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The H-H bond dissociation enthalpy of H2...

The H-H bond dissociation enthalpy of `H_2` is _________, is the highest for a single bond between two atoms of any elements.

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To answer the question regarding the H-H bond dissociation enthalpy of \( H_2 \), we can follow these steps: ### Step 1: Understand Bond Dissociation Enthalpy Bond dissociation enthalpy is the energy required to break a bond in a molecule. For \( H_2 \), this refers to the energy needed to separate the two hydrogen atoms. ### Step 2: Recognize the Stability of \( H_2 \) The \( H_2 \) molecule is very stable due to the strong bond between the two hydrogen atoms. This stability is a result of the high bond dissociation enthalpy. ### Step 3: Compare with Other Elements The bond dissociation enthalpy of \( H_2 \) is higher than that of any other single bond between two atoms of different elements. This means that the bond between hydrogen atoms is stronger than the bonds found in other diatomic molecules like \( O_2 \) or \( N_2 \). ### Step 4: Conclude the Value The bond dissociation enthalpy for \( H_2 \) is approximately 436 kJ/mol. This value indicates that a significant amount of energy is required to break the bond between the two hydrogen atoms. ### Final Answer The H-H bond dissociation enthalpy of \( H_2 \) is **436 kJ/mol**, which is the highest for a single bond between two atoms of any element. ---
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