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More Reactions

More Reactions. Acid-Base Reactions Oxidation-Reductions Reactions. Acids. Produce H + ions Ions disassociate in water Strong electrolytes (conduct electricity) HCl (g) ---> H + (aq) + Cl - (aq). Bases. Produces OH- (hydroxide) ions Strong Electrolytes

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More Reactions

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  1. More Reactions Acid-Base Reactions Oxidation-Reductions Reactions

  2. Acids • Produce H+ ions • Ions disassociate in water • Strong electrolytes (conduct electricity) HCl (g) ---> H+(aq) + Cl-(aq)

  3. Bases • Produces OH- (hydroxide) ions • Strong Electrolytes NaOH(s) ---> Na+ (aq) + OH-(aq) • Strong acid + Strong Base --> H2O(l) • Ionic compound (salt) in product HBr(aq) + NaOH(aq) ---> H2O(l) + NaBr(aq) H20

  4. Oxidation-Reduction • Electron transfer • Oxidation = loss of electrons • Reduction = gain of electrons • Electrons can transfer from metal to nonmetal 2Ca (s) + O2(g) --> 2CaO(s) Zn (s) + 2HCl (aq) --> H2(g) + ZnCl2 (aq)

  5. Oxidation Numbers Rules • The oxidation number of a free element = 0 • The oxidation number of a monatomic ion = charge on the ion 3. The oxidation number of hydrogen = +1 and rarely -1

  6. Oxidation Numbers • The oxidation number of oxygen = -2 and in peroxides -1 • The oxidation number of fluorine = -1 • The sum of the oxidation numbers in a polyatomic ion = charge on the ion 7. Elements in groups 1, 2, and aluminum are always indicated on the periodic table

  7. Sb2O5 CrO4-2 ClO4- NaBO3 MnO4- BrO3- ClO - Cr2O7-2 Oxidation NumbersExamples

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