Isoelectronic Species

Q.

The ionic radius of ${\mathrm{Na}}^{+}$ ion is $1.02\stackrel{\circ }{\mathrm{A}}$. The ionic radii (in $\stackrel{\circ }{\mathrm{A}}$) of ${\mathrm{Mg}}^{2+}$ and ${\mathrm{Al}}^{3+}$, respectively are:

1. $0.72\mathrm{and}0.54$

2. $0.68\mathrm{and}0.72$

3. $1.05\mathrm{and}0.99$

4. $0.85\mathrm{and}0.99$

Q.

Consider the following species: $N^{3–},O^{2–},F^{–},N{a}^{+},M{g}^{2+}andA{l}^{3+}$
(a)What is common in them?
(b)Arrange them in the order of increasing ionic radii.

Q. Amongst \(SF_4, ~ XeF_4, ~CF_4 ~\text{and}~ H_2O\), the number of species with two lone pair of electrons is _______

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.

What do you understand by isoelectronic species? Name a species that will be isoelectronic with each of the following atoms or ions.
(i) $F^{–}$

(ii) Ar

(iii) $M{g}^{2+}$

(iv)$R{b}^{+}$

Q. Which of these isoelectronic species has the smallest radius?

1. $B{r}^{-}$
2. $S{r}^{2+}$
3. $R{b}^{+}$
4. $S{e}^{2-}$

Q. Which one of the following sets of ions represents a collection of isoelectronic species?

1. $K^{+},C{l}^{-},C{a}^{2+},S{c}^{3+}$
2. $B{a}^{2+},S{r}^{2+},K^{+},S^{2-}$
3. $N^{3-},O^{2-},F^{-},S^{2-}$
4. $L{i}^{+},N{a}^{+},M{g}^{2+},C{a}^{2+}$

Q.

Which elements are non-reactive? Explain in terms of their electronic configuration?

Q.

Correct order of ionisation potentials of B, C, Al, Si is:

1. B < Al < Si < C

2. B < Si < Al < C

3. Al < B < Si < C

4. Al < Si < B < C

Q.

Give one word or a phrase for the following statement: The energy released when an electron is added to a neutral gaseous isolated atom to form a negatively charged ion.

Q.

Which of the following sets contain only isoelectronic ions?
(i) $Z{n}^{2+},C{a}^{2+},G{a}^{3+},A{l}^{3+}$

(ii) $K^{+},C{a}^{2+},S{c}^{3+},C{l}^{-}$

(iii) $P^{3-},S^{2-},C{l}^{-},K^{+}$

(iv) $T{i}^{4+},Ar,C{r}^{3+},v^{5+}$

Q.

The species with a radius less than of Ne is

a)Mg2+

b)F-

c)O2-

d)K+

Q.

Arrange the following species in the increasing order of their ionic radii giving reasons. ${\mathrm{Mg}}^{2+},{\mathrm{Al}}^{3+},{\mathrm{O}}^{2-},{\mathrm{Na}}^{+},{\mathrm{N}}^{3-},{\mathrm{F}}^{-}$.

Q. Q. Arrange the following species in the increasing order of their Ionic radius ( with reasons ) :
C^4+, S^2-, Cl^1-, K^1+, Ca^2+, Al^3+, Mg^2+, O^2-, F^1-

Q.

Question 20

In which of the following pairs, the ions are isoelectronic ?

(a) $N{a}^{+},M{g}^{2+}$ (b) $A{l}^{3+},O^{-}$ (c) $N{a}^{+},O^{2-}$ (d) $N^{3-},C{l}^{-}$

Q.

When does the nucleus of an atom tend to be radioactive?

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. Which of the following species is isoelectronic with $C{O}_2$?

1. $N_3^{-}$
2. $(CNO{)}^{-}$
3. $(NCN{)}^{2-}$
4. All of these

Q. $O^{2-}$ and $S{i}^{4+}$ are isoelectronic ions. If the ionic radius of $O^{2-}$ is $1.4\stackrel{\circ }{A}$, that of $S{i}^{4+}$ is

1. 
2. 
3. 
4. 

Q. Find the total number of species having bent shape.
$I_3^{-},N{O}_2^{+},H_{2}S,OC{l}_2,Xe{F}_2,S{O}_2,NOCl$

Q.

Why are nonmetals electronegative in nature?

Q.

Which of the following is not an isoelectronic species?

1. 

2. 

3. 

4. 

Q.

Chlorine has ______ electron affinity than fluorine.

Q. Predict the number of unpaired electrons in a square planar d8 ion. (Explain in detail to clear concept)

Q.

Statement - I: $C{l}^{-}andC{a}^{2+}$ are isoelectronic species.
Statement - II: Isoelectronic species should have same charges.

1. Statement - I is true; Statement - II is true; Statement - II is correct explanation for Statement - I

2. Statement - I is true; Statement - II is true; Statement - II is NOT the correct explanation for Statement - I

3. Statement - I is true; Statement - II is false

4. Statement - I is false; Statement - II is true

Q.

Consider the following species:

N^3–, O^2–, F^–, Na⁺, Mg²⁺ and Al³⁺

(a) What is common in them?

(b) Arrange them in the order of increasing ionic radii.

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. The ions $O^{2-},F^{-},N{a}^{+},M{g}^{2+}\text{and}A{l}^{3+}$ 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.

The size of isoelectronic species $F^{\ominus }$, $Ne$ and $N{a}^{\oplus }$ is affected by

1. Nuclear charge (Z)

2. Valence principal quantum number(n)

3. Electron-electron interaction in the outer orbitals

4. None