ap chemistry day 15 - ms. flemingflemingapchem.weebly.com/uploads/2/4/6/5/24658308/ap... · 2020....
TRANSCRIPT
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Monday,October9th,2017
APChemistryDay15
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CW/HWAssignments2. Ch.3NotesPartA10/9
3. Ch.3Packet10/9
PLANNER • Ch.3Packet• StudyCh.3+Ch.5• TurninUnitLogs• WriteunitstandardsforUnit3
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EssenMalknowledgestandards• 1.A.1:MoleculesarecomposedofspecificcombinaMonsofatoms;differentmoleculesare
composedofcombinaMonsofdifferentelementsandofcombinaMonsofthesameelementsindifferingamountsandproporMons
• 1.A.2:ChemicalanalysisprovidesamethodfordeterminingtherelaMvenumberofatomsinasubstance,whichcanbeusedtoidenMfythesubstanceordetermineitspurity
• 1.A.3:ThemoleisthefundamentalunitforcounMngnumbersofparMclesonthemacroscopiclevelandallowsquanMtaMveconnecMonstobedrawnbetweenlaboratoryexperiments,whichoccuratthemacroscopiclevel,andchemicalprocesses,whichoccurattheatomiclevel
• 1.D.2:AnearlymodeloftheatomstatedthatallatomsofanelementareidenMcal.Massspectrometrydatademonstrateevidencethatcontradictsthisearlymodel.
• 1.E.1:Physicalandchemicalprocessescanbedepictedsymbolically;whenthisisdone,theillustraMonmustconserveallatomsofalltypes.
• 1.E.2:ConservaMonofatomsmakesitpossibletocomputethemassesofsubstancesinvolvedinphysicalandchemicalprocesses.ChemicalprocessesresultintheformaMonofnewsubstances,andtheamountofthesedependsonthenumberandthetypesandmassesofelementsinthereactants,aswellastheefficiencyofthetransformaMon.
• 3.A.1:Achemicalchangemayberepresentedbyamolecular,ionic,ornetionicequaMon.
• 3.A.2:QuanMtaMveinformaMoncanbederivedfromstoichiometriccalculaMonsthatuMlizethemoleraMosfromthebalancedchemicalequaMons.Theroleofstoichiometryinreal-worldapplicaMonsisimportanttonote,sothatitdoesnotseemtobesimplyanexercisedoneonlybychemists.
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FLT• Iwillbeableto:– ConnectthenumberofparMcles,moles,mass,andvolumeofsubstancestooneanother,bothqualitaMvelyandquanMtaMvely
– ExpressthelawofconservaMonofmassquanMtaMvelyandqualitaMvelyusingsymbolicrepresentaMonsandparMculatedrawings
– ApplyconservaMonofatomstotherearrangementofatomsinvariousprocesses
– TranslateanobservedchemicalchangeintoabalancedchemicalequaMonandjusMfythechoiceofequaMontypeintermsofuMlityforthegivencircumstances
– UsestoichiometriccalculaMonstopredicttheresultsofperformingareacMoninthelaboratoryand/ortoanalyzedeviaMonsfromtheexpectedresults
– RelatequanMMestoidenMfystoichiometricrelaMonshipsforareacMon,includingsituaMonsinvolvinglimiMngreactantsandreacMonsthathavenotgonetocompleMon
• Bycomple1ngCh.3Notes
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Ch.3:Stoichiometry
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ChemicalQuanMMesReview
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Recall: Units • Whatareourunitsfor…
– Mass?• Grams!
– Volume?• Liters!
– Amount?• Moles!
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What is the mole?
We�re not talking about this kind of mole!
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The Mole § Mole (mol) = amount = defined as
the # of carbon atoms in exactly 12 g of carbon-12.
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Moles (is abbreviated: mol) § 1 mole = 6.022 x
1023 particles or atoms or molecules
§ Avogadro’s Number = 6.022 x 1023
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Similar Words for an amount § Just like a dozen is 12, or a pair is
two, a mole is an amount. § One dozen eggs = 12 eggs § One mole of eggs = 6.022 x 1023
eggs
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Figure3.4-One-MoleSamplesofSeveralElements
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Table3.1-Comparisonof1MoleSamplesofVariousElements
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Moles (is abbreviated: mol) § Writing conversions: mol à
particles
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Types of questions ■ Howmanyoxygenatomsinthefollowing?CaCO3Al2(SO4)3
3 atoms of oxygen
12 atoms of oxygen
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Ex/ § How many molecules of CO2 are
in 4.56 moles of CO2?
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Ex/ § How many moles of water is 5.87
x 1022 molecules?
