Question #67e72

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Question #67e72

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Answer 1 · 2014-04-02T02:56:40

Ionic compounds do not actually satisfy the octet rule.

The octet rule is that atoms of elements are most stable when the valence shell of $s^2$ and $p^6$ are filled with eight electrons, making the atom like a noble gas.

In order to accomplish this atoms release or take on electrons to fill these shells.

For example Calcium ( $1s^2 2s^2 2p^6 3s^2$ ) will readily lose the $3s^2$ electrons and becomes a $Ca^+2$ cation.
Fluorine ( $1s^2 2s^2 2p^5$ ) will readily take on an electron to fill $2p^6$ and become a $F^(-)$ anion.

In becoming ions the atoms fulfill the rule of octet.

Now as ions the $Ca^(+2)$ cation and the $F^(-)$ anion, have an electric attraction of opposites to become a $CaF_2$ ionic compound.

I hope this was helpful.
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Question #67e72

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