Question

It is believed that atoms combine with each other such that the outermost shell acquires a stable configuration of $8$ electrons. If stability were attained with $6$ electrons rather than $8$; what would be the formula of the stable fluoride ion?

• A. $F^{-}$
• B. $F^{+}$
• C. $F^{2+}$
• D. $F^{3+}$

Answer 1

Answer: (B)

$F^{+}$

Answer 2

If stability is attained with $6$ electrons, the stable ion will contain $6$ electrons in its valency shell...
Electronic configuration of...
[a] $F^{-}=2,8$
[b] $F^{+}=2,6$
[c] $F^{2+}=2,5$
[d] $F^{3+}=2,4$
Therefore, $F^{+}$ion will be the most stable ion.