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Periodic Table

Periodic Table. Kelter, Carr, Scott, Chemistry A Wolrd of Choices 1999, page 74. Electron Configurations and the Periodic Table. Periodic Patterns. Period # energy level (subtract for d & f) A/B Group # total # of valence e - Column within sublevel block # of e - in sublevel.

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Periodic Table

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  1. Periodic Table Kelter, Carr, Scott, Chemistry A Wolrd of Choices 1999, page 74

  2. Electron Configurations and the Periodic Table

  3. Periodic Patterns • 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. 1st column of s-block 1st Period s-block Periodic Patterns • Example - Hydrogen 1s1 Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  5. p s d (n-1) f (n-2) 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. 32 Ge 72.61 Periodic Patterns • Example -Germanium [Ar] 4s2 3d10 4p2 Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

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

  8. Stability • Electron Configuration Exceptions • Copper • EXPECT: [Ar] 4s2 3d9 • ACTUALLY: [Ar] 4s1 3d10 • Copper gains stability with a full d-sublevel. Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  9. Stability • Electron Configuration Exceptions • Chromium • EXPECT: [Ar] 4s2 3d4 • ACTUALLY: [Ar] 4s1 3d5 • Chromium gains stability with a half-full d-sublevel. Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  10. Stability • Ion Formation • Atoms gain or lose electrons to become more stable. • Isoelectronic with the Noble Gases. 3+ 1+ NA 2+ 1- 0 3- 2- Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  11. Stability • Ion Electron Configuration • Write the e- config for the closest Noble Gas • EX: Oxygen ion  O2-  Ne • O2- 10e- [He] 2s2 2p6 Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  12. Dmitri Mendeleev • Russian • Invented periodic table • Organized elements by properties • Arranged elements by atomic mass • Predicted existence of several unknown elements • Element 101 Dmitri Mendeleev

  13. Mendeleev’s Periodic Table

  14. Mendeleev’s Early Periodic Table TABELLE II GRUPPE I GRUPPE II GRUPPE III GRUPPE IV GRUPPE V GRUPPE VI GRUPPE VII GRUPPE VIII ___ ___ ___ ___ RH4 RH3 RH2 RH R2O RO R2O3 RO2 R2O5 RO3 R2O7 RO4 REIHEN 1 2 3 4 5 6 7 8 9 10 11 12 H = 1 Li = 7 Be = 9.4 B = 11 C = 12 N = 14 O = 16 F = 19 Na = 23 Mg = 24 Al = 27.3 Si = 28 P = 31 S = 32 Cl = 35.5 K = 39 Ca = 40 __ = 44 Ti = 48 V = 51 Cr = 52 Mn = 55 Fe = 56, Co = 59, Ni = 59, Cu = 63 (Cu = 63) Zn = 65 __ = 68 __ = 72 As = 75 Se = 78 Br = 80 Rb = 85 Sr = 87 ? Yt = 88 Zr = 90 Nb = 94 Mo = 96 __ = 100 Ru = 104, Rh = 104, Pd = 106, Ag = 108 (Ag = 108) Cd = 112 In = 113 Sn = 118 Sb = 122 Te = 125 J = 127 Cs = 133 Ba = 137 ? Di = 138 ? Ce = 140 __ __ __ __ __ __ __ ( __ ) __ __ __ __ __ __ __ __ ? Er = 178 ? La = 180 Ta = 182 W = 184 __ Os = 195, Ir = 197, Pt = 198, Au = 199 (Au = 199) Hg = 200 Tl= 204 Pb = 207 Bi = 208 __ __ __ __ __ Th = 231 __ U = 240 __ __ __ __ __ From Annalen der Chemie und Pharmacie, VIII, Supplementary Volume for 1872, p. 151.

  15. Elements Properties are Predicted O’Connor Davis, MacNab, McClellan, CHEMISTRY Experiments and Principles1982, page 119,

  16. Modern Periodic Table • H.G.J. Moseley • Arranged elements by increasing atomic number • Killed in WW I at age 28 (Battle of Gallipoli) 1887 - 1915

  17. Groups of Elements 1A 8A 1A 5A Nitrogen group Alkali metals H 1 2A 6A He 2 Alkali earth metals Oxygen group 1 1 2A 7A 3A 4A 5A 6A 7A Halogens Transition metals 3A 8A Noble gases Boron group Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 2 2 4A Carbon group Hydrogen Inner transition metals Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 3 3 8B 3B 4B 5B 6B 7B 1B 2B 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 4 4 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 5 5 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 * * 6 6 Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 W W 7 7 La 57 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 * Ac 89 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 W

  18. Groups of Elements Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3rd Edition, 1990, page 367

  19. He 2 Li 3 Be 4 N 7 O 8 F 9 Ne 10 Na 11 Mg 12 P 15 S 16 Cl 17 Ar 18 K 19 Ca 20 As 33 Se 34 Br 35 Kr 36 Rb 37 Sr 38 Sb 51 Te 52 I 53 Xe 54 Cs 55 Ba 56 Bi 83 Po 84 At 85 Rn 86 Fr 87 Ra 88 Groups of Elements 1 18 2 13 14 15 16 17 Alkali metals Oxygen family 1 16 Halogens Alkali earth metals 17 2 Noble gases Nitrogen family 18 15 Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3rd Edition, 1990, page 367

  20. Metalloids Metals and Nonmetals H 1 He 2 1 Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 Nonmetals 2 Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 3 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 4 METALS 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 5 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 * 6 Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 W 7 La 57 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 Ac 89 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

