Unhybrid "p" orbitals on linear overlap:
Correct answer: A. Always form Pi(π) bond
- A. Always form Pi(π) bond
- B. Always form Sigma(a) bond
- C. Neither form "a" nor "π" bond
- D. Form more reactive and more unstable "π" bond
Explanation
Unhybridized orbitals can only form π bonds upon sideways or parallel overlap and cannot form sigma bonds.
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Chemical bonding explains molecular shape through VSEPR theory and distinguishes sigma bonds from pi bonds. Questions involve hybridization, bond angles, dipole moment and bond energy, including how electron-pair repulsion determines geometry and how bond polarity differs from the overall polarity of a molecule.
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