Consider the following hydrocarbon:
d. Identify all the 120° bond angles in the molecule.

Verified step by step guidance

1. Identify the type of hydrocarbon given in the problem.
2. Recognize that 120° bond angles are characteristic of sp2 hybridized carbon atoms.
3. Determine which carbon atoms in the molecule are sp2 hybridized.
4. Look for carbon atoms that are part of double bonds or are in a trigonal planar geometry.
5. List all the bond angles around these sp2 hybridized carbon atoms that are 120°.

Key Concepts

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is determined by the number of bonding pairs and lone pairs of electrons around the central atom, which influences the angles between bonds. Understanding molecular geometry is crucial for predicting bond angles, such as the 120° angles typically found in trigonal planar structures.

VSEPR Theory

Valence Shell Electron Pair Repulsion (VSEPR) theory is a model used to predict the geometry of individual molecules based on the repulsion between electron pairs. According to VSEPR, electron pairs will arrange themselves to minimize repulsion, leading to specific bond angles. In hydrocarbons with trigonal planar geometry, the bond angles are approximately 120° due to the arrangement of three bonding pairs around a central atom.

Hybridization

Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate bonding. In the case of hydrocarbons with 120° bond angles, sp² hybridization occurs, where one s orbital and two p orbitals combine to form three equivalent sp² hybrid orbitals. This hybridization explains the planar structure and the specific bond angles observed in such molecules.