If stability were attained with $6$ electrons rather than with $8$ electrons, what would be the formula of the stable fluorine ion?

F^{3 +}

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F^{+}

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F^{-}

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F^{2 -}

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Solution

The correct option is B $F^{+}$
Electronic configuration of $F$ in atomic state is $1 s^{2} 2 s^{2} 2 p^{5}$ , i.e., $7$ electrons in outermost shell.
If stability is attained at $6$ electrons, it will lose $1$ electron to attain stability.

$F^{+} - 1 s^{2} 2 s^{2} 2 p^{4}$

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Similar questions

It is thought that atoms combine with each other such that the outermost orbit acquires a stable configuration of 8 electrons. If stability were attained with 6 electrons rather than with 8, what would be the formula of the stable fluoride ions?

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If stability were attained with 6 electrons rather than with 8 electrons, what would be the formula of the stable fluorine ion?

The correct option is B F+Electronic configuration of F in atomic state is 1s22s22p5, i.e., 7 electrons in outermost shell.If stability is attained at 6 electrons, it will lose 1 electron to attain stability.F+−1s22s22p4

If stability were attained with $6$ electrons rather than with $8$ electrons, what would be the formula of the stable fluorine ion?

The correct option is B $F^{+}$
Electronic configuration of $F$ in atomic state is $1 s^{2} 2 s^{2} 2 p^{5}$ , i.e., $7$ electrons in outermost shell.
If stability is attained at $6$ electrons, it will lose $1$ electron to attain stability.

$F^{+} - 1 s^{2} 2 s^{2} 2 p^{4}$