Predicting Reactions Predicting Reactions

Presented byPresented byMr. Mark LangellaMr. Mark Langella

AP Chemistry Instructor AP Chemistry Instructor College Board ConsultantCollege Board Consultant

Why do the reactions occur?Why do the reactions occur?

Gibbs Free Energy drives the Gibbs Free Energy drives the Spontaneous reactionsSpontaneous reactions Lower PE energyLower PE energy Formation of Stronger BondsFormation of Stronger Bonds Greater Entropy ( Formation of Gases)Greater Entropy ( Formation of Gases)

SolubilitySolubility Formation ConstantFormation Constant

Ways of Expressing Ways of Expressing CHEMICAL EQUATIONS CHEMICAL EQUATIONS

Word equationWord equation In word equations, the names of the In word equations, the names of the

reactants and products are written out. reactants and products are written out. The following example is a word equation:The following example is a word equation:

carbon + oxygen carbon dioxidecarbon + oxygen carbon dioxide

Formula equationsFormula equations Formula equations consist of formulas Formula equations consist of formulas

substituted for the names in the word substituted for the names in the word equation. The reaction above becomesequation. The reaction above becomes

C + OC + O22 CO CO22

Ionic equationsIonic equations In ionic equations, all water soluble compounds In ionic equations, all water soluble compounds

in an aqueous solution are separated into ions.in an aqueous solution are separated into ions. 2NaI2NaI(aq)(aq) + Pb(NO + Pb(NO33))22(aq) (aq) 2NaNO 2NaNO33(aq) + PbI(aq) + PbI22(s)(s)

2Na2Na++(aq) + 2I(aq) + 2I--(aq) + Pb(aq) + Pb2+2+(aq) + 2NO(aq) + 2NO33-(aq) -(aq) 2Na2Na++(aq) + 2NO(aq) + 2NO33--(aq)(aq) + PbI + PbI22(s)(s)

Spectator ionsSpectator ions - Spectator ions do not participate in the - Spectator ions do not participate in the chemical reaction. That is, they are identical on both chemical reaction. That is, they are identical on both sides of the equation.sides of the equation.

Net ionic equationsNet ionic equations The net ionic equation contains all of the The net ionic equation contains all of the

particles in the ionic equation less any particles in the ionic equation less any spectator ions.spectator ions.

2Na2Na++(aq) + 2I(aq) + 2I--(aq) + Pb(aq) + Pb2+2+(aq) + 2NO(aq) + 2NO33--(aq) 2Na(aq) 2Na++(aq) + 2NO(aq) + 2NO33

--(aq) + (aq) +

PbIPbI22(s)(s)

PbPb2+2+(aq) + 2I(aq) + 2I--(aq) PbI(aq) PbI22(s)(s)

ExamplesExamples 1. A strip of magnesium metal is added to an aqueous solution of 1. A strip of magnesium metal is added to an aqueous solution of

silver nitrate.silver nitrate.        Question: Which substance is oxidized in the reaction?        Question: Which substance is oxidized in the reaction?

2. Solid potassium chlorate is strongly heated.2. Solid potassium chlorate is strongly heated.        Question: What is the oxidation number of chlorine before and         Question: What is the oxidation number of chlorine before and after the reaction occurs?after the reaction occurs?

3. Solid silver chloride is added to a solution of concentrated 3. Solid silver chloride is added to a solution of concentrated hydrochloric acid to form a complex ion.hydrochloric acid to form a complex ion.        Question: Which species acts as a Lewis base in the reaction?         Question: Which species acts as a Lewis base in the reaction?  Explain. Explain.

4.  A solution of ethanoic (acetic) acid is added to a solution of 4.  A solution of ethanoic (acetic) acid is added to a solution of barium hydroxide.barium hydroxide.        Question: Explain why a mixture of equal volumes of equimolar         Question: Explain why a mixture of equal volumes of equimolar solutions of acetic acid and barium hydroxide is basic.solutions of acetic acid and barium hydroxide is basic.

ExamplesExamples 5. Ammonia gas is bubbled into a solution of hydrofluoric 5. Ammonia gas is bubbled into a solution of hydrofluoric

acid.acid.        Question: Identify a conjugate acid-base pair in the         Question: Identify a conjugate acid-base pair in the reaction.reaction.

6. Zinc metal is placed into a solution of copper (II) 6. Zinc metal is placed into a solution of copper (II) sulfate.sulfate.        Question: Describe the change in color that the         Question: Describe the change in color that the original solution undergoes as the reaction proceeds.original solution undergoes as the reaction proceeds.

7. Hydrogen phosphide (phosphine) gas is added to 7. Hydrogen phosphide (phosphine) gas is added to boron trichloride gas.boron trichloride gas.        Question: Which species acts as a Lewis acid in the         Question: Which species acts as a Lewis acid in the reaction? Explain.reaction? Explain.

ExamplesExamples

8. A solution of nickel (II) bromide is added 8. A solution of nickel (II) bromide is added to a solution of potassium hydroxide.to a solution of potassium hydroxide.        Question: Identify the spectator ions         Question: Identify the spectator ions in the reaction mixture.in the reaction mixture.

9. Hexane is combusted in air.9. Hexane is combusted in air.        Question: When one molecule of         Question: When one molecule of hexane is completely combusted, how hexane is completely combusted, how many molecules of products are formed?many molecules of products are formed?

BalancingBalancing

We were reminded (especially by the We were reminded (especially by the combustion reaction above) that the coefficients combustion reaction above) that the coefficients used for balancing should be the lowest possibleused for balancing should be the lowest possibleWHOLE NUMBER coefficients.  WHOLE NUMBER coefficients.  

