Periodic Table of the Elements Written by: Bill Byles - bylesb@internet4classrooms.com Modified by Jeff Christopherson - www.unit5.org/chemistry http://www.allperiodictables.com/apt/aptpages/apt_1_CC_Active.html

Groups of Elements 1A 8A H He 2A 3A 4A 5A 6A 7A Li Be B C N O F Ne Na Alkali metals 5A Nitrogen group H 1 2A Alkaline earth metals 6A Oxygen group He 2 1 1 2A Transition metals 7A Halogens 3A 4A 5A 6A 7A 3A Boron group 8A Noble gases 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 7 7 W W 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

Dmitri Mendeleev Russian Invented periodic table Organized elements by properties Arranged elements by atomic mass Predicted existence of several unknown elements Element 101 Dmitri Ivanovich Mendeleev (1834 – 1907) Arranged elements by increasing atomic mass. Proposed that properties of different elements repeat at regular intervals. 1860’s proposed new arrangements of elements. 1869 Published original periodic table Dmitri Mendeleev was the Russian chemist who invented the periodic table of the elements. He was born in Siberia and was the youngest of 17 children. Mendeleev missed receiving the Nobel prize in chemistry by just one vote in 1906, and died before the next year’s election. Element 101 (discovered in 1955) was named Mendelevium in his honor. Dmitri Mendeleev

H He H Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe hydrogen alkali metals alkaline earth metals transition metals poor metals nonmetals noble gases rare earth metals H 1 He 2 H 1 1 Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 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 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 7 W 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 http://www.elementsdatabase.com/

The Periodic Table * * Lanthanides Y Y Actinides Alkaline H He Li Be B Noble gases Alkaline earth metals Halogens 1 18 H 1 He 2 2 13 14 15 16 17 Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 Na 11 Mg 12 3 4 5 6 7 8 9 10 11 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 Transition metals 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 Alkali 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 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 Y Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 Uun 110 Uuu 111 Uub 112 Uuq 113 Uuh 116 Uuo 118 * Lanthanides 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 Y Actinides 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

Orbitals Being Filled Groups 1 8 2 1s 1 3 4 5 6 7 1s 2s 2 2p 3 3s 3p 3 4 5 6 7 1s 2s 2 2p 3 3s 3p Periods 4s 3d 4p 4 4d 5p 5 5s La 5d 6p 6 6s Ac 6d 7 7s 4f Lanthanide series 5f Actinide series Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 345

METALS Metals and Nonmetals Nonmetals Metalloids H He Li Be B C N O F 1 He 2 1 Li 3 Be 4 B 5 C 6 Nonmetals N 7 O 8 F 9 Ne 10 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 Metalloids 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 7 W 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

Metallic Characteristic metallic character increases nonmetallic character increases metallic character increases nonmetallic character increases

Periodic Table s s H He H p Li Be B C N O F Ne Na Mg d Al Si P S Cl Ar 1 He 2 H 1 p 1 1 Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 2 2 Na 11 Mg 12 d Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 3 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 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 7 7 W W f 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

Electron Filling in Periodic Table s s s s H 1s1 He 1s2 H 1s1 p p 1 1 Li 2s1 Be 2s2 B 2p1 C 2p2 N 2p3 O 2p4 F 2p5 Ne 2p6 2 2 Na 3s1 Mg 3s2 d d Al 3p1 Si 3p2 P 3p3 S 3p4 Cl 3p5 Ar 3p6 3 3 K 4s1 Ca 4s2 Sc 3d1 Ti 3d2 V 3d3 Cr 3d5 Mn 3d5 Fe 3d6 Co 3d7 Ni 3d8 Cu 3d10 Zn 3d10 Ga 4p1 Ge 4p2 As 4p3 Se 4p4 Br 4p5 Kr 4p6 4 4 Rb 5s1 Sr 5s2 Y 4d1 Zr 4d2 Nb 4d4 Mo 4d5 Tc 4d6 Ru 4d7 Rh 4d8 Pd 4d10 Ag 4d10 Cd 4p1 In 5p1 Sn 5p2 Sb 5p3 Te 5p4 I 5p5 Xe 5p6 5 5 Cs 6s1 Ba 6s2 Hf 5d2 Ta 5d3 W 5d4 Re 5d5 Os 5d6 Ir 5d7 Pt 5d9 Au 5d10 Hg 5d10 Tl 6p1 Pb 6p2 Bi 6p3 Po 6p4 At 6p5 Rn 6p6 6 6 * * Fr 7s1 Ra 7s2 Rf 6d2 Db 6d3 Sg 6d4 Bh 6d5 Hs 6d6 Mt 6d7 7 7 W W f f La 5d1 Ce 4f2 Pr 4f3 Nd 4f4 Pm 4f5 Sm 4f6 Eu 4f7 Gd 4f7 Tb 4f9 Dy 4f10 Ho 4f11 Er 4f12 Tm 4f13 Yb 4f14 Lu 4f114 * * Ac 6d1 Th 6d2 Pa 5f2 U 5f3 Np 5f4 Pu 5f6 Am 5f7 Cm 5f7 Bk 5f8 Cf 5f10 Es 5f11 Fm 5f14 Md 5f13 No 5f14 Lr 5f14 W W

