OxidationReduction Reactions Redox LEO SAYS GER Oxidation and

Oxidation and Reduction (Redox) q Electrons are transferred q Spontaneous redox rxns can transfer

Oxidation Reduction Reactions (Redox) Each sodium atom loses one electron: Each chlorine atom gains

LEO says GER : Lose Electrons = Oxidation Sodium is oxidized Gain Electrons =

Rules for Assigning Oxidation Numbers Rules 1 & 2 1. The oxidation number of

Rules for Assigning Oxidation Numbers Rules 3 & 4 3. The oxidation number of

Rules for Assigning Oxidation Number Rule 5 5. The sum of the oxidation numbers

Rules for Assigning Oxidation Numbers Rule 6 6. The sum of the oxidation numbers

The Oxidation Number Rules SIMPLIFIED 1. The sum of the oxidation numbers in ANYTHING

Not All Reactions are Redox Reactions in which there has been no change in

This slide refers to vocabulary that has been excluded from AP Chemistry by the

Trends in Oxidation and Reduction Active metals: Lose electrons easily Are easily oxidized Active

Redox Reaction Prediction #1 Reduced in reaction Formed in reaction Mn. O 4 -

Redox Reaction Prediction #2 Oxidized in reaction Formed in reaction Halide Ions Free Metals

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Oxidation-Reduction Reactions “Redox” LEO SAYS GER

Oxidation and Reduction (Redox) q Electrons are transferred q Spontaneous redox rxns can transfer energy q Electrons (electricity) q Heat q Non-spontaneous redox rxns can be made to happen with electricity

Oxidation Reduction Reactions (Redox) Each sodium atom loses one electron: Each chlorine atom gains one electron:

LEO says GER : Lose Electrons = Oxidation Sodium is oxidized Gain Electrons = Reduction Chlorine is reduced

Rules for Assigning Oxidation Numbers Rules 1 & 2 1. The oxidation number of any uncombined element is zero 2. The oxidation number of a monatomic ion equals its charge

Rules for Assigning Oxidation Numbers Rules 3 & 4 3. The oxidation number of oxygen in compounds is -2 4. The oxidation number of hydrogen in compounds is +1

Rules for Assigning Oxidation Number Rule 5 5. The sum of the oxidation numbers in the formula of a compound is 0 2(+1) + (-2) = 0 H O (+2) + 2(-2) + 2(+1) = 0 Ca O H

Rules for Assigning Oxidation Numbers Rule 6 6. The sum of the oxidation numbers in the formula of a polyatomic ion is equal to its charge X + 3(-2) = -1 N O X + 4(-2) = -2 S O X = +5 X = +6

The Oxidation Number Rules SIMPLIFIED 1. The sum of the oxidation numbers in ANYTHING is equal to its charge 2. Hydrogen in compounds is +1 3. Oxygen in compounds is -2

Not All Reactions are Redox Reactions in which there has been no change in oxidation number are not redox rxns. Examples:

This slide refers to vocabulary that has been excluded from AP Chemistry by the College Board, and will not be tested. Reducing Agents and Oxidizing Agents q The substance reduced is the oxidizing agent q The substance oxidized is the reducing agent Sodium is oxidized – it is the reducing agent Chlorine is reduced – it is the oxidizing agent

Trends in Oxidation and Reduction Active metals: Lose electrons easily Are easily oxidized Active nonmetals: Gain electrons easily Are easily reduced

Redox Reaction Prediction #1 Reduced in reaction Formed in reaction Mn. O 4 - (acid solution) Mn. O 4 - (basic solution) Mn. O 2 (acid solution) Cr 2 O 72 - (acid) Cr. O 42 HNO 3, concentrated HNO 3, dilute H 2 SO 4, hot conc Metallic Ions Free Halogens HCl. O 4 Na 2 O 2 H 2 O 2 Mn(II) Mn. O 2 Mn(II) Cr(III) NO 2 NO SO 2 Metallous Ions Halide ions Cl. OHO 2

Redox Reaction Prediction #2 Oxidized in reaction Formed in reaction Halide Ions Free Metals Metalous Ions Nitrite Ions Sulfite Ions Free Halogens (dil, basic sol) Free Halogens (conc, basic sol) C 2 O 42 - Halogens Metal Ions Metallic ions Nitrate Ions SO 42 Hypohalite ions Halate ions CO 2