All other rules for the balanced equations are the All other rules for the balanced equations are the same - omit spectator ions, assume a reaction same - omit spectator ions, assume a reaction occurs, write the formulas for molecular occurs, write the formulas for molecular compounds (e.g. HF) as undissociated species compounds (e.g. HF) as undissociated species in solution, etc.in solution, etc.

Synthesis or Combination Synthesis or Combination ReactionsReactions

In synthesis or combination reactions, two In synthesis or combination reactions, two or more substances combine together to or more substances combine together to form a single product.form a single product.

The general form is A + B CThe general form is A + B C The products must contain only those The products must contain only those

elements found in the reactants.elements found in the reactants.

Metal + Nonmetal SaltMetal + Nonmetal Salt

Magnesium ribbon is burned in oxygenMagnesium ribbon is burned in oxygen

A strip of magnesium metal is heated A strip of magnesium metal is heated strongly in pure nitrogen gasstrongly in pure nitrogen gas

Online DemosOnline Demos Reaction of Magnesium and OxygenReaction of Magnesium and Oxygen http://boyles.sdsmt.edu/magburn/magnesium_burning.htmhttp://boyles.sdsmt.edu/magburn/magnesium_burning.htm Reaction of Iron and SulfurReaction of Iron and Sulfur http://www.pc.chemie.uni-siegen.de/pci/versuche/english/v21-1.htmlhttp://www.pc.chemie.uni-siegen.de/pci/versuche/english/v21-1.html Reaction of Potassium and OxygenReaction of Potassium and Oxygen http://neon.chem.ox.ac.uk/vrchemistry/FilmStudio/alkalimetals/HTML/page08.hthttp://neon.chem.ox.ac.uk/vrchemistry/FilmStudio/alkalimetals/HTML/page08.ht

mm

Reaction of Lithium and OxygenReaction of Lithium and Oxygen http://neon.chem.ox.ac.uk/vrchemistry/FilmStudio/alkalimetals/HTML/http://neon.chem.ox.ac.uk/vrchemistry/FilmStudio/alkalimetals/HTML/

page02.htmpage02.htm Reaction of Lithium and ChlorineReaction of Lithium and Chlorine http://neon.chem.ox.ac.uk/vrchemistry/FilmStudio/alkalimetals/HTML/http://neon.chem.ox.ac.uk/vrchemistry/FilmStudio/alkalimetals/HTML/

page04.htmpage04.htm Reaction of Sodium and OxygenReaction of Sodium and Oxygen http://neon.chem.ox.ac.uk/vrchemistry/FilmStudio/alkalimetals/HTML/http://neon.chem.ox.ac.uk/vrchemistry/FilmStudio/alkalimetals/HTML/

page05.htmpage05.htm Reaction of Zinc and SulfurReaction of Zinc and Sulfur http://boyles.sdsmt.edu/znsulf/zincsul.htmhttp://boyles.sdsmt.edu/znsulf/zincsul.htm

Nonmetal + Nonmetal Molecular Nonmetal + Nonmetal Molecular compoundscompounds

Pure Solid Phosphorus (White Form) is Pure Solid Phosphorus (White Form) is burned in airburned in air

Reaction of Phosphorus and ChlorineReaction of Phosphorus and Chlorine WebsiteWebsite: :

http://boyles.sdsmt.edu/pwithcl/reaction_ofhttp://boyles.sdsmt.edu/pwithcl/reaction_of_white_phosphorus_and.htm_white_phosphorus_and.htm

Reaction of Hydrogen and Reaction of Hydrogen and OxygenOxygen

HydridesHydrides

Preparation of the Group 1 hydridesPreparation of the Group 1 hydrides These are made by passing hydrogen gas These are made by passing hydrogen gas

over the heated metal. For example, for over the heated metal. For example, for lithium hydride:lithium hydride:

2Li 2Li (s)(s) + H + H2(g)2(g) 2LiH 2LiH

Nonmetal Oxide + Water OxyacidNonmetal Oxide + Water Oxyacid

Oxy Acid= Contains H+ ions attached to Oxy Acid= Contains H+ ions attached to common Polyatomic ion of Nonmetal common Polyatomic ion of Nonmetal Oxide plus one more oxygenOxide plus one more oxygen

Solid dinitrogen pentoxide is added to Solid dinitrogen pentoxide is added to waterwater

Sulfur trioxide gas is bubbled into water Sulfur trioxide gas is bubbled into water

Phosphorus(V) oxide powder is sprinkled Phosphorus(V) oxide powder is sprinkled over dis tilled waterover dis tilled water

Sulfur dioxide gas is bubbled into distilled Sulfur dioxide gas is bubbled into distilled waterwater

Metal oxide + water metal hydroxideMetal oxide + water metal hydroxide

Solid Cesium Oxide is added to waterSolid Cesium Oxide is added to water

Solid sodium oxide is added to distilled waterSolid sodium oxide is added to distilled water

Powdered strontium oxide is added to distilled Powdered strontium oxide is added to distilled waterwater

Calcium oxide powder is added to distilled waterCalcium oxide powder is added to distilled water

Solid barium oxide is added to distilled waterSolid barium oxide is added to distilled water

DemoDemo

CmdCmd NaNa22OO MgOMgO AlAl33OO22 SiOSiO22 PP44OO1010 SOSO33 ClCl22OO77

%Ionic%Ionic 7979 6868 5656 4545 3232 1717 22

SolidSolid IonicIonic IonicIonic IonicIonic NetworkNetwork MolecularMolecular MolecularMolecular MolecularMolecular

Hydroxide Hydroxide FormulaFormula

NaOHNaOH Mg(OH)Mg(OH)22 Al(OH)Al(OH)33 Si(OH)Si(OH)44 OP(OH)OP(OH)33 OO22S(OH)S(OH)22 OO33Cl(OH)Cl(OH)

