Which resonance form is likely to contribute most to the correct structure of n2o?

Explanation:

- The atoms combine to form molecules and attain stability by completing their octet. The formation of compound can take place either by transfer of electron from one atom to other or by sharing of electrons between them.

- Resonance structure of a molecule is of two or more forms in which the distribution of electrons around the structure is different but the chemical connectivity is same.

- The total number of valence electrons VE in (N N O) is :

                                 VE = 2(5) + 6 = 16 electrons.

- Among the molecule, the electrons are distributed in atom in such a way that formation of triple bond will take place between two nitrogen atoms and a single bond will form between nitrogen and oxygen atom.

- The formal charge FC on each atom is determined as:

                                  FC = VE - NBE - BE/2

Where,

            NBE: Non-Bonding Electrons

            BE : Bonding Electrons.

- The formal charge on each atom is: the nitrogen atom in center will possess 1+ formal charge and oxygen will possess 1- charge (oxygen is electronegative atom). Thus, results in formation of neutral molecule.

- The structure of (N N O) is shown in attachment.

- The resonance form which is likely to contribute most to the correct structure of (N_2 O) is:

- Structure for (N N O)  showing one lone-pair of electrons on the terminal nitrogen atom, a triple bond between the two nitrogen atoms, a single bond between nitrogen and oxygen, and three lone-pairs of electrons on the terminal oxygen atom.

no simpler subs form complex ones. synthesise = make

i think its c if i'm wrong