Isoelectronic Species

Q. The ions $O^{2-}$, $F^{-}$, $N{a}^{+}$, $M{g}^{2+}$ and $A{l}^{3+}$ are isoelectronic. Their ionic radii show:

1. An increase from $O^{2-}$ to $F^{-}$ and then a decrease from $N{a}^{+}$ to $A{l}^{3+}$
2. A decrease from $O^{2-}$ to $F^{-}$ and then an increase from $N{a}^{+}$ to $A{l}^{3+}$
3. A significant increase from $O^{2-}$ to $A{l}^{3+}$
4. A significant decrease from $O^{2-}$ to $A{l}^{3+}$

Q.

Which among the following are isoelectronic $N{O}_3^{-},C{O}_3^{2-},Cl{O}_3^{-},S{O}_2$

1. $N{O}_3^{-},C{O}_3^{2-},Cl{O}_3^{-}$

2. $N{O}_3^{-},C{O}_3^{2-},S{O}_2$

3. $C{O}_3^{2-},Cl{O}_3^{-},S{O}_2$

4. None of these

Q.

In the iso electronic species the ionic radii ($A^O$) of $N^{3-}$, $O^{-2}$, $F^{-}$ are respectively given by

1. 1.36, 1.40, 1.71

2. 1.36, 1.71, 1.40

3. 1.71, 1.40, 1.36

4. 1.71, 1.36, 1.40

Q. Which one of following species are isoelectronic? $S^{2-},N{a}^{+},C{a}^{2+},C{l}^{-}$

1. $S^{2-},N{a}^{+},C{a}^{2+},C{l}^{-}$
2. $N{a}^{+},C{a}^{2+},C{l}^{-}$
3. $S^{2-},N{a}^{+},C{l}^{-}$
4. $S^{2-},C{a}^{2+},C{l}^{-}$

Q.

The number of isoelectronic species among the following are:
$C{a}^{2+},Ar,C{l}^{-},K^{+},Kr,F^{-}$

1. $2$
2. $4$
3. $5$
4. $6$

Q. In iso-electronic species $O^{2-}$, $F^{-}$ and $N{a}^{+}$, size is affected by:

1. Nuclear charge (Z) of the element
2. Valence principal quantum number
3. Electron-electron interactions in the outer orbitals
4. None of the factors because their size is the same

Q. Which of the following pairs of compounds is isoelectric and isostructural?

1. $BeC{l}_2,Xe{F}_2$
2. $Te{I}_2,Xe{F}_2$
3. $IB{r}_2^{-},Xe{F}_2$
4. $I{F}_3,Xe{F}_2$

Q.

Ionic radii of

1. $T{i}^{4+}<M{n}^{7+}$

2. ${}^{35}C{l}^{-}<{}^{37}C{l}^{-}$

3. $K^{+}>C{I}^{-}$

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

Q.

Which one of the following is an example of a positive ion and negative ion that is isoelectronic with $F^{-}$?

1. $S^{2-}$ and $M{g}^{2+}$ or $N{a}^{+}$

2. $O^{2-}$ and $C{a}^{2+}$ or $K^{+}$

3. $O^{2-}$ and $M{g}^{2+}$ or $L{i}^{+}$

4. $O^{2-}$ and $M{g}^{2+}$ or $N{a}^{+}$

Q. Assertion: ${\text{Mg}}^{2+}$and ${\text{Al}}^{3+}$ are isoelectronic but ionic radius ${\text{Al}}^{3+}$ is less than that of ${\text{Mg}}^{2+}$.
Reason: The effective nuclear charge on the outer-shell electrons in ${\text{Al}}^{3+}$ is more than that in ${\text{Mg}}^{2+}$.

1. Both assertion and reason are true. Reason is the correct explanation of assertion.
2. Both assertion and reason are true. Reason is not the correct explanation of assertion.
3. Assertion is true. Reason is false.
4. Assertion is false. Reason is true.

Q. Which of the following compound is isoelectronic with
$[H_{3}N:B{H}_3]$ ?

1. $B_2{H}_6$
2. $C_2{H}_6$
3. $C_2{H}_4$
4. $C_3{H}_6$

Q. In iso-electronic species $O^{2-}$, $F^{-}$ and $N{a}^{+}$, size is affected by:

1. Nuclear charge (Z) of the element
2. Valence principal quantum number
3. Electron-electron interactions in the outer orbitals
4. None of the factors because their size is the same