01:160:163 Lecture Notes - Lecture 30: Oxidation State, Electronegativity, Electrochemistry

• School: Rutgers University
• Department: Chemistry
• Course: 01:160:163
• Professor: Lauren Klein- Juneau

Document Summary

*****we did review problems for most of the class for chapter. Electrochemistry: redox reactions are chemical reactions during which electrons are transferred from one reactant to another. The reduction agent: the reagent that is oxidized (the one that is accepting electrons) The oxidizing agent: the reagent that is reduced (the one that is donation the electrons) Add e- and h+ respectively to balance the charges. Put the two balanced equations together by equalizing the e- and h+ with (each other) Oxidation number: the charge an atom has when electrons are transferred to the most electronegative atom. Figured out by looking at the final state of the element in the product to the initial charge of the atom in the reactant. Except also as -1/2 in superoxides (nao2)