Question

Arrange the following as stated:
(a) N2, O2, F2, Cl2 (Increasing order of bond dissociation energy).
Mention the appropriate reason

Answer 1

F2>Cl2>O2>NO2

Here bond length is increases if there is a single bond that its easy to break it double bond its hard as compared to first and triple its more hard.

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Answer 2

Increasing order of bond dissociation energy is as follows.

      $F_{2}$ < $Cl_{2}$ < $O_{2}$ < $N_{2}$

Explanation:

Bond dissociation energy is defined as strength of a chemical bond formed between two atoms. More is the number of bonds present between the two atoms more will be the heat energy required by it.

For example, $N_{2}$ has triple bonds so it will require high heat. $O_{2}$ has a double bond between the two oxygen atoms.

$F_{2}$ has smaller size as compared to $Cl_{2}$ atom. Therefore, there will be more repulsion between the electrons of fluorine gas due to its smaller size. Hence, its bond dissociation energy will be less than the bond dissociation energy of chlorine gas.

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