The drawing below shows the overlap of two hybrid orbitals to form a bond in a hydrocarbon. (a) Which of the following types of bonds is being formed: (i) C¬C s, (ii) C¬C p, or (iii) C¬H s?

Verified step by step guidance

1. Identify the types of hybrid orbitals involved in the bond formation.
2. Determine the type of bond formed based on the overlap of these hybrid orbitals.
3. Recall that sigma (\(\sigma\)) bonds are formed by the end-to-end overlap of orbitals, while pi (\(\pi\)) bonds are formed by the side-to-side overlap.
4. Consider the context of hydrocarbons, where carbon typically forms \(\sigma\) bonds with hydrogen and other carbon atoms.
5. Conclude which type of bond is formed based on the overlap and the elements involved, choosing from C-C \(\sigma\), C-C \(\pi\), or C-H \(\sigma\).

Key Concepts

Hybridization

Hybridization is the process by which atomic orbitals mix to form new hybrid orbitals that are suitable for the pairing of electrons to form chemical bonds. In hydrocarbons, carbon typically undergoes sp3, sp2, or sp hybridization, depending on its bonding environment, which influences the geometry and type of bonds formed.

Types of Bonds

In chemistry, bonds can be classified as sigma (σ) or pi (π) bonds. Sigma bonds are formed by the head-on overlap of orbitals, allowing for free rotation, while pi bonds result from the side-to-side overlap of p orbitals, restricting rotation. Understanding these bond types is crucial for analyzing molecular structure and reactivity.

Bonding in Hydrocarbons

Hydrocarbons are organic compounds consisting solely of carbon and hydrogen. The bonding in hydrocarbons involves carbon atoms forming bonds with each other and with hydrogen atoms. The type of bond formed (σ or π) depends on the hybridization of the carbon atoms and the specific arrangement of their orbitals, which is essential for determining the properties of the hydrocarbon.