36
http://lawrencekok.blogs pot.com Prepared by Lawrence Kok Tutorial on Electronic Configuration and Quantum Numbers.
| Date post: | 11-May-2015 |
| Category: |
Education |
| Upload: | lawrence-kok |
| View: | 777 times |
| Download: | 5 times |
2. Periodic Table of elements divided into s, p, d, f blocks 3. Periodic Table of elements divided into s, p, d, f blockss block s orbitals partially filld block d orbitals partially filled transition elementsf block f orbital partially fillp block p orbital partially fill 4. Electron filled according to 3 Principles 1Aufbau Principle electron occupy orbitals of lower energy first building up, construction from bottom up4BeHigh energy- 1s2 2s25B- 1s2 2s2 2p12p2p2s2s Click here to view simulation1s1s lower energyClick here to view simulationClick here to view simulation 5. Electron filled according to 3 Principles 1Aufbau Principle electron occupy orbitals of lower energy first building up, construction from bottom up4BeHigh energy- 1s2 2s25B- 1s2 2s2 2p12p2p2s2s Click here to view simulation1s1s lower energy2Hunds Principle electron occupy orbitals singly first before pairing up 7NHigh energy- 1s2 2s2 2p38O- 1s2 2s2 2p42p 2s 1sClick here to view simulation lower energyClick here to view simulation 6. Electron filled according to 3 Principles 1Aufbau Principle electron occupy orbitals of lower energy first building up, construction from bottom up4BeHigh energy- 1s2 2s25B- 1s2 2s2 2p12p2p2s2s Click here to view simulation1s1s lower energy2Hunds Principle electron occupy orbitals singly first before pairing up 7NHigh energy- 1s2 2s2 2p38O- 1s2 2s2 2p42p 2sClick here to view simulation1s 3lower energyPauli Exclusion Principle each orbital occupy by 2 electron opposite spin 4Be- 1s2 2s2High energy10Ne- 1s2 2s2 2p6Click here to view simulation lower energy 7. Electron configuration5B1s2 2s2 2p16C1s2 2s2 2p27N1s2 2s2 2p38O1s2 2s2 2p49F1s2 2s2 2p510Ne1s2 2s2 2p611Na1s2 2s2 2p6 3s112Mg1s2 2s2 2p6 3s213Al1s2 2s2 2p6 3s2 3p114Si1s215P1s2 2s2 2p6 3s2 3p316S1s2 2s2 2p6 3s2 3p417CI1s2 2s2 2p6 3s2 3p518Ar1s2 2s2 2p6 3s2 3p619K1s2 2s2 2p6 3s2 3p6 4s120Ca1s2 2s2 2p6 3s2 3p6 4s221Sc1s2 2s2 2p6 3s2 3p6 4s2 3d122Ti1s2 2s2 2p6 3s2 3p6 4s2 3d223V1s2 2s2 2p6 3s2 3p6 4s2 3d324Cr1s2 2s2 2p6 3s2 3p6 4s1 3d525Mn1s2 2s2 2p6 3s2 3p6 4s2 3d526Fe1s2 2s2 2p6 3s2 3p6 4s2 3d627Co1s2 2s2 2p6 3s2 3p6 4s2 3d728Ni1s2 2s2 2p6 3s2 3p6 4s2 3d829Cu1s2 2s2 2p6 3s2 3p6 4s1 3d1030Zn1s2 2s2 2p6 3s2 3p6 4s2 3d10Electron occupy 4s first then 3dEnergy level and sublevels2s22p64s energy level lower than 3d3s24s 3p 3p23s 18Ar 1s2 2s2 2p6 3s2 3p6 2p 2s 1s3d 8. Electron configuration5B1s2 2s2 2p16C1s2 2s2 2p27N1s2 2s2 2p38O1s2 2s2 2p49F1s2 2s2 2p510Ne1s2 2s2 2p611Na1s2 2s2 2p6 3s112Mg1s2 2s2 2p6 3s213Al1s2 2s2 2p6 3s2 3p114Si1s215P1s2 2s2 2p6 3s2 3p316S1s2 2s2 2p6 3s2 3p417CI1s218Ar1s2 2s2 2p6 3s2 3p619K1s220Ca1s2 2s2 2p6 3s2 3p6 4s221Sc1s2 2s2 2p6 3s2 3p6 4s2 3d122Ti1s2 2s2 2p6 3s2 3p6 4s2 3d223V1s2 2s2 2p6 3s2 3p6 4s2 3d324Cr1s2 2s2 2p6 3s2 3p6 4s1 3d525Mn1s2 2s2 