What is the predicted shape, bond angle, and hybridization for CH3+?
Correct answer: A. Trigonal planar, 120°, sp2
- A. Trigonal planar, 120°, sp2
- B. Trigonal planar, 120°, sp3
- C. Trigonal planar, 109.5°, sp2
- D. Trigonal pyramidal, 120°, sp2
Explanation
The correct answer is Option A: Trigonal planar, 120°, sp2. A carbocation like CH3+ has sp2 hybridization because the carbon atom is bonded to three hydrogen atoms and has a vacant p orbital. This hybridization results in a trigonal planar geometry with bond angles of 120°. Other options are incorrect because they either state incorrect hybridization, bond angles, or molecular shapes: sp3 hybridization would imply a tetrahedral shape, and incorrect bond angles (109.5°) do not match the trigonal planar shape.
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About Hybridization
Hybridization explains bonding by combining atomic orbitals to form equivalent hybrid orbitals with definite geometries. Coverage includes sp, sp², sp³, sp³d and sp³d² hybridization, their shapes and bond angles, and the relation of sigma and pi bonds to molecular structure.
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