1.Tutorial on s, p, d, f, successive ionization and electronic configuration.Prepared by Lawrence Kok http://lawrencekok.blogspot.com

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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 3. 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 fill 4. 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, 5. 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 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 energy 7. 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 1s 3Click here to view simulation lower energy 8. 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 9. 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 10. 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] 11. 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] 12. 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 13. 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 14. 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 15. 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 16. 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 17. 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 18. d blockException to d block elements 4s energy level lower than 3dElectron configuration d blockNoble gas notation Condensed configurationPositive Ions21Sc1s2 2s2 2p6 3s2 3p6 4s2 3d121Sc[Ar] 3d1 4s221Sc3+[Ar]22Ti1s2 2s2 2p6 3s2 3p6 4s2 3d222Ti[Ar] 3d2 4s222Ti4+[Ar]23V1s2 2s2 2p6 3s2 3p6 4s2 3d323V[Ar] 3d3 4s223V3+[Ar] 3d224Cr1s2 2s2 2p6 3s2 3p6 4s1 3d524Cr[Ar] 3d5 4s124Cr3+[Ar] 3d325Mn1s2 2s2 2p6 3s2 3p6 4s2 3d525Mn[Ar] 3d5 4s225Mn2+[Ar] 3d526Fe1s2 2s2 2p6 3s2 3p6 4s2 3d626Fe[Ar] 3d6 4s226Fe2+[Ar] 3d627Co1s2 2s2 2p6 3s2 3p6 4s2 3d727Co[Ar] 3d7 4s227Co2+[Ar] 3d728Ni1s2 2s2 2p6 3s2 3p6 4s2 3d828Ni[Ar] 3d8 4s228Ni2+[Ar] 3d829Cu1s2 2s2 2p6 3s2 3p6 4s1 3d1029Cu[Ar] 3d10 4s129Cu2+[Ar] 3d930Zn1s2 2s2 2p6 3s2 3p6 4s2 3d1030Zn[Ar] 3d10 4s230Zn2+[Ar] 3d10Electrons lost from 4s then 3d 19. d blockException to d block elements 4s energy level lower than 3dElectron configuration d blockNoble gas notation Condensed configurationPositive Ions21Sc1s2 2s2 2p6 3s2 3p6 4s2 3d121Sc[Ar] 3d1 4s221Sc3+[Ar]22Ti1s2 2s2 2p6 3s2 3p6 4s2 3d222Ti[Ar] 3d2 4s222Ti4+[Ar]23V1s2 2s2 2p6 3s2 3p6 4s2 3d323V[Ar] 3d3 4s223V3+[Ar] 3d224Cr1s2 2s2 2p6 3s2 3p6 4s1 3d524Cr[Ar] 3d5 4s124Cr3+[Ar] 3d325Mn1s2 2s2 2p6 3s2 3p6 4s2 3d525Mn[Ar] 3d5 4s225Mn2+[Ar] 3d526Fe1s2 2s2 2p6 3s2 3p6 4s2 3d626Fe[Ar] 3d6 4s226Fe2+[Ar] 3d627Co1s2 2s2 2p6 3s2 3p6 4s2 3d727Co[Ar] 3d7 4s227Co2+[Ar] 3d728Ni1s2 2s2 2p6 3s2 3p6 4s2 3d828Ni[Ar] 3d8 4s228Ni2+[Ar] 3d829Cu1s2 2s2 2p6 3s2 3p6 4s1 3d1029Cu[Ar] 3d10 4s129Cu2+[Ar] 3d930Zn1s2 2s2 2p6 3s2 3p6 4s2 3d1030Zn[Ar] 3d10 4s230Zn2+[Ar] 3d10Why electron fill 4s first? 