2p6 3s2 3p6 4s2 3d526Fe1s2 2s2 2p6 3s2 3p6 4s2 3d627Co1s2 2s2 2p6 3s2 3p6 4s2 3d728Ni1s2 2s2 2p6 3s2 3p6 4s2 3d829Cu1s2 2s2 2p6 3s2 3p6 4s1 3d1030Zn1s2 2s2 2p6 3s2 3p6 4s2 3d10Electron occupy 4s first then 3dEnergy level and sublevels2s22s22s22p62p62p64s energy level lower than 3d3s23s23s24s3d3p 3p23s 18Ar 1s2 2s2 2p6 3s2 3p6 2p 2s3p53p6 4s1Electrons fill 4s first3d 4s1s 3p 19K 1s2 2s2 2p6 3s2 3p6 4s13s 2p2s1s 9. Electron configuration5B1s2 2s2 2p16C1s2 2s2 2p27N1s2 2s2 2p38O1s2 2s2 2p49F1s2 2s2 2p510Ne1s2 2s2 2p611Na1s2 2s2 2p6 3s112Mg1s2 2s2 2p6 3s213Al1s2 2s2 2p6 3s2 3p114Si1s215P1s2 2s2 2p6 3s2 3p316S1s2 2s2 2p6 3s2 3p417CI1s218Ar1s2 2s2 2p6 3s2 3p619K1s220Ca1s2 2s2 2p6 3s2 3p6 4s221Sc1s2 2s2 2p6 3s2 3p6 4s2 3d122Ti1s2 2s2 2p6 3s2 3p6 4s2 3d223V1s2 2s2 2p6 3s2 3p6 4s2 3d324Cr1s2 2s2 2p6 3s2 3p6 4s1 3d525Mn1s2 2s2 2p6 3s2 3p6 4s2 3d526Fe1s2 2s2 2p6 3s2 3p6 4s2 3d627Co1s2 2s2 2p6 3s2 3p6 4s2 3d728Ni1s2 2s2 2p6 3s2 3p6 4s2 3d829Cu1s2 2s2 2p6 3s2 3p6 4s1 3d1030ZnElectron occupy 4s first then 3dEnergy level and sublevels1s2 2s2 2p6 3s2 3p6 4s2 3d102s22s22s22p62p62p64s energy level lower than 3d3s23s23s24s3d3p 3p23s 18Ar 1s2 2s2 2p6 3s2 3p6 2p 2s3p53p6 4s1Electrons fill 4s first3d 4s1s 3p 19K 1s2 2s2 2p6 3s2 3p6 4s13s 4s then 3d is fill2p 3d2s4s1s 21Sc3p 3s 1s2 2s2 2p6 3s2 3p6 4s2 3d1 2p2s 1s 10. Electron Notation Atom s, p, d, f notation Complete configuration10Ne1s2 2s2 2p611Na1s2 2s2 2p6 3s112Mg1s2 2s2 2p6 3s213Al1s2 2s2 2p6 3s2 3p114Si1s2 2s2 2p6 3s2 3p215P1s2 2s2 2p6 3s2 3p316S1s2 2s2 2p6 3s2 3p417CI1s2 2s2 2p6 3s2 3p518Ar1s2 2s2 2p6 3s2 3p619K1s2 2s2 2p6 3s2 3p6 4s120Ca1s2 2s2 2p6 3s2 3p6 4s221Sc1s2 2s2 2p6 3s2 3p6 4s2 3d122Ti1s2 2s2 2p6 3s2 3p6 4s2 3d223V1s2 2s2 2p6 3s2 3p6 4s2 3d324Cr1s2 2s2 2p6 3s2 3p6 4s1 3d525Mn1s2 2s2 2p6 3s2 3p6 4s2 3d526Fe1s2 2s2 2p6 3s2 3p6 4s2 3d627Co1s2 2s2 2p6 3s2 3p6 4s2 3d728Ni1s2 2s2 2p6 3s2 3p6 4s2 3d829Cu1s2 2s2 2p6 3s2 3p6 4s1 3d1030Zn1s2 2s2 2p6 3s2 3p6 4s2 3d10 11. Electron Notation Atom s, p, d, f notation Complete configurationNoble gas notation Condensed configuration10Ne1s2 2s2 2p610Ne[Ne]11Na1s2 2s2 2p6 3s111Na[Ne] 3s112Mg1s2 2s2 2p6 3s212Mg[Ne] 3s213Al1s2 2s2 2p6 3s2 3p113Al[Ne] 3s2 3p114Si1s2 2s2 2p6 3s2 3p214Si[Ne] 3s2 3p215P1s2 2s2 2p6 3s2 3p315P[Ne] 3s2 3p316S1s2 2s2 2p6 3s2 3p416S[Ne] 3s2 3p417CI1s2 2s2 2p6 3s2 3p517CI[Ne] 3s2 3p518Ar1s2 2s2 2p6 3s2 3p618Ar[Ar]19K1s2 2s2 2p6 3s2 3p6 4s119K[Ar] 4s120Ca1s2 2s2 2p6 3s2 3p6 4s220Ca[Ar] 4s221Sc1s2 2s2 2p6 3s2 3p6 4s2 3d121Sc[Ar] 4s2 3d122Ti1s2 2s2 2p6 3s2 3p6 4s2 3d222Ti[Ar] 4s2 3d223V1s2 2s2 2p6 3s2 3p6 4s2 3d323V[Ar] 4s2 3d324Cr1s2 2s2 2p6 3s2 3p6 4s1 3d524Cr[Ar] 4s1 3d525Mn1s2 2s2 2p6 3s2 3p6 4s2 3d525Mn[Ar] 4s2 3d526Fe1s2 2s2 2p6 3s2 3p6 4s2 3d626Fe[Ar] 4s2 3d627Co1s2 2s2 2p6 3s2 3p6 4s2 3d727Co[Ar] 4s2 3d728Ni1s2 2s2 2p6 3s2 3p6 4s2 3d828Ni[Ar] 4s2 3d829Cu1s2 2s2 2p6 3s2 3p6 4s1 3d1029Cu[Ar] 4s1 3d1030Zn1s2 2s2 2p6 3s2 3p6 4s2 3d1030Zn[Ar] 4s2 3d10[Ne][Ar] 12. Electron Notation AtomPositive/Negative Ions, p, d, f notation Complete configurationNoble gas