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Oxidation Numbers, Reactions in Aqueous Solutions, & Predicting Products I. Rules for Assigning Oxidation Numbers 1. The oxidation number of any uncombined element is 0. 2. The oxidation number of a monatomic ion equals the charge on the ion. 3. The more-electronegative element in a binary compound is assigned the number equal to the charge it would have if it were an ion. 4. The oxidation number of fluorine in a compound is always -1. 5. Oxygen has an oxidation number of -2 unless it is combined with F (when it is +2), or it is in a peroxide (such as H2O2 or Na2O2), when it is -1. 6. The oxidation state of hydrogen in most of its compounds is +1 unless it is combined with a metal, in which case it is -1. Oxidation vs. Reduction The sum of the oxidation states in a neutral compound must equal zero and must be equal to the overall charge in an ionic compound. Assign oxidation states to each of the atoms in the following compounds: = a. FeF2 Fe = +2, F = -1 b. H2O H = +1, O = -2 c. KMnO4 K+ = +1, Mn 1(+2) 2(-1) d. C2H6 2(+1) 1(-2) C = -3, H = +1 2(-3) 6(+1) 1(+1) +7 e. ICl5 I = +5, Cl = -1 +5 5(-1) f. SO42- 0 +3 -2 7, O = 2 S = +6, O = -2 +6 4(-2) = -2 Assign oxidation states to each atom in the equation. Fe2O3 + 2 Al Al2O3 + 2 Fe Fe gains electrons. +3 -2 4(-2) It has been REDUCED 0 Al lost electrons. It has been OXIDIZED II. REDOX Reactions Remember LEO GER: LOSE ELECTRONS OXIDATION GAIN ELECTRONS REDUCTION Something that is reduced is called an oxidizing agent. Something that is oxidized is called a reducing agent. For each reaction, identify that atoms that undergo reduction, or oxidation. a. 2 H2 0 b. Zn 0 c. (g) (s) 2 AgCl +1 -1 + O2 0 + Cu2+ +2 (s) (g) 2 H2O (g) oxidized: hydrogen (0 to +1) reduced: oxygen (0 to -2) (aq) Zn2+ + Cu + H2 0 (g) +1 -2 +2 (aq) 2 H+ +1 0 (aq) (s) + 2 Ag 0 oxidized: zinc (0 to +2) reduced: copper (+2 to 0) (s) + 2 Cl- (aq) -1 oxidized: hydrogen (0 to +1) reduced: silver (+1 to 0) d. 2 MnO4-(aq) + 16 H+(aq) + 5 C2O42-(aq) 2 Mn2+(aq) + 10 CO2(g) + 8 H2O(l) +7 -2 +1 +3 -2 +2 +4 -2 oxidized: carbon (+3 to +4) reduced: manganese (+7 to +2) +1 -2 Learning Check Assign oxidation states to each of the atoms in the following compounds: a. SO2 b. S c. SO3 Assign oxidation states to each atom in the equation. Determine which element was oxidized and which was reduced. 2 Al + 3 CuCl2 2 AlCl3 + 3 Cu III. Dissociation When a soluble ionic salt dissolves in water the ions separate and a hydration shell is formed around each ion (Dissociation) Ex. Ba(NO3)2 in water – Ba(NO3)2 (aq) Ba+2(aq) + 2 NO3-1(aq) Aluminum acetate Al(C2H3O2)3 (aq) Al+3(aq)+ 3 C2H3O2-1(aq) Aluminum carbonate Al2(CO3)3 (s) Al2(CO3)3 (s) or No RXN Draw a beaker of dissociated sodium chloride; a beaker of dissociated Aluminum nitrate; and a beaker of silver chloride. Na+1 NO3-1 Na+1 NO3-1 Cl-1 Cl-1 Cl-1 Cl-1 = sodium ion = chloride ion Al+3 Ag+1 Al+3 Na+1 Na+1 NO3-1 NO3-1 NO3-1 Al+3 NO3-1 NO3-1 Cl-1 Ag Cl-1 +1 Cl-1 Ag+1 Cl-1 Ag+1 = aluminum ion Ag+1 = silver ion = nitrate ion Cl-1 = chloride ion Learning check Write a dissociation equation for aluminum sulfate Draw a beaker of dissociated aluminum sulfate IV. Predicting Products A. Single Displacement reactions: an element and a compound combine to form a new element and compound. * Use the activity series. *If you don’t know the General Equation: charge use +2 A + YB Y + AB (Cation) Example: B + AZ Z + AB (Anion) Na+1 Pb+2 C2H3O2-1 Sodium + Lead (II) acetate 2 Na(s) + Pb(C2H3O2)2(aq) Pb(s) + 2 NaC2H3O2 (aq) Single Replacement Reactions: Activity Series Active metal elements can replace less active metals, active nonmetal elements can replace less active nonmetals. Use the Activity series (snoopy sheet) to determine whether or not the reaction will occur. Driving force is the transfer of electrons. Learning check Try these single displacement reactions: 3. copper + silver nitrate 4. bromine + sodium chloride Lab – Metal Activity and Reactivity B. Double Displacement reactions: two compounds combine to produce two Driving force = different compounds - Acid-Base liquid and Precipitation Reactions. Driving force = solid * Use solubility rules. AB + YZ AZ + YB General Equation: C2H3O2-1 Pb+2 Na+1 Cl-1 Example: Lead (II) acetate + sodium chloride Pb(C2H3O2)2 (aq) + 2 NaCl (aq) PbCl2 (s) + 2 NaC2H3O2 (aq) Learning check Try these double displacement reactions: sodium sulfate + lead (II) nitrate sulfuric acid + potassium hydroxide Complete Ionic and Net Ionic Equations Molecular Equation: shows the complete formula of all reactants and products Ex: Ag+1 NO3-1 Ba+2 Cl-1 Silver