Atomic Radii The atomic radius of a chemical element is a measure of the size of its atoms, usually the mean or typical distance from the nucleus to the boundary of the surrounding cloud of electrons.

Atomic Radii = 1 Angstrom IA IIA IIIA IVA VA VIA VIIA Li Be B C N O F 1.52 1.11 1.86 1.60 2.31 1.97 2.44 2.15 2.62 2.17 0.88 0.77 0.70 0.66 0.64 1.43 1.17 1.10 1.04 0.99 1.22 1.22 1.21 1.17 1.14 1.62 1.40 1.41 1.37 1.33 1.71 1.75 1.46 Na Mg Al Si P S Cl K Ca Ga Ge As Se Br Rb Sr In Sn Sb Te I Cs Ba Tl Pb Bi = 1 Angstrom

Ion An ion is an atom or a molecule in which the total number of electrons is not equal to the total number of protons, giving the atom or molecule a net positive or negative electrical charge. Ions can be created, by either chemical or physical means, via ionization.

Ionic Radii Ionic radius is the radius of an atom's ion.

Atomic Radii Ionic Radii = 1 Angstrom = 1 Angstrom 0.60 0.31 0.95 0.65 1.33 0.99 1.48 1.13 1.69 1.35 1.71 1.40 1.36 0.50 1.84 1.81 0.62 1.98 1.85 0.81 2.21 2.16 0.95 IA IIA IIIA IVA VA VIA VIIA = 1 Angstrom Li1+ Be2+ Na1+ Mg2+ Ba2+ Sr2+ Ca2+ K1+ Rb1+ Cs1+ Cl1- N3- O2- F1- S2- Se2- Br1- Te2- I1- Al3+ Ga3+ In3+ Tl3+ IA IIA IIIA IVA VA VIA VIIA Li Na K Rb Cs Cl S P Si Al Br Se As Ge Ga I Te Sb Sn In Tl Pb Bi Mg Ca Sr Ba Be F O N C B 1.52 1.11 1.86 1.60 2.31 1.97 2.44 2.15 2.62 2.17 0.88 0.77 0.70 0.66 0.64 1.43 1.17 1.10 1.04 0.99 1.22 1.22 1.21 1.17 1.14 1.62 1.40 1.41 1.37 1.33 1.71 1.75 1.46 = 1 Angstrom

