Question

$ {{O}_{2}}N-{{N}_{2}}O $ is homolysis or heterolysis? What is the product?

Answer 1

Hint: In chemistry, homolysis is the chemical breakdown of a molecular link into fragments, each of which maintains one of the initially bound electrons. Two free radicals are produced during homolytic fission of a neutral molecule with an even number of electrons. The two electrons involved in the initial bond are allocated across the two fragment species in this way. Bond dissociation energy is the energy involved in this process (BDE). Bond cleavage can also be accomplished by a process known as heterolysis.

Complete answer:
The "enthalpy (per mole) necessary to break a given bond of some particular molecular entity by homolysis," represented as D, is defined as the "enthalpy (per mole) required to break a given bond of some specific molecular entity by homolysis." The Bond Dissociation Energy is governed by the bond's strength, which is determined by parameters pertaining to the radical species' stability.
Homolysis happens predominantly in the following conditions due to the comparatively large energy required to break bonds in this manner:
Luminous environment (i.e.Ultraviolet radiation).
Heat.
Consider $ {{N}_{2}}{{O}_{4}}(g)\to 2N{{O}_{2}}(g) $
 $ N{{O}_{2}} $ is a radical species, which means that it has a single unpaired electron on the nitrogen centre. $ N{{O}_{2}} $ must have 17 valence electrons to spread among its three atoms ( 26 – 4 + 5 ). The nitrogen atom has a single electron and is cationic, whereas one of the oxygen atoms has a negative charge. Of course, we may create a new resonance structure in which the negative charge is carried by the other oxygen: $ O={{N}^{+}}-{{O}^{-}} $
Each atom possesses 6, 4, and 7 valence electrons, and has a formal charge of 0, $ {{1}^{+}} $ , and $ {{1}^{-}} $ from left to right. a pair When the single electrons on the nitrogen centres combine to create a nitrogen-nitrogen bond, i.e. $ {{O}^{-}}(O=){{N}^{+}}-N{{O}_{2}} $ , $ N{{O}_{2}} $ molecules can dimerize. Of course, each nitrogen centre still has a formal positive charge. Of course, the dimer's nitrogen-nitrogen link can hemolysis, yielding 2 equivalence $ N{{O}_{2}} $ , which is the solution to the question.
Hence homolysis is the answer.

Note:
The capacity of a molecule to absorb energy from light or heat, as well as the bond dissociation energy, drive homolytic cleavage (enthalpy). The energy of the Singly Occupied Molecular Orbital will be reduced, as would the bond dissociation energy, if the radical species is better able to stabilise the free radical. Multiple variables, such as electronegativity and polarisability, influence bond dissociation energy.