The correct order of ionic radii for the give | vedclass

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Question

(B) The given species are $K^{+}$,$Na^{+}$,$Mg^{2+}$,and $Al^{3+}$.$K^{+}$ has electrons in the $n=3$ shell,while $Na^{+}$,$Mg^{2+}$,and $Al^{3+}$ hav

Vedclass · Accepted Answer

$K^{+} > Na^{+} > Mg^{2+} > Al^{3+}$

Vedclass · Answer

(B) The given species are $K^{+}$,$Na^{+}$,$Mg^{2+}$,and $Al^{3+}$.$K^{+}$ has electrons in the $n=3$ shell,while $Na^{+}$,$Mg^{2+}$,and $Al^{3+}$ have electrons in the $n=2$ shell.Therefore,$K^{+}$ has the largest ionic radius.For the isoelectronic species $Na^{+}$,$Mg^{2+}$,and $Al^{3+}$,the ionic radius decreases as the nuclear charge (atomic number) increases.The atomic numbers are $Na (11)$,$Mg (12)$,and $Al (13)$.Thus,the order of ionic radii for these is $Na^{+} > Mg^{2+} > Al^{3+}$.Combining these,the correct order is $K^{+} > Na^{+} > Mg^{2+} > Al^{3+}$.

The correct order of ionic radii for the given species is:

Similar Questions

Identify the wrong statement in the following.

Which of the following ions has the smallest radius?

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.

Which of the following species is the smallest in size?

For which of the following ionic species would the radius be maximum?

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