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
Arrange the following elements in increasing order of their atomic radius: $Na$,$K$,$Mg$,$Rb$.
Medium
View SolutionThe correct order of atomic radii of $B, Be, N$ and $C$ is
Identify the correct orders regarding atomic radii:
$i$. $Cl > F > Li$
$ii$. $P > C > N$
$iii$. $Tm > Sm > Eu$
$iv$. $Sr > Ca > Mg$
$i$. $Cl > F > Li$
$ii$. $P > C > N$
$iii$. $Tm > Sm > Eu$
$iv$. $Sr > Ca > Mg$
The size of the species $Pb$,$Pb^{2+}$,and $Pb^{4+}$ decreases as:
Difficult
View SolutionIn $Cl_2$, the van der Waals radius is $180 \ pm$. What is the distance between the two atoms (in $pm$)?
Easy
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