Some of the given species (ions) has the same number of electrons Hence, the given species are isoelectronic, i.e
O2- has 8+2= 10 electrons
F- has 9+1 = 10 electrons
Mg2+ has 12-2 = 10 electrons
Al3+ has 13-3= 10 electrons
Ca2+ has 20-2 = 18 electrons
K1+ has 19-1 = 18 electrons
Cl 1- has 17+1=18 electrons
S 2- has 16+2 = 18 electrons
C 4+ has 6-4 = 2 electrons
Among these C 4+ is smallest
Then comes ions having 10 electrons .
Their order is
The ionic radii of isoelectronic species increases with a decrease in the magnitudes of nuclear charge.
The arrangement of the given species in order of their increasing nuclear charge is as follows:
O2– < F– < Mg2+ < Al3+
Nuclear charge = +8, +9 ,+12 ,+13
Therefore, the arrangement of the given species in order of their increasing ionic radii is as follows:
Al3+ < Mg2+ < F– < O2–
Then comes the ions with 18 number of electrons
Their order is
The ionic radii of isoelectronic species increases with a decrease in the magnitudes of nuclear charge.
The arrangement of the given species in order of their increasing nuclear charge is as follows:
S 2– < Cl– < K+ < Ca 2+
Nuclear charge = +10,+11, +13,+14
Therefore, the arrangement of the given species in order of their increasing ionic radii is as follows:
Ca2+ < K+ < Cl - < S2–
So over all increasing order of ionic radii is
C4+<Al3+<Mg2+<F-<O2-<Ca2+<K+<Cl-<S2-<