notation Condensed configurationNoble gas notation Complete configuration10Ne1s2 2s2 2p610Ne[Ne]10Ne1s2 2s2 2p6 /[Ne]11Na1s2 2s2 2p6 3s111Na[Ne] 3s111Na+1s2 2s2 2p6 / [Ne]12Mg1s2 2s2 2p6 3s212Mg[Ne] 3s212Mg2+1s2 2s2 2p6 / [Ne]13Al1s2 2s2 2p6 3s2 3p113Al[Ne] 3s2 3p113Al3+1s2 2s2 2p6 / [Ne]14Si1s2 2s2 2p6 3s2 3p214Si[Ne] 3s2 3p214Si4+1s2 2s2 2p6 / [Ne]15P1s2 2s2 2p6 3s2 3p315P[Ne] 3s2 3p315P3-1s2 2s2 2p6 3s2 3p6 /[Ar]16S1s2 2s2 2p6 3s2 3p416S[Ne] 3s2 3p416S2-1s2 2s2 2p6 3s2 3p6 /[Ar]17CI1s2 2s2 2p6 3s2 3p517CI[Ne] 3s2 3p517CI-1s2 2s2 2p6 3s2 3p6/ [Ar]18Ar1s2 2s2 2p6 3s2 3p618Ar[Ar]19[Ne]18Ar[Ar]K[Ar]4s119K+1s2 2s2 2p6 3s2 3p6 /[Ar]20Ca[Ar] 4s220Ca2+1s2 2s2 2p6 3s2 3p6 / [Ar]21Sc[Ar] 4s2 3d122Ti[Ar] 4s2 3d21s2 2s2 2p6 3s2 3p6 4s2 3d323V[Ar] 4s2 3d3Cr1s2 2s2 2p6 3s2 3p6 4s1 3d524Cr[Ar] 4s1 3d525Mn1s2 2s2 2p6 3s2 3p6 4s2 3d525Mn[Ar] 4s2 3d526Fe1s2 2s2 2p6 3s2 3p6 4s2 3d626Fe[Ar] 4s2 3d627Co1s2 2s2 2p6 3s2 3p6 4s2 3d727Co[Ar] 4s2 3d728Ni1s2 2s2 2p6 3s2 3p6 4s2 3d828Ni[Ar] 4s2 3d829Cu1s2 2s2 2p6 3s2 3p6 4s1 3d1029Cu[Ar] 4s1 3d1030Zn1s2 2s2 2p6 3s2 3p6 4s2 3d1030Zn[Ar] 4s2 3d10K1s22s22p63s23p6 4s11920Ca1s2 2s2 2p6 3s2 3p6 4s221Sc1s2 2s2 2p6 3s2 3p6 4s2 3d122Ti1s2 2s2 2p6 3s2 3p6 4s2 3d223V24[Ar] 13. d blockException to d block elements 4s energy level lower than 3d3d4s 3p Electron configuration d block21Sc1s2 2s2 2p6 3s2 3p6 4s2 3d122Ti V1s2 2s2 2p6 3s2 3p6 4s2 3d324Cr1s2 2s2 2p6 3s2 3p6 4s1 3d525Mn1s2 2s2 2p6 3s2 3p6 4s2 3d526Fe1s2 2s2 2p6 3s2 3p6 4s2 3d627Co1s2 2s2 2p6 3s2 3p6 4s2 3d728Ni1s2 2s2 2p6 3s2 3p6 4s2 3d829Cu1s2 2s2 2p6 3s2 3p6 4s1 3d1030Zn1s2 2s2 2p6 3s2 3p6 4s2 3d1021Sc 1s2 2s2 2p6 3s2 3p6 4s2 3d12p1s2 2s2 2p6 3s2 3p6 4s2 3d2233s 2s 1s4s energy level lower than 3d 14. d blockException to d block elements 4s energy level lower than 3d3d4s 3p Electron configuration d block21Sc1s2 2s2 2p6 3s2 3p6 4s2 3d122Ti V24Cr25Mn1s2 2s2 2p6 3s2 3p6 4s2 3d526Fe1s2 2s2 2p6 3s2 3p6 4s2 3d627Co Ni1s2 2s2 2p6 3s2 3p6 4s2 3d829Cu1s2 2s2 2p6 3s2 3p6 4s1 3d1030Zn1s2 2s2 2p6 3s2 3p6 4s2 3d102s22p63s23p6 4s13d54s energy level lower than 3d2p1s2 2s2 2p6 3s2 3p6 4s2 3d728 1s2 2s2 2p6 3s2 3p6 4s2 3d11s2 2s2 2p6 3s2 3p6 4s2 3d31s221Sc1s2 2s2 2p6 3s2 3p6 4s2 3d2233s 2s 1s 24Cr 1s2 2s2 2p6 3s2 3p6 4s13d524Cr 1s2 2s2 2p6 3s2 3p6 4s2 3d43d 4s 3p 3s 2p 2s1sHalf fill energetically more stable 15. d blockException to d block elements 4s energy level lower than 3d3d4s 3p Electron configuration d block21Sc1s2 2s2 2p6 3s2 3p6 4s2 3d122Ti V24Cr25Mn1s2 2s2 2p6 3s2 3p6 4s2 3d526Fe1s2 2s2 2p6 3s2 3p6 4s2 3d627Co Ni1s2 2s2 2p6 3s2 3p6 4s2 3d829Cu1s2 2s2 2p6 3s2 3p6 4s1 3d1030Zn1s2 2s2 2p6 3s2 3p6 4s2 3d102s22p63s23p6 4s13d54s energy level lower than 3d2p1s2 2s2 2p6 3s2 3p6 4s2 3d728 1s2 2s2 2p6 3s2 3p6 4s2 3d11s2 2s2 2p6 3s2 3p6 4s2 3d31s221Sc1s2 2s2 2p6 3s2 3p6 4s2 3d2233s 2s 1s 24Cr 1s2 2s2 2p6 3s2 3p6 4s13d524Cr 1s2 2s2 2p6 3s2 3p6 4s2 3d43d 4s 3p 3sHalf fill energetically more stable2p 2s1s29Cu29Cu1s2 2s2 2p6 3s2 3p6 4s1 3d10 1s2 2s2 2p6 3s2 3p6 4s2 3d9 4s 3p 3sHalf fill energetically more