chemistry day 18
TRANSCRIPT
Do-Now: “Ch. 11 Inquiry Demo” 1. Write down today’s FLT 2. What was wrong with Rutherford’s atomic
model? 3. Sketch a diagram of Bohr’s model (without
looking at your notes). Label it. 4. Summarize Bohr’s model in 1-2 sentences. 5. Explain what happens when electrons move
up or down an energy level.
Take out your planner and ToC
FLT • I will be able to describe the quantum
atomic model by completing Ch. 11 Notes B
Standard HS-PS1-1:Usetheperiodictableasamodeltopredicttherelativepropertiesofelementsbasedonthepatternsofelectronsintheoutermostenergylevelofatoms.
Bohr Model • ShortcomingsoftheBohrModel:
– e-scan’torbitthenucleus– Onlyexplainedthebehaviorofhydrogenatomsàdidnotexplainthepropertiesoflargeratoms
The Quantum Mechanical Model • Thequantummechanicalmodelisbasedonquantumtheory
• Scientists,suchasSchrödinger,notedthatmattercanbehavelikewaves,anddevelopedcomplexmathematicalequationsthatcoulddescribethebehaviorofe-s
The Quantum Mechanical Model • QuantumTheoryandHeisenberg:• UncertaintyPrinciple=it’simpossibletoknowboththeexactpositionandmomentumofane-atthesametime
The Quantum Mechanical Model • QuantumMechanicalModel–Determinestheallowedenergiesane-canhaveandhowlikelyitistofindthee-invariouslocationsaroundthenucleus
The Quantum Mechanical Model • Inthequantummechanicalmodel,theprobabilityoffindinganelectronwithinacertainvolumeofspacesurroundingthenucleuscanberepresentedasafuzzycloud
• Thecloudismoredensewheretheprobabilityoffindingtheelectronishigh.
The Quantum Mechanical Model • Insteadoforbits,themodelusesorbitals• AtomicOrbitals=regionsofspaceinwhichthereisahighprobabilityoffindingane-
• Orbitalsaresometimescallede-clouds
Pair-Share-Respond 1. What was wrong with Bohr’s atomic
model?
2. State the uncertainty principle. 3. What does the quantum model use instead
of orbits?
4. Define the term “atomic orbital”5. Are atomic orbitals actually part of an
atom?
Quantum Numbers • Fournumbers,calledquantumnumbers,describethecharacteristicsofelectronsandtheirorbitals
Quantum Numbers • n=PrincipalQuantumNumber• l=AngularMomentumQuantumNumber• ml=MagneticQuantumNumber• ms=SpinQuantumNumber
Quantum Numbers • n=PrincipalQuantumNumber
– nrepresentsthespecificenergylevelandthesizeoftheorbital(higherenergylevelsarelarger)
– n=1,2,3,…– Ex/n=2meanselectronsinthe2ndenergylevel
– n=3means…?– n=5means…?
Quantum Numbers • n=PrincipalQuantumNumber• Thetotalnumberofe-sthatanenergylevelcanholdis2n2
• Ex/n=2isthe2ndenergylevel.Itcanhold2(2)2electronsà8electronstotal
• Howmanyelectronscanbeonthe3rdenergylevel?
Quantum Numbers • l=AngularMomentumQuantumNumber
– Thisspecifiestheshapeoftheorbital:s,p,d,orf
– l =0,…,n-1– Ex/ifn=1,thenl=0àsorbitals– Ex/Ifn=3…? l=0 l=1 l=2 l=3
s p d f
Quantum Numbers • l=AngularMomentumQuantumNumber
– Ifn=2,lcanbe0or1(upton-1)– Ifn=3,lcanbe0,1,or2– Ifn=4?
l=0 l=1 l=2 l=3s p d f
Quantum Numbers • Ex/Ifn=3andl=0,thenitisthe3ssublevel
– Thismeansthesorbitalonthe3rdenergylevel
• Ex/Ifn=2andl=1,then• …Itisthe2psublevel• Ex/Ifn=4andl=2,then• …Itisthe4dsublevel
Quantum Numbers • ml =MagneticQuantumNumber• Describestheorientationoftheorbitals• Maybe–l…,0,…+l• Ex/n=2andl=1àsoml=-1,0,+1(3orbitals)
• Whatifn=3andl=2?
