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Why B(2) is paramagnetic in nature while...

Why `B_(2)` is paramagnetic in nature while `C_(2)` is not?

Text Solution

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The molecular orbital electronic configuration of both `B_(2) and C_(2)` are:
`B_(2):[sigma1s]^(2)[sigma^(**)1s]^(2)[sigma^(**)2s]^(2)[sigma^(**)2s]^(2)[pi2p_(x)]^(1)[pi2p_(y)]^(1)`
`B_(2):[sigma1s]^(2)[sigma^(**)1s]^(2)[sigma^(**)2s]^(2)[sigma^(**)2s]^(2)[pi2p_(x)]^(2)[pi2p_(y)]^(2)`
Since `B_(2)` has two unpaired electrons, therefore, `B_(2)` is paramagnetic.
`C_(2)` has no unpaired electron, therefore, `C_(2)` is diamagnetic.
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Knowledge Check

  • Assertion (A): B_(2), O_(2), NO are paramagnetic in nature.

    A
    Both (A) and (R) are correct and (R) is the correct explanation of (A).
    B
    Both (A) and (R) are correct but (R) is not the correct explanation of (A).
    C
    (A) is correct but (R) is wrong.
    D
    (A) is wrong but (R) is corTect.

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    `[Zn(NH_3)_4]^(2+)`
    B
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    C
    `[Ni(H_2O)_6]^(2+)`
    D
    `[Ni(CN)_4]^(2-)`

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