Assertion :Dihydrogen is inert at room temperature Reason: The $H - H$ bond dissociation enthalpy is the highest for a single bond between two atoms of an element

Both Assertion and Reason are correct and Reason is the correct explanation for Assertion

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Solution

The correct option is A Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
Dihydrogen is inert at room temperature.
This can be attributed to the highest $H - H$ bond dissociation enthalpy for a single bond between two atoms of any element. The strength of a chemical bond is measured by bond-dissociation enthalpy.
It is the standard enthalpy change accompanying the cleavage by homolysis of a bond. The higher the bond dissociation enthalpy, the higher will be the strength of the chemical bond.
The bond enthalpy of $H - H$ bond is due to the small size and high electronegativity of a hydrogen atom.
Due to highest bond dissociation enthalpy, the cleavage of bond does not take place at room temperature & the $H_{2}$ becomes inert.

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