FormulaFormula SiOSiO22+2H+2H22OO HH33POPO44 HH22SOSO44 HClOHClO33

Very Very BasicBasic

BasicBasic Ampho.Ampho. Slightly Slightly acidicacidic

AcidicAcidic Stronger Stronger AcidAcid

Very AcidicVery Acidic

Hydrogen-Nonmetal + Water Acidic SolutionHydrogen-Nonmetal + Water Acidic Solution

Hydrogen Chloride gas bubbled into waterHydrogen Chloride gas bubbled into water

Metal oxide + nonmetal oxide metal ion attached to common Metal oxide + nonmetal oxide metal ion attached to common polyatomic ionpolyatomic ion

Metal oxide + carbon dioxide metal Metal oxide + carbon dioxide metal carbonatecarbonate

Carbon dioxide gas is passed over hot, solid Carbon dioxide gas is passed over hot, solid sodium oxide sodium oxide

Metal oxide + sulfur dioxide Metal Metal oxide + sulfur dioxide Metal sulfitesulfite

Sulfur Dioxide is passed over solid calcium oxideSulfur Dioxide is passed over solid calcium oxide

DECOMPOSITION REACTIONSDECOMPOSITION REACTIONS

Substances break down by means of Substances break down by means of decomposition reactionsdecomposition reactions

The general form of a decomposition The general form of a decomposition reaction isreaction is

C A + BC A + B Decomposition reactions are the opposite Decomposition reactions are the opposite

of combination or synthesis reactionsof combination or synthesis reactions

Decomposition of Metal CarbonateDecomposition of Metal Carbonate

Heating a metal carbonate always yields Heating a metal carbonate always yields the metal oxide and carbon dioxide.the metal oxide and carbon dioxide.

MCOMCO33 MO + CO MO + CO22

Powdered magnesium carbonate is Powdered magnesium carbonate is heated strongly heated strongly

Solid calcium carbonate is strongly heatedSolid calcium carbonate is strongly heated

Metal Hydrogen Carbonate Metal Hydrogen Carbonate DecompositionDecomposition

Heating a metal bicarbonate gives the Heating a metal bicarbonate gives the metal oxide, carbon dioxide, and water.metal oxide, carbon dioxide, and water.

MHCOMHCO33 MO + H MO + H22O + COO + CO22

http://www.chemguide.co.uk/inorganic/http://www.chemguide.co.uk/inorganic/group1/compounds.htmlgroup1/compounds.html

Solid Sodium Hydrogen Carbonate is Solid Sodium Hydrogen Carbonate is strongly heatedstrongly heated

Heating the nitratesHeating the nitrates

Most nitrates tend to decompose on heating to give the metal oxide, Most nitrates tend to decompose on heating to give the metal oxide, brown fumes of nitrogen dioxide, and oxygen.brown fumes of nitrogen dioxide, and oxygen.

For example, a typical For example, a typical Group 2 nitrateGroup 2 nitrate like magnesium nitrate like magnesium nitrate decomposes like this:decomposes like this:

In In Group 1Group 1, lithium nitrate behaves in the same way - producing , lithium nitrate behaves in the same way - producing lithium oxide, nitrogen dioxide and oxygen.lithium oxide, nitrogen dioxide and oxygen.

The rest of the Groups, however, don't decompose so completely The rest of the Groups, however, don't decompose so completely (at least not at Bunsen temperatures) - producing the metal nitrite (at least not at Bunsen temperatures) - producing the metal nitrite and oxygen, but no nitrogen dioxide.and oxygen, but no nitrogen dioxide.

2 Mg(NO3)2 = 2 MgO + 2 NO2 + 3 O2

Decomposition of Metal HydroxidesDecomposition of Metal Hydroxides

Heating a metal hydroxide gives the metal Heating a metal hydroxide gives the metal oxide and wateroxide and water

MOH MO + HMOH MO + H22OO

Metal Sulfite DecompositionMetal Sulfite Decomposition

Heating a metal sulfite produces a metal Heating a metal sulfite produces a metal oxide and sulfur dioxideoxide and sulfur dioxide

MSOMSO33 MO + SO MO + SO22

Solid calcium sulfite is heated in a vacuumSolid calcium sulfite is heated in a vacuum

Metal Chlorate DecompositionMetal Chlorate Decomposition

Heating a metal chlorate gives the metal chloride Heating a metal chlorate gives the metal chloride plus oxygen.plus oxygen.

MClOMClO33 MCl + O MCl + O22

Electrolysis of Binary CompoundElectrolysis of Binary Compound

Electrolysis of a molten salt (ionic Electrolysis of a molten salt (ionic compound) separates the substance into compound) separates the substance into its elements.its elements.

MN M + NMN M + N

Ammonium Compound Ammonium Compound DecompositionDecomposition

Ammonium Ammonium CarbonatesCarbonates

Solid ammonium Solid ammonium carbonate is heatedcarbonate is heated

Ammonium HydroxideAmmonium Hydroxide

4 3 2NH OH NH + H O

(NH4)2CO3 = 2NH3 + 2CO2 + H2O

2007 Questions2007 Questions

(NH4)2CO3 = 2NH3 + 2CO2 + H2O

Peroxide DecompositionPeroxide Decomposition

Elephant’s ToothpasteElephant’s Toothpaste WebsiteWebsite: :

http://boyles.sdsmt.edu/tphttp://boyles.sdsmt.edu/tpaste/elephants.htmaste/elephants.htm

Genie in a Bottle DemoGenie in a Bottle Demo WebsiteWebsite: :

http://boyles.sdsmt.edu/ghttp://boyles.sdsmt.edu/geniebot/genie.htmeniebot/genie.htm

Reactions Based on Reduction Potentials Reactions Based on Reduction Potentials EMF PotentialEMF Potential

