Give the approximate values for the indicated bond angles in the following molecules: (a)

Verified step by step guidance

1. Identify the central atom in the molecule.
2. Determine the electron domain geometry around the central atom using the VSEPR theory, which considers both bonding and non-bonding electron pairs.
3. Count the number of bonding pairs and lone pairs around the central atom to predict the molecular geometry.
4. Use the molecular geometry to estimate the bond angles. For example, tetrahedral geometries have bond angles of about 109.5°, trigonal planar geometries have bond angles of about 120°, and linear geometries have bond angles of about 180°.
5. Consider any deviations from ideal bond angles due to factors such as lone pairs or double bonds, which can slightly alter the angles.

Key Concepts

Bond Angles

Bond angles are the angles formed between two adjacent bonds at a central atom in a molecule. They are crucial for understanding molecular geometry and are influenced by the arrangement of electron pairs around the central atom, which can be predicted using VSEPR (Valence Shell Electron Pair Repulsion) theory.

VSEPR Theory

VSEPR theory is a model used to predict the geometry of individual molecules based on the repulsion between electron pairs surrounding a central atom. According to this theory, electron pairs will arrange themselves to minimize repulsion, leading to specific bond angles characteristic of different molecular shapes, such as linear, trigonal planar, or tetrahedral.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is determined by the number of bonding and non-bonding electron pairs around the central atom, which influences the bond angles. Common geometries include linear (180°), trigonal planar (120°), and tetrahedral (109.5°), each with distinct bond angles.