The drawing below shows the overlap of two hybrid orbitals to form a bond in a hydrocarbon. (b) Which of the following could be the identity of the hydrocarbon: (i) CH4, (ii) C2H6, (iii) C2H4, or (iv) C2H2?

Verified step by step guidance

1. Identify the type of hybrid orbitals shown in the diagram. The diagram shows the overlap of two sp hybrid orbitals.
2. Recall the types of bonds formed by different hybridizations: sp hybridization forms a triple bond or a single bond with two lone pairs, sp2 hybridization forms a double bond, and sp3 hybridization forms a single bond.
3. Determine the type of hydrocarbon that can have sp hybridization. Hydrocarbons with sp hybridization include those with triple bonds, such as acetylene (C2H2).
4. Analyze the given options: (i) CH4 (sp3 hybridization), (ii) C2H6 (sp3 hybridization), (iii) C2H4 (sp2 hybridization), and (iv) C2H2 (sp hybridization).
5. Conclude that the hydrocarbon with sp hybridization, which matches the diagram, is C2H2.

Key Concepts

Hybridization

Hybridization is the process of combining atomic orbitals to form new hybrid orbitals that can accommodate bonding. In hydrocarbons, carbon typically undergoes sp3, sp2, or sp hybridization, depending on the number of bonds it forms. This concept is crucial for understanding the geometry and bonding characteristics of molecules.

Types of Hydrocarbons

Hydrocarbons are organic compounds consisting solely of carbon and hydrogen. They can be classified into alkanes (single bonds), alkenes (at least one double bond), and alkynes (at least one triple bond). Identifying the type of hydrocarbon is essential for determining its structure and reactivity, which is relevant to the question.

Bond Formation

Bond formation occurs when atomic orbitals overlap to create a stable connection between atoms. The image depicts the overlap of hybrid orbitals, indicating the formation of a sigma bond. Understanding how bonds form helps in predicting the molecular structure and properties of the hydrocarbon in question.