Reduction and OxidationReduction and Oxidation Single replacementSingle replacement

Cation ReplacementCation Replacement

There are two types of single replacement There are two types of single replacement reactions, in one, a metal or hydrogen reactions, in one, a metal or hydrogen replaces a positive ionreplaces a positive ion

MM00 + A + A++BB-- M M++BB-- + A + A00

Replacement of HydrogenReplacement of Hydrogen Reaction of Magnesium and Different Concentrations of AcidsReaction of Magnesium and Different Concentrations of Acids WebsiteWebsite: :

http://boyles.sdsmt.edu/kinetic/mercadokinetics.htmhttp://boyles.sdsmt.edu/kinetic/mercadokinetics.htm Hydrochloric Acid(g) + Magnesium(s) Hydrochloric Acid(g) + Magnesium(s) Magnesium(II)Chloride(aq) Magnesium(II)Chloride(aq)

+ Hydrogen(g)+ Hydrogen(g) 2HCl(g) + Mg(s) 2HCl(g) + Mg(s) MgCl MgCl22(aq) + H(aq) + H22(g)(g)

Small piece of sodium metal is added to distilled waterSmall piece of sodium metal is added to distilled water WebsiteWebsite: :

http://boyles.sdsmt.edu/sodwat/reaction_of_sodium_and_water.htmhttp://boyles.sdsmt.edu/sodwat/reaction_of_sodium_and_water.htm Sodium(s) + Water(l) Sodium(s) + Water(l) Sodium Hydroxide(aq) + Hydrogen(g) Sodium Hydroxide(aq) + Hydrogen(g) 2Na(s) + 2H2Na(s) + 2H22O(l) O(l) 2NaOH(aq) + H 2NaOH(aq) + H22(g)(g)

) ) Reaction of Potassium and WaterReaction of Potassium and Water WebsiteWebsite: :

http://www.chem.shef.ac.uk/webelements-moov/K_H2O.movhttp://www.chem.shef.ac.uk/webelements-moov/K_H2O.mov Potassium(s) + Water(l) Potassium(s) + Water(l) Potassium Hydroxide(aq) + Hydrogen(g) Potassium Hydroxide(aq) + Hydrogen(g) 2K(s) + 2H2K(s) + 2H22O O 2KOH + H 2KOH + H22(g) (g)

A strip of zinc is added to a solution of 6.0-molar hydrobromic acidA strip of zinc is added to a solution of 6.0-molar hydrobromic acid

Group I with water videoGroup I with water video http://video.google.com/videoplay?docid=-http://video.google.com/videoplay?docid=-

2134266654801392897&q=rubidium+water2134266654801392897&q=rubidium+water

2007 Question2007 Question

Cation ReplacementCation Replacement

Reaction of Zinc and Tin (II) ChlorideReaction of Zinc and Tin (II) Chloride WebsiteWebsite: :

http://www.chemtopics.com/lectures/unit02http://www.chemtopics.com/lectures/unit02/lecture1/displace.htm/lecture1/displace.htm

Zinc(s) + Tin (II) Chloride(aq) Zinc(s) + Tin (II) Chloride(aq) Tin(s) + Tin(s) + Zinc (II) Chloride(aq)Zinc (II) Chloride(aq)

Zn(s) + SnClZn(s) + SnCl22(aq) (aq) Sn(s) + ZnCl Sn(s) + ZnCl22(aq)(aq)

Thermite ReactionThermite Reaction

2Al(s) + Fe2Al(s) + Fe22OO33 (s) (s) Al Al22OO33 (s) + 2Fe(l) (s) + 2Fe(l)

http://boyles.sdsmt.edu/thermite/therm.htmhttp://boyles.sdsmt.edu/thermite/therm.htm http://www2.chemie.uni-erlangen.de/http://www2.chemie.uni-erlangen.de/

education/medprak/videos/thermit_v.mpgeducation/medprak/videos/thermit_v.mpg

A solution of copper (II) sulfate is spilled onto a A solution of copper (II) sulfate is spilled onto a sheet of freshly polished aluminum metal.sheet of freshly polished aluminum metal.

Bar of strontium metal is immersed in a 1.0 M Bar of strontium metal is immersed in a 1.0 M copper (II) nitrate solution. copper (II) nitrate solution.

A piece of copper wire is placed in a solution of A piece of copper wire is placed in a solution of silver nitratesilver nitrate

A small piece of calcium metal is added to hot A small piece of calcium metal is added to hot distilled waterdistilled water

A solution of tin (II) nitrate is added to a solution A solution of tin (II) nitrate is added to a solution of silver nitrateof silver nitrate

A mixture of powdered iron (III) oxide and A mixture of powdered iron (III) oxide and powdered aluminum metal is heat powdered aluminum metal is heat strongly.strongly.

A bar of zinc metal is immersed in a A bar of zinc metal is immersed in a solution of copper (II) sulfatesolution of copper (II) sulfate

A piece of nickel metal is immersed in a A piece of nickel metal is immersed in a solution of copper (II) sulfatesolution of copper (II) sulfate

Solutions of tin (II) chloride and iron (III) Solutions of tin (II) chloride and iron (III) chloride are mixedchloride are mixed

Cu+2 (aq) + Fe(s) Cu+2 (aq) + Fe(s) Cu(s) + Fe+2 Cu(s) + Fe+2

Cu+2 (aq) + Zn(s) Cu+2 (aq) + Zn(s) Cu(s) + Zn+2 Cu(s) + Zn+2

Growing Crystals in Gels are a Growing Crystals in Gels are a great activity you can use to great activity you can use to demonstrate single replacement demonstrate single replacement reactions.reactions.

