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21 October, 08:51

What is the maximum number of electrons that can occupy each of the following subshells?

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Answers (2)
  1. 21 October, 09:09
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    Using paulis exclusive principle which states that no two electrons can have the same four electronic quantum numbers,

    A. 3 p

    3p is in the 3rd shell (m), p orbital has 3 orbitals which contain only 2 electrons. Therefore, total electrons in the p orbital = 2 * 3

    = 6 orbitals.

    B. 5 d

    5 d is in the 5th shell, d orbital has 5 orbitals which contain only 2 electrons. Therefore, total electrons in the p orbital = 2 * 5

    = 10 orbitals.

    C. 2 s

    2 s is in the 2nd shell (l), s orbital has 1 orbitals which contain only 2 electrons. Therefore, total electrons in the p orbital = 2 * 1

    = 2 orbitals.

    D. 4 f

    4 f is in the 4th shell (n), f orbital has 7 orbitals which contain only 2 electrons. Therefore, total electrons in the p orbital = 2 * 7

    = 14 orbitals.
  2. 21 October, 09:14
    0
    s (l = 0) only two electrons

    p (l = 1) sublevel six (6) electrons fit

    d (l = 2) sub-level has 10 electrons

    f (l = 3) has 7 has 14 electrons

    Explanation:

    The electrons have an odd spin, so they must comply with the Pauli principle, therefore only two electrons fit in a given sublevel.

    Sub level s (l = 0) only two electrons

    Sub level p (l = 1) has three orbitals in which two electrons fit, therefore in the sublevel six (6) electrons fit

    Sub-level d (l = 2) has 5 orbitals each with two electrons, the sub-level has 10 electors

    Sub-level f (l = 3) has 7 orbitals and two electrons each, the sub-level has 14 electrons
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