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SampleQuesMon• WhichofthefollowingisthemostaccuratedescripMonofamole?a. Massofcarboninameasuredsampleofcarbon
b. Numberofatomsinanygivenmassofanelement
c. Numberofsodiumionsin58.44gofsodiumchloride
d. AtleasttwooftheseareaccuratedescripMonsofamole
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SampleQuesMon• Whichofthefollowingisclosesttotheaveragemassofoneatomofcopper?a. 63.55g
b. 52.00g
c. 58.93g
d. 65.38g
e. 1.055×10–22g
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MolarMass
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Atomic & Molar Mass § Molar mass = Mass of 1 mole (g/mol) § Allows us to convert from mol ßà g § Ex/ Molar mass of Carbon
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Ex/ § What is the mass of 2.34 moles of
carbon?
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MolarMassforFormulas
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Calculating Formula Mass
Calculate the formula mass of magnesium carbonate, MgCO3.
24.3 g + 12 g + 3 x (16.00 g) = 84.3 g
Thus, 84.3 grams is the formula mass for MgCO3.
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MolarMass• Example
• Calciumcarbonate(CaCO3),alsocalledcalcite,istheprincipalmineralfoundinlimestone,marble,chalk,pearls,andtheshellsofmarineanimalssuchasclamsa. Calculatethemolarmassofcalciumcarbonate
b. Acertainsampleofcalciumcarbonatecontains4.86moles
• Whatisthemassingramsofthissample?
• WhatisthemassoftheCO32–ionspresent?
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MolarMass• SoluMon(a)
• Thus,themassof1moleofCaCO3(1moleofCa2+plus1moleofCO3
2-)is100.09g
• Thisisthemolarmass
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MolarMass• SoluMon(b)• Massof1moleofCaCO3is100.09g
– Samplecontainsnearly5moles,orcloseto500g
– Exactamountisdeterminedasfollows:
• Tofindthemassofcarbonateions(CO32–)presentinthis
sample,realizethat4.86molesofCaCO3contains4.86molesofCa2+ionsand4.86molesofCO3
2–ions
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MolarMass• SoluMon(b)
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MolarMass• Exercise:• Calculatethemolarmassofthefollowingsubstances:
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MolarMass• Exercise:• Whatnumberofnitrogenatomsarepresentin1.00gofeachofthefollowingcompounds?
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SampleQuesMon• Whichofthefollowing100.0-gsamplescontainsthegreatestnumberofatoms?a. Magnesium
b. Zinc
c. Silver
d. Calcium
e. Allsamplescontainthesamenumberofatoms
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SampleQuesMon• Forwhichofthefollowingcompoundsdoes1.0grepresent2.27×10–2mol?a. H2O
b. CO2
c. NH3
d. C2H6
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SampleQuesMon• Massof0.82molofadiatomicmoleculeis131.3g
– IdenMfythemolecule
a. F2
b. Cl2
c. Br2
d. I2
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SampleQuesMon• Whichofthefollowing100.0-gsamplescontainsthegreatestnumberofoxygenatoms?a. H2O
b. N2O
c. C3H6O2
d. CO2
e. Allofthesampleshavethesamenumberofoxygenatoms
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Recall
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MassSpectrometer• Helpstoaccuratelycomparethemassesofatoms
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MassSpectrometer
• Helpsdetermineaccuratemassvaluesforindividualatoms
• DeterminestheisotopiccomposiMonofnaturalelements
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AverageAtomicMass
• Knownasatomicweight(asperIUPAC’sdeclaraMon),whichisdimensionlessbycustom– IUPAC-InternaMonalUnionofPureandAppliedChemistry
• Sinceelementsoccurinnatureasmixturesofisotopes,atomicmassesareusuallyaveragevalues
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SampleQuesMon
• Ex/TheatomicnumberofIndiumis49anditsatomicmass114.8g– Naturallyoccurringindiumcontainsamixtureofindium-112andindium-115,respecMvely,inanatomicraMoofapproximately:
a. 6:94
b. 25:75
c. 50:50
d. 75:25
e. 94:6
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SampleQuesMon• Ex/Youhaveasampleofzinc(Zn)andasampleofaluminum(Al)– Eachsamplecontainsthesamenumberofatoms
– Whichofthefollowingstatementsconcerningthemassesofthesamplesistrue?a. Massofthezincsampleismorethantwiceasgreatasthe
massofthealuminumsample
b. Massofthezincsampleismorethanthemassofthealuminumsample,butitisnottwiceasgreat
c. Massofthealuminumsampleismorethantwiceasgreatasthemassofthezincsample
d. Massofthealuminumsampleismorethanthemassofthezincsample,butitisnottwiceasgreat
e. Massesofthetwosamplesareequal
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PercentComposiMon
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PercentComposiMon• WaystoDescribeaCompound’sComposiMon:
• Intermsofthenumbersofthecompound’sconsMtuentatoms
• Intermsofmasspercent(weightpercent)
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PercentComposiMon• Ex/CalculaMngMassPercent
• Carvoneisasubstancethatoccursintwoformshavingdifferentarrangementsoftheatomsbutthesamemolecularformula(C10H14O)andmass– OnetypeofcarvonegivescarawayseedstheircharacterisMcsmell,andtheothertypeisresponsibleforthesmellofspearmintoil
• Computethemasspercentofeachelementincarvone
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PercentComposiMon• Ex/CalculaMngMassPercent-SoluMon
• Wherearewegoing?– Tofindthemasspercentofeachelementincarvone
– Whatdoweknow?• MolecularformulaisC10H14O
– WhatinformaMondoweneedtofindthemasspercent?• Massofeachelement(we’lluse1moleofcarvone)
• Molarmassofcarvone
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PercentComposiMon• Ex/CalculaMngMassPercent-SoluMon
• Howdowegetthere?– Determinethemassofeachelementin1moleofC10H14O
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PercentComposiMon• Ex/CalculaMngMassPercent-SoluMon
– WhatisthemolarmassofC10H14O?