stable2p 2s 1s3d 16. s block elements s orbitals partially fill1H Hep block elements p orbital partially fill51s2 n = 2 period 2B[He] 2s2 2p161s12Periodic Table s, p d, f blocks elementsC[He] 2s2 2p27N[He] 2s2 2p33Li[He] 2s18O[He] 2s2 2p44Be[He] 2s29F[He] 2s2 2p510Ne[He] 2s2 2p613Al[Ne] 3s2 3p13s111Na[Ne]12Mg[Ne] 3s214 19 20K CaSi[Ne] 3s2 3p2[Ar]4s115P[Ne] 3s2 3p3[Ar]4s216S[Ne] 3s2 3p417CI[Ne] 3s2 3p518Ar[Ne] 3s2 3p6 17. s block elements s orbitals partially fill1H Hep block elements p orbital partially fill51s2 n = 2 period 2B[He] 2s2 2p161s12Periodic Table s, p d, f blocks elementsC[He] 2s2 2p27N[He] 2s2 2p33Li[He] 2s18O[He] 2s2 2p44Be[He] 2s29F[He] 2s2 2p510Ne[He] 2s2 2p613Al[Ne] 3s2 3p13s111Na[Ne]12Mg[Ne] 3s214 20K Ca[Ne] 3s2 3p2[Ar]15P[Ne] 3s2 3p3[Ar]4s216S[Ne] 3s2 3p41719Si4s1CI[Ne] 3s2 3p518Ar[Ne] 3s2 3p6d block elements d orbitals partially fill transition elements21Sc[Ar] 4s2 3d122Ti[Ar] 4s2 3d223V[Ar] 4s2 3d1324Cr[Ar] 4s1 3d525Mn[Ar] 4s2 3d526Fe[Ar] 4s2 3d627Co[Ar] 4s2 3d728Ni[Ar] 4s2 3d829Cu[Ar] 4s1 3d1030Zn[Ar] 4s2 3d10 18. s block elements s orbitals partially fill1H Hep block elements p orbital partially fill51s2 n = 2 period 2B[He] 2s2 2p161s12Periodic Table s, p d, f blocks elementsC[He] 2s2 2p27N[He] 2s2 2p33Li[He] 2s18O[He] 2s2 2p44Be[He] 2s29F[He] 2s2 2p510Ne[He] 2s2 2p613Al[Ne] 3s2 3p13s111Na[Ne]12Mg[Ne] 3s214 20K Ca[Ne] 3s2 3p2[Ar]15P[Ne] 3s2 3p3[Ar]4s216S[Ne] 3s2 3p41719Si4s1CI[Ne] 3s2 3p518Ar[Ne] 3s2 3p6d block elements d orbitals partially fill transition elements21Sc[Ar] 4s2 3d122Ti[Ar] 4s2 3d223V[Ar] 4s2 3d1324Cr[Ar] 4s1 3d525Mn[Ar] 4s2 3d526Fe[Ar] 4s2 3d627Co[Ar] 4s2 3d728Ni[Ar] 4s2 3d829Cu[Ar] 4s1 3d1030Zn[Ar] 4s2 3d10f block elements f orbitals partially fillVideo on electron configurationClick here electron structureClick here video on s,p,d,f notationClick here video s,p,d,f blocks, 19. Periodic Table s, p d, f blocks elements Electron structure Chromium d block (Period 4)Electron structure Germanium p block, Gp 4 (Period 4)Electron structure Iodine p block, Gp 7 (Period 5)1s2 2s2 2p6 3s2 3p6 4s1 3d5 [Ar] 4s1 3d51s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2 [Ar] 4s2 3d10 4p21s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p5 [Kr] 5s2 4d10 5p5d block d partially filledGp 4 -4 valence electronGp 7 - 7 valence electron 20. Periodic Table s, p d, f blocks elements Electron structure Chromium d block (Period 4)Electron structure Germanium p block, Gp 4 (Period 4)Electron structure Iodine p block, Gp 7 (Period 5)1s2 2s2 2p6 3s2 3p6 4s1 3d5 [Ar] 4s1 3d51s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2 [Ar] 4s2 3d10 4p21s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p5 [Kr] 5s2 4d10 5p5d block d partially filledElectron structure Cadmium d block (Period 5)1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 [Kr] 5s2 4d10 d block d partially filledGp 4 -4 valence electronElectron structure Mercury d block (Period 6)1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p6 6s2 4f14 5d10 [Xe] 6s2 4f14 5d10 