Solutions:Solutions: 1.1. Saturated Sodium Saturated Sodium

metasilicate- Flinn Scientific (CAT metasilicate- Flinn Scientific (CAT No. S0102) – Needs to be diluted No. S0102) – Needs to be diluted to a density of 1.06 g/ml. About to a density of 1.06 g/ml. About 158 ml of the commercial solution 158 ml of the commercial solution diluted to one liter of solution will diluted to one liter of solution will yield a proper density.yield a proper density.

2.2. Commercial White Commercial White VinegarVinegar

3.3. 1.0 M CuCl2 1.0 M CuCl2 (13.5g/100ml H2O)(13.5g/100ml H2O)

4.4. 1.0 M Pb(NO3)2 1.0 M Pb(NO3)2 (33.1g/100ml H2O)(33.1g/100ml H2O)

Pb+2(aq) + Zn(s) Zn+2(aq) + Pb(s)

Anion ReplacementAnion Replacement

In the second, a halogen replaces another In the second, a halogen replaces another halogen as the negative ion.halogen as the negative ion.

NN2200 + A + A++BB-- A A++NN-- + B + B22

00

Chlorine gas is bubbled through a solution of Chlorine gas is bubbled through a solution of potassium bromidepotassium bromide

Liquid bromine is shaken with 0.5Liquid bromine is shaken with 0.5MM sodium sodium iodide solutioniodide solution

Chlorine gas is bubbled into a solution of sodium Chlorine gas is bubbled into a solution of sodium bromidebromide

Halogen Replacement Halogen Replacement

To prepare a saturated solution of aqueous bromine, mix equal volumes of 1.28 M NaBr, 1.28 M HCl, and household bleach. Prepare only as much solution as you need to the activity in working fume hood to avoid unnecessary exposure to bromine vapor. There is no need to store the bromine water since it is easily prepared. It may also be helpful to mix the solutions in a clear glass bottle allowing your students to view the color of elemental bromine.

Discussion: Since the solubility of bromine in water at 25EC is 0.214 moles/liter , a saturated

aqueous bromine solution can easily be prepared as needed by mixing equal volumes of a 1.28 M sodium or potassium bromide solution, a 1.28 M hydrochloric acid solution, and common household bleach. The three reagents react according to the equation:

The reaction between bleach and hydrochloric acid produces elemental chlorine The reaction between bleach and hydrochloric acid produces elemental chlorine which then will replace the bromine in sodium bromide producing bromine and which then will replace the bromine in sodium bromide producing bromine and sodium chloride.sodium chloride.

A saturated solution of aqueous chlorine can be prepared in the same fashion. To A saturated solution of aqueous chlorine can be prepared in the same fashion. To prepare 100 ml a saturated aqueous solution of chlorine, mix 1.5 ml of concentrated prepare 100 ml a saturated aqueous solution of chlorine, mix 1.5 ml of concentrated HCl with 13 ml of bleach in 84 ml of water. The solubility of chlorine at 25EC is 0.092 HCl with 13 ml of bleach in 84 ml of water. The solubility of chlorine at 25EC is 0.092 M (2)M (2)

NaClO(aq) 2HCl(aq) Cl (aq) NaCl(aq) H O( )2 2Cl (g) 2NaBr(aq) 2NaCl(aq) Br (aq)2 2

2007 Question2007 Question

Special Red-ox ReactionsSpecial Red-ox Reactions

Hydrogen reacts with hot metallic oxide to Hydrogen reacts with hot metallic oxide to produce the elemental metal and waterproduce the elemental metal and water

Hydrogen gas is passed over hot iron(II) Hydrogen gas is passed over hot iron(II) oxide powderoxide powder

Oxygen react with Metal Sulfides to Oxygen react with Metal Sulfides to produce Metallic Oxides and Sulfur produce Metallic Oxides and Sulfur DioxideDioxide

Copper reacts with Copper reacts with Concentrated Sulfuric Concentrated Sulfuric AcidAcid

Copper Reacts with Copper Reacts with Concentrated Nitric Concentrated Nitric AcidAcid

2 4 4 2 2Cu + 2 H SO CuSO +SO +2 H O

3 3 2 23Cu + 8HNO Cu(NO ) + NO + 4H O

Typical ReactionsTypical Reactions

Oxidation States of ManganeseOxidation States of Manganese

ProcedureProcedure Place 10 ml of a Water into Four Graduated CylindersPlace 10 ml of a Water into Four Graduated Cylinders Place one tablet #1 into each CylinderPlace one tablet #1 into each Cylinder .01 M KMnO.01 M KMnO44 solution is in four small cylinders labeled A solution is in four small cylinders labeled A

, B, N ( Place Tablet 1/10 ml water), B, N ( Place Tablet 1/10 ml water) To Flask A, Add 10 ml of 3M HTo Flask A, Add 10 ml of 3M H22SOSO44

MnOMnO44- + H+- + H+ To Flask B, add 10 ml of 5 M NaOH. To Flask B, add 10 ml of 5 M NaOH. MnOMnO44- + OH-- + OH- To Flask N add nothing.To Flask N add nothing. MnOMnO44--

To Flask A add .01M NaHSO3 ( Tablet 2) slowly To Flask A add .01M NaHSO3 ( Tablet 2) slowly till you get a colorless Mn2+ ion.till you get a colorless Mn2+ ion.

MnOMnO44-- + 5H + 5H+++ HSO+ HSO33

-- 3H 3H22O + 2MnO + 2Mn2+2+ + 5SO + 5SO442-2-

To Flask N add .01M NaHSO3 ( Tablet 2)until a To Flask N add .01M NaHSO3 ( Tablet 2)until a brown precipitate forms.brown precipitate forms.

2MnO2MnO44-- + 3HSO + 3HSO33

- - 3SO 3SO442- 2- + H + H+++ H+ H22O +MnOO +MnO22

To Flask B slowly add .01M NaHSO3 ( Tablet 2) To Flask B slowly add .01M NaHSO3 ( Tablet 2) until a green solution forms.until a green solution forms.

