see the chart on page 156 for rules about oxidation numbers you need these so you can tell if you are gaining or losing electrons reactions are an exchange of electrons. some atoms lose, some atoms gain. o2 cl Mn+3 reduction is the gaining of electrons ( ) oxidation is the losing of electrons ( becoming more +) Na + SO4 try some! KClO3 H 2O UF6 MnO4 reducing agent cause another atom to be reduced by donating electrons oxidizing agent often oxygen, it is the atom that takes electrons and causes another atom to lose them. see pg 156 for rules now try them in a reaction H2 + O2 = H2O element = o ion = charge oxygen = 2 hydrogen =1 flourine =1 last element treat as an ion ( or 1st if need be) balance 1st so total is zero if polyatomic ion, balance to charge + try some! Mg +2 KClO3 H 2O Cl2 (g) UF6 MnO4 +2 +1, +5, 2 +1, 2 0 +6 1 +8, 2 3 ways to look at oxidation oxidizing agent remember that originally oxidation always meant where oxygen had been added, like the creation of rust or tarnishing of silver Fe + O2 2Fe2O3 figure oxidation states, see what the job of the oxygen is? so oxidation it also means it is also means to add oxygen to lose electrons the increase of oxidation number!!! it is a good idea to know the chart next page for some common oxidizing and reducing agents!!! try pg 922 111 reduction agent O2, H2, Halogens F2, Cl 2,I2 halogen ions F, Cl, I Cr+3 Cr2O7 2 MnO4 Mn+2 metals, C quiz over oxidation/reduction numbers For the following reactions, assign oxidation numbers, then list the oxidizing agent 1. KClO3 KCl + O2 2. H2 + I2 HI single replacement reactions when you have an element and a compound, and the element becomes part of the product compound, oxidation states have altered. remember net ionic equations? write it out, seperate the ionic compounds, get rid of everything that doesn't change. that is great for redox, cause you can look at just the exchange of electrons AgNO3 + Cu s CuNO3 + Ags better yet Ag + + Cus Cu+ + Ags 3. Cu + AgNO3 Ag + CuNO3 activity series this is a list of metals in order of most reactive to least reactive. it will also help you figure out how a single replacement reaction should occur. good for oxidation reduction cause that is what most are! K Ca react with water Na Mg Al Zn Fe react with acid Ni Sn Pb H2 Cu Hg very unreactive Ag Au F can replace all I replaces nothing. so can the following occur? K + Ca(CO3) KCl + F2 Mg + H20? Mg + HCl? Ca + NaOH Al + ZnS H2 + KCl Ca + K2CO3
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