Ionization Energies Period H He Mg Li Be B C N O F Ne Na Mg Al Si P S Group 1 18 H 1312 Symbol First Ionization Energy (kJ/mol) He 2372 1 1 Mg 738 2 13 14 15 16 17 Li 520 Be 900 B 801 C 1086 N 1402 O 1314 F 1681 Ne 2081 2 2 Na 496 Mg 738 Al 578 Si 787 P 1012 S 1000 Cl 1251 Ar 1521 3 3 3 4 5 6 7 8 9 10 11 12 Period K 419 Ca 590 Sc 633 Ti 659 V 651 Cr 653 Mn 717 Fe 762 Co 760 Ni 737 Cu 746 Zn 906 Ga 579 Ge 762 As 947 Se 941 Br 1140 Kr 1351 4 4 Rb 403 Sr 550 Y 600 Zr 640 Nb 652 Mo 684 Tc 702 Ru 710 Rh 720 Pd 804 Ag 731 Cd 868 In 558 Sn 709 Sb 834 Te 869 I 1008 Xe 1170 5 5 Cs 376 Ba 503 La 538 * Hf 659 Ta 761 W 770 Re 760 Os 839 Ir 878 Pt 868 Au 890 Hg 1007 Tl 589 Pb 716 Bi 703 Po 812 At -- Rn 1038 6 6 Linus Pauling (1901 - 1994) awarded Nobel Prize in chemistry in 1954 for his 1939 text, The Nature of the Chemical Bond, and also won the Nobel Peace Prize in 1962 for his fight to control nuclear weapons. The greater the electronegativity of an atom in a molecule, the more strongly it attracts the electrons in a covalent bond. Fr -- Ra 509 Ac 490 y Rf -- Db -- Sg -- Bh -- Hs -- Mt -- Ds -- Uuu -- Uub -- Uut -- Uuq -- Uup -- Uuo -- 7 * Lanthanide series Ce 534 Pr 527 Nd 533 Pm 536 Sm 545 Eu 547 Gd 592 Tb 566 Dy 573 Ho 581 Er 589 Tm 597 Yb 603 Lu 523 y Actinide series Th 587 Pa 570 U 598 Np 600 Pu 585 Am 578 Cm 581 Bk 601 Cf 608 Es 619 Fm 627 Md 635 No 642 Lr --

First Ionization Energies (in kilojoules per mole) H 1312.1 He 2372.5 Li 520.3 Be 899.5 B 800.7 C 1086.5 N 1402.4 O 1314.0 F 1681.1 Ne 2080.8 Na 495.9 Mg 737.8 Al 577.6 Si 786.5 P 1011.8 S 999.7 Cl 1251.2 Ar 1520.6 Metals have low ionization energy; nonmetals have high ionization energy. This experimental data gives evidence for: 1) effect of increasing nuclear charge 2) stability of octet 3) effect of increased radius 4) s & p sublevel in outer level SUGGESTION: Emphasize that theories came from experimental evidence! K 418.9 Ca 589.9 Ga 578.6 Ge 761.2 As 946.5 Se 940.7 Br 1142.7 Kr 1350.8 Rb 402.9 Sr 549.2 In 558.2 Sn 708.4 Sb 833.8 Te 869.0 I 1008.7 Xe 1170.3 Smoot, Price, Smith, Chemistry A Modern Course 1987, page 188

First Ionization Energies (kJ/mol) p H 1312.1 He 2372.5 Li 520.3 Be 899.5 B 800.7 C 1086.5 N 1402.4 O 1314.0 F 1681.1 Ne 2080.8 Na 495.9 Mg 737.8 Al 577.6 Si 786.5 P 1011.8 S 999.7 Cl 1251.2 Ar 1520.6 Metals have low ionization energy; nonmetals have high ionization energy. This experimental data gives evidence for: 1) effect of increasing nuclear charge 2) stability of octet 3) effect of increased radius 4) s & p sublevel in outer level SUGGESTION: Emphasize that theories came from experimental evidence! K 418.9 Ca 589.9 Ga 578.6 Ge 761.2 As 946.5 Se 940.7 Br 1142.7 Kr 1350.8 Rb 402.9 Sr 549.2 In 558.2 Sn 708.4 Sb 833.8 Te 869.0 I 1008.7 Xe 1170.3 Smoot, Price, Smith, Chemistry A Modern Course 1987, page 188

Ionization Energies (kJ/mol) Element Na Mg Al Si P S Cl Ar 1st 498 736 577 787 1063 1000 1255 1519 2nd 4560 1445 1815 1575 1890 2260 2295 2665 3rd 6910 7730 2740 3220 2905 3375 3850 3945 4th 9540 10,600 11,600 4350 4950 4565 5160 5770 5th 13,400 13,600 15,000 16,100 6270 6950 6560 7320 6th 16,600 18,000 18,310 19,800 21,200 8490 9360 8780 Ionization energy increases with the removal of each additional electron. Metals have low ionization energy; nonmetals have high ionization energy. This experimental data gives evidence for: 1) effect of increasing nuclear charge 2) stability of octet 3) effect of increased radius 4) s & p sublevel in outer level SUGGESTION: Emphasize that theories came from experimental evidence! Herron, Frank, Sarquis, Sarquis, Cchrader, Kulka, Chemistry 1996, Heath, page Shaded area on table denotes core electrons.

