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(D) Bond dissociation energy is inversely proportional to the bond length,which in turn depends on the atomic size of the bonded atoms.Smaller atoms f

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$D$

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(D) Bond dissociation energy is inversely proportional to the bond length,which in turn depends on the atomic size of the bonded atoms.Smaller atoms form shorter,stronger bonds,resulting in higher bond dissociation energy.Comparing the given values: $485 \ kJ \ mol^{-1} > 328 \ kJ \ mol^{-1} > 276 \ kJ \ mol^{-1} > 240 \ kJ \ mol^{-1}$.Since element $D$ has the highest bond dissociation energy $(485 \ kJ \ mol^{-1})$,it must have the smallest atomic size among the given elements.

$Bond$	$E_{diss} (kJ \ mol^{-1})$
$C-A$	$240$
$C-B$	$328$
$C-C$	$276$
$C-D$	$485$

The table shown below gives the bond dissociation energies $E_{diss}$ for single covalent bonds of carbon $C$ atoms with elements $A, B, C$ and $D.$ Which element has the smallest atoms?

$Bond$ $E_{diss} (kJ \ mol^{-1})$

$C-A$ $240$

$C-B$ $328$

$C-C$ $276$

$C-D$ $485$

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The table shown below gives the bond dissociation energies $E_{diss}$ for single covalent bonds of carbon $C$ atoms with elements $A, B, C$ and $D.$ Which element has the smallest atoms? $Bond$ $E_{diss} (kJ \ mol^{-1})$ $C-A$ $240$ $C-B$ $328$ $C-C$ $276$ $C-D$ $485$