(a) Draw Lewis structures for chloromethane 1CH3Cl2, chloroethene 1C2H3Cl2, and chloroethyne 1C2HCl2. Draw Lewis structures for chloromethane 1CH3Cl2.

Key Concepts

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent electrons and lines to represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting the reactivity of compounds.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in determining how atoms bond with each other. The number of valence electrons influences the formation of bonds and the overall structure of a molecule. For example, carbon has four valence electrons, which allows it to form four bonds, while chlorine has seven, allowing it to form one bond.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is influenced by the number of bonds and lone pairs around the central atom, which can affect the molecule's physical and chemical properties. Understanding molecular geometry is important for predicting the behavior of molecules in reactions and their interactions with other substances.