Buy this as a periodic table poster!periodic table poster

Why is the periodic table so important? Why is the periodic table shaped the way it's shaped? What are the major names groups on the periodic table? What are the shared characteristics of these groups?

HOW TO ORGANIZE ELEMENTS… PERIODIC TABLE DESIGNS

Baseball Cards: year, team, player, card number, value ($). Elements: when they were discovered, family, reactivity, state of matter, metal vs. non-metal, atomic mass, atomic number. alphabetically, mass, value, density, solid or liquid or gas Which way is CORRECT to organize the elements? Is it possible to organize the elements correctly in more than one way?

Look carefully at the drawings of the ‘aliens’. Organize all the aliens into a meaningful pattern

Law of Triads Law of Octaves Elements could be classified into groups of three, or triads. Trends in physical properties such as density, melting point, and atomic mass were observed. Arranged the 62 known elements into groups of seven according to increasing atomic mass. He proposed that an eighth element would then repeat the properties of the first element in the previous group. J.W. Döbereiner (1829) J.A.R. Newlands (1864) Lothar Meyer (1830 – 1895) Invented periodic table independently of Mendeleev his work was not published until one year after Mendeleev's

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

Period 1 Group I IIIIIIVVVIVIIVIII H = 1 2 Li = 7Be= 9.4B = 11C = 12N = 14O = 16F = 19 3 Na = 23Mg = 24Al = 27.3Si = 28P = 31S = 32C = K = 39Ca = 40? = 44Ti = 48V = 51Cr = 52Mn = 55 Fe =56, Co = 59, Ni = 59 5 Cu = 63Zn = 65? = 68? = 72As = 75Se = 78Br = 80 6 Rb = 85Sr = 87? Yt = 88Zr = 90Nb = 94Mo = 96? = 100 Ru= 104, Rh = 104, Pd = Ag = 108Cd = 112In = 113Sn = 118Sb = 122Te = 125J = Cs = 133Ba = 137?Di = 138?Ce = ?Er = 178?La = 180Ta = 182W = 184 Os = 195, Ir = 197, Pt = Au = 199Hg = 200Tl = 204Pb = 207Bi = Th = 231U = 240

 Henry G.J. Moseley  Determined the atomic numbers of elements from their X -ray spectra (1914)  Arranged elements by increasing atomic number  Killed in WW I at age 28 (Battle of Gallipoli in Turkey)

INTRODUCTION TO THE PERIODIC TABLE  Elements are arranged in seven horizontal rows, in order of increasing atomic number from left to right and from top to bottom.  Rows are called periods and are numbered from 1 to 7.  Elements with similar chemical properties form vertical columns, called groups, which are numbered from 1 to 18.  Groups 1, 2, and 13 through 18 are the main group elements.  Groups 3 through 12 are in the middle of the periodic table and are the transition elements.  The two rows of 14 elements at the bottom of the periodic are the lanthanides and actinides. Copyright 2007 Pearson Benjamin Cummings. All rights reserved.

GROUPS OF ELEMENTS

PERIODIC TABLE 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 A 2A Alkali metals Alkali earth metals Transition metals Boron group Nonmetals Noble gases 3B 5B6B7B 8B 1B2B 3A4A5A6A7A 8A 4B Lanthanoid Series 6 7 Actinoid Series C Solid Br Liquid H Gas

    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   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

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 Alkali metals Alkaline earth metals Nitrogen family Oxygen family Halogens Noble gases

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 P 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 S Tl

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

The alkali metals (Group 1) - The alkali metals are lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr). - Hydrogen is placed in Group 1 but is not a metal. - The alkali metals react readily with nonmetals to give ions with a +1 charge. - Compounds of alkali metals are common in nature and daily life. CHEMISTRY OF THE GROUPS Copyright 2007 Pearson Benjamin Cummings. All rights reserved. H1H1 Li 3 Na 11 K 19 Rb 37 Cs 55 Fr 87 1

