# (a) Principal quantum no. n is de6ned as 1, 2, 3.... (b) Azimuthal quantum no.l is defined as 1 lo n + 2 in integral steps.(c) Magnetic quantum no. m is defined -l/2 to l/2 (including zero, if any, in integral steps). (d) Spin quantum no. s has six possible values (-2,-1, - 1/2,+1,+2)(e)The subsell corresponding to l=1,2,3,4,5,.....designated as F, G, H, I, J, k.... respectively.(f) The values of m for a given values of l give the number of orbitals in a sub-shell.(g) The principle for filling of  ${\mathrm{e}}^{-}$ in the shells remains unchanged.The no. of orbitals and maximum no. of ${\mathrm{e}}^{-}$that can be filled in a J-subshell respectively will be :

1. A

6, 36

2. B

5, 30

3. C

4, 24

4. D

7, 42

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### Solution:

In the subshell J,
$l=5$

The values of m,

$m=-\frac{5}{2},-\frac{3}{2},-\frac{1}{2},+\frac{1}{2},+\frac{3}{2},+\frac{5}{2}$

Number of orbital=6.

So, the no. of orbitals and maximum no. of ${\mathrm{e}}^{-}$that can be filled in a J-subshell respectively will be 6,36.

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