14s fill first 4s2 4s greater penetration/closer to nucleus 4s lower in energy3d4s 20Ca [Ar] 4s2 3d0Electrons lost from 4s then 3d 20. d blockException to d block elements 4s energy level lower than 3dNoble gas notation Condensed configurationElectron configuration d blockPositive Ions21Sc1s2 2s2 2p6 3s2 3p6 4s2 3d121Sc[Ar] 3d1 4s221Sc3+[Ar]22Ti1s2 2s2 2p6 3s2 3p6 4s2 3d222Ti[Ar] 3d2 4s222Ti4+[Ar]23V1s2 2s2 2p6 3s2 3p6 4s2 3d323V[Ar] 3d3 4s223V3+[Ar] 3d224Cr1s2 2s2 2p6 3s2 3p6 4s1 3d524Cr[Ar] 3d5 4s124Cr3+[Ar] 3d325Mn1s2 2s2 2p6 3s2 3p6 4s2 3d525Mn[Ar] 3d5 4s225Mn2+[Ar] 3d526Fe1s2 2s2 2p6 3s2 3p6 4s2 3d626Fe[Ar] 3d6 4s226Fe2+[Ar] 3d627Co1s2 2s2 2p6 3s2 3p6 4s2 3d727Co[Ar] 3d7 4s227Co2+[Ar] 3d728Ni1s2 2s2 2p6 3s2 3p6 4s2 3d828Ni[Ar] 3d8 4s228Ni2+[Ar] 3d829Cu1s2 2s2 2p6 3s2 3p6 4s1 3d1029Cu[Ar] 3d10 4s129Cu2+[Ar] 3d930Zn1s2 2s2 2p6 3s2 3p6 4s2 3d1030Zn[Ar] 3d10 4s230Zn2+[Ar] 3d10Why electron fill 4s first? 14s fill first 4s2 4s greater penetration/closer to nucleus 4s lower in energy3d23d filled 3d higher energy3d4s 20Ca4s [Ar] 4s2 3d021Sc [Ar] 4s2 3d1Electrons lost from 4s then 3d 21. d blockException to d block elements 4s energy level lower than 3dNoble gas notation Condensed configurationElectron configuration d blockPositive Ions21Sc1s2 2s2 2p6 3s2 3p6 4s2 3d121Sc[Ar] 3d1 4s221Sc3+[Ar]22Ti1s2 2s2 2p6 3s2 3p6 4s2 3d222Ti[Ar] 3d2 4s222Ti4+[Ar]23V1s2 2s2 2p6 3s2 3p6 4s2 3d323V[Ar] 3d3 4s223V3+[Ar] 3d224Cr1s2 2s2 2p6 3s2 3p6 4s1 3d524Cr[Ar] 3d5 4s124Cr3+[Ar] 3d325Mn1s2 2s2 2p6 3s2 3p6 4s2 3d525Mn[Ar] 3d5 4s225Mn2+[Ar] 3d526Fe1s2 2s2 2p6 3s2 3p6 4s2 3d626Fe[Ar] 3d6 4s226Fe2+[Ar] 3d627Co1s2 2s2 2p6 3s2 3p6 4s2 3d727Co[Ar] 3d7 4s227Co2+[Ar] 3d728Ni1s2 2s2 2p6 3s2 3p6 4s2 3d828Ni[Ar] 3d8 4s228Ni2+[Ar] 3d829Cu1s2 2s2 2p6 3s2 3p6 4s1 3d1029Cu[Ar] 3d10 4s129Cu2+[Ar] 3d930Zn1s2 2s2 2p6 3s2 3p6 4s2 3d1030Zn[Ar] 3d10 4s230Zn2+[Ar] 3d10Why electron fill 4s first? 1Why electrons lost from 4s first4s fill first 4s2 4s greater penetration/closer to nucleus 4s lower in energy3d23d filled 3d higher energy33d once filled 3d e attracted by increasing nuclear charge 3d orbitals lower in energy - shield 4s e3d4s4s 20Ca4s [Ar] 4s2 3d0Electrons lost from 4s then 3d21Sc [Ar] 4s2 3d13d 21Sc [Ar] 3d2 4s2 22. d blockException to d block elements 4s energy level lower than 3dNoble gas notation Condensed configurationElectron configuration d blockPositive Ions21Sc1s2 2s2 2p6 3s2 3p6 4s2 3d121Sc[Ar] 3d1 4s221Sc3+[Ar]22Ti1s2 2s2 2p6 3s2 3p6 4s2 3d222Ti[Ar] 3d2 4s222Ti4+[Ar]23V1s2 2s2 2p6 3s2 3p6 4s2 3d323V[Ar] 3d3 4s223V3+[Ar] 3d224Cr1s2 2s2 2p6 3s2 3p6 4s1 3d524Cr[Ar] 3d5 4s124Cr3+[Ar] 3d325Mn1s2 2s2 2p6 3s2 3p6 4s2 3d525Mn[Ar] 3d5 4s225Mn2+[Ar] 3d526Fe1s2 2s2 2p6 3s2 3p6 4s2 3d626Fe[Ar] 3d6 4s226Fe2+[Ar] 3d627Co1s2 2s2 2p6 3s2 3p6 4s2 3d727Co[Ar] 3d7 4s227Co2+[Ar] 3d728Ni1s2 2s2 2p6 3s2 3p6 4s2 3d828Ni[Ar] 3d8 4s228Ni2+[Ar] 3d829Cu1s2 2s2 2p6 3s2 3p6 4s1 3d1029Cu[Ar] 3d10 4s129Cu2+[Ar] 3d930Zn1s2 2s2 2p6 3s2 3p6 4s2 3d1030Zn[Ar] 3d10 4s230Zn2+[Ar] 3d10Why electron fill 4s first? 