A molecule with the formula AB₃ has a trigonal pyramidal geometry. How many electron groups are on the central atom (A)?

Verified step by step guidance

1. insert step 1> Identify the molecular geometry given in the problem, which is trigonal pyramidal.
2. insert step 2> Recall that a trigonal pyramidal geometry typically arises from a tetrahedral electron geometry with one lone pair.
3. insert step 3> Understand that the central atom (A) in a trigonal pyramidal molecule has three bonded atoms (B) and one lone pair.
4. insert step 4> Count the total number of electron groups around the central atom, which includes both bonding pairs and lone pairs.
5. insert step 5> Conclude that the central atom (A) has four electron groups: three bonding pairs and one lone pair.

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. In the case of AB3 with trigonal pyramidal geometry, the arrangement is influenced by the presence of lone pairs that repel bonding pairs, leading to a specific shape.

Electron Groups

Electron groups include both bonding pairs of electrons (shared between atoms) and lone pairs (non-bonding electrons) around a central atom. The total number of electron groups determines the molecular geometry according to the VSEPR (Valence Shell Electron Pair Repulsion) theory. For a trigonal pyramidal shape, the central atom must have four electron groups.

VSEPR Theory

VSEPR (Valence Shell Electron Pair Repulsion) theory is a model used to predict the geometry of molecules based on the repulsion between electron pairs. According to this theory, electron groups will arrange themselves as far apart as possible to minimize repulsion. In the case of AB3, the presence of one lone pair leads to a trigonal pyramidal shape, indicating that there are four electron groups around the central atom.