The hypochlorite ion, ClO^-, is the active ingredient in bleach. The perchlorate ion, ClO₄^-, is a main component of rocket propellants. Draw Lewis structures for both ions. (c) What is the oxidation number of Cl in the hypochlorite ion? (d) What is the oxidation number of Cl in the perchlorate ion, assuming the Cl—O bonds are all single bonds?

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 help visualize the arrangement of electrons and the connectivity of atoms, which is crucial for understanding molecular geometry and reactivity. In the case of ions like hypochlorite and perchlorate, drawing their Lewis structures allows us to identify the formal charges and the overall electron distribution.

Oxidation Numbers

Oxidation numbers are a way to keep track of electron transfer in chemical reactions, indicating the degree of oxidation of an atom in a compound. They are assigned based on a set of rules, such as the oxidation number of oxygen is typically -2, and the sum of oxidation numbers in a neutral compound is zero. Understanding oxidation numbers is essential for determining the oxidation state of chlorine in the hypochlorite and perchlorate ions.

Ionic Compounds and Bonding

Ionic compounds are formed when atoms transfer electrons, resulting in the formation of charged ions that attract each other due to electrostatic forces. In the context of hypochlorite and perchlorate ions, recognizing that chlorine is bonded to oxygen through ionic interactions helps in understanding the stability and reactivity of these ions. This knowledge is fundamental when analyzing their roles in various chemical processes, such as in bleach and rocket propellants.