1Why electrons lost from 4s first4s fill first 4s2 4s greater penetration/closer to nucleus 4s lower in energy3d23d filled 3d higher energy344s higher in energy 4s e lost first4s4s4s [Ar] 4s2 3d04S FIRST IN FIRST OUT3d once filled 3d e attracted by increasing nuclear charge 3d orbitals lower in energy - shield 4s e3d20CaElectrons lost from 4s then 3d21Sc [Ar] 4s2 3d13d3d 21Sc [Ar] 3d2 4s2lose 2 electron21Sc2+ [Ar] 3d2 4s0 23. d blockd block elements and ions 4s energy level lower than 3dElectron configuration d block Electron lost from 4s then 3d21Sc22Ti[Ar] 3d2 4s223V Cr25Mn[Ar] 3d5 4s226Fe[Ar] 3d6 4s227Co[Ar] 3d7 4s228Ni[Ar] 3d8 4s229Cu[Ar] 3d10 4s130Zn[Ar] 3d10 4s2lose 3 e3d3d4s4s lose 2 e3d3d[Ar]V3+[Ar] 3d224Cr3+[Ar] 3d3Mn2+[Ar] 3d5264sTi4+254s[Ar]Fe2+[Ar] 3d627[Ar] 3d5 4s13dSc3+233d21 22lose 3 e[Ar] 3d3 4s2244s4s[Ar] 3d1 4s2Positive IonsCo2+[Ar] 3d728Ni2+[Ar] 3d829Cu2+[Ar] 3d930Zn2+[Ar] 3d10 24. d blockd block elements and ions 4s energy level lower than 3dElectron configuration d block Electron lost from 4s then 3d21Sc22Ti[Ar] 3d2 4s223V Cr25Mn[Ar] 3d5 4s226Fe[Ar] 3d6 4s227Co28Ni[Ar] 3d8 4s229Cu[Ar] 3d10 4s130Zn[Ar] 3d10 4s23d3d4s4s lose 2 e3d3dV3+[Ar] 3d224Cr3+[Ar] 3d3Mn2+[Ar] 3d5Fe2+[Ar] 3d6Co2+[Ar] 3d728Ni2+[Ar] 3d829Cu2+[Ar] 3d930[Ar] 3d7 4s2lose 3 e[Ar]264sTi4+254s[Ar]27[Ar] 3d5 4s13dSc3+233d21 22lose 3 e[Ar] 3d3 4s2244s4s[Ar] 3d1 4s2Positive IonsZn2+[Ar] 3d10Video on Ionization energyClick here to view IEClick here to view IEClick here to view IE 25. Ionization energy (IE) 1st Ionization energy Min energy to remove 1 mole e from 1 mole of element in gaseous state M(g) M+ (g) + e2nd Ionization energy Min energy to remove 1 mole e from 1 mole of +1 ion to form +2 ion M+(g) M2+ (g) + eIonization energyWhy IE increases across the period? Why IE decreases down a group ? 26. Ionization energy (IE) 1st Ionization energy Min energy to remove 1 mole e from 1 mole of element in gaseous state M(g) M+ (g) + e2nd Ionization energy Min energy to remove 1 mole e from 1 mole of +1 ion to form +2 ion M+(g) M2+ (g) + eIonization energyFactors affecting ionization energy1Distance from nucleus electronDistance near to nucleus IE High Distance far away nucleus IE Low Distance near Strong electrostatic forces attraction bet nucleus and e IE High Why IE increases across the period? Why IE decreases down a group ? 27. Why IE increases across the period? Why IE decreases down a group ?Ionization energy (IE) 1st Ionization energy Min energy to remove 1 mole e from 1 mole of element in gaseous state M(g) M+ (g) + e2nd Ionization energy Min energy to remove 1 mole e from 1 mole of +1 ion to form +2 ion M+(g) M2+ (g) + eIonization energyFactors affecting ionization energy12Distance from nucleusNuclear chargeelectron+3+4+5+6Nuclear charge increaseDistance near to nucleus IE High Distance far away nucleus IE Low Nuclear charge high (more proton) IE High Nuclear charge low (less proton) IE Low +6Distance nearNuclear charge Strong electrostatic forces attraction bet nucleus and eStrong electrostatic forces attraction bet nucleus and eIE High IE High 28. Why IE increases