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
Identify the element having the smallest atomic radius from the following:
Assertion $(A)$: The ionic radii of $Na^{+}$ and $F^{-}$ are same.
Reason $(R)$: Both $Na^{+}$ and $F^{-}$ are isoelectronic species.
The correct answer is:
Reason $(R)$: Both $Na^{+}$ and $F^{-}$ are isoelectronic species.
The correct answer is:
Which ion has the largest radius?
Medium
View SolutionExplain why cations are smaller and anions larger in radii than their parent atoms.
Medium
View SolutionThe correct order of increasing atomic radius of the following elements is
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