Electron Configuration 4 Be Beryllium Beryllium N Name: Beryllium Symbol: Be Atomic Number: 4 Atomic Mass: 9.012182 amu Melting Point: 1278.0 °C (1551.15 °K, 2332.4 °F) Boiling Point: 2970.0 °C (3243.15 °K, 5378.0 °F) What is Beryllium? Grey metallic element of group 2 of the periodic table. Is toxic and can cause severe lung diseases and dermatitis. Shows high covalent character. It was isolated independently by F. Wohler and A.A. Bussy in 1828. Electron Configuration Be = 1s22s2

Electron Configuration 6 C Carbon Carbon N Name: Carbon Symbol: C Atomic Number: 6 Atomic Mass: 12.0107 amu Melting Point: 3500.0 °C (3773.15 °K, 6332.0 °F) Boiling Point: 4827.0 °C (5100.15 °K, 8720.6 °F) What is Carbon? Carbon is a member of group 14 of the periodic table. It has three allotropic forms of it, diamonds, graphite and fullerite. Carbon-14 is commonly used in radioactive dating. Carbon occurs in all organic life and is the basis of organic chemistry. Carbon has the interesting chemical property of being able to bond with itself, and a wide variety of other elements. Electron Configuration C = 1s22s22p2

Electron Configuration 10 Ne Neon Neon N pslawinski, wikipedia.org Name: Neon Symbol: Ne Atomic Number: 10 Atomic Mass: 20.1797 amu Melting Point: -248.6 °C (24.549994 °K, -415.48 °F) Boiling Point: -246.1 °C (27.049994 °K, -410.98 °F) What is Neon? Colorless gaseous element of group 18 on the periodic table (noble gases). Neon occurs in the atmosphere, and comprises 0.0018% of the volume of the atmosphere. It has a distinct reddish glow when used in discharge tubes and neon based lamps. It forms almost no chemical compounds. Neon was discovered in 1898 by Sir William Ramsey and M.W. Travers. Electron Configuration Ne = 1s22s22p6

Electron Configuration 24 Cr Chromium Chromium N Name: Chromium Symbol: Cr Atomic Number: 24 Atomic Mass: 51.9961 amu Melting Point: 1857.0 °C (2130.15 °K, 3374.6 °F) Boiling Point: 2672.0 °C (2945.15 °K, 4841.6 °F) Link What is Chromium? Hard silvery transition element. Used in decorative electroplating. Discovered in 1797 by Vauquelin. Electron Configuration Cr = 1s22s22p63s23p6 4s13d5

Radon Gas Radon gas occurs naturally from the radioactive decay of radium. Radium is found in small amounts in rock. SOURCES OF RADON “Radon, the heaviest noble gas, was first observed as the gas produced by the radioactive element radium when it decayed. Some granites used for building houses have been found to give off tiny amounts of radon, which can accumulate in confined areas.” Eyewitness Science “Chemistry” , Dr. Ann Newmark, DK Publishing, Inc., 1993, pg 33 Ra  Rn + radiation Predicted fraction of homes over 4 picocuries/liter radon

Magnesium Mg Atomic Mass 24 amu melting point = silver gray metal 24.305 12 Magnesium Atomic Mass 24 amu melting point = silver gray metal used in flash bulbs, bombs,and flares 8th most abundant element (2.2% of Earth’s crust) lack of Mg produces same biological effect as alcoholism (delirium tremens) FLASH PHOTOGRAPHY “Magnesium metal was produced commercially from the 1860s as wire or ribbon. It readily burns in air, the metal being oxidized to magnesium oxide. The brightness of the white flame made it useful in photography to provide studio lighting.” Eyewitness Science “Chemistry” , Dr. Ann Newmark, DK Publishing, Inc., 1993, pg 40