1. Chemical Symbols Ancient Astronomical Symbols Sun MoonMars Venus SaturnJupiterMercury Symbols used in the 16 th and 17 th Century Gold SilverIron Copper LeadTinMercury Alchemical Symbols used in the 15 th Century Fire AirEarthWater

2. Chemical Symbols Symbols used in the 18 th Century Antimony WaterSulfuric acidCopperSulfur Symbols used by John Dalton Carbon Hydrogen Oxygen Silver Sulfur Nitrogen S Lead Mercury Copper C L Gold Potassa Soda G WaterCarbon dioxideAlcohol

3. Origin of the Names of Elements Title Number of Elements Pre-chemical Names10 Names from celestial bodies 8 Names from mythology / superstition10 Names from minerals / ores, other than geographical names13 Names from colors 9 Names from properties other than color 8 Geographical names from the domicile or workplace of the discoverer(s)13 Geographical names from minerals / ores10 Constructed names16 Names from persons10

4. Names and Symbols of Selected Elements Name*SymbolName*Symbol AluminumAlLead (plumbum)Pb ArgonArLithiumLi BariumBaMagnesiumMg BoronBMercury (hydrargyrum)Hg BromineBrNeonNe CadmiumCdNickelNi CalciumCaNitrogenN CarbonCOxygenO ChlorineClPhosphorusP CobaltCoPotassium (kalium)K Copper (cuprum)CuSiliconSi FluorineFSilver (argentum)Ag Gold (aurum)AuSodium (natrum)Na HeliumHeStrontiumSr HydrogenHSulfurS IodineITin (stannum)Sn Iron (ferrum)FeZincZn *Names given in parentheses are ancient Latin or Greek words from which the symbols are derived.

5. Map of Elements Discovered

6. Several Synthetic Elements Man-made Bk = Berkelium Cf = Californium Am = Americium Synthetic – All made by nuclear bombardment at Berkeley, California, U.S.A.

7. How to Organize Elements… Periodic Table Designs

8. Dutch Periodic Table 106 107 108 109 110 111 112 113 114 115 116 117 118

9. “Mayan” Periodic Table

11. Stowe’s Periodic Table

13. Benfey’s Periodic Table

14. Law of Triads Name Atomic Mass Name Atomic Mass Name Atomic Mass Calcium 40 Barium 137 Average 88.5 Strontium 87.6 Chlorine 35.5 Iodine 127 Average 81.3 Bromine 79.9 Sulfur 32 Tellurium 127.5 Average 79.8 Selenium 79.2 Johann Döbereiner ~1817 Elements could be classified into groups of three, or triads based on trends in physical properties such as density, melting point, and atomic mass were observed.

15. Newlands Law of Octaves 1 Li Na K John Newlands ~1863 2 Be Mg 3 B Al 4 C Si 5NP5NP 6OS6OS 7 F Cl Arranged the 62 known elements into groups of seven according to increasing atomic mass and proposed that an eighth column would then repeat the properties of the first element in the previous group.

16. Dmitri Mendeleev Russian Invented periodic table Organized elements by properties Arranged elements by atomic mass Predicted existence of several unknown elements Noted some discrepancies with atomic mass Dmitri Mendeleev

17. Mendeleev’s Early Periodic Table GRUPPE I GRUPPE II GRUPPE III GRUPPE IV GRUPPE V GRUPPE VI GRUPPE VII GRUPPE VIII ___ ___ ___ ___ RH 4 RH 3 RH 2 RH R 2 O RO R 2 O 3 RO 2 R 2 O 5 RO 3 R 2 O 7 RO 4 REIHEN 1 2 3 4 5 6 7 8 9 10 11 12 Annalen der Chemie und Pharmacie From Annalen der Chemie und Pharmacie, VIII, Supplementary Volume for 1872, p. 151. 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 __ __ __ __ __ TABELLE II ? ? ?

18. Elements Properties are Predicted PropertyMendeleev’s Predictions in 1871Observed Properties Molar Mass Oxide formula Density of oxide Solubility of oxide Scandium (Discovered in 1877) 44 g M 2 O 3 3.5 g / ml Dissolves in acids 43.7 g Sc 2 O 3 3.86 g / ml Dissolves in acids Molar mass Density of metal Melting temperature Oxide formula Solubility of oxide Gallium (Discovered in 1875) 68 g 6.0 g / ml Low M 2 O 3 Dissolves in ammonia solution 69.4 g 5.96 g / ml 30 0 C Ga 2 O 3 Dissolves in ammonia Molar mass Density of metal Color of metal Melting temperature Oxide formula Density of oxide Chloride formula Density of chloride Boiling temperature of chloride Germanium (Discovered in 1886) 72 g 5.5 g / ml Dark gray High MO 2 4.7 g / ml MCl 4 1.9 g / ml Below 100 o C 71.9 g 5.47 g / ml Grayish, white 900 0 C GeO 2 4.70 g / ml GeCl 4 1.89 g / ml 86 0 C O’Connor Davis, MacNab, McClellan, CHEMISTRY Experiments and Principles 1982, page 119,

