The charge/size ratio of a cation determines its polarizing power. Which one of the following sequences represents the increasing order of the polarizing power of the cationic species, 

$K^{+}, C{a}^{+2}, M{g}^{+2}, B{e}^{+2}$

(1) $B{e}^{+2}<K^{+}<C{a}^{+2}<M{g}^{+2}$                     

(2) $K^{+}<C{a}^{+2}<M{g}^{+2}<B{e}^{+2}$

(3) $C{a}^{+2}<M{g}^{+2}<B{e}^{+2}<K^{+}$                     

(4) $M{g}^{+2}<B{e}^{+2}<K^{+}<C{a}^{+2}$

 

The molecule having the smallest bond angle is-

Which of the following statement is true for $I{O}_2{F_2}^{-}$according to VSEPR theory?

(A) The lone pair and two I-O double bonds occupy the equatorial positions of trigonal
bipyramid.

(B) It has $s{p}^3$ hybridization and is T-shaped.

(C)  Its structure is analogous to $S{F}_4$.

(D) (A) and (C) both

No S-S bonds are present in?

1. \(S_{2}O_{3}^{2-}\)                                           

2. \(S_{2}O_{4}^{2-}\)

3. \(S_{2}O_{5}^{2-}\)                                                

4. \(S_{2}O_{7}^{2-}\)

A diatomic molecule has a dipole moment of 1.2 D. If its bond length is equal to 10 ^-10 m , then the fraction of an electronic charge on each atom will be:

1. 42%
2. 52%
3. 37%
4. 25%

Most covalent compound among the following is :

The correct order of covalent bond character among
LiCl, BeCl₂, BCl₃ and CCl₄, is:

1. LiCl < BeCl₂ > BCl₃ > CCl₄

2. LiCl > BeCl₂ < BCl₃ < CCl₄

3. LiCl < BeCl₂ < BCl₃ < CCl₄

4. LiCl > BeCl₂ > BCl₃ > CCl₄

Which of the following conversions demonstrates an increase in bond order and a change in magnetic behaviour?

1. $NO\to N{O}^{+}$                                 

2. $O_2\to O_2+$

3. $N_2\to N_2^{+}$                                   

4. $C_2\to C_2^{+}$

The ionisation energy will be maximum for the process:

(a) $Ba\to B{a}^{2+}$

(b) $Be\to B{e}^{2+}$

(c) $Cs\to C{s}^{+}$

(d) $Li\to L{i}^{+}$

$N{F}_3$ is:

(1) non-polar compound 

(2) electrovalent compound 

(3) having low value of dipole moment than $N{H}_3$

(4) having more dipole moment than $N{H}_3$