2MnO2MnO44-- + OH + OH--+ HSO+ HSO33

-- 2MnO 2MnO442-2- + 2H + 2H22O + O +

SOSO442-2-

Sulfite ion is readily oxidized to sulfate. On Sulfite ion is readily oxidized to sulfate. On prolonged exposure to air, this oxidation prolonged exposure to air, this oxidation occurs with atmospheric oxygen:occurs with atmospheric oxygen:

2SO2SO3322-(aq) + O-(aq) + O22(g) --> 2SO(g) --> 2SO44

2-2-(aq)(aq) Sulfite or sulfur dioxide will decolorize Sulfite or sulfur dioxide will decolorize

permanganate. This de-colorization serves permanganate. This de-colorization serves as a convenient test for sulfur dioxide:as a convenient test for sulfur dioxide:

2MnO2MnO44--(aq) + 5SO(aq) + 5SO22(g) + 2H(g) + 2H22O(l) --> 5SOO(l) --> 5SO44

2-2-

(aq) + 2Mn(aq) + 2Mn2+2+(aq) + 4H(aq) + 4H++(aq)(aq)

2007 Question2007 Question

) ) Formation of a Silver MirrorFormation of a Silver Mirror WebsiteWebsite: :

http://boyles.sdsmt.edu/agmirror/agmir.hthttp://boyles.sdsmt.edu/agmirror/agmir.htmm

: : Preparing Oxygen from BleachPreparing Oxygen from Bleach WebsiteWebsite: :

http://boyles.sdsmt.edu/prepoxyg/preparatihttp://boyles.sdsmt.edu/prepoxyg/preparation_of_oxygen_gas_from_b.htmon_of_oxygen_gas_from_b.htm

An acidic solution of potassium dichromate is An acidic solution of potassium dichromate is added to a solution of iron (II) nitrate. added to a solution of iron (II) nitrate.

Acidified solutions of potassium permanganate Acidified solutions of potassium permanganate and iron (II) nitrate are mixed togetherand iron (II) nitrate are mixed together

Solution of iron (II) chloride is added to an Solution of iron (II) chloride is added to an acidified solution of sodium dichromateacidified solution of sodium dichromate

A concentrated solution of hydrochloric acid is A concentrated solution of hydrochloric acid is added to solid potassium permanganate.added to solid potassium permanganate.

A solution of potassium dichromate is added to A solution of potassium dichromate is added to an acidified solution of iron(II) chloride.an acidified solution of iron(II) chloride.

A concentrated solution of hydrochloric acid is A concentrated solution of hydrochloric acid is added to solid potassium permanganate.added to solid potassium permanganate.

Solutions of potassium permanganate and Solutions of potassium permanganate and sodium oxalate are mixed.sodium oxalate are mixed.

A solution of sodium bromide is added to an A solution of sodium bromide is added to an acidified solution of potassium bromateacidified solution of potassium bromate

Reactions Driven byReactions Driven by

Solubility and PrecipitationSolubility and Precipitation Formation of Gases ( Increase in entropy)Formation of Gases ( Increase in entropy) Formation of WaterFormation of Water Coordinate Covalent Bond Formation Coordinate Covalent Bond Formation

( Lewis Acid-Base)( Lewis Acid-Base) Formation ConstantsFormation Constants

Formation of WaterFormation of Water

Metal Oxide + an Acid Salt + WaterMetal Oxide + an Acid Salt + Water Metal Hydroxide + an Acid Salt + WaterMetal Hydroxide + an Acid Salt + Water (a special type of reaction called (a special type of reaction called neutralization)neutralization) A 0.1 M nitrous acid solution is added to the A 0.1 M nitrous acid solution is added to the

same volume of a 0.1 M sodium hydroxide same volume of a 0.1 M sodium hydroxide solutionsolution

A 0.02 A 0.02 M M hydrochloric acid solution is mixed with hydrochloric acid solution is mixed with an equal volume of a 0.01 an equal volume of a 0.01 M M calcium hydroxide calcium hydroxide solution.solution.

Lewis Acid-Base Reactions (Coordinate Lewis Acid-Base Reactions (Coordinate Covalent Bond Formation)Covalent Bond Formation)

Ammonia gas is mixed with hydrogen Ammonia gas is mixed with hydrogen chloride gas. chloride gas.

Methylamine gas is bubbled into distilled Methylamine gas is bubbled into distilled waterwater

phosphine (phosphorus trihydride) gas is phosphine (phosphorus trihydride) gas is bubbled into liquid boron trichloridebubbled into liquid boron trichloride

Formation of Gas and WaterFormation of Gas and Water

Metal Carbonate + an Acid Metal Carbonate + an Acid Salt + Salt + Carbon Dioxide + WaterCarbon Dioxide + Water

Hydrogen iodide gas is bubbled into a Hydrogen iodide gas is bubbled into a solution of lithium carbonatesolution of lithium carbonate

Solid zinc carbonate is added to 1.0 M Solid zinc carbonate is added to 1.0 M sulfuric acid.sulfuric acid.

Carbon dioxide and Water- Carbon Carbon dioxide and Water- Carbon Dioxide is easily produced by the reaction Dioxide is easily produced by the reaction of sodium bicarbonate and vinegar.of sodium bicarbonate and vinegar.

2007 Question2007 Question

Metal hydrides + Water Metal Metal hydrides + Water Metal Hydroxide + Hydrogen GasHydroxide + Hydrogen Gas

Solid calcium hydride is added to distilled Solid calcium hydride is added to distilled waterwater

Solid sodium hydride is added to waterSolid sodium hydride is added to water

Metal Bicarbonate (Hydrogen Carbonate) Metal Bicarbonate (Hydrogen Carbonate) ++ an Acid Salt + Carbon Dioxide + an Acid Salt + Carbon Dioxide + WaterWater

Excess hydrobromic acid solution is added Excess hydrobromic acid solution is added to a solution of potassium hydrogen to a solution of potassium hydrogen carbonate.carbonate.