19. Modern Periodic Table Determined the atomic numbers of elements from their X -ray spectra (1914) Resolved discrepancies in Mendeleev’s arrangement. Arranged elements by increasing atomic number Henry G.J. Moseley 1887 - 1915

20. Describing the Periodic Table Periodic Law – the properties of elements repeat in a predictable pattern. Periods are ROWs; Numbered from 1 to 7. NUMBER the PERIODS on your periodic tables Group/Family are COLUMNs; Numbered from 1 to 18 (share similar chemical properties), NUMBER the GROUPS on your periodic tables Main Group Elements: Groups 1, 2, & 13 through 18; “s” & “p” block

21. Diatomic Elements ` H2H2 N2N2 O2O2 F2F2 Cl 2 Br 2 I2I2 Tl At S Li Na K Fr Be Mg Ca Ra Sc Ac He Ne Ar Kr Rn Ti V Cr Mn Fe Co Ni Cu ZnGa Ge As Se Rb Sr Y Xe Zr Nb Mo Tc Ru Rh Pd Ag CdIn Sn Sb Te Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Pb Bi Po Al Si P4P4 B C Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er TmYb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm MdNo Lr S8S8 Tl Diatomic Molecules Unable to stand alone; bonded to their identical twin Others: Sulfur = 8 ; Phosphorus = 4

22. Stop & Stations

24. Metals, Nonmetals, & Metalloids 1 2 3 4 5 6 7 Metals Metalloids Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 349 Nonmetals Pattern: Metals = blank Metalliods = diagonal Nonmetals = dot

25. Properties of Metals Good conductors of heat and electricity. Lustrous Ductile (stretched into thin wires) Malleable (pounded into thin sheets) Chemical property: Reaction with water which results in corrosion Chemical Reactions: lose electrons to form positively charged ions All are solids except for mercury

26. Properties of Non-Metals Poor Conductors of heat and electricity. Dull Not ductile Not malleable Solid non-metals are brittle Can be gases, liquids or solids. Tend to gain electrons to form negatively charged ions Share electrons in reaction with other non-metals. Sulfur

27. Properties of Metalloids Metalloids (metal-like) Exhibit properties of both metals and non-metals Solids that can be shiny or dull. Conduct heat and electricity better than non-metals but not as well as metals. Ductile and malleable. Silicon

28. Li 3 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   Hydrogen Alkali metals Alkaline Earth Metals Coinage Metals Other Transition Elements Metalloids (B, Si, Ge, As, Sb, Te, At) Halogens Noble Gases Other Nonmetals Lanthanides Actinides Other metals  

29. Groups of Elements 1 2 3 4 5 6 7     Li 3 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   1A 2A 1A 2A 3A 4A 5A 6A 7A 8A Alkali metals Alkali earth metals Transition metals Inner transition metals Boron group Carbon group Nitrogen group Oxygen group Halogens Noble gases Hydrogen 3B 5B6B7B 8B 1B2B 3A4A5A6A7A 8A 4B

30. Groups of Elements Dorin, Demmin, Gabel, Chemistry The Study of Matter, 3 rd Edition, 1990, page 367 N7N7 P 15 As 33 Sb 51 Bi 83 O8O8 S 16 Se 34 Te 52 Po 84 F9F9 Cl 17 Br 35 I 53 At 85 He 2 Ne 10 Ar 18 Kr 36 Xe 54 Rn 86 Li 3 Na 11 K 19 Rb 37 Cs 55 Fr 87 Be 4 Ca 20 Sr 38 Ba 56 Ra 88 Mg 12 1 2 1 2 15 16 17 18 Alkali metals Alkaline earth metals Nitrogen family Oxygen family Halogens Noble gases 1314151617 18

31. Hydrogen is in a class of its own. only needs 2 electrons to complete its valence shell. Characteristics Gas at room temperature. Flammable

