Which of the following ions is most unlikely to exist?

L i^{+}

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B e^{-}

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B^{-}

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F^{-}

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Solution

The correct option is B $B e^{-}$
It is $B e^{-}$
The electronic configurations for $L i^{+}, B e^{-}, B^{-}$ & $F^{-}$ are given by,
$L i^{+} : 1 s^{2}$ $B^{-} = 1 s^{2} 2 s^{2} 2 p^{2}$
$B e^{-} : 1 s^{2} 2 s^{2} 2 p^{1}$ $F^{-} = 1 s^{2} 2 s^{2} 2 p^{6}$
Half filled & fulfilled orbitals are more stable. In $B e^{-}$ it is unlikely that already fulfilled orbitals in $B e$ accept electrons to form $B e^{-}$ .

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