HOMEWORK PROBLEM 2.19

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april_bussey_1C
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Joined: Fri Apr 06, 2018 11:02 am

HOMEWORK PROBLEM 2.19

Postby april_bussey_1C » Sun Apr 29, 2018 11:41 pm

2.19 (a) How many values of the quantum number l are
possible when n  7? (b) How many values of ml are allowed
for an electron in a 6d-subshell? (c) How many values of ml
are allowed for an electron in a 3p-subshell? (d) How many
subshells are there in the shell with n  4?

Im not fully understanding the correlation between l and n. How do we know what l is when we're given n (part a for this question)? and vice versa? same with ml (part b and c)? and how do we know the relationship between subshells when given n (part d for this question)?

Hannah Lee 1B
Posts: 26
Joined: Fri Apr 06, 2018 11:03 am

Re: HOMEWORK PROBLEM 2.19

Postby Hannah Lee 1B » Mon Apr 30, 2018 3:10 pm

n is the principal quantum number (energy level/shell) while L describes the subshell (s, p, d, f).
For part a:
Values for L (subshells) ranges from 0 - (n-1), so when n=7, L could be anything from 0-7. Thus, 8 values are possible. You can work backward as well.
For parts b and c:
ml describes the different orbitals and goes from -L - L. For example since p subshell corresponds with L=1, ml could be -1, 0, or 1.
Part d:
is basically asking the same thing as part a since subshells correspond with quantum number L

Andrew Berard 1F
Posts: 21
Joined: Fri Apr 06, 2018 11:01 am

Re: HOMEWORK PROBLEM 2.19

Postby Andrew Berard 1F » Wed May 02, 2018 12:45 pm

For part a, wouldn't it be 0-6, as the range is from 0 - (n-1)

Yeo Bin Yook 1K
Posts: 30
Joined: Fri Apr 06, 2018 11:05 am

Re: HOMEWORK PROBLEM 2.19

Postby Yeo Bin Yook 1K » Thu May 03, 2018 6:09 pm

For part a, l would be 0~6 which makes it 7 numerical values in total. You know it is 0~6 because n=7 and l=0,...n-1.


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