32. Alkali Metals, Group 1 H N OF Cl Br I Li Na K Fr Be Mg Ca Ra Sc Ac He Ne Ar Kr Rn Ti V Cr Mn Fe Co Ni Cu ZnGa Ge As Se Rb Sr Y Xe Zr Nb Mo Tc Ru Rh Pd Ag CdIn Sn Sb Te Cs Ba La Hf Ta W Re Os Ir Pt Au HgTl Pb Bi PoAt Al Si P S B C Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er TmYb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm MdNo Lr

33. Alkali Metals Most REACTIVE metals. Characteristics Soft (Clay consistency) Dull Silver color Low Density Low Melting Point React violently with water React w/ halogens to form salt ns 1 valence electron configuration

34. Alkaline Earth Metals, Group 2 H N OF Cl Br I Li Na K Fr Be Mg Ca Ra Sc Ac He Ne Ar Kr Rn Ti V Cr Mn Fe Co Ni Cu ZnGa Ge As Se Rb Sr Y Xe Zr Nb Mo Tc Ru Rh Pd Ag CdIn Sn Sb Te Cs Ba La Hf Ta W Re Os Ir Pt Au HgTl Pb Bi PoAt Al Si P S B C Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er TmYb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm MdNo Lr

35. Alkaline Earth Metals Characteristics Soft Shiny silver color Low Density Found naturally as a compound Glow different colors “ns 2 ” valence electron configuration

36. Transition Metals Column 11 is known as “coinage metals” contains copper, silver & gold.

37. Transition Metals usually brightly colored often used to color paints. Characteristics High Density High Melting/Boiling Pt Good Catalysts Hard, Tough & Strong Multiple oxidation (charge) states Form compounds called oxides

38. Group 13: Boron Family 3 valence electrons forms +3 charged ions. Family includes a metalloid (boron), and the rest are metals. Family includes the most abundant metal in the earth’s crust; aluminum. Highly reactive & form stable compounds with oxygen “ns 2 np 1 ” valence electron configuration

39. Group 14: Carbon Family 4 valence electrons forms 3 oxidation states -4, +4 & +2 (loss of two np 2 gives a filled ns 2 subshell) Family includes a non-metal, metalloids, and metals. Carbon is called the “basis of life.” “ns 2 np 2 ” valence-electron configuration.

40. Group 15: Pnicogens H N OF Cl Br I Li Na K Fr Be Mg Ca Ra Sc Ac He Ne Ar Kr Rn Ti V Cr Mn Fe Co Ni Cu ZnGa Ge As Se Rb Sr Y Xe Zr Nb Mo Tc Ru Rh Pd Ag CdIn Sn Sb Te Cs Ba La Hf Ta W Re Os Ir Pt Au HgTl Pb Bi PoAt Al Si P S B C Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er TmYb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm MdNo Lr

41. Group 15: Nitrogen Family 5 valence electrons forms 3 oxidation states -3, +5 & +3 (three np electrons lost to give a filled ns2 subshell) Family includes non-metals, metalloids and metals Nitrogen makes up 79% of our atmosphere. “ns 2 np 3 ” valence electron configuration

42. Group 16: Chalcogens H N OF Cl Br I Li Na K Fr Be Mg Ca Ra Sc Ac He Ne Ar Kr Rn Ti V Cr Mn Fe Co Ni Cu ZnGa Ge As Se Rb Sr Y Xe Zr Nb Mo Tc Ru Rh Pd Ag CdIn Sn Sb Te Cs Ba La Hf Ta W Re Os Ir Pt Au HgTl Pb Bi PoAt Al Si P S B C Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er TmYb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm MdNo Lr

43. Group 16: Oxygen Family 6 valence electrons forms 3 oxidation states -2, +6 & +4 (four np electrons lost give filled ns 2 subshell) Oxygen is the most abundant element in the earth’s crust. It is extremely active and combines with almost all elements. “ns 2 np 4 ” valence-electron configuration O8O8 S 16 Se 34 Te 52 Po 84

44. Halogens, Group 17 H N OF Cl Br I Li Na K Fr Be Mg Ca Ra Sc Ac He Ne Ar Kr Rn Ti V Cr Mn Fe Co Ni Cu ZnGa Ge As Se Rb Sr Y Xe Zr Nb Mo Tc Ru Rh Pd Ag CdIn Sn Sb Te Cs Ba La Hf Ta W Re Os Ir Pt Au HgTl Pb Bi PoAt Al Si P S B C Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er TmYb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm MdNo Lr

45. Group 17: Halogen (Salt Makers) Family Most active non-metals. - never found free in nature Only group in all 3 states of matter React with alkali metals to form SALTS High electronegativity Non-metal qualities – dull, brittle, non- conductor “ns2np5” valence electron configuration