PREDICTIONS BASED ON PREDICTIONS BASED ON SOLUBILITYSOLUBILITY

If one or both of the products in the double If one or both of the products in the double replacement reaction is replacement reaction is insolubleinsoluble in in water, the reaction water, the reaction willwill occur. occur.

SOLUBILITY RULES FOR COMMON IONIC SOLUBILITY RULES FOR COMMON IONIC COMPOUNDS IN WATERCOMPOUNDS IN WATER

1.1. All nitrates, chlorates, and acetates are All nitrates, chlorates, and acetates are soluble soluble in water. Silver in water. Silver acetate is sparingly soluble.acetate is sparingly soluble.

2.2. Most common acids are Most common acids are solublesoluble in water. in water. 3.3. All common IA, and ammonium compounds are All common IA, and ammonium compounds are soluble soluble in water.in water. 4.4. All chlorides, bromides, and iodides are All chlorides, bromides, and iodides are solublesoluble in water except in water except

silver, mercury (I), and lead. HgI2 and HgBr2 are insoluble in water.silver, mercury (I), and lead. HgI2 and HgBr2 are insoluble in water. 5.5. All sulfates are All sulfates are solublesoluble in water except CaSO4, SrSO4, BaSO4, in water except CaSO4, SrSO4, BaSO4,

PbSO4, Hg2SO4. Ag2SO4 is sparingly soluble in water.PbSO4, Hg2SO4. Ag2SO4 is sparingly soluble in water. 6.6. All carbonates, phosphates, oxides, and sulfites are All carbonates, phosphates, oxides, and sulfites are insolubleinsoluble in in

water but soluble in dilute acids except the IA and ammonium compounds. water but soluble in dilute acids except the IA and ammonium compounds. 7.7. The sulfides of all metals are The sulfides of all metals are insolubleinsoluble in water except the IA, IIA, in water except the IA, IIA,

and ammonium sulfides.and ammonium sulfides. 8.8. All hydroxides are All hydroxides are insolubleinsoluble in water except the IA, Ca(OH)2, in water except the IA, Ca(OH)2,

Sr(OH)2, and Ba(OH)2 hydroxides.Sr(OH)2, and Ba(OH)2 hydroxides.

Nonmetal Oxide and Metal Nonmetal Oxide and Metal HydroxideHydroxide

) ) Reaction of Carbon Dioxide and Reaction of Carbon Dioxide and LimewaterLimewater

WebsiteWebsite: : http://boyles.sdsmt.edu/respira/respir.htmhttp://boyles.sdsmt.edu/respira/respir.htm

COCO22(g) + Ca(OH)(g) + Ca(OH)22(aq) (aq) CaCO CaCO33(s) + H(s) + H22O(l)O(l)

A solution of sodium phosphate is added A solution of sodium phosphate is added to a solution of aluminum nitrateto a solution of aluminum nitrate

A solution of potassium phosphate is A solution of potassium phosphate is mixed with a solution of calcium acetatemixed with a solution of calcium acetate

A solution of sodium Iodide is added to a A solution of sodium Iodide is added to a solution of lead (II) acetatesolution of lead (II) acetate

A solution of lead(II) nitrate is added to a A solution of lead(II) nitrate is added to a solution of potassium sulfate. solution of potassium sulfate.

2007 Question2007 Question

Complex Ion FormationComplex Ion Formation

Often an ion in water solution is in a more complex Often an ion in water solution is in a more complex species, in which the ion is bound to several water species, in which the ion is bound to several water molecules molecules

A complex ion consists of a central ion to which are A complex ion consists of a central ion to which are bonded two, four, or six neutral or ionic species bonded two, four, or six neutral or ionic species called ligands called ligands

AMPHOTERICAMPHOTERIC Lead and Zinc form complexes with hydroxide Lead and Zinc form complexes with hydroxide The hydroxides of lead and zinc are soluble in both The hydroxides of lead and zinc are soluble in both

acidic and basic solutions acidic and basic solutions Hydroxides that have this property are called Hydroxides that have this property are called

amphotericamphoteric

Halide complexesHalide complexes

AlAl3+3+ + 6 F + 6 F-  -  <----------> [AlF<----------> [AlF66]]

3-3- 2.5 x 102.5 x 1044

AlAl3+3+ + 4 F + 4 F-  -  <---------->  [AlF<---------->  [AlF44]]

-1-1 2.0 x 102.0 x 1088

  BeBe2+2+ + 4 F + 4 F--  <---------->  [BeF  <---------->  [BeF44]]

2-2- 1.3 x 101.3 x 101313

SnSn4+4+ + 6 F + 6 F--  <---------->  [SnF  <---------->  [SnF66]]

2-2- 1.0 x 101.0 x 102525

CuCu++ + 2 Cl + 2 Cl-  -  <---------->  [CuCl<---------->  [CuCl22]]

-1-1 3.0 x 103.0 x 1055

AgAg++ + 2 Cl + 2 Cl-  -  <---------->  [AgCl<---------->  [AgCl22]]

-1-1 1.8 x 101.8 x 1055

PbPb2+2+ + 4 Cl + 4 Cl-  -  <---------->  [PbCl<---------->  [PbCl44]]

2-2- 2.5 x 102.5 x 101515

ZnZn2+2+ + 4 Cl + 4 Cl-  -  <---------->  [ZnCl<---------->  [ZnCl44]]