  21. Metals, Nonmetals, & Metalloids 1 Nonmetals 2 3 4 Metals 5 6 7 Metalloids Zumdahl, Zumdahl, DeCoste, World of Chemistry2002, page 349

  22. Properties of Metals, Nonmetals, and Metalloids METALS malleable, lustrous, ductile, good conductors of heat and electricity NONMETALS gases or brittle solids at room temperature, poor conductors of heat and electricity (insulators) METALLOIDS (Semi-metals) dull, brittle, semi-conductors (used in computer chips)

  23. 1894-1918 Ancient Times H He Midd. -1700 1923-1961 1965- 1735-1843 1843-1886 Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Rf Db Sg Bh Hs Mt Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Discovering the Periodic Table Journal of Chemical Education, Sept. 1989

  24. Electron Filling in Periodic Table metallic character increases nonmetallic character increases metallic character increases nonmetallic character increases

  25. Melting Points He 0.126 H -259.2 He -269.7 Mg 650 1 1 Symbol Melting point oC Li 180.5 Be 1283 B 2027 C 4100 N -210.1 O -218.8 F -219.6 Ne -248.6 2 2 > 3000 oC 2000 - 3000 oC Na 98 Mg 650 Al 660 Si 1423 P 44.2 S 119 Cl -101 Ar -189.6 3 3 K 63.2 Ca 850 Sc 1423 Ti 1677 V 1917 Cr 1900 Mn 1244 Fe 1539 Co 1495 Ni 1455 Cu 1083 Zn 420 Ga 29.78 Ge 960 As 817 Se 217.4 Br -7.2 Kr -157.2 4 4 Rb 38.8 Sr 770 Y 1500 Zr 1852 Nb 2487 Mo 2610 Tc 2127 Ru 2427 Rh 1966 Pd 1550 Ag 961 Cd 321 In 156.2 Sn 231.9 Sb 630.5 Te 450 I 113.6 Xe -111.9 5 5 Cs 28.6 Ba 710 La 920 Hf 2222 Ta 2997 W 3380 Re 3180 Os 2727 Ir 2454 Pt 1769 Au 1063 Hg -38.9 Tl 303.6 Pb 327.4 Bi 271.3 Po 254 At Rn -71 6 6 Ralph A. Burns, Fundamentals of Chemistry , 1999, page 1999

  26. Densities of Elements H 0.071 He 0.126 1 1 Li 0.53 Be 1.8 B 2.5 C 2.26 N 0.81 O 1.14 F 1.11 Ne 1.204 2 2 Na 0.97 Mg 1.74 Al 2.70 Si 2.4 P 1.82w S 2.07 Cl 1.557 Ar 1.402 3 3 K 0.86 Ca 1.55 Sc (2.5) Ti 4.5 V 5.96 Cr 7.1 Mn 7.4 Fe 7.86 Co 8.9 Ni 8.90 Cu 8.92 Zn 7.14 Ga 5.91 Ge 5.36 As 5,7 Se 4.7 Br 3.119 Kr 2.6 4 4 Rb 1.53 Sr 2.6 Y 5.51 Zr 6.4 Nb 8.4 Mo 10.2 Tc 11.5 Ru 12.5 Rh 12.5 Pd 12.0 Ag 10.5 Cd 8.6 In 7.3 Sn 7.3 Sb 6.7 Te 6.1 I 4.93 Xe 3.06 5 5 Cs 1.90 Ba 3.5 La 6.7 Hf 13.1 Ta 16.6 W 19.3 Re 21.4 Os 22.48 Ir 22.4 Pt 21.45 Au 19.3 Hg 13.55 Tl 11.85 Pb 11.34 Bi 9.8 Po 9.4 At --- Rn 4.4 6 6 8.0 – 11.9 g/cm3 12.0 – 17.9 g/cm3 > 18.0 g/cm3 Mg 1.74 Symbol Density in g/cm3C, for gases, in g/L W Ralph A. Burns, Fundamentals of Chemistry , 1999, page 200

  27. Periodic Trends in Atomic Radii LeMay Jr, Beall, Robblee, Brower, Chemistry Connections to Our Changing World , 1996, page 175

  28. Relative Size of Atoms Zumdahl, Zumdahl, DeCoste, World of Chemistry2002, page 350

  29. Shielding Effect Valence Kernel electrons block the attractive force of the nucleus from the valence electrons + - - nucleus - Electrons - Electron Shield “kernel” electrons

  30. Atomic Radii

  31. Atomic Radii vs. Ionic Radii

  32. First Ionization Energy Plot

  33. First Ionization Energy Plot

  34. First Ionization Energy Plot

  35. sodium ion Na+ e- e- e- e- 11p+ e- e- e- e- e- e- Formation of Cation sodium atom Na e- e- e- e- e- e- loss of one valence electron 11p+ e- e- e- e- e- e-

  36. chloride ion Cl1- e- e- e- e- e- e- e- 17p+ e- e- e- e- e- e- e- e- e- Formation of Anion chlorine atom Cl gain of one valence electron e- e- e- e- e- e- e- e- 17p+ e- e- e- e- e- e- e- e- e- e-

  37. Summary of Periodic Trends Shielding is constant Atomic radius decreases Ionization energy increases Electronegativity increases Nuclear charge increases 1A 0 Nuclear charge increases Shielding increases Atomic radius increases Ionic size increases Ionization energy decreases Electronegativity decreases 2A 3A 4A 6A 7A 5A Ionic size (cations) Ionic size (anions) decreases decreases

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