This document provides an overview of redox (reduction-oxidation) reactions, including definitions of key terms like oxidation, reduction, oxidizing agents, reducing agents, and disproportionation reactions. It discusses identifying oxidation and reduction based on changes in oxygen, hydrogen, or electron content. Methods for determining oxidation states and balancing redox reactions using the half-reaction method are also described. Real-world examples of redox processes like corrosion and the blue bottle experiment are mentioned.

1. REDOX REACTIONS A.k.a. A study on why things explode

7. Redox gain of electrons loss of electrons gain in hydrogen loss of hydrogen loss of oxygen gain in oxygen Reduction Oxidation

15. Common Oxidation States Chemical species Oxidation state and remarks Any element eg Fe, O 2 , S 8 zero Oxygen in any compound -2 except in peroxides example H 2 O 2 or Na 2 O 2 then oxygen atom has oxidation state of -1 or in F 2 O , then oxygen atom has oxidation state of +2 Fluorine in any compound -1 being most electronegative Hydrogen in any compound +1 except in metal hydrides example NaH then hydrogen atom has oxidation state of -1 as metals have a greater tendency to lose electrons Chlorine, bromine, iodine -ve oxidation state if bonded to less electronegative element eg NaCl; then Cl = -1. +ve oxidation state if bonded to more electronegative element eg ClO - , then Cl = +1; ClO 3 - , then Cl = +5

28. Interlude: More real-life redox!

34. End of Lecture 1 of Redox “ I have never let my schooling interfere with my education.” Mark Twain