d block d partially filledGp 7 - 7 valence electronElectron structure Lead p block, Gp 4 (Period 6)1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p6 6s2 4f14 5d106p2 [Xe] 6s2 4f14 5d10 6p2 Gp 4 -4 valence electron 21. s block elements s orbitals partially fill1H Hep block elements p orbital partially fill51s2 n = 2 period 2B[He] 2s2 2p161s12Periodic Table s, p d, f blocks elementsC[He] 2s2 2p27N[He] 2s2 2p33Li[He] 2s18O[He] 2s2 2p44Be[He] 2s29F[He] 2s2 2p510Ne[He] 2s2 2p613Al[Ne] 3s2 3p114Si[Ne] 3s2 3p215P[Ne] 3s2 3p316S[Ne] 3s2 3p417CI[Ne] 3s2 3p518Ar[Ne] 3s2 3p63s111Na[Ne]12Mg[Ne] 3s219 20K Ca[Ar]4s1[Ar]4s21s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p6 6s2 4f14 5d106p2 [Xe] 6s2 4f14 5d10 6p2 22. Periodic Table s, p d, f blocks elementss block elements s orbitals partially fill1H He51s2 n = 2 period 2B[He] 2s2 2p161s12p block elements p orbital partially fillC[He] 2s2 2p27N[He] 2s2 2p33Li[He] 2s18O[He] 2s2 2p44Be[He] 2s29F[He] 2s2 2p510Ne[He] 2s2 2p613Al[Ne] 3s2 3p114Si[Ne] 3s2 3p215P[Ne] 3s2 3p316S[Ne] 3s2 3p417CI[Ne] 3s2 3p518Ar[Ne] 3s2 3p63s111Na[Ne]12Mg[Ne] 3s219K201Ca[Ar] [Ar]1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p6 6s2 4f14 5d106p2 [Xe] 6s2 4f14 5d10 6p24s1 4s2Identify position elements P, Q, R, S and T Electron configuration : P 3s2 3p6 Q 4s2 4p5 R 3s2 3p6 4s2 S 1s2 2s2 2p6 3s2 3p6 3d3 4s2 T 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6AnswerElement2Write electron configuration for X, Y and Z ElementGroupPeriodX23Y152Z183AnswerGrou pPeriodClassificationP8/183Noble gasQ7/174p blockR24s blockS54d blockT8/184Noble gasX 1s2 2s2 2p6 3s2 Y 1s2 2s2 2p3 Z 1s2 2s2 2p6 3s2 3p63Write electron structure for ions: O - 1s2 2s2 2p4 O2- V - 1s2 2s2 2p6 3s2 3p6 4s2 3d3 V3+ Cu - 1s2 2s2 2p6 3s2 3p6 4s2 3d9 Cu2+ -AnswerWrite electron structure for ions: O - 1s2 2s2 2p4 O2- -1s2 2s2 2p6 V - 1s2 2s2 2p6 3s2 3p6 4s2 3d3 V 3+ - 1s2 2s2 2p6 3s2 3p6 4s0 3d2 Cu - 1s2 2s2 2p6 3s2 3p6 4s2 3d9 Cu 2+ - 1s2 2s2 2p6 3s23p6 4s0 3d9 23. Four Quantum Numbers 1Electrons arrange in specific energy level and sublevels Orbitals of electrons in atom differ in size, shape and orientation. Allow states call orbitals, given by four quantum number 'n', 'l', 'ml' and ms - (n, l, ml, ms)Principal Quantum Number (n): n = 1, 2, 3,.. Energy of electron and size of orbital/shell Distance from nucleus, (higher n higher energy) Larger n - farther e from nucleus larger size orbital n=1, 1stprincipal shell ( innermost/ground shell state)No TWO electron have same 4 quantum number 24. Four Quantum Numbers Electrons arrange in specific energy level and sublevels Orbitals of electrons in atom differ in size, shape and orientation. Allow states call orbitals, given by four quantum number 'n', 'l', 'ml' and ms - (n, l, ml, ms)1Principal Quantum Number (n): n = 1, 2, 3,.. Energy of electron and size of orbital/shell Distance from nucleus, (higher n higher energy) Larger n - farther e from nucleus larger size orbital n=1, 1stprincipal shell ( innermost/ground shell