Chapter 10 Chemical Reactions.

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Presentation transcript:

Chapter 10 Chemical Reactions

Evidence of Chemical Reactions Chemical Reaction: The process of one or more substances being rearranged to form a different substance AKA – Chemical Change Evidence: Temperature change Absorption of Heat (endothermic reaction) Release of heat (exothermic reaction) Color Change Sometimes, reactions are so subtle they are hard to detect.

Representing Chemical Reactions Reactants – Starting Substances (on the LEFT- HAND SIDE of the Equation) Products – Ending Substances (on the RIGHT- HAND SIDE of the Equation) Unlike in mathematics, where things are (=) equaled, in chemistry, reactions are directional () Reactant 1 + Reactant 2  Product 1 + Product 2

Representing Chemical Reactions Reactant 1 + Reactant 2  Product 1 + Product 2 More correct Reactant 1 (state) + Reactant 2 (state)  Product 1 (state) + Product 2 (state) States are denotes as follows: (s) means solid (aq) means liquid (g) Means gas

Representing Chemical Equations in Words Word Equations are used to indicate products and reactants of chemical reactions Iron(s) + Chlorine(g)  Iron(III) Chloride (s) In Word Equations: Iron and Chlorine react to produce Iron (III) Chloride

Iron(s) + Chlorine(g)  Iron(III) Chloride (s) Skeleton Equations The skeleton equation gives more information than the word equation It uses the chemical formulas (symbols) to describe a reaction NOTE: THESE ARE NOT BALANCED EQUATIONS!!! More information includes basic amounts of each element Iron(s) + Chlorine(g)  Iron(III) Chloride (s) Fe(s) + Cl2  FeCl3

Practice Working independently on your white board, write skeleton equations for the following word problems: hydrogen(g) +bromine(g)  hydrogen bromide (g) Carbon monoxide (g) + oxygen (g)  carbon dioxide (g) Potassium Chlorate (s)  Potassium Chloride(s) + Oxygen (g)

Practice Answers Working independently on your white board, write skeleton equations for the following word problems: hydrogen(g) +bromine(g)  hydrogen bromide (g) H2(g) + Br2(g)  HBr (g) 2) Carbon monoxide (g) + oxygen (g)  carbon dioxide (g) CO(g) + O2(g)  CO2 (g) 3) Potassium Chlorate (s)  Potassium Chloride(s) + Oxygen (g) KClO3(g)  KCl(s) + O2(g)

Chemical Equations The Process: Write a skeleton equation Remember the conservation of mass (matter is neither created nor destroyed, but can change shape and form) Balance the equation so that the reactants and products are equal When these three steps are complete, the product should be a balanced chemical reaction

How to Balance Chemical Reactions Coefficient The number written before either the products and/or reactants. These are whole numbers A “one” (1) is presumed Coefficients start at “two” 2 H2 + Cl2  2HCl The 2 in front of the HCl is the Coefficient

How to Balance Chemical Reactions Write the skeleton equation for the reaction. Count the atoms (number) of elements in the reactants Count the atoms (number) of elements in the products Change the coefficients to make the numbers of atoms of each element equal on both sides of the equation. Note: Never change the subscript Write the coefficients in their lowest possible ratio Check your work

How to Balance Equations – The T-Method Equation: NaOH (aq) + CaBr2(aq)  Ca(OH)2(s) + NaBr(aq) Reactants on this Side Products on This Side 1- Na 1-OH 1-Ca 2-Br NaOH (aq) + CaBr2(aq) 2NaOH (aq) + CaBr2(aq) 2- Na 2-OH 1-Ca 2-Br They are Equal 1- Na 2-OH 1-Ca 1-Br Ca(OH)2(s) + 2NaBr(aq) 2- Na 2-OH 1-Ca 2-Br They are Equal NOTE: Only Change 1 Coefficient, 1 Side at a Time.