– Whatisthemasspercentofeachelement?• FindthefracMonofthetotalmasscontributedbyeachelementandconvertittoapercentage
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PercentComposiMon• Ex/CalculaMngMassPercent-SoluMon
• Realitycheck– Individualmasspercentvaluesshouldtotalto100%withinround-offerrors
• Inthiscase,percentagesaddupto100%
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PercentComposiMon• TryThese:• CalculatethepercentcomposiMonbymassofthefollowingcompoundsthatareimportantstarMngmaterialsforsyntheMcpolymers:a. C3H4O2(acrylicacid,fromwhichacrylicplasMcsare
made)
b. C4H6O2(methylacrylate,fromwhichPlexiglasismade)
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SampleProblem• Whichofthefollowing100.0-gsamplescontainsthehighestpercentoxygenbymass?a. H2O
b. N2O
c. C3H6O2
d. CO2
e. Allofthesampleshavethesamepercentoxygenbymass
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DeterminingtheFormulaofaCompound
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DeterminingtheFormulaofaCompound
• Weighthesampleofthecompoundby:– DecomposingthesampleintoitsconsMtuentelements
– ReacMngitwithoxygen• ResulMngsubstancesarethencollectedandweighed– ThistypeofanalysisisdonebyacombusMondevice
– Resultsofsuchanalysesprovidethemassofeachtypeofelementinthecompound,whichcanbeusedtodeterminethemasspercentofeachelement
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DeterminingtheFormulaofaCompound
• CombusMonDevice
• Usedtoanalyzesubstancesforhydrogenandcarbon
• Helpsdeterminethemasspercentofeachelementinacompound
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DeterminingtheFormulaofaCompound
• EmpiricalFormula
• Anymoleculethatcanberepresentedas(CH5N)nhastheempiricalformulaCH5N– n-Integer– Molecularformula:Exactformulaofthemoleculespresentinasubstance
• Molecularformula=(empiricalformula)n• Requirestheknowledgeofthemolarmass
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DeterminingtheFormulaofaCompound
EmpiricalFormula�HowtoSolve1. Assumeyouhave100gofyoursubstance(since
masspercentagegivesthenumberofgramsofaparMcularelementper100gofcompound)
– Eachpercentwillthenrepresentthemassingramsofthatelement
2. Determinethenumberofmolesofeachelementpresentin100gofcompoundusingtheatomicmassesoftheelementspresent
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DeterminingtheFormulaofaCompound
EmpiricalFormula�HowtoSolve3. Divideeachvalueofthenumberofmolesbythe
smallestofthevalues– IfeachresulMngnumberisawholenumber(arerappropriaterounding),thesenumbersrepresentthesubscriptsoftheelementsintheempiricalformula
– Ifthenumbersobtainedarenotwholenumbers,mulMplyeachnumberbyanintegersothattheresultsareallwholenumbers
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DeterminingtheFormulaofaCompound
MolecularFormula:1. Obtaintheempiricalformula
2. Calculatethemassoftheempricalformula
3. CalculatetheraMo:n=MolarMass/EmpiricalFormulaMass
• Integerfromtheprevioussteprepresentsthenumberofempiricalformulaunitsinonemolecule
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DeterminingtheFormulaofaCompound• Example
• Awhitepowderisanalyzedandfoundtocontain43.64%phosphorusand56.36%oxygenbymass– Compoundhasamolarmassof283.88g/mol
• Whatarethecompound’sempiricalandmolecularformulas?
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DeterminingtheFormulaofaCompound• Example–SoluMon
• Assume100g• MassofP=43.64g
• MassofO=56.36g
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DeterminingtheFormulaofaCompound• Example-SoluMon
– Whatarethemolesofeachelementin100.00gofcompound?
