291st one is also wrong
when l=0 then m shud be equal to zero..
Which of the following set of quantum numbers is impossible for an electron?
n=1,l=0,ml=1,ms=+1/2
n=3,l=2,ml= -3,ms=+1/2
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8 Answers
11the 2nd one..
n-3 max. d subshell is max..
m=-2 is least possible m value in d..
m=-3 is posssible in f only...but thats not possible with n=3.
1Neither of thetwo is possible,
Basic rules of quantum numbering are
a l =[0,n]
b ml= [-l,l]
c ms={-1/2,1/2}
The second rule is not adhered to in both the cases
1both r wrong
because m can only take values from -L to +L through 0
so when m is 0 l can only be 0
when m is 2 l can be -2,-1,0,1,2
1For given n,l can take integral values fron 0 to (n-1)
For given l,m can take integral values between -l and +l
in case 1, l=0 so m can have only 1 possible value: 0 but not 1 as given in the question.
in case 2, l=2 so m can have values -2,-1,0,1,2 but not -3 as given in the question.
Thus,both are not possible.
