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URL:https://www.learndesk.us/class/6031358776311808/lesson/d65499d94f23ece11940eaf3e99fb8cc?ref=outlook-calendar
SUMMARY:UNIT 11 
DTSTART;TZID=America/Los_Angeles:20260501T190000
DTEND;TZID=America/Los_Angeles:20260501T200000
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DESCRIPTION: Redox reactions are a type of chemical reaction that involves the change in the oxidation state of atoms. These reactions involve the actual or formal transfer of electrons from one species known as the reducing agent to another species known as the oxidising agent. The transfer of electrons is responsible for the changing oxidation number in each species. There are a number of rules that govern the oxidation number of an atom undergoing a redox reaction: A free element is given an oxidation number of 0 In a compound or ion, the sum of all the oxidations numbers is equal to the total charge of the compound or ion Group 1 and group 2 metals are given an oxidation number of 0 Hydrogen is given an oxidation number of +1 unless it is bonded as a hydride to metals Oxygen is commonly given an oxidation number of -2 Halogens are commonly given an oxidation number of -1

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