The set of isomers of ${\mathrm{C}}_6{\mathrm{H}}_4{\mathrm{Cl}}_2$ that have an equal dipole moment with ${\mathrm{C}}_6{\mathrm{H}}_5\mathrm{Cl}$ & C₆H₆ respectively is : 

1.	Ortho and Meta	2.	Meta and Para
3.	Ortho and Para	4.	Para and Ortho

Which of the following set of molecules will have zero dipole moment?

A molecule that cannot exist is:

Isoelectronic species among the following is/ are :

l. \(NH_{3}\)

ll. \(CH_{3}^{+}\)${{}^{}}_{\mathrm{}}$

lll. \(NH_{2}^{-}\)

lV. \(NH_{4}^{+}\)

Electron deficient species among the following is: 

1. ${\mathrm{PH}}_3$

2. ${\left(C{H}_3\right)}_2$

3. ${\mathrm{BH}}_3$

4. ${\mathrm{NH}}_3$

Xe F${}_2$ is isostructural with : 

1. ${\mathrm{SbCl}}_3$

2. ${\mathrm{BCl}}_3$

3. ${\mathrm{TeF}}_2$

4. ${\mathrm{ICl}}_2^{-}$

Non-Zero dipole moment is shown by : 

1. ${\mathrm{CO}}_2$

2. p-Dichlorobenzene

3. Carbontetrachloride

4. Water.

An incorrect statement regarding resonating structures is : 

An ion having  the shortest bond length among the following is -

1. $O_2^{+}$

2. $O_2^{-}$

3. $O_2^{2-}$

4. $O_2^{2+}$

Assuming that Hund's rule is violated, the bond order and magnetic nature of the diatomic molecule $B_2$ is: