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?

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)  F2+  (D)  F3+

Tardigrade Admin · Accepted Answer

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] F2+=2,5 [d] F3+=2,4 Therefore, F+ion will be the most stable ion.

Q. 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?

$F^{-}$

$F^{+}$

$F^{2 +}$

$F^{3 +}$

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.

Q. 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?

F−

F+

F2+

F3+