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AFMC AFMC Solved Paper-2003

  • question_answer
    How many electrons can be accommodated in a p sub-orbital?

    A) 6 electrons         

    B) 2 electrons

    C) 4 electrons         

    D) none of these

    Correct Answer: B

    Solution :

    Each electron in an orbit of an atom is designated by a set of four quantum numbers. Principle quantum number (n): It tells the energy level in which the electron lie and the  size of the atom, various shell are denoted by K, L, M, N.... etc., (1, 2, 3. 4.... shell). Angular momentum quantum number or azimuthal quantum number (l): It has value from 0 to n -1. The sub-shells are designated as s, p, d f...........
    Value of \[l\] Sub ? shell
    0 S
    1 P
    2 D
    3 F
    4 G
         5?. h?.
    \[n=1,\,\,l=0\] only s \[n=2,\,\,l=0,\,1s,\]sub-shell only \[n=3,\,l=0,\,1,\,2s,\,p,d\]sub-shell only magnetic quantum number \[({{m}_{e}})\] refers to different orientations of electron in a particular sub-shell. Its value ranges from\[+\,l\]through 0 to \[+\,l\]with total \[2l+1\] values. The spin quantum number \[({{m}_{s}})\] determine the orientation of spin angular momentum and has two values \[+\frac{1}{2}\] and \[-\frac{1}{2}.\]In the above question for p orbital \[l=1\] \[\therefore \]  \[{{m}_{e}}\]has \[(2l+1)=3\] values, thus p orbital has only 3 sub-orbital for d, \[l=2\]i.e., 5 values of \[{{m}_{e}}\]thus 5 sub-orbitals As \[{{m}_{s}}\]has two values thus two electrons with opposite spin occupy one sub-orbital.


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