across the period? Why IE decreases down a group ?Ionization energy (IE) 1st Ionization energy Min energy to remove 1 mole e from 1 mole of element in gaseous state M(g) M+ (g) + e2nd Ionization energy Min energy to remove 1 mole e from 1 mole of +1 ion to form +2 ion M+(g) M2+ (g) + eIonization energyFactors affecting ionization energy12Distance from nucleus3Nuclear chargeelectron+3+4+5+6Effective Nuclear Charge (ENC)/(Zeff) Screening effect/shielding Effective nuclear charge (ENC)/(Zeff) (Zeff) = Nuclear charge (Z) shielding effect Net positive charge felt by valence electrons.Nuclear charge increaseDistance near to nucleus IE High Distance far away nucleus IE Low Nuclear charge high (more proton) IE High Nuclear charge low (less proton) IE Low +6Inner electron shield valence e from positive charge Distance nearNuclear charge Higher electron/electron repulsionStrong electrostatic forces attraction bet nucleus and eStrong electrostatic forces attraction bet nucleus and eEasier valence e to leaveIE High IE High IE Low 29. IE drop from Be to B and N to OIonization Energy- Period 2Why IE increases across the period 2? IE increases across period 2 Nuclear charge increase Strong electrostatic forces attraction bet nucleus and eIE High LiBeBCNOFNe2p 2s 1s 1s2 2s11s2 2s21s2 2s2 2p11s2 2s2 2p21s2 2s2 2p31s2 2s2 2p41s2 2s2 2p51s2 2s2 2p6 30. IE drop from Be to B and N to OIonization Energy- Period 2Why IE increases across the period 2? IE increases across period 2 Nuclear charge increase Strong electrostatic forces attraction bet nucleus and eIE High LiBeBCNOFNe2p 2s 1s 1s2 2s11s2 2s21s2 2s2 2p11s2 2s2 2p2IE drop from Be to BElectron in p sublevel of B further away from nucleusWeak electrostatic force attraction between nucleus and electronIE - Low period 21s2 2s2 2p31s2 2s2 2p41s2 2s2 2p51s2 2s2 2p6 31. IE drop from Be to B and N to OIonization Energy- Period 2Why IE increases across the period 2? IE increases across period 2 Nuclear charge increase Strong electrostatic forces attraction bet nucleus and eIE High LiBeBCNOFNe2p 2s 1s 1s2 2s11s2 2s21s2 2s2 2p11s2 2s2 2p2IE drop from Be to B1s2 2s2 2p31s2 2s2 2p4IE drop from N to OElectron in p sublevel of B further away from nucleus2 electrons in same p orbital - Greater e/e repulsionWeak electrostatic force attraction between nucleus and electronEasier to remove e IE - Low IE - Low period 21s2 2s2 2p51s2 2s2 2p6 32. IE drop from Mg to AI and P to SIonization Energy- Period 3Why IE increases across the period 3? IE increases across period 3 Nuclear charge increase Strong electrostatic forces attraction bet nucleus and eIE High NaMgAISiPSCIAr3p3s [Ne] 3s1[Ne] 3s2[Ne] 3s2 3p1[Ne] 3s2 3p2[Ne] 3s2 3p3[Ne] 3s2 3p4[Ne] 3s2 3p5[Ne] 3s2 3p6 33. IE drop from Mg to AI and P to SIonization Energy- Period 3Why IE increases across the period 3? IE increases across period 3 Nuclear charge increase Strong electrostatic forces attraction bet nucleus and eIE High