Concept:Bond length is the internuclear distance between two bonded atoms. It is physically determined by orbital size, bond order, and electrostatic polarity.
Formula:$$ \text{Bond Length} \propto \text{Radius} + \text{Radius} - \text{Polarity corrections} $$
Solution:- Multiple bonds: Increase bond order, pulling atoms closer (decreases length).
- Hybridization: More s-character (e.g., sp vs sp3) makes orbitals smaller, decreasing bond length.
- Electronegativity diff: Creates partial charges causing electrostatic attraction, shortening the bond (Schomaker-Stevenson rule).
- Ionization energy: While related to general atomic properties, it does not directly act as a mechanical factor altering the geometric distance of a formed covalent bond.
Why other options are incorrect:- Option A, Option B, Option C: These are the three primary, direct determinants of covalent bond length.
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