What is the hybridization state of the carbon atom in methane (${\mathrm{CH}}_4$)?

• A. ${\mathrm{sp}}^2$
• B. ${\mathrm{sp}}^1$
• C. ${\mathrm{sp}}^{3d}$
• D. ${\mathrm{sp}}^3$

Answer: (D)

Verified step by step guidance

1. Identify the central atom in methane (CH4), which is carbon.
2. Determine the number of sigma bonds formed by the carbon atom. In CH4, carbon forms four sigma bonds with four hydrogen atoms.
3. Recall that the hybridization state of an atom is determined by the number of sigma bonds and lone pairs around it. For carbon in CH4, there are four sigma bonds and no lone pairs.
4. Use the formula for hybridization: Hybridization = number of sigma bonds + number of lone pairs. For carbon in CH4, this is 4 + 0 = 4.
5. Recognize that a hybridization number of 4 corresponds to sp3 hybridization, which involves one s orbital and three p orbitals combining to form four equivalent sp3 hybrid orbitals.