NaMgAISiPSCIAr3p3s [Ne] 3s1[Ne] 3s2[Ne] 3s2 3p1[Ne] 3s2 3p2IE drop from Mg to AIElectron in p sublevel of AI further away from nucleus Weak electrostatic force attraction between nucleus and electronIE - Low Period 3[Ne] 3s2 3p3[Ne] 3s2 3p4[Ne] 3s2 3p5[Ne] 3s2 3p6 34. IE drop from Mg to AI and P to SIonization Energy- Period 3Why IE increases across the period 3? IE increases across period 3 Nuclear charge increase Strong electrostatic forces attraction bet nucleus and eIE High NaMgAISiPSCIAr3p3s [Ne] 3s1[Ne] 3s2[Ne] 3s2 3p1[Ne] 3s2 3p2IE drop from Mg to AI[Ne] 3s2 3p3[Ne] 3s2 3p4IE drop from P to SElectron in p sublevel of AI further away from nucleus2 electrons in same p orbital - Greater e/e repulsionWeak electrostatic force attraction between nucleus and electronEasier to remove e IE - Low IE - Low Period 3[Ne] 3s2 3p5[Ne] 3s2 3p6 35. IE for Period 2 and 3Ionization Energy- Period 2 and 3Why IE period 3 lower than 2? Period 3 3 shells/energy levelperiod 2 Period 3Valence e further from nucleusHigh shielding effect more inner eWeaker electrostatic forces attraction bet nucleus and e IE Lower period 2 LiBeBCNOFNe2p 2s 1s 1s2 2s11s2 2s21s2 2s2 2p11s2 2s2 2p21s2 2s2 2p31s2 2s2 2p41s2 2s2 2p51s2 2s2 2p6Period 3 NaMgAISiPS[Ne] 3s2 3p1[Ne] 3s2 3p2[Ne] 3s2 3p3[Ne] 3s2 3p4CIAr3p 3s 2p 2s 1s [Ne] 3s1[Ne] 3s2[Ne] 3s2 3p5[Ne] 3s2 3p6 36. IE for Period 2 and 3Ionization Energy- Period 2 and 3Why IE period 3 lower than 2? Period 3 3 shells/energy levelperiod 2 Period 3Valence e further from nucleusHigh shielding effect more inner eWeaker electrostatic forces attraction bet nucleus and e IE Lower period 2 LiBeBCNOFNe2p 2s 1s 1s2 2s11s2 2s21s2 2s2 2p11s2 2s2 2p21s2 2s2 2p31s2 2s2 2p41s2 2s2 2p51s2 2s2 2p6Period 3 NaMgAISiPS[Ne] 3s2 3p1[Ne] 3s2 3p2[Ne] 3s2 3p3[Ne] 3s2 3p4CIAr3rd level3p 3s 2p 2s 1s [Ne] 3s1[Ne] 3s2[Ne] 3s2 3p5[Ne] 3s2 3p6 37. IE for Ne and ArIonization Energy- Period 2 and 3Why Ne and Ar have HIGH IE ? Full electron configuration, 2.8/2.8.8neon argonMost energetically stable structure Difficult to lose electronIE High period 2 LiBeBCNOFNe2p 2s 1s 1s2 2s11s2 2s21s2 2s2 2p11s2 2s2 2p21s2 2s2 2p31s2 2s2 2p41s2 2s2 2p51s2 2s2 2p6Period 3 NaMgAISiPS[Ne] 3s2 3p1[Ne] 3s2 3p2[Ne] 3s2 3p3[Ne] 3s2 3p4CIAr3p3s 2p 2s 1s [Ne] 3s1[Ne] 3s2[Ne] 3s2 3p5[Ne] 3s2 3p6 38. Successive Ionization Energy (IE) for Mg ( 2.8.2) 1st Ionization energy Min energy to remove 1 mole e from 1 mole of element in gaseous state M(g) M+(g) + e2nd Ionization energy Min energy to remove 1 mole e from 1 mole of +1 ion to form +2 ion M+(g) M2+(g) + eMg 3rd energy level1st + 2nd electron 3s 2p2nd energy level3rd to 8th electron9th to 10th electron 2s1st energy level11th to 12th electron 1s1s2 2s2 2p6 3s2Successive Ionization Energy (IE) for magnesium 39. Successive Ionization Energy (IE) for Mg ( 2.8.2)Successive Ionization Energy (IE) for magnesium1st Ionization energy Min energy to remove 1 mole e from 1 mole of element in gaseous state