46. Noble Gases, Group 18 H N OF Cl Br I Li Na K Fr Be Mg Ca Ra Sc Ac He Ne Ar Kr Rn Ti V Cr Mn Fe Co Ni Cu ZnGa Ge As Se Rb Sr Y Xe Zr Nb Mo Tc Ru Rh Pd Ag CdIn Sn Sb Te Cs Ba La Hf Ta W Re Os Ir Pt Au HgTl Pb Bi PoAt Al Si P S B C Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er TmYb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm MdNo Lr

47. Group 18: Noble Gases Characteristics Inert (Non-reactive) due to their filled octet Colorless gas Odorless Tasteless Nonflammable Non-metal qualities – dull, brittle, non-conductor Found in small amounts in the earth's atmosphere. “ns 2 np 6 ” valence electron configuration

48. Lanthanide Series H N OF Cl Br I Li Na K Fr Be Mg Ca Ra Sc Ac He Ne Ar Kr Rn Ti V Cr Mn Fe Co Ni Cu ZnGa Ge As Se Rb Sr Y Xe Zr Nb Mo Tc Ru Rh Pd Ag CdIn Sn Sb Te Cs Ba La Hf Ta W Re Os Ir Pt Au HgTl Pb Bi PoAt Al Si P S B C Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er TmYb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm MdNo Lr La

49. Actinide Series H N OF Cl Br I Li Na K Fr Be Mg Ca Ra Sc Ac He Ne Ar Kr Rn Ti V Cr Mn Fe Co Ni Cu ZnGa Ge As Se Rb Sr Y Xe Zr Nb Mo Tc Ru Rh Pd Ag CdIn Sn Sb Te Cs Ba La Hf Ta W Re Os Ir Pt Au HgTl Pb Bi PoAt Al Si P S B C Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er TmYb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm MdNo Lr La

50. Rare Earth (Inner Transition) Elements Rare earth elements not particularly rare but long & tedious processes were required to purify the metals from their oxides prior to 1945 One element of the lanthanide series & most of the elements in the actinide series are called trans- uranium, which means synthetic or man-made. Characteristics High melting points Reactivity varies Usually bonded to non-metals Tarnish readily in air High electrical conductivity

51. Chemistry of the Groups 1 2 3 4 5 6 7     Li 3 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   1A 2A 3B 5B6B7B 8B 1B2B 3A4A5A6A7A 8A 4B Transition Metals Actinides Lanthanides

52. Metallic Characteristics metallic character increases nonmetallic character increases metallic character increases nonmetallic character increases

53. Extra Slides...

54. 1 2 3 4 5 6 Li 180.5 He -269.7 C 4100 N -210.1 O -218.8 F -219.6 Ne -248.6 Na 98 B 2027 Be 1283 H -259.2 Al 660 Si 1423 P 44.2 S 119 Cl -101 Ar -189.6 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 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 Cs 28.6 Ba 710 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 Mg 650 Mg 650 1 2 3 4 5 6 Melting Points Symbol Melting point o C > 3000 o C2000 - 3000 o C La 920 He 0.126 Ralph A. Burns, Fundamentals of Chemistry, 1999, page 1999

55. Elements with Highest Densities Year Density Element Discovered (g/cm 3 ) Osmium1804 22.59 Iridium1804 22.56 Platinum1784 21.45 Rhenium1925 21.01 Neptunium1940 20.47 Plutonium1940 20.26 Goldprehistoric 19.32 Tungsten1783 19.26 Uranium1789 19.05 Tantalum1802 16.67

56. 1 2 3 4 5 6  Li 0.53 He 0.126 C 2.26 N 0.81 O 1.14 F 1.11 Ne 1.204 Na 0.97 B 2.5 Be 1.8 H 0.071 Al 2.70 Si 2.4 P 1.82w S 2.07 Cl 1.557 Ar 1.402 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 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 Cs 1.90 Ba 3.5 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 Mg 1.74 1 2 3 4 5 6 Densities of Elements Mg 1.74 Symbol Density in g/cm 3 C, for gases, in g/L 8.0 – 11.9 g/cm 3 12.0 – 17.9 g/cm 3 > 18.0 g/cm 3 La 6.7

57. Oxidation States of Elements 1 3 4 5 6 7 Groups 8 2 F 1- Br 1- I 1- Cl 1- Transition metals form cations with various charges. O 2- S 2- Se 2- Te 2- Be 2+ Te 2- Li 1+ Na 1+ K 1+ Rb 1+ Cs 1+ Al 3+ Ga 3+ In 3+ Zn 2+ Ag 1+