Classifying Chemical Reactions 5 Main Types of Chemical Reactions Synthesis Reaction Combustion Reaction Decomposition Reaction Single-Replacement Reaction Double-Replacement Reaction

Synthesis Reaction A chemical reaction in which two or more products react to form a single product A + B  AB Synthesis can occur between elements and/or compounds Element + Elements  Compound Compound + Compound  Compound Element + Compound  Compound

Synthesis Reaction Examples 2Mg + O2 ---> 2MgO 2H2 + O2 ---> 2H2O 2K + Cl2 ---> 2KCl 4Fe + 3O2 ---> 2Fe2O3 CaO + CO2 ---> CaCO3 Na2O + CO2 ---> Na2CO3 2KCl + 3O2 ---> 2KClO3 Ba(ClO3)2 ---> BaCl2 + 3O2

Predicting Products of Chemical Reactions Class of Reaction Reactants Probable Products Synthesis Two or more substances One compound

Combustion Reaction Oxygen combines with substance and releases energy in the form of heat and light Majority of combustion reactions are synthesis reactions Not ALL combustion reactions are synthesis reactions

Combustion Reaction Examples CxHy + O2 ---> CO2 + H2O CH4 + O2 ---> CO2 + H2O C2H6 + O2 ---> CO2 + H2O C6H12O6 + O2 ---> CO2 + H2O C2H5OH + O2 ---> CO2 + H2O C21H24N2O4 + O2 ---> CO2 + H2O + NO2 C2H5SH + O2 ---> CO2 + H2O + SO2

Predicting Products of Chemical Reactions Class of Reaction Reactants Probable Products Synthesis Two or more substances One compound Combustion A metal and oxygen A non-metal and oxygen A compound and oxygen The oxide of a metal The oxide of a non-metal Two or more oxides

Decomposition Reaction A single compound breaks down into one or more elements and/or compounds Opposite of the synthesis reaction AB  A + B Often require an energy source to occur. Heat, light, electricity are some examples of energy

Decomposition Reaction Examples HgO ---> Hg + O2 H2O ---> H2 + O2 MgCl2 ---> Mg + Cl2 FeS ---> Fe + S CaCO3 ---> CaO + CO2 Na2CO3 ---> Na2O + CO2 KClO3 ---> KCl + O2 Ba(ClO3)2 ---> BaCl2 + O2

Predicting Products of Chemical Reactions Class of Reaction Reactants Probable Products Synthesis Two or more substances One compound Combustion A metal and oxygen A non-metal and oxygen A compound and oxygen The oxide of a metal The oxide of a non-metal Two or more oxides Decomposition Two or more elements and/or compounds

Single Replacement Reaction Also Called a Replacement Reaction A reaction in which the atoms of one element replace the atoms of another element in a compound A + BX  AX + B One metal might replace another metal Lithium and water is an example of a single replacement reaction

Single Replacement Reaction Examples Cu + AgNO3 ---> Ag + Cu(NO3)2 Fe + Cu(NO3)2 ---> Fe(NO3)2 + Cu Ca + H2O ---> Ca(OH)2 + H2 Zn + HCl ---> ZnCl2 + H2 ZnS + O2 ---> ZnO + S K + H2O ---> KOH + H2 Fe + HCl ---> FeCl3 + H2 NaI + Br2 ---> NaBr + I2

Predicting Products of Chemical Reactions Class of Reaction Reactants Probable Products Synthesis Two or more substances One compound Combustion A metal and oxygen A non-metal and oxygen A compound and oxygen The oxide of a metal The oxide of a non-metal Two or more oxides Decomposition Two or more elements and/or compounds Single-replacement A metal and a compound A non-metal and a compound A new compound and the replaced metal. A new compound and the replaced non-metal

Double Replacement Reaction The exchange of ions between TWO compounds AY + BX  AX + BY A and B would be cations Y and X are anions ALL products of a double-replacement reaction are either a precipitate, gas or water. Precipitate: A solid produced during a chemical reaction

Guidelines for Double Replacement Reaction Write the components of the reactants in a skeleton equation Identify the cations and anions Pair up each cation with the anion in the other compound Write the formulas for the products using pairs from step 3. Write the complete equation for the double-replacement reaction Balance the equation

Double Replacement Reaction Examples KOH + H2SO4 ---> K2SO4 + H2O FeS + HCl ---> FeCl2 + H2S NaCl + H2SO4 ---> Na2SO4 + HCl AgNO3 + NaCl ---> AgCl + NaNO3 CaCO3 + HCl ---> CaCl2 + CO2 + H2O K2SO3 + HNO3 ---> KNO3 + SO2 + H2O NH4Cl + NaOH ---> NaCl + NH3 + H2O

