When the molecules ${\mathrm{N}}_2,{\mathrm{O}}_2,{\mathrm{F}}_2$ are arranged in order of increasing bond strength, which order is correct?

Triple bonds connect the$\mathrm{N}$ atoms in ${\mathrm{N}}_2$. ${\mathrm{O}}_2$ contains two double-bonded $\mathrm{O}$ atoms. Single bonds connect the molecules of ${\mathrm{F}}_2$ and ${\mathrm{Cl}}_2$.
The bond energy will increase as the number of bonds between atoms increases. Because the atoms in ${\mathrm{F}}_2$ are closer together and exhibit stronger repulsion, ${\mathrm{Cl}}_2$ has a higher bond energy than ${\mathrm{F}}_2$.${\mathrm{F}}_2$ has a lower bond energy as a result.
∴ Bond enthalpies are as follows: $={\mathrm{N}}_2>{\mathrm{O}}_2>{\mathrm{F}}_2$
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