22. Consider the isoelectronic species, Na+, Mg2+, F-and 02. The
correct order of increasing length of their radii is
(0) F< 02 < Mg2+ <Na
(ii) Mg2+< Na*< F-< 02-
(iii) 02-< F-< Na < Mg2+
(iv) 02-< F- < Mg2+< Na-
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Answer:
For isoelectronic species, ionic radii decrease with an increase in nuclear charge (i.e., no. of protons). Thus, for isoelectronic species, the cation with the greater +ve charge will have a smaller radius and the anion with greater -ve charge will have a larger radius.
Thus, the correct order of increasing ionic radii is Mg
2+
< Na
+
<F
−
< O
2−
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