Bond dissociation energy of `F_2` is less than `Cl_2`.

Explain why Bond dissociation energy of F_2 is less than that of Cl_2 ?

Account for the following : Bond energy of F_2 is less than Cl_2 .

What is dissociation energy?

F_2 has lower bond dissociation enthalpy than Cl_2 . Why?

Ozone in the upper atmoshphere absorbs ultraviolet radiation which induces the following chemical reaction O_(3)(g)rightarrowO_(2)(g)+O(g) O_(2) produced in the above photochemical dissociation undergoes further dissociation into one normal oxygen atom (O) and more energetic oxygen atom O** . O_(2)(g) rightarrowO+O** (O**) has 1 eV more energy than(O) and normal dissociation energy of O_(2) is 480 kJ "mol"^(-1) . [1 eV/Photon =96 kJ "mol"^(-1) ] What is the maximum wavelength effective for the photochemical dissociation of O_(2) molecule

The negative electron gain enthalpy of F is less/more than Cl.

Ozone in the upper atmoshphere absorbs ultraviolet radiation which induces the following chemical reaction O_(3)(g)rightarrowO_(2)(g)+O(g) O_(2) produced in the above photochemical dissociation undergoes further dissociation into one normal oxygen atom (O) and more energetic oxygen atom O** . O_(2)(g) rightarrowO+O** (O**) has 1 eV more energy than(O) and normal dissociation energy of O_(2) is 480 kJ "mol"^(-1) . [1 eV/Photon =96 kJ "mol"^(-1) ] If dissociation of O_(3) into O_(2) and O requires 400kJ mol^(-1) and O_(2) produced in this reaction is further dissociated to O and O** then the total energy required to for the dissociation of O_(3) into O and O** is :

Give reasons for the following: Bond enthalpy of F_2 is lower than that of Cl_2 .