Medium
Consider the following species: $N^{3-}, O^{2-}, F^{-}, Na^{+}, Mg^{2+}, Al^{3+}$
$(a)$ What is common in them?
$(b)$ Arrange them in the order of increasing ionic radii.
$(a)$ What is common in them?
$(b)$ Arrange them in the order of increasing ionic radii.
(N/A) All these ions have the same number $(10)$ of electrons. Therefore,these are called isoelectronic species.
$(b)$ Since the number of electrons is the same,the ionic size decreases with an increase in nuclear charge. Therefore,the ions can be arranged in increasing order of ionic radii as $Al^{3+} < Mg^{2+} < Na^{+} < F^{-} < O^{2-} < N^{3-}$.
$(b)$ Since the number of electrons is the same,the ionic size decreases with an increase in nuclear charge. Therefore,the ions can be arranged in increasing order of ionic radii as $Al^{3+} < Mg^{2+} < Na^{+} < F^{-} < O^{2-} < N^{3-}$.
Explore More
Similar Questions
For $Na^{+}$,$Mg^{2+}$,$F^{-}$,and $O^{2-}$; the correct order of increasing ionic radii is
$Na^{+}$,$Mg^{2+}$,$Al^{3+}$,and $Si^{4+}$ are isoelectronic. Their ionic size follows the order:
Choose the incorrect trend in the atomic radii $(r)$ of the elements $:$
Which ion has the largest radius from the following ions?
Medium
View SolutionThe ionic radii of $Li^{+}$,$Be^{2+}$,and $B^{3+}$ follow the order:
Medium
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo