AP Chemistry Chapter 89AP化学章89.docx
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AP Chemistry Chapter 89AP化学章89.docx
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APChemistryChapter89AP化学章89
APChemistry:
Chapter8StudentNotes—Bonding
Objectives
☑8.1:
TypesofChemicalBonds
☑8.2:
Electronegativity
☑8.3:
BondPolarityandDipoleMoments
☑8.4:
Ions:
ElectronConfigurationsandSizes
☑8.5:
FormationofBinaryIonicCompounds
☑8.8:
CovalentBondEnergies
☑8.10:
LewisStructures
☑8.11:
ExceptionstotheOctetRule
☑8.12:
Resonance
☑8.13:
VSEPRModelandShapes
☑9.1:
HybridizationandtheLocalizedElectronModel
8.1:
TypesofChemicalBonds
IntroductiontoBondingType
TheKey:
Coulomb’sLaw
Whatholdsthingtogetheris
_______________attraction
IonicBondDiagram
____________ofvalenceelectrons
CovalentBondDiagram
____________ofvalenceelectrons
MetallicBondDiagram
____________ofvalenceelectrons
BondEnergyandBondDistanceofaCovalentBond
8.2:
Electronegativity
Definition
Trend
8.3:
BondPolarityandDipoleMoments
Dipole=
DipoleMoment=
Polarbond=
PolarMolecule
Bondmustbe_________________
Shapemustnot________________
ExamplesofPolarmolecules
H2Oispolar
NH3ispolar
CO2isnotpolar
8.4:
Ions:
ElectronConfigurationsandSizes
Ionshave__________________sizesthan____________________
Cationsofthesameelementare___________________.
Anionsofthesameelementare____________________.
Why?
Drawpictureshereanddiscusselectronsandelectronclouds.
Example1:
Rankthefollowinginorderfromsmallesttolargest:
Na+,Mg2+,Al3+O2-,F-,Ne
8.5:
FormationofBinaryIonicCompounds
Thissectionlooksthattheenergiesinvolvedintheformationofionicbonds
LatticeEnergy:
____________________________________
FortheReaction:
M+(g)+X-(g)MX(s)
Stepstomakethishappen:
Startwiththemetalinit’sstandardstateandtheanioninitsstandardstate:
Eachsteprequiresenergy(orreleasesinsomecases)
Example:
Theformationoflithiumfluoride
8.8:
CovalentBondEnergies
Fourwaystocalculate∆H
1.HessLawversion1:
2.HessLawVersion2:
AddReactionsMethod
3.Calorimetry:
4.BondEnergies:
Thisiswhatthissectionisabout
∆H=BondsBroken–BondsFormed
=Reactantsbonds–ProductsBonds
AQuickLessoninOrganicChemistry—DrawingStructuralFormulas
Chemical
NumberofBonds
Halides+Hydrogen
1
Oxygen,Sulfur
2
Nitrogen,Phosphorous
3
Carbon
4
Examples
CalculatingBondEnergies:
Example1
Calculate∆Hforthefollowingreaction:
CH4(g)+2Cl2(g)+2F2(g)CF2Cl2(g)+2HF(g)+2HCl(g)
Example2:
Calculate∆Hforthefollowingreaction:
5N2O4+4N2H3CH312H2O+9N2+4CO2
Example3:
UsethefollowingstandardenthalpiesofformationtoestimatetheN-Hbondenergyinammonia:
N(g),472.7kJ/mol,H(g),216.0kJ/mol,NH3(g),-46.1kJ/mol.Compareyourvaluetotheoneinthetable.Accountfordifferences.
8.10:
LewisStructures
Definition:
LewisStructure
Definition:
OctetRule
RulesforDrawingLewisStructures
1.Countthetotalnumberofvalenceelectrons(Includingelectronsrelatedtopolyatomicions)
2.Distributeonebondtoallnecessaryconnections
3.Distributepairsofelectronstoexternalatoms
4.Allextraelectronsgoonthecentralatom.
5.Ifnecessaryadddoubleortriplebondstofulfilltheoctetrule.
Examples
8.11:
ExceptionstotheOctetRule
Whathappenswhenyouhavemore/lesselectronsthan8?
Examples
8.12:
Resonance
Definition:
Resonance
Definition:
ResonanceStructures
Examples
FormalCharge
Assignaformalchargetoeachatominamoleculeorionby:
1.NumberofValenceElectronsTypicallyassociatedwiththatatom
2.Subtractthetotalnumberofelectronsaroundthatatom
3.Subtractthenumberofbondsconnectedtothatatom.
TheBeststructureshavetheformalchargesclosesttozeroforallatoms
Example1:
Sulfate
Example2:
HCN
Example3:
ClO3-
8.13:
VSEPRModelandShapes
Shapes=MolecularGeometry=molecularstructure
VSEPR=
Thismeansthatvalenceelectrons__________________________________
Why?
Italldependsonthenumberof“clouds”(effectivepairs)aroundanatom.
Activity:
SpheresandShapes.
MolecularShapes.
APChemistry
Sp
2
LinearDiatomic,UsuallynonpolarCO2,HCN
Rememberthatinmoleculeswheretheoutsidemoleculesaredifferent,shapesthattendtobenonpolarusuallybecomepolar.
Sp2
3
TrigonalPlanar:
BF3,SO32-,NO3-120˚
Bent,12O˚Usuallypolar
NO2-
Also:
Ifthereeverisatwomoleculeatom(diatomic)thatmolecule’spolaritydependsupontheelectronegativitydifferenceoftheatoms
Sp3
4
Tetrahedral;109˚:
UsuallynonpolarCH4CF4
Pyrimidal:
107˚Usuallypolar:
NH3,PCl3
Bent:
104.5˚
Usuallypolar:
H2O,OF2
Remembertocountthenumberof“effectivepairs”ofelectrons,nottheactualnumberofelectrons.Adoubleortriplebondcountsasoneeffectivepair.
Sp3d
5
Trigionalbipyrimidal:
Usuallynonpolar120˚and90˚:
PCl5
See-saw:
Usuallypolar:
120˚,90˚,SeF4
T-Shaped:
Usuallypolar,90˚bondangles
LinearTriatomic:
Usuallynonpolar:
180˚,90˚
Sp3d2
6
Octahedral:
Usuallynonpolar:
90˚,PCl6
SbF6
SquarePyrimidal:
Usuallypolar,90˚,IF5
SquarePlanar:
Usuallynonpolar,90˚
XeF4
T-Shaped:
Usuallypolar
90˚bondangles
LinearTriatomic:
Usuallynonpolar:
180˚,90˚
I31-
ShapesandPolarity
DrawtheLewisstructuresofeach:
Determinethemoleculargeometry(shape),andthepolarity.
9.1:
HybridizationandtheLocalizedElectronModel
Definition:
Hybridization
HybridOrbitals:
Hastodowithatomshavingdifferentorbitals(s,p,d,f)shapesthanmolecules(molecularorbitals)
sp3
sp2
SigmaBond=
PiBond=
sp
dsp3
d2sp3
APStyleQuestions
d)Determine
a.Thenumberofsigmapibondsinbothpropaneandmethanonicacid.
b.Thehybridizationaroundeachcarboninpropane
c.ThehybridizationaroundtheOinmethanoicacid
10.1:
IntermolecularForces
PolarMolecules:
Dipole-dipole:
SketchHere
HydrogenBonding:
SketchHere:
WhatdoesE.T.say:
E.T.______________________________
NonpolarSubstances:
LondonDispersionForces
SketchHere:
O2
WhichmoleculesexhibitLDFforces?
LDFandSize
TheBiggerthemoleculethe___________theattractiveforcesandthe____________theboilingpoint.
LargevsSmallMolecules
10.4:
MetallicBonding
Thekeyplayeristhe__________________________________
Definingpropertyofmetalsthe_____________electrons(andheat)
Sketch:
Explain:
Seaofrovingvalenceelectronsholdsmetalstogether
Otherinterestingthingsaboutmetals:
Alloys
SubstitutionalAlloy
InterstitialAlloy
WhyMalleable?
10.5:
NetworkSolids
Moleculeswithall_________________________________
OnlyCompoundsthatcontain_____________&_________________
Examples
10.6:
MolecularSolids(S8,O2,CO2)
APStyleQuestions
Explaineachofthefollowingintermsofatomicandmolecularstructuresand/orintermolecularforces.
(a)SolidKconductsanelectriccurrent,whereassolidKNO3doesnot.
(b)SbCl3hasmeasurabledipolemoment,whereasSbCl5doesnot.
(c)ThenormalboilingpointofCCl4is77˚C,whereasthatofCBr4is190˚C.
(d)NaI(s)isverysolubleinwater,whereasI2(s)hasasolubilityofonly0.03gramper100gramsofwater.
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- AP Chemistry Chapter 9AP化学章8 化学