Which of the following sets of ions represents a group of isoelectronic species?
- A$Na^{+}, Mg^{2+}, Al^{3+}, Cl^{-}$
- B$Na^{+}, Ca^{2+}, Sc^{3+}, F^{-}$
- C$K^{+}, Cl^{-}, Mg^{2+}, Sc^{3+}$
- D$K^{+}, Ca^{2+}, Sc^{3+}, Cl^{-}$
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Similar Questions
Observe the following data. Ion Radius $(pm)$ $Q^{a+}$ $53$ $X^{b+}$ $66$ $Y^{c+}$ $40$ $Z^{d+}$ $100$
$Q^{a+}, X^{b+}, Y^{c+}, Z^{d+}$ are respectively
| Ion | Radius $(pm)$ |
|---|---|
| $Q^{a+}$ | $53$ |
| $X^{b+}$ | $66$ |
| $Y^{c+}$ | $40$ |
| $Z^{d+}$ | $100$ |
Which of the following represents the incorrect order of ionic or atomic radii?
Easy
View SolutionWhich of the following is the correct increasing order of ionic radii for $N^{3-}$,$Na^+$,$F^-$,$O^{2-}$,and $Mg^{2+}$?
Easy
View SolutionThe correct order of ionic radii for the given species is:
Among the elements $Li$,$N$,$C$ and $Be$,the one with the largest atomic radius is
MediumKVPY 2016
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