1E » Sat Nov 07, 2020 7:49 pm

For the number part, just use the n value. For the letter, it depends on the l value.
l = 0 is s
l = 1 is p
l = 2 is d
l = 3 is f

Kelly Ha 1K
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Re: Textbook 1D #21

Postby Kelly Ha 1K » Sat Nov 07, 2020 7:52 pm

To add on to the previous answer, the number of orbitals simply corresponds to the subshell (letter) you identified:
s subshell has one orbital
p subshell has three orbitals
d subshell has five orbitals
f subshell has seven orbitals

Crystal Pan 2G
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Re: Textbook 1D #21

Postby Crystal Pan 2G » Sat Nov 07, 2020 9:08 pm

n gives the energy level, and every orbital can hold up to two electrons. l=0 would correspond to s sublevel, l=1 would be p, l=2 would be d, and l=3 would be f, etc. for instance, n=5 l=2 would be 5d based on the definition we gave for n and l.

Mahnoor_Wani_1I
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Re: Textbook 1D #21

Postby Mahnoor_Wani_1I » Sat Nov 07, 2020 9:15 pm

Just out of curiosity, If it is more than 5 orbitals, do we go by alphabet order or is there a specific order you need to go by

Rachel Kho Disc 2G
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Re: Textbook 1D #21

Postby Rachel Kho Disc 2G » Sun Nov 08, 2020 9:33 pm

A tip my TA gave me was super helpful in understanding the relationship between l and s,p,d,f orbitals.

when l = 0 --> s
when l = 1 --> p
when l = 2 --> d
when l = 3 --> f

a) l = 2 corresponds to the d orbital.
b) l = 0 corresponds to the s orbital.
c) l = 2 corresponds to the d orbital.
d) l = 3 corresponds to the f orbital.

And whatever n equals, that is the number you put in front. So your answers should be a) 5d, b) 1s, etc. Another good tip to study for the midterm is what would the ml values be for each of these questions?

Hope this helps!


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