What is the hybridization of the central atom in methane (CH4)?

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Multiple Choice

What is the hybridization of the central atom in methane (CH4)?

Explanation:
Four equivalent C–H bonds around the carbon in CH4 require four identical hybrid orbitals. That happens with sp3 hybridization, where one 2s and three 2p orbitals mix to form four degenerate sp3 hybrids. Each of these hybrids overlaps with a hydrogen 1s orbital to create a sigma bond, giving a tetrahedral arrangement with bond angles around 109.5°. D-orbital participation isn’t needed here, and using sp or sp2 would yield linear or trigonal planar geometries, which don’t match methane. So the central carbon is sp3 hybridized.

Four equivalent C–H bonds around the carbon in CH4 require four identical hybrid orbitals. That happens with sp3 hybridization, where one 2s and three 2p orbitals mix to form four degenerate sp3 hybrids. Each of these hybrids overlaps with a hydrogen 1s orbital to create a sigma bond, giving a tetrahedral arrangement with bond angles around 109.5°. D-orbital participation isn’t needed here, and using sp or sp2 would yield linear or trigonal planar geometries, which don’t match methane. So the central carbon is sp3 hybridized.

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