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

1.	Boron trifluoride, hydrogen fluoride,  carbon dioxide, 1 3-dichlorobenzene
2.	Nitrogen trifluoride, beryllium difluoride,  water, 1 3 -dichlorobenzene
3.	Boron trifluoride, beryllium difluoride, carbon dioxide, 1 4-dichlorobenzene
4.	Ammonia, beryllium difluoride, water,  1, 4-dichlorobenzene

Match the following:

Which of the following is the correct option? 

A molecule that cannot exist is-

1. ${\mathrm{Li}}_2$

2. ${\mathrm{C}}_2$

3. ${\mathrm{O}}_2$

4. ${\mathrm{He}}_2$

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:

The species having pyramidal shape is:

(1) $S{O}_3$

(2) $Br{F}_3$

(3) $Si{O}_3^{2-}$

(4) OSF₂