VI. Oxidation-Reduction (Redox)

A. Some simple combination reactions such as two elements (see Part I: A)

B. Single replacement (see Part III)

C. Combustion (see Part V)

D. Reactions between oxidizers (oxidizing agents) and reducers (reducing agents) (Remember: One species is oxidized and another is reduced.)

bulletCommon Oxidizing Agent Formed in Reaction

(reduced to )

bulletMnO4-, MnO2 in acid Mn2+
bulletMnO4- in neutral or base MnO2
bulletCr2O72- in acid Cr3+
bulletHNO3, conc. NO2
bulletHNO3, dilute NO
bulletH2SO4, conc. SO2
bulletMetal-ic ions Metal-ous ions
bulletH2O2 H2O
bulletMetal ions Free metals
bulletCommon Reducing Agent Formed in Reaction

(oxidized to )

bulletHalide ions Free halogen
bulletFree metals Metal ions
bulletSulfite, sulfide, SO2 , S2O32- Sulfate ion
bulletS2O32- (with I2) S4O62-
bulletMetal-ous ions Metal-ic ions
bulletFree halogen, dil. basic Hypohalite ion*
bulletFree halogen, conc. basic Halate ion
bulletNitrite Nitrate
bulletH2O2 (with st. ox. agent) O2
bulletH2 H2O
bulletC, hydrocarbon CO2

* If free halogen such as Cl2 is reacted with only dilute NaOH, the Cl2 is both oxidized and reduced, giving ClO- and Cl-.

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