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Reactions in Aqueous Solutions, Predicting Products and Classifying Types of Chemical Reactions

Reactions in Aqueous Solutions, Predicting Products and Classifying Types of Chemical Reactions. I. Predicting Whether a Reaction Will Occur. A. Four Driving Forces Formation of a solid (precipitate) Formation of water Transfer of electrons Formation of a gas

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Reactions in Aqueous Solutions, Predicting Products and Classifying Types of Chemical Reactions

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  1. Reactions in Aqueous Solutions, Predicting Products and Classifying Types of Chemical Reactions

  2. I. Predicting Whether a Reaction Will Occur A. Four Driving Forces • Formation of a solid (precipitate) • Formation of water • Transfer of electrons • Formation of a gas B. If a driving force occurs the reaction will take place.

  3. Predicting States of Substances 1. Soluble solid – readily dissolves in water 2. Insoluble and slightly soluble solid – a solid where such a tiny amount dissolves in water that it is undetectable to the naked eye 3. Solubility is temperature dependent State is aqueous - (aq) State is solid - (s) States of reactants can be manipulated

  4. Solubility Rules(on snoopy sheet) Ex. Predict whether the following substances are soluble or insoluble. Solubility Rules Mainly water soluble (aq) All nitrates are soluble. All acetates are soluble. All chlorates are soluble. All chlorides are soluble except AgCl, Hg2Cl2, and PbCl2 All bromides are soluble except AgBr, Hg2Br2, PbBr2, and HgBr2 All iodides are soluble except AgI, Hg2I2, PbI2, and HgI2 All sulfates are soluble except CaSO4, SrSO4, BaSO4, PbSO4, Hg2SO4, and Ag2SO4 Mainly water insoluble (s) All sulfides are insoluble except those of 1A and 2A elements and (NH4)2S All carbonates are insoluble except those of 1A and (NH4)2CO3 All phosphates are insoluble except those of 1A and (NH4)3PO4 All hydroxides are insoluble except those of 1A, Ba(OH)2, Sr(OH)2 and Ca(OH)2 AgNO3 (aq) Al(OH)3 (s) ZnSO4 (aq) Li2CO3 (aq) Cu3PO4 (s)

  5. 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

  6. Cl-1 Cl-1 Cl-1 Cl-1 Cl-1 Cl-1 Na+1 Na+1 Na+1 Na+1 Na+1 NO3-1 NO3-1 NO3-1 NO3-1 NO3-1 NO3-1 NO3-1 Ag+1 Cl-1 Ag+1 Cl-1 Cl-1 Cl-1 Ag+1 Ag+1 = sodium ion Al+3 = aluminum ion Ag+1 = silver ion = chloride ion = nitrate ion Cl-1 = chloride ion Draw a beaker of dissociated sodium chloride; a beaker of dissociated Aluminum nitrate; and a beaker of silver chloride. Al+3 Al+3 Na+1

  7. Special Rules 1. Acids are aqueous 2. Most metal oxides are solids 3. Most non-metal oxides are gases

  8. III. Types of Reactions Double Displacement: Single Displacement: Decomposition: Synthesis: Combustion: AB +YZ  AZ + YB Reactants are: 2 compounds A +YB  Y + AB Reactants are: 1 element & 1 Compound AB  A + B Reactant is: 1 compound A + B  AB Reactants are: 2 elements or 2 oxides CxHx + O2 CO2 + H2O Reactants are: hydrocarbon and oxygen

  9. IV. Predicting Products • Double Displacement reactions: two compounds combine to produce two different compounds - Acid-Base and Precipitation Reactions. * Use solubility rules. General Equation: Example: Driving force = liquid Driving force = solid AB + YZ  AZ + YB C2H3O2-1 Pb+2 Na+1 Cl-1 Lead (II) acetate + sodium chloride Pb(C2H3O2)2 + 2 NaCl  PbCl2 + 2 NaC2H3O2 (aq) (aq) (s) (aq)

  10. B.Single Replacement Reactions: Activity Series Single Displacement reactions: an element and a compound combine to form a new element and compound. * Use the activity series. General Equation: Example: *If you don’t know the charge use +2 A + YB  Y + AB (Cation) 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) 

  11. 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.

  12. 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. General Equation: Example: 2. Decomposition of a base into a metal-oxide and water. General Equation: Example:  Δ = heat or electricity AB  A + B Sodium Chloride 2 NaCl(aq)  2 Na(s) + Cl2(g) Base = Compound that contains hydroxide (OH-1) AOH  AO + H2O Sodium Hydroxide Metal-oxide = solid 2 NaOH(aq)  Na2O(s) + H2O (l)

  13. A is metal/cation, B is nonmetal/anion nonmetal-oxide = gas HBO  BO + H2O 3. Decomposition of a ternary acid into a nonmetal-oxide and water. General Equation: Example: 4. Decomposition of a metallic carbonate into a metal-oxide and carbon dioxide. General Equation: Example: sulfuric acid H2SO4(aq)  SO3(g) + H2O (l) ACO3 AO + CO2 Sodium Carbonate Na2CO3(aq)  Na2O (s) + CO2(g)

  14. A is metal/cation, B is nonmetal/anion AClO3 ACl + O2  5. Decomposition of a metallic chlorate into a metal-chloride and oxygen gas. General Equation: Example: 6. Decomposition of a tertiary salt into a metal-oxide and a non-metal oxide General Equation: Example: Sodium Chlorate 2 NaClO3(aq)  2 NaCl (aq) + 3 O2(g) ABO  AO+ BO Sodium Phosphate 2 Na3PO4(aq)  3 Na2O(s) + P2O5(g)

  15. 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

  16. D. 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: Example: 2.Combining a metal-oxide and water to produce a base. General Equation: Example: A + B  AB Sodium + Chlorine 2 Na(s) + Cl2(g)  2 NaCl(aq) AO + H2O  AOH Barium oxide + water BaO(s) + H2O(l)  Ba(OH)2(aq)

  17. A is metal/cation, B is nonmetal/anion BO + H2O  HBO 3.Combining a nonmetal–oxide and water to produce a tertiary acid. General Equation: Example: 4.Combining a metal-oxide and a nonmetal-oxide to produce a tertiary salt. General Equation: Example: dinitrogen pentoxide + water N2O5(g) + H2O(l)  2 HNO3(aq) AO + BO  ABO Barium oxide + dinitrogen pentoxide BaO(s) + N2O5(g)  Ba(NO3)2(aq)

  18. E. 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: Example: 2.Incomplete combustion - combining a hydrocarbon with limited oxygen to produce carbon monoxide and water. General Equation: Example: CxHx + O2 CO2 + H2O CH4(g) + O2(g) 2 CO2(g) + 2 H2O(g) CxHx + limited O2 CO + H2O 2 CH4(g) + limited O2(g) 3 2 CO(g) + 4 H2O(g)

  19. 2 NaCl(aq)  2 Na(s) + Cl2(g) 2 Na(s) + Cl2(g)  2 NaCl(aq) F.Oxidation Reduction reactions: (redox) • Driving Force = Transfer of electron • Always in single displacement reactions • Sometimes in Synthesis and Decomposition • Never in Double Displacement Example: Anytime a single element is present a reaction is also classified as redox decomposition & redox synthesis & redox Zn(NO3)2(aq) + 2 Na(s) 2NaNO3(aq) + Zn(s) single displacement & redox

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