nitrate + barium chloride 2 AgNO3 (aq) + BaCl2 (aq) 2 AgCl (s) + Ba(NO3)2 (aq) Complete Ionic Equation: represents aqueous compounds as ions Ex: 2 Ag+1(aq) + 2NO3-1(aq) + Ba+2(aq) + 2Cl-1(aq) 2AgCl(s) + Ba+2(aq) + 2NO3-1(aq) Net Ionic Equation: includes only those components directly involved in the reaction. Ions present on both sides on the equation and do not participate directly in the reaction are called Spectator Ions Ex: 2Ag+1(aq) + 2Cl-1(aq) 2AgCl(s) Ex: Write the molecular, complete ionic and net ionic equations for the following reaction. Na+1 Zn+2 NO3-1 Sodium + Zinc Nitrate Molecular – 2 Na(s) + Zn(NO3)2(aq) Zn(s) + 2NaNO3(aq) Complete 2 Na(s) + Zn+2(aq) + 2 NO3-1(aq) Zn(s) + 2 Na+1(aq) + 2 NO3-1(aq) Net – 2 Na(s) + Zn+2(aq) Zn(s) + 2 Na+1(aq) C. Decomposition reactions: a single compound is broken down into more than one product. There are six different types. A is metal/cation, B is nonmetal/anion 1. Decomposition of a binary compound into its elements. * Usually requires heat or electricity. Δ = heat or electricity General Equation: AB A + B Example: Sodium Chloride 2 NaCl(aq) 2 Na(s) + Cl2(g) 2. Decomposition of a base into a metal-oxide and water. Base = Compound General Equation: AOH AO + H2O Example: that contains hydroxide (OH-1) Sodium Hydroxide Metal-oxide = solid 2 NaOH(aq) Na2O(s) + H2O (l) A is metal/cation, B is nonmetal/anion 3. Decomposition of a ternary acid into a nonmetal-oxide and water. nonmetal-oxide = gas General Equation: HBO BO + H2O Example: sulfuric acid H2SO4(aq) SO3(g) + H2O (l) 4. Decomposition of a metallic carbonate into a metal-oxide and carbon dioxide. General Equation: ACO3 AO + CO2 Example: Sodium Carbonate Na2CO3(aq) Na2O (s) + CO2(g) A is metal/cation, B is nonmetal/anion 5. Decomposition of a metallic chlorate into a metal-chloride and oxygen gas. General Equation: AClO3 ACl + O2 Example: Sodium Chlorate 2 NaClO3(aq) 2 NaCl (aq) + 3 O2(g) 6. Decomposition of a tertiary salt into a metaloxide and a non-metal oxide General Equation: ABO AO+ BO Example: Sodium Phosphate 2 Na3PO4(aq) 3Na2O(s)+ P2O5(g) Special Situations Whenever H2CO3, H2SO3, or NH4OH is a product it will decompose immediately as follows: H2CO3 H2O + CO2 H2SO3 H2O + SO2 NH4OH H2O + NH3 Learning check Try these decomposition reactions: 5. Calcium chlorate 6. Phosphoric acid 7. Barium hydroxide 8. Tin (IV) carbonate Synthesis reactions: two substances combine to form one product. There are four different types. A is metal/cation, B is nonmetal/anion 1. Two elements combine to form a binary compound. General Equation: A + B AB Example: Sodium + Chlorine 2 Na(s) + Cl2(g) 2 NaCl(aq) 2. Combining a metal-oxide and water to produce a base. General Equation: AO + H2O AOH Example: Barium oxide + water BaO(s) + H2O(l) Ba(OH)2(aq) A is metal/cation, B is nonmetal/anion 3. Combining a nonmetal–oxide and water to produce a tertiary acid. General Equation: BO + H2O HBO Example: dinitrogen pentoxide + water N2O5(g) + H2O(l) 2 HNO3(aq) 4. Combining a metal-oxide and a nonmetaloxide to produce a tertiary salt. General Equation: AO + BO ABO Example: Barium oxide + dinitrogen pentoxide BaO(s) + N2O5(g) Ba(NO3)2(aq) Learning check Try these synthesis reactions: 9. Water + magnesium oxide 10. Water + dinitrogen trioxide 11. Bromine + sodium Combustion reactions: Certain organic compounds (Hydrocarbons – compound containing Carbon and Hydrogen or Carbon, Hydrogen and Oxygen) burn to produce specific products. There are two types. 1. Complete combustion – combining a hydrocarbon with excess oxygen to produce carbon dioxide and water. * if the equation does not indicate limited oxygen assume complete combustion General Equation: C H + O CO + H O x Example: x 2 CH4(g) + 2 O2(g) 2 2 CO2(g) + 2 H2O(g) 2. Incomplete combustion - combining a hydrocarbon with limited oxygen to produce carbon monoxide and water. General Equation: C H + limited O CO + H O x Example: 2 CH 4(g) x 2 2 + limited 3 O2(g) 2 CO(g) + 4 H2O(g) Learning check Try these combustion reactions: 12. C8H18 + oxygen 13. C2H2 + oxygen V. Reaction Rates Reaction rate depends on the collisions between reacting particles. Successful collisions occur if the particles... collide with each other have the correct orientation have enough kinetic energy to break bonds To speed up the rate of the reaction: Increase surface area (smaller particles or dissolve in water) Increase concentration (add more reactant) Increase temperature (add heat source) Add catalyze/enzyme VI. Heat in Reactions Exothermic reactions release heat Heat is a product Feels hot Endothermic reactions absorb heat Heat is a reactant Feels cold