2. s p d (n-1) f (n-2) 6767 Periodic Patterns 1s1s1s1s 2s2s2s2s 3s3s3s3s 4s4s4s4s 5s5s5s5s 6s6s6s6s 7s7s7s7s 3d3d3d3d 4d4d4d4d 5d5d5d5d 6d6d6d6d 1s1s1s1s 2p2p2p2p 3p3p3p3p 4p4p4p4p 5p5p5p5p 6p6p6p6p 7p7p7p7p 4f4f4f4f 5f5f5f5f 12345671234567

3. Period # –energy level (subtract for d & f) A/B Group # –total # of valence e - Column within sublevel block –# of e - in sublevel Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

4. s-block1st Period 1s 1 1 st column of s-block Periodic Patterns Example - Hydrogen Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

5. Periodic Patterns Shorthand Configuration –Core electrons: Go up one row and over to the Noble Gas. –Valence electrons: On the next row, fill in the # of e - in each sublevel. Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

6. [Ar]4s 2 3d 10 4p 2 Periodic Patterns GermaniumExample - Germanium Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem Ge 72.61 32

7. Full energy level Full sublevel (s, p, d, f) Half-full sublevel Stability Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

8. Electron Configuration Exceptions –Copper EXPECT :[Ar] 4s 2 3d 9 ACTUALLY :[Ar] 4s 1 3d 10 –Copper gains stability with a full d-sublevel. Stability Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

9. Electron Configuration Exceptions –Chromium EXPECT :[Ar] 4s 2 3d 4 ACTUALLY :[Ar] 4s 1 3d 5 –Chromium gains stability with a half-full d-sublevel. Stability Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

10. Electron Filling in Periodic Table K4s1K4s1 Ca 4s 2 Sc 3d 1 Ti 3d 2 V3d3V3d3 Mn 3d 5 Fe 3d 6 Co 3d 7 Ni 3d 8 Cr 3d 4 Cu 3d 9 Zn 3d 10 Ga 4p 1 Ge 4p 2 As 4p 3 Se 4p 4 Br 4p 5 Kr 4p 6 1 2 3 4 s d p s Cr 4s 1 3d 5 Cu 4s 1 3d 10 4f4f 4d4d 4p4p 4s4s n = 4 3d3d 3p3p 3s3s n = 3 2p2p 2s2s n = 2 1s1sn = 1 Energy 4s3d Cr 4s 1 3d 5 4s3d Cu 4s 1 3d 10 Cr 3d 5 Cu 3d 10

11. Stability Ion Formation –Atoms gain or lose electrons to become more stable. –Isoelectronic with the Noble Gases. Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

12. O 2- 10e - [He] 2s 2 2p 6 Stability Ion Electron Configuration –Write the e - config for the closest Noble Gas –EX: Oxygen ion  O 2-  Ne Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

13. http://www.unit5.org/christjs/tempT 27dFields-Jeff/Atom1.htm Electron Configurations Electron Configuration WSElectron Configuration WS Pattern Electron Configuration WSElectron Configuration WS PatternPattern

14. Orbital Diagrams for Nickel 2s2s2p2p 3s3s 3p3p4s4s3d3d1s1s2s2s2p2p 3s3s 3p3p4s4s3d3d1s1s2s2s2p2p 3s3s 3p3p4s4s3d3d1s1s 2s2s2p2p 3s3s 3p3p4s4s3d3d1s1s Excited State Pauli Exclusion Hund’s Rule Ni 58.6934 28 2 2 6 2 6 2 8 2 2 6 2 6 1 9

15. Orbital Diagrams for Nickel 2s2s2p2p 3s3s 3p3p4s4s3d3d1s1s2s2s2p2p 3s3s 3p3p4s4s3d3d1s1s2s2s2p2p 3s3s 3p3p4s4s3d3d1s1s 2s2s2p2p 3s3s 3p3p4s4s3d3d1s1s Excited State VIOLATES Pauli Exclusion VIOLATES Hund’s Rule Ni 58.6934 28 2 2 6 2 6 2 8 2 2 6 2 6 1 9

16. Write out the complete electron configuration for the following: 1) An atom of nitrogen 2) An atom of silver 3) An atom of uranium (shorthand) Fill in the orbital boxes for an atom of nickel (Ni) 2s2s2p2p 3s3s 3p3p4s4s3d3d1s1s Which rule states no two electrons can spin the same direction in a single orbital? Extra credit: Draw a Bohr model of a Ti 4+ cation. Ti 4+ is isoelectronic to Argon. POP QUIZ

17. Write out the complete electron configuration for the following: 1) An atom of nitrogen 2) An atom of silver 3) An atom of uranium (shorthand) Fill in the orbital boxes for an atom of nickel (Ni) 2s2s2p2p 3s3s 3p3p4s4s3d3d1s1s Which rule states no two electrons can spin the same direction in a single orbital? 1s 2 2s 2 2p 3 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 9 [Rn]7s 2 6d 1 5f 3 Extra credit: Draw a Bohr model of a Ti 4+ cation. 22+ n = n Pauli exclusion principle Ti 4+ is isoelectronic to Argon. Answer Key

