Test: Covalent and Co-ordinate Bonding - JEE MCQ

In P = O bond, π - bond is formed by the sidewise overlapping of d - orbital of P and p - orbital of oxygen. Hence, it is formed by pπ and dπ overlapping.
In nitrogen and carbon, no vacant d-orbital is present. So, they do not form pπ − dπ bond.

The delocalised pπ − pπ bonding between filled p -orbital of F and vacant p -orbital of B leads to shortening of B−F bond length which results in higher bond dissociation energy of the B-F bond.

In ion, formal charge on each -atom of
bond

NH₄Cl contains both covalent and ionic

According to the question, radical is an exception case to the octet rule which occurs when there is an odd number of electrons in an atom.
In case of nitrogen oxide, it has  Odd electrons (seven valency electrons of nitrogen and eight valency electrons of oxygen), so this species work as radical. 
In case of , the total electrons are  (even), in case of nitro ion, total valency electrons are  (even), In case of cyanide ion, total valency electrons are  (even).

The increasing order is

Due to resonance in O₃, the O − O bond length will be in between O = O and O − O

The shape of BF₃ is trigonal planar

and hence it is non polar.
The shape of is pyramidal

and hence it is polar.

The structure of is
i.e, one and two bonds

In bond will have ionic character due to electron attracting tendency of P-carrying positive charge and least covalent.

The average distance between the centre of nuclei of the two bonded atoms in a molecule is known as bond length. It depends upon the size of atoms, hybridisation, steric effect, resonance etc.
Usually bond length of polar bond is smaller as compared to a non-polar bond. Therefore, C − C bond length is longest among given options.