– Whatistheempiricalformulaforthecompound?• Dividingeachmolevaluebythesmalleronegives
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DeterminingtheFormulaofaCompound• Example-SoluMon
• Sincewehave1Pand2.5O,wemulMplyby2togetwholenumbers
• Thisgivesus2Pand5O• SoourempiricalformulaisP2O5
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DeterminingtheFormulaofaCompound• Whatisthemolecularformula?
– Whatisthemolecularformulaforthecompound?• Comparetheempiricalformulamasstothemolarmass
• Molecularformulais(P2O5)2,orP4O10
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SampleProblem• EmpiricalformulaofstyreneisCH;itsmolarmassis104.1g/mol– Whatisthemolecularformulaofstyrene?
a. C2H4
b. C8H8
c. C10H10
d. C6H6
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SampleProblem:• Acompoundcontains47.08%carbon,6.59%hydrogen,and46.33%chlorinebymass– Molarmassofthecompoundis153g/mol
• Whataretheempiricalandmolecularformulasofthecompound?
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Mole�VolumeRelaMonship
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Mole-Volume Relationship § Volume may be affected by
§ (1) Temperature § (2) Pressure
§ Consequently, we need to compare gases at a constant temperature and pressure for consistency
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Mole-Volume Relationship § Standard
Temperature and Pressure (STP): § 1 atm of
pressure and 273 K (0°C)
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Mole-Volume Relationship § Molar Volume:
§ At STP, 1 mole of any gas occupies a volume of 22.4 L
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SampleProblems
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Example § What is the volume of 4.59 mole of
CO2 gas at STP?
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Recall § Density = mass/volume (g/L)
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Example § The density of a gas is 1.964 g/L
at STP. What is the molar mass of the gas?
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CHEMICALEQSREVIEW
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Chemical Equations • Chemical Equation = Shorthand for a
chemical rxn using formulas and symbols
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Chemical Equations
• There are two parts to a reaction: 1. Reactants = substances you start
with 2. Products = substances you end up
with
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Symbols • à = “yields” or “reacts to form”
Reactants à Products
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Symbols • + = “and”
Cu + Cl2 à CuCl2
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Symbols • States of matter = indicated with
subscripts (s), (l), (g), or (aq)
2H2(g) + O2(g) à 2H2O(l)
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Symbols • aq = aqueous = dissolved in water
NaCl(aq) à Na+ + Cl-
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Symbols • Double arrow = reversible rxn
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Symbols • Others: Heat (Δ), energy, and
catalysts can be indicated on arrows
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Symbols • A catalyst is a substance that is
added to speed up a reaction, but is not used or consumed by the reaction
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WriMngEquaMons
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Writing Equations • Ex 1/ Bromine and potassium iodide
react to form potassium bromide and iodine
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***NOTE*** • Diatomic gases =
H, N, O, F, Cl, Br, I • Write as diatomic if
they are by themselves in a chemical equation
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Writing Equations • Ex 2/ Iron and oxygen react to form
iron (III) oxide
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Now, read these equations:
Fe(s)+O2(g)→Fe2O3(s)
Cu(s)+AgNO3(aq)→Ag(s)+Cu(NO3)2(aq)
NO2(g)N2(g)+O2(g)→
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ConservaMonofMass
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Law of Conservation of Mass • Law of Conservation of Mass =
mass in a closed system can neither be created nor destroyed
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Law of Conservation of Mass • What does this mean for us?
– In a balanced chemical equation, the number and kinds of atoms on each side of the equation should be equal.
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Law of Conservation of Mass
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Balancing Equations • A balanced equation has the same
number of each element on both sides of the equation
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Balancing Equations • We use coefficients to indicate
multiples of molecules or compounds
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Balancing Equations • Coefficients are multiples of the
entire formula • How does this affect each atom?
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Coefficients • How many of each type of atom? 1. 3H2O 2. 2NO3 3. 3Ca(NO3)2
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Rules 1. Write out correct formulas (if not
already written) Ex/ Li + H3PO4 à H2 + Li3PO4
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Rules 2. Count the # of atoms of each type on both sides
– If possible, keep polyatomic ions together
Ex/ Li + H3PO4 à H2 + Li3PO4
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Rules 3. Balance the elements one at a time by adding coefficients in front.
à Generally, balance H, O, & monatomic atoms last
Ex/ Li + H3PO4 à H2 + Li3PO4
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Rules 4. Double-check ��always Ex/ Li + H3PO4 à H2 + Li3PO4
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Rules Never’s: • Never add or change subscripts on
formulas • Never put a coefficient in the middle of a
formula
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Try These: • AgNO3+Cu→Cu(NO3)2+Ag
• Mg+N2→Mg3N2
• P+O2→P4O10
• CH4+O2→CO2+H2O
• C3H8 + O2 à H2O + CO2
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CW • Ch.3Packet