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(D) The ionic radius depends on the effective nuclear charge and the number of shells.$(A)$ $Ti^{4+}$ $(Z=22)$ and $Mn^{7+}$ $(Z=25)$ are isoelectroni

Vedclass · Accepted Answer

$P^{3+} > P^{5+}$

Vedclass · Answer

(D) The ionic radius depends on the effective nuclear charge and the number of shells.$(A)$ $Ti^{4+}$ $(Z=22)$ and $Mn^{7+}$ $(Z=25)$ are isoelectronic ($18$ electrons). As nuclear charge increases,size decreases,so $Ti^{4+} > Mn^{7+}$.$(B)$ $^{35}Cl^{-}$ and $^{37}Cl^{-}$ are isotopes. Isotopes have the same number of electrons and protons,so their ionic radii are equal.$(C)$ $K^{+}$ and $Cl^{-}$ are isoelectronic ($18$ electrons). $K^{+}$ has a higher nuclear charge $(Z=19)$ than $Cl^{-}$ $(Z=17)$,so $K^{+} $(D)$ $P^{3+}$ and $P^{5+}$ are ions of the same element. $P^{5+}$ has lost more electrons than $P^{3+}$,resulting in a higher effective nuclear charge per electron,making $P^{3+} > P^{5+}$.Thus,the correct statement is $(D)$.

Which of the following represents the correct order of ionic radii?

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Assertion $(A)$: $Na^{+}$ and $Mg^{2+}$ ions are isoelectronic but the ionic radius of $Na^{+}$ is greater than that of $Mg^{2+}$.
Reason $(R)$: The effective nuclear charge of $Na^{+}$ ion is less than that of $Mg^{2+}$ ion.

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