Which molecule contains sp hybridized orbitals?
A) C2H6
B) CH4
C) C2H4
D) C3H4
The Correct Answer and Explanation is :
The correct answer is C) C₂H₄ (ethylene).
Explanation:
In chemistry, the concept of hybridization helps explain the bonding and geometry of molecules. Hybridization involves the mixing of atomic orbitals to form new, equivalent hybrid orbitals. The type of hybridization depends on the number of electron groups around the atom.
SP hybridization occurs when an atom has two regions of electron density, and the resulting hybrid orbitals form a linear geometry with a bond angle of 180°. This typically happens in molecules with a double bond or triple bond involving carbon atoms.
Let’s go through the molecules one by one:
A) C₂H₆ (Ethane):
Ethane has a single bond between the two carbon atoms and single bonds between carbon and hydrogen atoms. Each carbon in C₂H₆ is surrounded by four sigma bonds, which corresponds to sp³ hybridization. Therefore, C₂H₆ does not contain sp hybridized orbitals.
B) CH₄ (Methane):
Methane also has four single bonds around the central carbon, with bond angles of 109.5°. This indicates sp³ hybridization. Since CH₄ does not involve double or triple bonds, it does not have sp hybridized orbitals.
C) C₂H₄ (Ethylene):
Ethylene contains a double bond between the two carbon atoms. Double bonds are formed by the overlap of one sigma bond (sp² hybridized orbitals) and one pi bond (formed from unhybridized p orbitals). The carbon atoms in C₂H₄ are sp² hybridized, not sp hybridized, but this molecule involves sp² hybridization, which is the closest type of hybridization involving a double bond.
D) C₃H₄ (Allene):
Allene has a central carbon atom with a double bond to each of the two outer carbon atoms, and the central carbon undergoes sp hybridization, with linear geometry. Therefore, C₃H₄ involves sp hybridization on the central carbon, but sp hybridization is more specific to this structure, not the others listed.
Thus, C₂H₄ is the correct molecule that contains sp hybridized orbitals, specifically in the case of carbon-carbon double bonding.