The following quantum numbers are possible for how many orbital(s) n = 3 ,l = 2 and m = +2 are possible ?

Question

The following quantum numbers are possible for how many orbital(s) n = 3 ,l = 2 and m = +2 are possible ? (A) 1 (B) 2 (C) 3 (D) 4

Tardigrade Admin · Accepted Answer

n = 3,l = 2,m = + 2,s = ± 1/2 These values of quantum numbers are possible for only one of the five 3d-orbitaIs as +2 value of m is possible only for one orbital.

Q. The following quantum numbers are possible for how many orbital(s) $n = 3$ , $l = 2$ and $m = + 2$ are possible ?

1

2

3

4

$n = 3, l = 2, m = + 2, s = \pm 1/2$
These values of quantum numbers are possible for only one of the five $3 d$ -orbitaIs as $+ 2$ value of m is possible only for one orbital.

Q. The following quantum numbers are possible for how many orbital(s) n=3 ,l=2 and m=+2 are possible ?

1

2

3

4

n=3,l=2,m=+2,s=±1/2 These values of quantum numbers are possible for only one of the five 3d-orbitaIs as +2 value of m is possible only for one orbital.

Q. The following quantum numbers are possible for how many orbital(s) $n = 3$ , $l = 2$ and $m = + 2$ are possible ?

$n = 3, l = 2, m = + 2, s = \pm 1/2$
These values of quantum numbers are possible for only one of the five $3 d$ -orbitaIs as $+ 2$ value of m is possible only for one orbital.