M(g) M+(g) + e 12nd Ionization energy Min energy to remove 1 mole e from 1 mole of +1 ion to form +2 ion M+(g) M2+(g) + eMg 3rd energy level1st + 2nd electron 3s 2p2nd energy level3rd to 8th electron9th to 10th electron 2s1st energy level11th to 12th electron 1s1s2 2s2 2p6 3s2 1Successive (IE) Mg (2.8.2) show IE increase when e removed Ion become increasingly more positive as more e are removed Electron-electron repulsion decrease as more e removedHigh electrostatic forces attractionIE High 40. Successive Ionization Energy (IE) for Mg ( 2.8.2)Successive Ionization Energy (IE) for magnesium1st Ionization energy Min energy to remove 1 mole e from 1 mole of element in gaseous state M(g) M+(g) + e 12nd Ionization energy Min energy to remove 1 mole e from 1 mole of +1 ion to form +2 ion M+(g) M2+(g) + e2Mg 3rd energy level1st + 2nd electron 3s 2p2nd energy level3rd to 8th electron9th to 10th electron 2s1st energy level11th to 12th electron 1s1s2 2s2 2p6 3s2 1Successive (IE) Mg (2.8.2) show IE increase when e removed2Successive (IE) Mg (2.8.2) show High jump in 2nd to 3rd IE High jump in 10th to 11th IE Ion become increasingly more positive as more e are removed Electron-electron repulsion decrease as more e removedHigh jump in IE presence of new inner shellHigh electrostatic forces attractionElectron nearer to nucleus High electrostatic forces attractionIE High IE High 41. Successive Ionization Energy (IE) for Mg ( 2.8.2)Successive Ionization Energy (IE) for magnesium1st Ionization energy Min energy to remove 1 mole e from 1 mole of element in gaseous state M(g) M+(g) + e 12nd Ionization energy Min energy to remove 1 mole e from 1 mole of +1 ion to form +2 ion M+(g) M2+(g) + e2Mg33rd energy level1st + 2nd electron 3s 2p2nd energy level3rd to 8th electron9th to 10th electron 2s1st energy level11th to 12th electron 1s1s2 2s2 2p6 3s2 1Successive (IE) Mg (2.8.2) show IE increase when e removed2Successive (IE) Mg (2.8.2) show High jump in 2nd to 3rd IE High jump in 10th to 11th IE3Successive (IE) Mg (2.8.2) show Presence of 3 energy level Ion become increasingly more positive as more e are removed Electron-electron repulsion decrease as more e removedHigh jump in IE presence of new inner shell1st + 2nd e outmost shell (3rd level)High electrostatic forces attractionElectron nearer to nucleus High electrostatic forces attraction3rd to 10th e 2nd shell (2nd level)IE High IE High 11th to 12th e innermost shell (1st level) 42. Successive Ionization Energy (IE) for Mg ( 2.8.2)Successive Ionization Energy (IE) for magnesium1st Ionization energy Min energy to remove 1 mole e from 1 mole of element in gaseous state M(g) M+(g) + e42s and 2p2nd Ionization energy Min energy to remove 1 mole e from 1 mole of +1 ion to form +2 ion M+(g) M2+(g) + eMg 3rd energy level1st + 2nd electron 3s 2p2nd energy level3rd to 8th electron9th to 10th electron 2s1st energy level11th to 12th electron 1s1s2 2s2 2p6 3s2 4Successive (IE) Mg (2.8.2) show Presence of sublevel, 2s + 2pSlow gradual increase in IE from 3rd to 10th e3rd to 8th e in 2p orbital9th to 10th e inner 2s orbital 43. Successive Ionization Energy (IE) for Mg ( 2.8.2)Successive Ionization Energy (IE) for magnesium1st Ionization energy Min energy to remove 1 mole e from 1 mole of element in gaseous state M(g) M+(g) + e542s and 2p2nd Ionization energy Min energy to remove 1 mole e from 1 mole of +1 ion to form +2 ion M+(g) M2+(g) + eMg 3rd energy level1st + 2nd electron 3s 2p2nd energy level3rd to 8th electron9th to 10th electron 2s1st energy level11th to 12th electron 1s1s2 2s2 2p6 3s2 4Successive (IE) Mg (2.8.2) show Presence of sublevel, 2s + 2p5Successive (IE) Mg (2.8.2) show Succesive IE increasingSlow gradual increase in IE from 3rd to 10th eSpecies form increase in proton/e ratio by losing e3rd to 8th e in 2p orbital9th to 10th e inner 2s orbitalSpecies becomes more positively chargedIE High 44. Successive Ionization Energy (IE) for Mg ( 2.8.2) 1st Ionization energy Min energy to remove 1 mole e from 1 mole of element in gaseous state M(g) M+(g) + eSuccessive Ionization Energy (IE) for magnesium5 6 42s and 2p2nd Ionization energy Min energy to remove 1 mole e from 1 mole of +1 ion to form +2 ion M+(g) M2+(g) + eMg 3rd energy level1st + 2nd electron 3s 2p2nd energy level3rd to 8th electron9th to 10th electron 2s1st energy level11th to 12th electron 1s1s2 2s2 2p6 3s2 Slow gradual increase in IE from 3rd to 10th e4Successive (IE) Mg (2.8.2) show Presence of sublevel, 2s + 2p5Successive (IE) Mg (2.8.2) show Succesive IE increasingSpecies form increase in proton/e ratio by losing e6Successive (IE) Mg (2.8.2) show More difficult to lose eM(g) M+(g) + eM+ M2++ e3rd to 8th e in 2p orbital9th to 10th e inner 2s orbitalSpecies becomes more positively chargedM2+ M3++ eMore energy need to lose eIE High IE High 45. IB Questions on IEs 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] 3s219 201K Ca[Ar]4s1[Ar]1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p6 6s2 4f14 5d106p2 [Xe] 6s2 4f14 5d10 6p24s2Identify 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 4p62Write electron configuration for X, Y and Z ElementGroupPeriodX23Y152Z1833Write 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+ - 46. IB Questions on IEs 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 47. IB Questions on IEs 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] 3s219 204K Ca[Ar] [Ar]1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p6 6s2 4f14 5d106p2 [Xe] 6s2 4f14 5d10 6p24s1 4s2Successive IE of X is shown below Predict the group and arrange in order of increasing proton number Element1st IE2nd IE3rd IE4th IEP7461423768910456Q92017681457821343R587113448906453S5421045412154125Successive IE of X is shown below Determine electron structure of XSuccessive IE (kJ/mol)131433025436743610647137687156484736 48. IB Questions on IEs 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] 