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Use Hund's rule to derive the electronic...

Use Hund's rule to derive the electronic configuration of `Ce^(3+)` ion, and calculatel its magntic moment on the basis of spin-only formula.

Text Solution

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`._(58)Ce= [Xe]^(54) 4f^(1) 5d^(1) 6s^(2)`
`Ce^(3+) = [Xe]^(54) 4f^(1) , i.e., `there is only one unpaired electron , i.e., `n=1`. Hence,
`mu = sqrt(n(n+2)) BM = sqrt(1( 1+2)) = sqrt( 3) BM= 1.73BM`
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Use Hund's rule to derive the electronic configuration of Ca^(3+) ion, and calculate its magnetic moment on the basis of 'spin-only' formula.

(a) Use Hund’s rule to derive the electronic configuration of Ce^(+3) ions and calculate its magnitude moment.

Knowledge Check

  • Transition metals and many of their compounds show paramagnetic behaviour where there are unpaired electron or electrons. The magnetic moment arises from the spin and orbital motions in ions or molecule. Magnetic moment of n unpaired electrons is given as mu=sqrt(n(n+2)) Bohr magneton Magnetic moment increases as the number of unpaired electrons increases. Q. There are three unpaired electrons in [Co(H_2O)_6]^(2+) and calculated value of magnetic moment on the basis of sqrt(n(n+2)) formula is 3.87 BM. which is lower than the expermental value of 4.40 BM. The reason for this difference is due to

    A
    increase in number of unpaired electrons during determination
    B
    Some contribution of the orbital motion of the electrons to the magnetic moment
    C
    d-d transition
    D
    Experimental error

  • The atomic number of cerium (Ce) is 58. The correct electronic configuration of Ce^(3+) ion is

    A
    `[Xe]4f^(1)`
    B
    `[Kr]4f^(-1)`
    C
    `[Xe]4f^(-13)`
    D
    `[Kr]4d^(1)`

  • the atomic number of cerium ( Ce ) is 58 . The correct electronic configuration of Ce^(3+) ion is

    A
    `[Xe] 4f^(1)`
    B
    `[Kr]4f^(1)`
    C
    `[Xe] 4f^(13)`
    D
    `[Kr] 4d^(1)`

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