CH111 Lecture Notes - Lecture 12: Oxidation State, Oxidizing Agent, Ionic Compound
25 Dec 2018
Department
Course
Professor
Document Summary
Redox reaction- a reaction that involves a transfer of electrons: examples of redox reactions: all single-replacement reactions, all combustion reactions, and some synthesis or decomposition reactions. Oxidation- the process of losing an electron (charge increases). Reduction- the process of gaining an electron (charge decreases). It oxidizes another substance; in the process, it is reduced. It reduces another substance; in the process, it is oxidized. The number of electrons lost or gained by an atom/group of atoms when it forms an ion. Why do we use oxidation numbers: to keep track of how electrons are transferred during a reaction, to tell which reactant is oxidized and which one is reduced, to find the coefficients to balance equations. # of an uncombined element is zero: ex: o2, cl2, fe, etc, the ox. # of a mono-atomic ion is the charge of that ion: ex: the ox. # of na+ is +1: ex: the ox. # of al3+ is +3: the ox.