3s219 204K Ca[Ar] [Ar]1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p6 6s2 4f14 5d106p2 [Xe] 6s2 4f14 5d10 6p24s1 4s2Successive IE of X is shown below Predict the group and arrange in order of increasing proton number Element1st IE2nd IE3rd IE4th IEP7461423768910456Q92017681457821343R587113448906453S542104541215412Answer All in Gp 2 2 valence electron Order increasing proton number Q, P, R, S ReasonGp 2, cause 1st and 2nd IE low Q Highest IE (less shell/energy level) S Lowest IE (more shell/energy level)5Successive IE of X is shown below Determine electron structure of XSuccessive IE (kJ/mol)131433025436Answer: X = 6 outermost electron, Gp 6, 2.6 Reason - 1st IE to 6th IE are low.743610647137687156484736 49. IB Questions on IE 6Successive IE of sodium is shown below: State full electron structure and explain how the successive IE are related to Its electron configuration.8Successive IE for 4 element shown below a) Which element form charge +1 b) Predict C in periodic table c) Which element requires least amt energy to charge a gaseous ion which carry charge +3 d) Which element belong to same group? Element1st IE2nd IE3rd IE4th IEA423302146575867B7541431774110432C5571814273511843D5971104494263427Successive IE of magnesium is shown below: Explain the large increase in 10th and 11th IE and the general trend of Increasing successive IE for Mg. 50. IB Questions on IE 6Successive IE of sodium is shown below: State full electron structure and explain how the successive IE are related to Its electron configuration.7Successive IE of magnesium is shown below: Explain the large increase in 10th and 11th IE and the general trend of Increasing successive IE for Mg.11th electron10th electronAnswer: 1s2 2s2 2p6 3s1 Reason: 1st electron easiest to remove, or 1st e in outmost shell/n= 3 energy level Large increase in IE bet 1st and 2nd as 2nd electron located in inner level, n=2 Next 8 electrons more difficult to remove as the ion now is positively charged Large increase in IE between 9th and 10th , two innermost electron 10th/11th in n=1 (close to nucleus) 8Successive IE for 4 element shown below a) Which element form charge +1 b) Predict C in periodic table c) Which element requires least amt energy to charge a gaseous ion which carry charge +3 d) Which element belong to same group? Element1st IE2nd IE3rd IE4th IEA423302146575867B7541431774110432C5571814273511843D597110449426342Answer: Reason: 10th electron comes from 2nd energy level, (n=2) and 11th electron from n=1 Electron in 1st energy level (n=1) closer to nucleus/ not shielded by inner electrons Successive IE high as it is more difficult to remove e from a positively charged ion.Answer: A Gp 1, B - Gp 2, C Gp 3, D Gp 2 a) A- Gp 1 lose 1 electron foming +1 b) C Gp 3 c) Total IE = 1st IE + 2nd IE + 3rd IE A = 8101 B= 9926 C = 5106 D = 6643 C requires least Gp 3 lose 3 e easily d) B and D 51. 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