ࡱ> BDA bjbj & 4BBBB$f$B4!!!:<<<<<<$"^`@!`Wuqqq^:q:qq:,PW> &0HR"^"8"T!Lm6q,*!!!``[!!!"!!!!!!!!! : OXIDATION STATE Oxidation state: The imaginary charge an atom would have if shared electrons were divided equally between identical atoms bound to one another, or, for different atoms, if electrons were all assigned to the atom in each bond that has the greater attraction for electrons. Rules for Assigning Oxidation States: The oxidation number of all atoms adds up to the charge on the molecule or ion. The oxidation state of an element is zero. i.e. Na(s), K(s), Hg(l), Ag(s); these can also be written as Na0, K0, etc. diatomic molecules: H2 (g), N2 (g), F2 (g), O2 (g), I2 (s), Cl2 (g), Br2 (l), (mnemonic: Have No Fear Of Ice Cold Beer) The oxidation number of: an alkali metal is +1 an alkaline earth metal is +2 metals in group IIIA (B, Al, etc) is +3 The oxidation number of hydrogen +1 in covalent compounds with nonmetals: ex) CH4 (g), HCl (aq), NH3 (g), H2SO4 (aq), etc 1 when combined with metals (especially alkali & alkaline earth metals): ex) NaH, LiH, AlH3 Halides (F, Cl, Br, and I) usually have an oxidation number of 1. The fluoride ion has a -1 oxidation state, except when paired with oxygen. The oxidation number of oxygen and other group VIA elements is 2 in covalent compounds. Exception: oxygen has an oxidation state of 1 in peroxides (H2O2 or Na2O2 where oxygen is O22-) and in superoxides -1/2 (NaO2 where oxygen is O2-). Non-integer oxidation states do exist ex) In Fe3O4, iron has an oxidation state of +8/3 Convention for showing oxidation states and charges: Oxidation state is represented as +n or n (i.e. +3, -2) Charge is written as n+ or n- (i.e. 3-, or 2- as in CO22-) Oxidation corresponds to an increase in the oxidation number (n ( 0 ( +n) The compound being oxidized is the reducing agent. gain in electrons The reducing agent causes a loss of oxygen atoms gain of hydrogen atoms Reduction corresponds to a decrease in oxidation number (+n ( 0 ( n) The compound being reduced is the oxidizing agent.  loss of electrons The oxidizing agent causes a gain of oxygen atoms loss of hydrogen atoms mnemonics: Oxidation Is Loss of electrons. Reduction Is Gain of electrons. OIL RIG Loss of Electrons is Oxidation. Gain of Electrons is Reduction. LEO GER BALANCING HALF REACTIONS Step 1: Write the skeletal net ionic equation. (This is usually given.) Step 2: Make two half reactions, one for the species being oxidized the other for the species being reduced. Step 3: Balance all atoms except for the hydrogen and oxygen atoms. Step 4: Balance the hydrogen and oxygen atoms In acidic conditions: Balance the hydrogen atoms by adding hydrogen ions (H+) Balance the oxygen atoms by adding water (H2O) In basic conditions: Balance the oxygen atoms by adding hydroxide ions (OH-) Balance the hydrogen atoms by adding water (H2O) Step 5: To balance charge add electrons to the side with greater positive charge. Step 6: Multiply each half reaction by an appropriate whole number so that the number of electron in each half reaction is equal. Step 7: Add the two balanced half reactions together, and cancel out species that appear on both sides of the equation. 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