Using the following data estimate the bond dissociation energy (BDE) of H-Cl: BDE (Cl-Cl)= 242kJ/ mol;BDE (H-H)= 434 kJ/mol; χp (Cl)= 3.2 and χp (H)=2.2 (1.0 eV = 96.5kJ/mol)
Question
Using the following data estimate the bond dissociation energy (BDE) of H-Cl: BDE (Cl-Cl)= 242kJ/ mol;BDE (H-H)= 434 kJ/mol; χp (Cl)= 3.2 and χp (H)=2.2 (1.0 eV = 96.5kJ/mol)
Solution
To estimate the bond dissociation energy (BDE) of H-Cl, we can use the concept of electronegativity and the given data.
The BDE of a heteronuclear diatomic molecule like H-Cl can be estimated using the following equation:
BDE (A-B) = 1/2 [BDE (A-A) + BDE (B-B)] - 0.1 (χp (A) - χp (B))^2
where:
- BDE (A-B) is the bond dissociation energy of the A-B bond
- BDE (A-A) and BDE (B-B) are the bond dissociation energies of the A-A and B-B bonds, respectively
- χp (A) and χp (B) are the Pauling electronegativities of atoms A and B, respectively
Substituting the given values into the equation:
BDE (H-Cl) = 1/2 [BDE (H-H) + BDE (Cl-Cl)] - 0.1 (χp (H) - χp (Cl))^2 = 1/2 [434 kJ/mol + 242 kJ/mol] - 0.1 (2.2 - 3.2)^2 = 1/2 [676 kJ/mol] - 0.1 (1.0)^2 = 338 kJ/mol - 0.1 * 1.0 = 338 kJ/mol - 0.1 kJ/mol = 337.9 kJ/mol
So, the estimated bond dissociation energy of H-Cl is approximately 337.9 kJ/mol.
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