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Question

In the ground state electronic configuration of Mn (Z=25):

A

the number of electrons having n+l = 4 are 5

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B
the number of electrons having m=0 are 13
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C

the electron is first filled in 3d then in 4s subshell

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D

the number of electrons having l=1 are 10

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Solution

The correct option is B the number of electrons having m=0 are 13

Ground state electronic configuration for Mn is:
Mn=1s22s22p63s23p63d54s2
Now let’s check n+l value for each subshell involved i.e
1s1+0=1
2s2+0=2
2p2+1=3
3s3+0=3
3p3+1=4
3d3+2=5
4s4+0=4
So there are two cases for which n+l=4 i.e. 3p and 4s. Hence, total no of electrons are 8. So (a) option is incorrect.
m will be zero for electrons in all s subshell, one orbital each in each p subshell and d subshell. For Mn, total number of electrons having m = 0 is 13. Hence (b) option is correct.

In ground state electron is first filled in 4s than in 3d because 4s is of lower energy than 3d as per (n+l) rule. Hence (c) is incorrect.

The electrons having l=1 (p subshell) are 12. Hence (d) option is incorrect.


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