Predicting Products of Chemical Reactions Class of Reaction Reactants Probable Products Synthesis Two or more substances One compound Combustion A metal and oxygen A non-metal and oxygen A compound and oxygen The oxide of a metal The oxide of a non-metal Two or more oxides Decomposition Two or more elements and/or compounds Single-replacement A metal and a compound A non-metal and a compound A new compound and the replaced metal. A new compound and the replaced non-metal Double-Replacement Two compounds Two different compounds, one of which is often a sold, water or a gas

Reactions in Aqueous Solutions Solutes: What is dissolved in a solution Solvent: The liquid in which the solutes are dissolved Aqueous Solution: A solution in which the solvent is water HCl(g)  H+(aq) + Cl-(aq) When HCl is dissolved in H2O, it dissociates into its separate parts of Hydrogen (Cation) and Chlorine (Anion)

Reactions that Form Precipitates When the solutes mixed with the aqueous solvent have a solid product (precipitate) 2 AgNO3(aq) + MgBr2 → 2 AgBr(s) + Mg(NO3)2(aq) AB(aq) + CD(aq)  AD + CB AB = Cation + Anion (in water) CD = Cation + Anion (in water) AD = Cation + Anion CB = Cation + Anion Use the Solubility Rules to determine if solid or aqueous

Solubility Rules for Ionic Compounds in Aqueous Solutions All Salts of Group 1A are soluble All Nitrates are Soluble Chlorate, perchlorate and acetate are soluble Majority of Chlorides, Bromides and Iodides are soluble. The exceptions are those made with Silver, Lead and Mercury. The majority of Sulfates are soluble. The exceptions include barium, lead and strontium. The majority of carbonates are insoluble. The exceptions are NH4+ and those of Group 1A. The majority of hydroxides are insoluble. The exceptions are Barium, Strontium and the slightly insoluble Calcium and those of Group 1A. The majority of Sulfides are insoluble. The exceptions are NH4+ and those of Group 1A and 2A.

Reactions that Form Precipitates The majority of reactions within an aqueous solution are ionic The ions completely dissociate into their separate identities NaOH might become Na+ and OH- Complete Ionic Equation: An ionic equation that shows al of the particles in a solution as they realistically exist within the solution Spectator Ions: Ions that do not participate in a reaction and are usually not shown in ionic equations.

Three Types of Ionic Equations Complete Ionic Equation: An ionic equation that shows all of the particles in a solution as they realistically exist within the solution Spectator Ions: Ions that do not participate in a reaction and are usually not shown in ionic equations. Net Ionic Equations: Ionic equations that only include the elements that participate in the reaction

Net Ionic Equation Example 2Na+ (aq) + 2OH-(aq) + Cu2+ (aq) + Cl- (aq)  2Na+ (aq) + 2Cl-(aq) + Cu(OH)2(s) NET IONIC EQUATION 2OH-(aq) + Cu2+ (aq)  Cu(OH)2(s)

Reactions that Form Water Double-replacement reaction that occurs in an aqueous solution Water is a product Water molecules produced increase the amount of solvent within a solution HBr (aq) + NaOH (aq)  H2O(l) + NaBr(aq) H+ +Br- (aq) + Na+ + OH- (aq)  H2O(l) + Na+ + Br-(aq) H+ + OH- (aq)  H2O(l)

Reactions that Form Gases Double-replacement reaction that occurs in an aqueous solution Gas is the product Hydrogen gas of some form is often a product 2HI (aq) + Li2S(aq)  H2S(g) + 2LiI(aq) 2H+ + 2I- (aq) + 2Li+ + S2- (aq)  H2S(g) + 2Li+ + 2I-(aq) 2H+ + S2- (aq)  H2S(g)

Combining Reactions into a Single Chemical Equation Overall Equation: The process of combining and representing two reactions into a single chemical equation Process: Reactants of the two reactions are written on the reactant side Products of the two reactions are written on the products side Any substances that are on both sides are crossed out and eliminated. You know have a streamlined equation

Combining Reactions into a Single Chemical Equation 4FeS2 + 11O2  2Fe2O3 + 8SO2  8SO2 + 4O2  8SO3  8SO3 + 8H20  8H2SO4  Reactants Any Duplicates on BOTH Sides of the Eqation Products 4FeS2 + 11O2 SO2 2Fe2O3 + 8SO2 8SO2 + 4O2 SO3 8SO3  8SO3 + 8H20 8H2SO4  4FeS2 + 15O2 + 8H20  2Fe2O3 + 8H2SO4