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The size of isoelectronic species O^(-2)...

The size of isoelectronic species `O^(-2) F^(-)` and `Na^(+)` is affected by:

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`Mg^(2+) lt Na^(+) lt F^(-) lt O^(2-)`
This order can be justified on the basis of the fact that a negative anion is larger than its neutral atom due to a decrease in effective nuclear charge. As the valence electrons now experience weaker attractions from the nucleus, its size must be largest. On the contrary, a cation will have smaller size than its neutral atom due to an increase in effective nuclear charge. Higher the positive charge, smaller the cation.
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