2-2- 1.6 1.6 

HgHg2+2+ + 4 Cl + 4 Cl--  <---------->  [HgCl  <---------->  [HgCl44]]

2-2- 5.0 x 105.0 x 101515

CuCu++ + 2 Br + 2 Br--  <---------->  [CuBr  <---------->  [CuBr22]]

-1-1 8.0 x 108.0 x 1055

AgAg++ + 2 Br + 2 Br--  <---------->  [AgBr  <---------->  [AgBr22]]

-1-1 1.0 x 101.0 x 101111

Ammonia complexesAmmonia complexes

AgAg++ + 2 NH + 2 NH33  <---------->    [Ag(NH  <---------->    [Ag(NH

33))22]]++ 1.6 x 101.6 x 1077

ZnZn2+2+ + 4 NH + 4 NH33  <---------->   [Zn(NH  <---------->   [Zn(NH

33))44]]2+2+ 7.8 x 107.8 x 1088

CuCu2+2+ + 4 NH + 4 NH33  <---------->  [Cu(NH  <---------->  [Cu(NH

33))44]]2+2+ 1.1 x 101.1 x 101313

HgHg2+2+ + 4 NH + 4 NH33  <---------->  [Hg(NH  <---------->  [Hg(NH

33))44]]2+2+ 1.8 x 101.8 x 101919

CoCo2+2+ + 6 NH + 6 NH33  <---------->  [Co(NH  <---------->  [Co(NH

33))66]]2+2+ 5.0 x 105.0 x 1044

CoCo3+3+ + 6 NH + 6 NH33  <---------->  [Co(NH  <---------->  [Co(NH

33))66]]3+3+ 4.6 x 104.6 x 103333

CdCd2+2+ + 6 NH + 6 NH33  <---------->  [Cd(NH  <---------->  [Cd(NH

33))66]]2+2+ 2.6 x 102.6 x 1055

NiNi2+2+ + 6 NH + 6 NH33  <---------->   [Ni(NH  <---------->   [Ni(NH

33))66]]2+2+ 2.0 x 102.0 x 1088

Cyanide complexesCyanide complexes

FeFe2+2+ + 6 CN + 6 CN--  <---------->  [Fe(CN)  <---------->  [Fe(CN)66]]

4-4- 1.0 x 101.0 x 102424

FeFe3+3+ + 6 CN + 6 CN--  <---------->  [Fe(CN)  <---------->  [Fe(CN)66]]

3-3- 1.0 x 101.0 x 103131

AgAg++ + 2 CN + 2 CN--  <---------->  [Ag(CN)  <---------->  [Ag(CN)22]]

-1-1 5.3 x 105.3 x 101818

CuCu++ + 2 CN + 2 CN--  <---------->  [Cu(CN)  <---------->  [Cu(CN)22]]

-1-1 1.0 x 101.0 x 101616

CdCd2+2+ + 4 CN + 4 CN--  <---------->  [Cd(CN)  <---------->  [Cd(CN)44]]

2-2- 7.7 x 107.7 x 101616

AuAu++ + 2 CN + 2 CN--  <---------->    <---------->  [Au(CN)[Au(CN)22]]

-1-1 2.0 x 102.0 x 103838

Complexes with other monodentate Complexes with other monodentate ligandsligands

AgAg++ + 2 CH + 2 CH33NHNH

22  <--------->  [Ag(CH  <--------->  [Ag(CH33NHNH

22))22]]+1+1 7.8 x 107.8 x 1066

CdCd2+2+ + 4 SCN + 4 SCN--  <---------->  [Cd(SCN)  <---------->  [Cd(SCN)44]]

2-2- 1.0 x 101.0 x 1033

CuCu2+2+ 2 SCN 2 SCN--  <---------->  [Cu(SCN)  <---------->  [Cu(SCN)22] ]  5.6 x 105.6 x 1033

FeFe3+3+ 3 SCN 3 SCN--  <---------->  [  <---------->  [Fe(SCN)Fe(SCN)33]] 2.0 x 102.0 x 1066

HgHg2+2+ 4 SCN 4 SCN--  <---------->  [Hg(SCN)  <---------->  [Hg(SCN)44]]

2-2- 5.0 x 105.0 x 102121

CuCu2+2+ 4 OH 4 OH--  <---------->  [Cu(OH)  <---------->  [Cu(OH)44]]

2-2- 1.3 x 101.3 x 101616

ZnZn2+2+ 4 OH 4 OH--  <---------->  [Zn(OH)  <---------->  [Zn(OH)44]]

2-2- 2.0 x 102.0 x 102020

Excess concentrated aqueous ammonia is Excess concentrated aqueous ammonia is added to a solution of nickel (II) bromideadded to a solution of nickel (II) bromide

Excess concentrated hydrochloric acid is added Excess concentrated hydrochloric acid is added to a 1.0 M solution of cobalt (II) chlorideto a 1.0 M solution of cobalt (II) chloride

A drop of potassium thiocyanate solution is A drop of potassium thiocyanate solution is added to a solution of iron (III) nitrate.added to a solution of iron (III) nitrate.

Excess concentrated ammonia solution is added Excess concentrated ammonia solution is added to a solution of nickel (II) sulfateto a solution of nickel (II) sulfate

Excess sodium cyanide solution is added to a Excess sodium cyanide solution is added to a solution of silver nitratesolution of silver nitrate

Balancing Red-Ox ReactionsBalancing Red-Ox Reactions

Red-Ox ContinuedRed-Ox Continued

Red-Ox Under Basic ConditionsRed-Ox Under Basic Conditions

Red-Ox continuedRed-Ox continued

OrganicOrganic

Where in The Curriculum?Where in The Curriculum? ThermochemistryThermochemistry StoichiometryStoichiometry Bonding and Molecular StructureBonding and Molecular Structure