Pre-AP Chemistry 11 Atomic Theory II
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Pre-AP Chemistry 11 Atomic Theory II Name: Date: Block: 1. Electronic Structure 2. Electron Configuration 3. EC Relationship to Periodic Table 4. Core Notation 5. Electron Configuration of Ions Electronic Structure What you should already know… BOHR DIAGRAMS: Example: Calcium • First shell has 2 electrons • Second, third shell has 8 electrons Energy level • A specific amount of ____________ which an ____________ in an atom can possess Bohr’s Postulate #1 • The hydrogen atom had only certain allowed ___________________________ or stationary states. • The lowest (smallest) orbit was called the “________________________” and designated n = 1. • The larger orbits were called “________________________” and designated as n = 2, n = 3, n = 4, etc. Bohr’s Postulate #2 • As long as the electron moved within the same energy level, the electron did not radiate or absorb energy Bohr’s Postulate #3 • The electron could only move from one allowed energy level to another if it _____________________ or _____________________ an amount of energy equal to the energy different between the two energy level.
Transcript of Pre-AP Chemistry 11 Atomic Theory II
Pre-APChemistry11AtomicTheoryII
Name:Date:Block:
1. ElectronicStructure2. ElectronConfiguration3. ECRelationshiptoPeriodicTable4. CoreNotation5. ElectronConfigurationofIons
ElectronicStructureWhatyoushouldalreadyknow…BOHRDIAGRAMS:Example:Calcium
• Firstshellhas2electrons• Second,thirdshellhas8electrons
Energylevel
• Aspecificamountof____________whichan____________inanatomcanpossess
Bohr’sPostulate#1
• Thehydrogenatomhadonlycertainallowed___________________________orstationarystates.• Thelowest(smallest)orbitwascalledthe“________________________”anddesignatedn=1.• Thelargerorbitswerecalled“________________________”anddesignatedasn=2,n=3,n=4,etc.
Bohr’sPostulate#2
• Aslongastheelectronmovedwithinthesameenergylevel,theelectrondidnotradiateorabsorbenergy
Bohr’sPostulate#3
• Theelectroncouldonlymovefromoneallowedenergyleveltoanotherifit_____________________or_____________________anamountofenergyequaltotheenergydifferentbetweenthetwoenergylevel.
ExpandingBohr’sTheory
• Eachenergylevelissplitupinto___________________and___________________.
AtomicOrbitals• SHELL(sciencehallway)àSUBSHELL(room212)àORBITAL(rowintheclassroom)• Eachorbitalcanhold______electrons• Weusedtodrawelectronsas“dots”butnowwewilldrawthemasarrows:• “s”subshell=____orbital=canholdamaximumof____electrons
Ø Ex:1ssubshelllookslikethis:• “p”subshell=____orbitals=canholdamaximumof____electrons
Ø Ex:2psubshelllookslikethis:• “d”subshell=____orbitals=canholdamaximumof____electrons
Ø Ex:3dsubshelllookslikethis:• “f”subshell=____orbitals=canholdamaximumof____electrons
Ø Ex:4fsubshelllookslikethis:
• IntheBohrmodel,theshellsincreaseinnumericalorder=toosimplistic!
• Orbitalsincreaseinenergybutnotnumerically…
Ø Electronsfillorbitalsfromthelowestenergy
Ø Canyoureadthediagramontheright?o Followthearrows…
1s2s2p3s3p4s3d4p5s4d5p6s4f5d6p7s5f6d7p
Howcanwerememberthisorder…?
Don’tworry!IthastodowiththewaythePeriodicTableisorganized!!!Staytuned…ElectronConfiguration&OrbitalDiagrams
• Showswheretheelectronsarelocatedwithintheorbitals.
• Therearethree“rules”thatwemustremember:
Rule#1:AufbauPrinciple
• Means_______________________inGerman• Whenfillingorbitalsthe_____________________energyorbitalsavailablearealwaysfilledfirst.
Rule#2:PauliExclusionPrinciple
• Eachorbitalcanholdamaximumof___________electrons.
Rule#3:Hund’sRule
• Whenorbitalsof________________energyarebeingfilled,electronsaremoststablewhenorbitalis_____________________-occupiedbeforeanyorbitalis____________________-occupied.
• Ex:Carbonhas_________electrons.
1s 2s 2p
Let’spractice!Element Numberof
electronsFullElectronConfiguration OrbitalDiagram
Lithium 3
Beryllium 4
Boron
Carbon
Nitrogen
Oxygen
Fluorine
Neon
1s 2s
1s 2s 2p
ElectronConfigurationRelationshiptoPeriodicTable
CoreNotationSometimesweneedashortcuttowritetheelectronconfiguration.WeuseNOBLEGASEStoelectronconfigurationtowriteoutCORENOTATION.Example:Magnesium
Ø FullElectronconfiguration:
1s22s22p63s2
Ø Corenotation:Practice:
1. Co
2. Rh
3. Ir
4. K
5. Rb
6. Cs
7. Cl
8. Br
9. I
10. N
11. P
12. As
13. Doyounoticeanypatterns?
ElectronConfigurationofIonsNegativeIons:
• Example:
PositiveIons:
• TwoRules:1.
2.
• Writethecorenotationfortheatom,thenremoveelectronsintheorder:Example:
Practice:1.Writetheelectronconfigurationofthefollowingions,usingcorenotation:
1.H- 2.Sr2+
3.Br- 4.N3+
5.Ti2+ 6.N2-
7.Mn2+ 8.Ge4+
9.Fe3+ 10.Ge2+
11.Ru3+ 12.Sb3+
2.Usetheperiodictabletocompletethefollowingtable:AtomorIon ElectronConfiguration CoreNotation
Ge
Zn2+
Sr
Br-
Sn
In3+
3. Usetheperiodictabletoidentifytheneutralatomshavingthefollowingelectronconfigurations:
ElectronConfiguration ElementName
[Ne]3s2
[Ar]4s23d5
[Kr]5s24d105p3
[Xe]6s24f7
4. Considerthefollowingsixions:N3-O2-F-Na+Mg2+Al3+a) Howmanyelectronsarepresentineachion?
b) Writeasingleelectronconfigurationrepresentingalloftheions.
c) Whichneutralatompossessthiselectronconfiguration?
5. Completethefollowingtableforsomeelementsintwofamiliesoftheperiodictable:Alkalimetals CoreNotation #OuterElectrons Halogens CoreNotation #OuterElectrons
Lithium
Fluorine
Sodium
Chlorine
Potassium
Bromine
Rubidium
Iodine
a) Considerthenumberofouterelectronspresentandsuggestareasonwhyelementsbelongingto
thesamechemicalfamilydemonstratesimilarchemicalbehavior.
b) Whatchangeoccursintheatomsaswemovedowneachchemicalfamily?
