Question

Which of the following is a possible set of quantum numbers for an electron?

(1, 1, 0, +½)

(2, 1, 1, +½)

(3, 2, 3, -½)

(3, -1, 0, -½)

Answer 1

@ganeshie8 @Hero

Answer 2

any ideas .-. i dont even understand this

Answer 3

(n, l, m, s)

Answer 4

n is a natural number
l is a whole number and l = 0, 1, 2 ... (n-1)

Answer 5

so you can eliminate first and last options cuz :
1) first option n=l which is impossible
2) last option has l = negative number, which is also impossible

Answer 6

where are we getting the numbers from .-.

Answer 7

please don't ask tough questions lol im very bad in chem :o

Answer 8

the magnetic quantum number m ranges from -l to l,
so you can eliminate one other option, can you guess ?

Answer 9

so we eliminate d.... then what?

Answer 10

we have eliminated A and D earlier

Answer 11

we don't need to eliminate it again.

Answer 12

the reason for eliminating A and D options is \(l\) - the angular momentum quantum number, it has to be less than \(n\)

Answer 13

options A and D fail that requirement, if that makes any sense...

Answer 14

but c has two of the same numbers so that one cant be it right? so its b :D

Answer 15

@ganeshie8

Answer 16

b is correct !
but c doesn't work for a different reason

Answer 17

the magnetic quantum number \(m\) ranges from \(-l\) to \(l\), but in option C, the value of \(m\) is greater than \(l\) so option C is impossible

Answer 18

this site has nice explanation :
http://chemwiki.ucdavis.edu/Physical_Chemistry/Quantum_Mechanics/Quantum_Theory/Trapped_Particles/Atoms/Quantum_Numbers

Answer 19

do you wana get alot more chem medals? :D

Answer 20

lol you're forcing me to learn chem! :D

Answer 21

yussss but at least im not into the hard stuff yet XD