state)2Angular Momentum Quantum Number (l): l = 0 to n-1. Orbital Shape Divides shells into subshells/sublevels. Letters (s, d, p, f) s orbitalp orbitald orbitalNo TWO electron have same 4 quantum number 25. Four Quantum Numbers Electrons arrange in specific energy level and sublevels Orbitals of electrons in atom differ in size, shape and orientation. Allow states call orbitals, given by four quantum number 'n', 'l', 'ml' and ms - (n, l, ml, ms)1Principal Quantum Number (n): n = 1, 2, 3,.. Energy of electron and size of orbital/shell Distance from nucleus, (higher n higher energy) Larger n - farther e from nucleus larger size orbital n=1, 1stprincipal shell ( innermost/ground shell state)2Angular Momentum Quantum Number (l): l = 0 to n-1. Orbital Shape Divides shells into subshells/sublevels. Letters (s, d, p, f) s orbitalp orbitald orbital3No TWO electron have same 4 quantum numberMagnetic Quantum Number (ml): ml = -l, 0, +l. Orientation orbital in space/direction m range from to , = 0 -> m = 0 > s sublevel -> 1 orbital = 1 -> m = -1, 0, +1 -> p sublevel -> 3 diff p orbitals = 2 -> m = -2, -1, 0, +1, +2 -> d sublevel -> 5 diff d orbitals (2l+ 1 ) quantum number for each value 26. Four Quantum Numbers Electrons arrange in specific energy level and sublevels Orbitals of electrons in atom differ in size, shape and orientation. Allow states call orbitals, given by four quantum number 'n', 'l', 'ml' and ms - (n, l, ml, ms)1Principal Quantum Number (n): n = 1, 2, 3,.. Energy of electron and size of orbital/shell Distance from nucleus, (higher n higher energy) Larger n - farther e from nucleus larger size orbital n=1, 1stprincipal shell ( innermost/ground shell state)2Angular Momentum Quantum Number (l): l = 0 to n-1. Orbital Shape Divides shells into subshells/sublevels. Letters (s, d, p, f) s orbitalp orbital34No TWO electron have same 4 quantum numberMagnetic Quantum Number (ml): ml = -l, 0, +l. Orientation orbital in space/direction m range from to , = 0 -> m = 0 > s sublevel -> 1 orbital = 1 -> m = -1, 0, +1 -> p sublevel -> 3 diff p orbitals = 2 -> m = -2, -1, 0, +1, +2 -> d sublevel -> 5 diff d orbitals (2l+ 1 ) quantum number for each valueSpin Quantum Number (ms): ms = +1/2 or -1/2 Each orbital 2 electrons, spin up/down Pair electron spin opposite direction One spin up, ms = +1/2 One spin down, ms = -1/2 No net spin/cancel out each other diamagnetic electron writing electron spin electron spin up/downd orbital 27. Principal and Angular Momentum Quantum numbers Electrons arrange in specific energy level and sublevels Orbitals of electrons in atom differ in size, shape and orientation. Allow states call orbitals, given by four quantum number 'n', 'l', 'ml' and ms - (n, l, ml, ms)1Principal Quantum Number (n): n = 1, 2, 3, , Energy of electron and size of orbital /shell Distance from nucleus, (higher n higher energy) Larger n - farther e from nucleus larger size orbital n=1, 1stprincipal shell ( innermost/ground shell state)2Angular Momentum Quantum Number (l): l = 0, ..., n-1. Orbital Shape Divides shells into subshells (sublevels) Letters (s,p,d,f) < less than n-1Sublevels, l 28. Principal and Angular Momentum Quantum numbers Electrons arrange in specific energy level and sublevels Orbitals of electrons in atom differ in size, shape and orientation. Allow states call orbitals, given by four quantum number 'n', 'l', 'ml' and ms - (n, l, ml, ms)1Principal Quantum Number (n): n = 1, 2, 3, , Energy of electron and size of orbital /shell Distance from nucleus, (higher n higher energy) Larger n - farther e from nucleus larger size orbital n=1, 1stprincipal shell ( innermost/ground shell state)2Angular Momentum Quantum Number (l): l = 0, ..., n-1. Orbital Shape Divides shells into subshells (sublevels) Letters (s,p,d,f) < less than n-1Sublevels, lQuantum number, n and ll=12p sublevell=02s subleveln= 2n= 1 1Principal Quantum #, n (Size , energy)l=0 21s sublevelAngular momentum quantum number, l (Shape of orbital)1Principal Quantum Number (n)2Angular Momentum Quantum Number (l) 29. Principal and Angular Momentum Quantum numbers Electrons arrange in specific energy level and sublevels Orbitals of electrons in atom differ in size, shape and orientation. Allow states call orbitals, given by four quantum number 'n', 'l', 'ml' and ms - (n, l, ml, ms)1Principal Quantum Number (n): n = 1, 2, 3, , Energy of electron and size of orbital /shell Distance from nucleus, (higher n higher energy) Larger n - farther e from nucleus larger size orbital n=1, 1stprincipal shell ( innermost/ground shell state)2Angular Momentum Quantum Number (l): l = 0, ..., n-1. Orbital Shape Divides shells into subshells (sublevels) Letters (s,p,d,f) < less than n-1Sublevels, lQuantum number, n and ll=12p sublevell=02s subleveln= 2n= 1 1Principal Quantum #, n (Size , energy)l=0 21s sublevelAngular momentum quantum number, l (Shape of orbital) 2p sublevel contain 2p orbital2nd energy levelHas TWO sublevels 2s sublevel contain 2s orbital1st energy levelHas ONE sublevel1s sublevel contain 1s orbital1Principal Quantum Number (n)2Angular Momentum Quantum Number (l) 30. Electronic Orbitals n = 1, 2, 3,.Allowed valuesl = 0 to n-1Allowed valuesml = -l, 0, +l- (2l+ 1 ) for each value ml =+2 ml =+1 ml = 0l=13px orbitalml = 03s sublevel3py orbital3s orbitalml =+1l=03pz orbitalml = 03p sublevel3dxy orbitalml =-1l=13dxz orbitalml =+1 n= 33dz2 orbitalml =-23d sublevel3dyz orbitalml =-1l=2 Energy Level3dx2 y2 orbital2py orbitalml = 02p sublevel2pz orbitalml =-1n= 22px orbitall=01Principal Quantum #, n (Size , energy)2ml =02s orbitall=0n= 12s sublevel1s sublevelml =01s orbitalAngular momentum quantum number, l (Shape of orbital)3Magnetic Quantum Number (ml) (Orientation orbital) 31. Electronic Orbitals Simulation Electronic Orbitals n = 1, 2, 3,.Allowed valuesl = 0 to n-1Allowed valuesml = -l, 0, +l- (2l+ 1 ) for each value ml =+2 ml =+1 ml = 0l=13px orbitalml = 03s sublevel3py orbital3s orbitalml =+1l=03pz orbitalml = 03p sublevel3dxy orbitalml =-1l=13dxz orbitalml =+1 n= 33dz2 orbitalml =-23d sublevel3dyz orbitalml =-1l=2 Energy Level3dx2 y2 orbital2py orbitalml = 02p sublevel2pz orbitalml =-1n= 22px orbitall=01Principal Quantum #, n (Size , energy)22s sublevelml =01s sublevelml =0Click here to view simulation2s orbitall=0n= 1Click here to view simulation1s orbitalAngular momentum quantum number, l (Shape of orbital)3Magnetic Quantum Number (ml) (Orientation orbital)Click here to view simulation 32. Quantum Numbers and Electronic Orbitals ml =+2Energy Level3dx2 y2orbitalml =+13dz2 orbital3dxz orbitalml =-23d sublevelml = 0ml =-1l=23dyz orbital3dxy orbitaln= 3ml =+1l=13s sublevel2p subleveln= 23pz orbital 3px orbitalml = 03s orbitalml =+1l=03p sublevelml = 0 ml =-1l=13py orbital2py orbitalml = 02pz orbitalml =-12px orbitall=0n= 12s sublevelml =02s orbitall=01s sublevelml =01s orbital 33. Quantum Numbers and Electronic Orbitals ml =+23dx2 y2orbitalSimulation Electronic Orbitals Energy Levelml =+13d sublevelml = 03dz2 orbitalml =-1l=23dyz orbital3dxz orbital Click here to view simulationn= 3 ml =-23dxy orbitalml =+1 3p sublevelml = 03pz orbitalml =-1l=13py orbital3px orbitalClick here to view simulation l=02p subleveln= 2ml = 03s orbitalml =+1 l=13s sublevel2py orbitalml = 02pz orbitalml =-12px orbitall=0n= 12s sublevelml =02s orbitall=01s sublevelml =01s orbitalClick here to view simulation 34. Concept MapNo TWO electron have same 4 quantum numberQuantum numberQuantum number = genetic code for electronWhat are these 4 numbers? (1, 0, 0, +1/2) 0r (3, 1, 1, +1/2) 4 numbersnlSize/distanceShapeNumber + lettermlOrientationmsElectron spinElectron has special number codes 35. Concept MapNo TWO electron have same 4 quantum numberQuantum numberQuantum number = genetic code for electronWhat are these 4 numbers? (1, 0, 0, +1/2) 0r (3, 1, 1, +1/2) 4 numbersnlSize/distanceShapemlOrientationmsElectron has special number codesElectron spinNumber + letter1Electron with quantum number given below(n,l,ml,,ms) (1, 0, 0, +1/2)(n,l,ml,,ms) (3, 1, 1, +1/2)21s orbital3py orbitalWhat values of l, ml, allow for n = 3? How many orbitals exists for n=3?Video on Quantum numbersFor n=3 -> l = n -1 =2 -> ml = -l, 0, +l -> -2, -1, 0, +1, +2 m range from to , = 0 -> m = 0 > s sublevel -> 1 orbital = 1 -> m = -1, 0, +1 -> p sublevel -> 3 diff p orbitals = 2 -> m = -2, -1, 0, +1, +2 -> d sublevel -> 5 diff d orbitals (2l+ 1 ) quantum number for each value Answer = nine ml values 9 orbitals/ total # orbitals = n 2 Click here video on quantum numberClick here video on quantum number 36. Acknowledgements Thanks to source of pictures and video used in this presentation http://crescentok.com/staff/jaskew/isr/tigerchem/econfig/electron4.htm http://pureinfotech.com/wp-content/uploads/2012/09/periodicTable_20120926101018.pngThanks to Creative Commons for excellent contribution on licenses http://creativecommons.org/licenses/Prepared by Lawrence Kok Check out more video tutorials from my site and hope you enjoy this tutorial http://lawrencekok.blogspot.com
