CHEM 1A03 Lecture Notes - Lecture 9: Iron(Iii) Oxide, Aluminium Oxide, Oxidation State

• School: McMaster University
• Department: Chemistry
• Course: CHEM 1A03
• Professor: All

Document Summary

3. 3 reduction-oxidation reactions (redox: lose electrons oxidize; gain electrons reduced, calculate oxidation numbers to see which species gets oxidized and which gets reduced, reducing agent causes reduction and gets oxidized; oxidizing agent causes oxidation and gets reduced. 3. 4 redox reactions and terminology: goldschmidt reaction (termite reaction, the termite reaction is a classic redox reaction with historical significance, whe(cid:374) (cid:271)uildi(cid:374)g the (cid:396)ail(cid:449)ay a(cid:272)(cid:396)oss ca(cid:374)ada the (cid:449)o(cid:396)ke(cid:396)s did(cid:374)"t ha(cid:448)e po(cid:396)ta(cid:271)le welding equipment. Instead, they did on-the-spot chemistry to do spot welding. They would ignite a mixture of finely powdered iron (iii) oxide, or rust, with finely powdered aluminum and it would produce aluminum oxide and elemental iron. To prevent this, a salt bridge containing mobile ions allows cations to flow towards the cathode, and anions to flow towards the anode: this maintains electroneutrality for the electrochemical cell, and so it functions spontaneously.