(a) Boron trichloride 1BCl32 and the carbonate ion 1CO3 2- 2 are both described as trigonal. What does this indicate about their bond angles?

Key Concepts

Trigonal Geometry

Trigonal geometry refers to a molecular shape where a central atom is bonded to three other atoms, forming a planar structure. This arrangement typically results in bond angles of approximately 120 degrees, as seen in molecules like boron trichloride (BCl3) and the carbonate ion (CO3^2-). The trigonal shape arises from the repulsion between electron pairs around the central atom, which seeks to maximize distance between them.

Bond Angles

Bond angles are the angles formed between two adjacent bonds at a central atom. In trigonal planar molecules, the ideal bond angle is 120 degrees due to the symmetrical arrangement of the bonded atoms around the central atom. Variations in bond angles can occur due to factors such as lone pairs of electrons or differences in electronegativity among the bonded atoms, which can distort the ideal geometry.

VSEPR Theory

Valence Shell Electron Pair Repulsion (VSEPR) theory is a model used to predict the geometry of molecules based on the repulsion between electron pairs surrounding a central atom. According to VSEPR, electron pairs, whether bonding or non-bonding, will arrange themselves to minimize repulsion, leading to specific molecular shapes, such as trigonal planar for BCl3 and CO3^2-. This theory helps explain the observed bond angles in these molecules.