explain briefly why each of the following is NOT a possible set of quantum numbe

Question

explain briefly why each of the following is NOT a possible set of quantum numbers for an electron in an atom -

a) n=4, l=2, ml=0, ms= 0
b) n=3, l=1, ml= (-3) , ms= (-1/2)
c) n=3, l=3, ml= (-3), ms= +1/2
d) n=2, l=3, ml= 0 , ms= +1/2
e) n=2, l=1, ml= (-1), ms= 0
f) n=3, l=1 ml=+2, ms=+1/2

what is the max number of electrons that can be identified with each of the following sets of quantym numbers? in some cases, the answer may be "none"

a) n=3
b) n=3, l=2
c) n=4, l=1, ml= (-1), ms= +1/2
d) n=5, l=0, ml= +1
e) n=4, l=3
f) n=6, l=1 ml= (-1)
g) n=3, l=3, ml= (-3)

predict the electron configuration for each of the following

a) Ge

b) Cd

c) Gd

d) Sr

Explanation / Answer

Ge 1s2 2s2 2p6 3s2 3p6 4s2 3d10

Cd 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10

Gd 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f7 5d1

Sr 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2

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