18. Periodic Table – Filling Order

19. Electron Configurations and the Periodic Table

20. Orbitals Being Filled 1s1s 2s2s 3s3s 4s4s 5s5s 6s6s 7s7s 3d3d 4d4d 5d5d 6d6d 2p2p 3p3p 4p4p 5p5p 6p6p 1s1s La Ac 1 3 4 5 6 7 4f4f 5f5f Lanthanide series Actinide series Groups 8 Periods 1 2 2 3 4 5 6 7

21. Electron Filling in Periodic Table 1 2 3 4 5 6 7 s d p s f    

22. Li 3 H1H1 He 2 C6C6 N7N7 O8O8 F9F9 Ne 10 Na 11 B5B5 Be 4 H1H1 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24 Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36 Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag 47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 Cs 55 Ba 56 Hf 72 Ta 73 W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At 85 Rn 86 Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 Mg 12 Ce 58 Pr 59 Nd 60 Pm 61 Sm 62 Eu 63 Gd 64 Tb 65 Dy 66 Ho 67 Er 68 Tm 69 Yb 70 Lu 71 Th 90 Pa 91 U 92 Np 93 Pu 94 Am 95 Cm 96 Bk 97 Cf 98 Es 99 Fm 100 Md 101 No 102 Lr 103 La 57 Ac 89 1 2 3 4 5 6 7 s d p s f    

23. 1 2 3 4 5 6 7 s d p s f     Electron Filling in Periodic Table Li 2s 1 H 1s 1 He 1s 2 C 2p 2 N 2p 3 O 2p 4 F 2p 5 Ne 2p 6 Na 3s 1 B 2p 1 Be 2s 2 H 1s 1 Al 3p 1 Si 3p 2 P 3p 3 S 3p 4 Cl 3p 5 Ar 3p 6 K 4s 1 Ca 4s 2 Sc 3d 1 Ti 3d 2 V 3d 3 Cr 3d 5 Mn 3d 5 Fe 3d 6 Co 3d 7 Ni 3d 8 Cu 3d 10 Zn 3d 10 Ga 4p 1 Ge 4p 2 As 4p 3 Se 4p 4 Br 4p 5 Kr 4p 6 Rb 5s 1 Sr 5s 2 Y 4d 1 Zr 4d 2 Nb 4d 4 Mo 4d 5 Tc 4d 6 Ru 4d 7 Rh 4d 8 Pd 4d 10 Ag 4d 10 Cd 4p 1 In 5p 1 Sn 5p 2 Sb 5p 3 Te 5p 4 I 5p 5 Xe 5p 6 Cs 6s 1 Ba 6s 2 Hf 5d 2 Ta 5d 3 W 5d 4 Re 5d 5 Os 5d 6 Ir 5d 7 Pt 5d 9 Au 5d 10 Hg 5d 10 Tl 6p 1 Pb 6p 2 Bi 6p 3 Po 6p 4 At 6p 5 Rn 6p 6 Fr 7s 1 Ra 7s 2 H 1s 1 H 1s 1 H 1s 1 H 1s 1 H 1s 1 H 1s 1 Mg 3s 2 Ce 4f 2 Pr 4f 3 Nd 4f 4 Pm 4f 5 Sm 4f 6 Eu 4f 7 Gd 4f 7 Tb 4f 9 Dy 4f 10 Ho 4f 11 Er 4f 12 Tm 4f 13 Yb 4f 14 Lu 4f 114 Th 6d 2 Pa 5f 2 U 5f 3 Np 5f 4 Pu 5f 6 Am 5f 7 Cm 5f 7 Bk 5f 8 Cf 5f 10 Es 5f 11 Fm 5f 14 Md 5f 13 No 5f 14 Lr 5f 14 La 5d 1 Ac 6d 1 1 2 3 4 5 6 7 s d p s f    

24. Electron Filling in Periodic Table K4s1K4s1 Ca 4s 2 Sc 3d 1 Ti 3d 2 V3d3V3d3 Mn 3d 5 Fe 3d 6 Co 3d 7 Ni 3d 8 Cr 3d 4 Cu 3d 9 Zn 3d 10 Ga 4p 1 Ge 4p 2 As 4p 3 Se 4p 4 Br 4p 5 Kr 4p 6 1 2 3 4 s d p s Cr 4s 1 3d 5 Cu 4s 1 3d 10 4f4f 4d4d 4p4p 4s4s n = 4 3d3d 3p3p 3s3s n = 3 2p2p 2s2s n = 2 1s1sn = 1 Energy 4s3d Cr 4s 1 3d 5 4s3d Cu 4s 1 3d 10 Cr 3d 5 Cu 3d 10

25. Electron Configurations of First 18 Elements:

26. Electron Dot Diagrams H Li Na K Be Mg Ca B Al Ga C Si Ge N P As O S Se F Cl Br Ne Ar Kr He Group 1A 2A 3A 4A 5A 6A 7A 8A = valence electron s1s1 s2s2 s2p2s2p2 s2p3s2p3 s2p4s2p4 s2p5s2p5 s2p6s2p6 s2p1s2p1

27. First Four Energy Levels n = 1 n = 2 n = 3 n = 4 Energy

28. Sublevels

29. Principal Level 2 Divided

30. 4f4f 4d4d 4p4p 4s4s n = 4 3d3d 3p3p 3s3s n = 3 2p2p 2s2s n = 2 1s1s n = 1 Energy Sublevels

31. Metals, Nonmetals, Metalloids

32. Periodic Table