What type of hybridization occurs in the carbon atom of ethylene (C2H4)?

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Q: What type of hybridization occurs in the carbon atom of ethylene (C2H4)?

Solution: The carbon atoms in ethylene undergo sp2 hybridization, resulting in a planar structure.

Steps: 8

Step 1: Identify the molecular formula of ethylene, which is C2H4. This means there are 2 carbon atoms and 4 hydrogen atoms.
Step 2: Understand that each carbon atom in ethylene forms bonds with other atoms. Each carbon atom needs to form 4 bonds to satisfy the tetravalency of carbon.
Step 3: Determine the type of bonds in ethylene. Each carbon atom forms 2 single bonds with hydrogen atoms and 1 double bond with the other carbon atom.
Step 4: Recognize that a double bond consists of one sigma bond and one pi bond. The sigma bond is formed by the overlap of hybrid orbitals, while the pi bond is formed by the overlap of unhybridized p orbitals.
Step 5: Conclude that to form 3 sigma bonds (2 with hydrogen and 1 with another carbon), the carbon atoms must undergo hybridization.
Step 6: Identify the type of hybridization. In ethylene, each carbon atom uses one s orbital and two p orbitals to form three sp2 hybrid orbitals.
Step 7: Note that the remaining unhybridized p orbital is used to form the pi bond in the double bond between the carbon atoms.
Step 8: Conclude that the carbon atoms in ethylene are sp2 hybridized, which results in a planar structure.