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Postby ClaireHW » Wed Nov 01, 2017 6:07 pm

How many electrons can have to following electrons in an atom:
a) n=2, l=1
b) n=4, l=2, m=-2
c) n=2
d) n=3, l=2, m=+1

I'm confused about the logic behind solving these problems.

(Claire Woolson Dis. 3J)

Ashley Chipoletti 1I
Posts: 20
Joined: Fri Sep 29, 2017 7:04 am

Re: 2.29

Postby Ashley Chipoletti 1I » Wed Nov 01, 2017 6:23 pm

So basically to figure out how many electrons are designated you can see what are the possible electrons that have these quantum numbers. For a) n=2 designates the second shell and l=1 designates p. Therefore, since this is the 2p orbital, 6 electrons can have these quantum numbers. For b) the subshell is 2, which designates d, and m=-2 designates a specific orbital. Each orbital can hold two electrons, which means only 2 electrons can possibly have these quantum numbers.

Guadalupe T 1E
Posts: 58
Joined: Fri Sep 29, 2017 7:04 am

Re: 2.29

Postby Guadalupe T 1E » Wed Nov 01, 2017 6:29 pm

For a) the alphabetical letter for l=1 is p. Also the quantum/group number is given (4) So it is 4p. The most # of electrons 4p can have is six.
For c, the group number is given 2. The most number of electrons that group 2 can have is 8. (2s2 4p6) 2+6=8
I am not sure how to find the others because it seems that m has something to do with it and I don't know why.

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