Quantum Numbers • ml =MagneticQuantumNumber• Justremember:
– ssublevelhasoneorbitals– psublevelhasthreeorbitals– dsublevelhasfiveorbitals– fsublevelhassevenorbitals
Quantum Numbers • ms=SpinQuantumNumber
– Thisdescribesthedirectionoftheelectron–eitherclockwiseorcounterclockwise
– Onlytwovalues:+1/2or-1/2– Therefore,therecanonlybeuptotwoe-sineachspecificorbitalwithoppositespins• Ex/OnesorbitalcanholduptoTWOelectrons• Ex/OneporbitalcanholduptoTWOelectrons• Ex/Oneforbitalcanholdupto…youguessedit…
– TWOelectrons
• Note:Thefewerthequantumnumbers,thelessweknowabouttheelectrons.– Ex/Ifn=3,Icouldbetalkingabout2n2or18electronsonthe3rdenergylevel
• TheMOREquantumnumberswehave,themoreweknowabouttheelectrons.– Ex/Ifn=3andl=2,Icouldbetalkingaboutanyelectronsinthedorbitals.Sincethereare5dorbitals,thismeansIcouldbetalking
about10electrons.– Ex/Ifn=3,l=2,andml=0,thenIamtalkingaboutonespecificdorbital,andtherefore2electrons.
– Ex/Ifn=3,l=2,ml=0,andms=+½thenIamonlytalkingaboutoneelectron.
Atomic Orbitals • Differentatomicorbitalsaredenotedbyletters.Thesorbitalsarespherical,andporbitalsaredumbbell-shaped.
FLT • I will be able to express the arrangements
of e-s in atoms using orbital notation and electron configurations by completing Ch. 11 Notes C
Standard HS-PS1-1:Usetheperiodictableasamodeltopredicttherelativepropertiesofelementsbasedonthepatternsofelectronsintheoutermostenergylevelofatoms.
Arrangement of Electrons in Atoms • e-sassumeanarrangementthatgivestheatomthelowestenergypossible(morestable)
Electron Configurations
2p4 EnergyLevel
Sublevel
Numberofelectronsinthesublevel
1s22s22p63s23p64s23d104p65s24d105p66s24f14…etc.
Three Principles • AufbauPrinciple=e-soccupythelowestEorbitalavailable.
• Thediagonalrulegivesusanideaoftheorder
Three Principles • PauliExclusionPrinciple=Nomorethantwoe-scanoccupyasingleorbital
• Wenotethisusingarrowsinoppositedirections
Rules 1)Determinethenumberofe-sbylookingupZ(atomicnumber)• Assumetheatomisneutralunlessstatedotherwise(moreonthislater).Draworbitalsfirsttohelpyou.
• Ex/Nitrogen
Rules 2)StartfillingorbitalsinorderofincreasingEaccordingtotheAufbauPrinciple.• Asingleorbitalcanholdamaxof2e-s
OrbitalType NumberofOrbitals
s 1p 3d 5f 7
Rules 3)Hund’sRule&PauliExclusionApply:Drawallorbitalsforeachtype,andfillinONEe-ineachorbitalbeforedoublingup.Doubledupelectronshaveoppositespin.
Shorthand Electron Notation
• Wecanabbreviateourlonge-configurationsbyusingournoblegases
• ThisisbecauseourNobleGaseshavecompletefullporbitals– Note:onlyuseshorthandwhenaskedto
Shorthand e- Notation 1. Findtheclosestnoblegastoyouratomwitha
smallerZandputin[]2. FillorbitalsfromwheretheNobleGasleftoffEx/Na
Do-Now: “Ch. 11 Quiz Day Do-Now” 1. Write down today’s FLT 2. What are our four types of orbitals? 3. How many orientations does each type of orbital
have? 4. How many electrons can one orbital hold? 5. How many TOTAL electrons can the 5th energy
level hold (n = 5) 6. How many TOTAL electrons can there be if n =
3 and l = 2? 7. What four quantum numbers describe an
electron in the 4s orbital spinning clockwise? Take out your planner and ToC
FLT • I will be able to demonstrate my
understanding of modern atomic models and electron configurations by completing Ch. 11 Quiz
Standard HS-PS1-1:Usetheperiodictableasamodeltopredicttherelativepropertiesofelementsbasedonthepatternsofelectronsintheoutermostenergylevelofatoms.