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Arrange the ions Na^(+), O^(2-) and F^(-...

Arrange the ions `Na^(+), O^(2-) and F^(-)` in the decreasing order of their ionic radius.

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`{:(,O^(2-)gt,F^(-)gt,Na^(+)),("Number of electrons",10,10,10),("Number of protons",8,9,11):}`
All the ions contain same number of electrons. Due to the presence of greatest number of protons in `Na^(+)` its effective nuclear charge `(Z_("eff.))` is highest and, therefore, its radius is smallest. `O^(2-)` contains smallest number of protons. Its effective nuclear charge is lowest and therefore, its ionic radius is largest. Greater is the ratio of Z/e, smaller is the radius of the ion. Z= number of protons, e=number of electrons
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