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

The alkaline earths (Group 2) - The alkaline earths are beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra). - All are metals that react readily with nonmetals to give ions with a +2 charge. CHEMISTRY OF THE GROUPS Copyright 2007 Pearson Benjamin Cummings. All rights reserved. Be 4 Ca 20 Sr 38 Ba 56 Ra 88 Mg 12 2

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

The halogens (Group 17) - The halogens are fluorine (F), chlorine (Cl), bromine (Br) iodine (  ), and astatine (At). - They react readily with metals to form ions with a  1 charge. CHEMISTRY OF THE GROUPS Copyright 2007 Pearson Benjamin Cummings. All rights reserved. F9F9 Cl 17 Br 35 I 53 At Fluorine F 19.0 F 2 pale-yellow gas Chlorine Cl 35.5 Cl 2 greenish-yellow gas Bromine Br 79.9 Br 2 red-brown liquid 58.0 Iodine I I 2 black solid (m.p.113 o C) Element At. Mass Normal Form at STP b.p., o C Astatine At (210)

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

The noble gases (Group 18) - are helium (He), neon (Ne), argon, (Ar), krypton (Kr), xenon (Xe), and radon (Rn); - are monatomic; - are unreactive gases at room temperature and pressure; - are called inert gases. CHEMISTRY OF THE GROUPS Copyright © 2007 Pearson Benjamin Cummings. All rights reserved. He 2 Ne 10 Ar 18 Kr 36 Xe 54 Rn 86 18

CHALCOGENS, GROUP 16 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

Group 16, the Chalcogens – The chalcogens are oxygen, sulfur, selenium, tellurium, and polonium. All of the chalcogens have ns 2 np 4 valence-electron configurations. Their chemistry is dominated by three oxidation states: 1. –2, in which two electrons are added to achieve the closed-shell electron of the next noble gas , in which all six valence electrons are lost to give the closed-shell electron configuration of the preceding noble gas , in which only the four np electrons are lost to give a filled ns 2 subshell. CHEMISTRY OF THE GROUPS Copyright © 2007 Pearson Benjamin Cummings. All rights reserved. O8O8 S 16 Se 34 Te 52 Po 84 16

PNICOGENS, GROUP 15 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

CHEMISTRY OF THE GROUPS Copyright © 2007 Pearson Benjamin Cummings. All rights reserved. Group 15, the Pnicogens – The pnicogens are nitrogen, phosphorus, arsenic, antimony, and bismuth. – All the pnicogens have ns 2 np 3 valence-electron configurations, leading to three common oxidation states: 1. –3, in which three electrons are added to give the closed-shell electron configuration of the next noble gas 2. +5, in which all five valence electrons are lost to give the closed-shell electron configuration of the preceding noble gas 3. +3, in which only the three np electrons are lost to give a filled ns 2 subshell N7N7 P 15 As 33 Sb 51 Bi 83 15

Group 14 – Group 14 elements straddle the diagonal line that divides nonmetals from metals. – Carbon is a nonmetal, silicon and germanium are semimetals, and tin and lead are metals. – Group-14 elements have the ns 2 np 2 valence-electron configuration. – Group-14 elements have three oxidation states: 1. –4, in which four electrons are added to achieve the closed-shell electron configuration of the next noble gas 2. +4, in which all four valence electrons are lost to give the closed-shell electron configuration of the preceding noble gas 3. +2, in which the loss of two np 2 electrons gives a filled ns 2 subshell CHEMISTRY OF THE GROUPS Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.

Group 13 – Of the Group-13 elements, only the lightest, boron, lies on the diagonal line that separates nonmetals and metals, it is a semimetal and possesses an unusual structure. – The rest of Group 13 are metals (aluminum, gallium, indium, and thallium) and are typical metallic solids. – Elements of Group 13 are highly reactive and form stable compounds with oxygen. – Elements of Group 13 have ns 2 np 1 valence-electron configurations. CHEMISTRY OF THE GROUPS Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.

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

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 Ac