Understanding Molecular Shapes
Molecular shape is determined by the arrangement of electron pairs around a central atom. The most common shapes are:
* Linear: Two electron pairs around the central atom, resulting in a straight line.
* Bent/V-shaped: Two bonding pairs and two lone pairs of electrons around the central atom, creating a bent shape.
* Trigonal planar: Three electron pairs around the central atom, forming a flat triangle.
* Tetrahedral: Four electron pairs around the central atom, forming a pyramid with a triangular base.
Identifying the Compound
To determine which compound is not bent, we need to look at the central atom and its bonding and lone pair electrons. Here are some common examples:
* Water (H₂O): The central atom is oxygen, which has two lone pairs and two bonding pairs. This results in a bent shape.
* Carbon Dioxide (CO₂): The central atom is carbon, which has two double bonds to oxygen atoms. These bonds are linear, resulting in a linear molecule.
* Ammonia (NH₃): The central atom is nitrogen, which has one lone pair and three bonding pairs. This results in a trigonal pyramidal shape.
* Methane (CH₄): The central atom is carbon, which has four bonding pairs. This results in a tetrahedral shape.
Answer
The compound that does not have a bent molecular shape is Carbon Dioxide (CO₂) .
