Q. 124.3( 44 Votes )
Consider the foll
A. In the given examples of isoelectronic species have a same number of electrons which is equal to 10. Hence, the given species are isoelectronic, i.e.
N3- has 7+3 = 10 electrons
O2- has 8+2 = 10 electrons
F- has 9+1 = 10 electrons
Na+ has 11-1 = 10 electrons
Mg2+ has 12-2 = 10 electrons
AL3+ has 13-3 = 10 electrons
B. As the magnitude of the effective nuclear decreases, the ionic radii of the ions increase.
The following arrangement denotes the elements arranged in the order of increasing nuclear charge:
N3- < O2- < F- < Na+ < Mg2+ < AL3+
Nuclear charge = +7 +8 +9 +11 +12 +13
The following arrangement denotes the elements arranged in the order of increasing ionic radii:
AL3+ < Mg2+ < Na+ < F- < O2- < N3-
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