Section 1 – History of the Periodic Table Objectives:

1. Section 1 – History of the Periodic Table Objectives: Explore the scientific theory of atoms (also known as the atomic theory) by describing changes in the atomic model over time and why those changes were necessary based on new evidence. Become familiar with the scientists that helped these changes come about. Explore the differences between modern periodic table and the historic periodic tables.

2. By 1860, more than 60 elements had been discovered. • Chemists had a hard time determining properties of the elements and compounds that the elements formed. • They also had no accurate way to determine atomic mass or the number of atoms that made up an element, so each scientist used a different atomic mass – making it nearly impossible for one chemist to understand the results of another. • In 1860, chemists assembled at the First International Congress of Chemists in Germany to settle the issue of atomic mass.

3. Mendeleev and Chemical Periodicity: • Russian chemist Dmitri Mendeleev included the new values from the conference in a chemistry textbook that he was writing. • He hoped to organize the elements according to their properties. • He did this by placing the elements on cards and arranged them according to atomic mass and properties, looking for trends. • He noticed that when the elements were arranged by increasing atomic mass, similarities in the chemical properties appeared at regular intervals – these patterns are periodic.

4. Brainstorming: List 3 examples of phenomena that occur periodically: 1. 2. 3.

5. Brainstorming: List 3 examples of phenomena that occur periodically: 1. Phases of the moon 2. Magazine Publications (monthly) 3. Tides (high tide & low tide) **Keep these examples in mind as we cover the arrangement of the elements on the periodic table**

6. Mendeleev and Chemical Periodicity Cont.: • Mendeleev created a table in which the elements were grouped together by similar properties – a periodic table of elements. • This table was published in 1869 and the properties were similar as you read horizontally across the table. • This procedure left many empty spaces, but he predicted that elements would be discovered and would fill those places - all three were discovered by 1886.

7. Moseley and the Periodic Law: • Moseleywas working with 38 different metals and discovered a pattern that was had not been recognized – elements fit better when they were arranged by increasing nuclear charge (# of protons in nucleus) • Moseley’s work led to: • Modern definition of atomic number • Recognition that atomic number – NOT atomic mass – is basis for organization of periodic table • Periodic Law– the physical and chemical properties of the elements are periodic functions of their atomic numbers (# of protons).

8. 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

9. 1 H 94 67 93 49 31 91 90 39 50 41 70 21 68 71 85 10 18 46 109 108 27 20 97 98 38 65 24 26 64 63 28 78 60 59 47 107 58 66 3 22 81 103 102 88 101 56 99 2 4 12 105 86 23 15 16 35 17 13 48 9 5 14 52 6 8 83 29 51 33 30 7 82 25 34 54 106 32 36 37 89 57 19 72 74 11 75 76 77 104 55 44 42 87 41 80 79 43 84 45 Es Md No Bh F Kr Te Gd Dy Cf Th Pu Np Pa Lu Yb Er Ho Tb Cl Sg Bk Db Nb Ac Eu Sb Bi N Pb Tc O Hg Se As Po Rf Hs Mo Ru Rh Ir Os Re W Hf La Mt Nd Ra Ce Cr Au P Ca Zn K Pr Sc Be Ag Cs Cu Ge Ti Ba Pt Na Si Sr B Y Al Ga Fr Zr He Ne Pd Li Xe Rn At Br V Lr Sn Ar Rb Mg Ni Fe C Mn Tl S Co Cd In 53 I 73 Ta 62 61 69 Sm Pm Tm 96 100 92 95 Cm Fm U Am Other Physical DATA

10. The Modern Periodic Table • Periodic table– an arrangement of the elements in order of their atomic number so that elements with similar properties fall in the same column or group. • The Noble Gases - 1894 • Noble gases were the most significant addition to the periodic table. • John William Strutt and Sir William Ramsay discovered Argon – a gas in the atmosphere that had not been noticed because it is unreactive – and Helium – a component of the sun. • Ramsey added a new group to the table to fit these gases.

11. Lanthanides/ Actinides – early 1900s • These are the 14 elements with atomic number from 58 to 71 (lanthanides) and 90 to 103 (actinides) that have very similar properties. • They are placed below the table to save space

12. Dutch Periodic Table 118 117 116 115 114 113 112 111 110 109 108 107 106 Strong, Journal of Chemical Education, Sept. 1989, page 743

13. Chinese Periodic Table http://www.limestone.on.ca/ibuild/davies/chinesept.html

14. Stowe’s Periodic Table

15. Benfrey’s Periodic Table

16. developed by Mohd Abubakr, Hyderabad, India

17. Misconceptions: - Something does not have to very uniformly to be periodic. It just has to have a similar pattern. - As you read through the articles, make sure you are aware that changes have been made - the periodic table has been modified to fit new evidence.

18. Group assignments: • Individually read the two articles that you have been given. • Once you have read the articles, please discuss them with your group members and create two charts on your bell ringer paper : • 1. Venn Diagram: • Compare historic periodic tables vs. the Modern Periodic table • The overlap will represent what has stayed the same. • 2. Concept Map: • Periodic Table is your Heading • Relate it to: • The scientists involved • Problems/predictions that occurred • Changes made over time

19. Groups for Assignment: • Group 1 • 1. Anna Ashley • 2. Bobby Beeton • 3. KayleeMadere • Group 2 • 1. Kellie Fahy • 2. Rachel Loughney • 3. Nicholas White • Group 3: • 1. Joey Winston • 2. Madeline Mulder • 3. Sierra Lloyd • Group 4 • 1. Zach Jowers • 2. Matthew Holt • 3. ChanteriaHamm • Group 5 • 1. MoriahFobbs • 2. Cody Frizzelle • 3. Garret Siegel • Group 6 • 1. Noah Mobley • 2. EdinMcKuhen • 3. Jonah Hooton • Group 7 • 1. Zachary Bradley • 2. Sean Chancellor • 3. Victoria Worley • Group 8 • 1. Spencer Carr • 2. Brandon Castelin • 3. Alex Hill • 4. Nancy Tanner

20. Section 2 – Electron Configuration and the Periodic Table Objectives: Relate the properties of atoms and their position in the periodic table to the arrangement of their electrons. The student will organize information to show understanding or relationships among facts, ideas, and events (representing key points within text through charting, mapping, paraphrasing, summarizing, comparing, contrasting, or outlining)

21. Groups of Elements 1A 8A 1A 5A Nitrogen group Alkali metals H 1 2A 6A He 2 Alkaline 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

22. Groups of Elements H 1 He 2 1 1 IA IIA IIIB IVB VB VIB VIIB VIIIB IB IIB IIIA IVA VA VIA VIIA VIIIA 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 Alkali metals Halogens 2 2 Other non-metals Alkaline earth metals Lanthanides Transition metals Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 Other metals Actinides 3 3 Noble gases 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