Journal: Choose one of these Periodic Table ideas or come up with your own. Explain what different CATEGORIES/SECTIONS you would make to group your “Elements” by similarities (ex. Heroes section, villains section) Explain what TRENDS you would create in your table (ex. Characters on the far left are terrible villains, as we go right they get less bad, and the far right side is amazing heroes OR hair color is light in the top rows and gets darker as we go down rows)

Trend Videos: https://betterlesson.com/lesson/619487/periodic-table-trends https://www.youtube.com/watch?time_continue=40&v=fmiz6Ypl3Cc https://www.youtube.com/watch?time_continue=13&v=pisA4O7jw34 https://www.youtube.com/watch?v=OgAEnuYKcPg

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

Atomic Radii of Representative Elements (nm) 1A 2A 3A 4A 5A 6A 7A Li Be B C N O F 0.1.52 0.111 0.088 0.077 0.070 0.066 0.064 Na Mg Al Si P S Cl 0.186 0.160 0.143 0.117 0.110 0.104 0.099 K Ca Ga Ge As Se Br 0.231 0.197 0.122 0.122 0.121 0.117 0.114 Rb Sr In Sn Sb Te I 0.244 0.215 0.162 0.140 0.141 0.137 0.133 Cs Ba Tl Pb At Bi Po 0.262 0.217 0.171 0.175 0.146 0.140 0.140 LeMay Jr, Beall, Robblee, Brower, Chemistry Connections to Our Changing World , 1996, page 175

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

Electronegativities Period H B P As Se Ru Rh Pd Te Os Ir Pt Au Po At 2.1 B 2.0 P As Se 2.4 Ru 2.2 Rh Pd Te Os Ir Pt Au Po At 2.0 - 2.4 1 1 2A 3A 4A 5A 6A 7A Actinides: 1.3 - 1.5 Li 1.0 Ca Sc 1.3 Sr Y 1.2 Zr 1.4 Hf Mg La 1.1 Ac 1.0 - 1.4 Lanthanides: 1.1 - 1.3 * y Be 1.5 Al Si 1.8 Ti V 1.6 Cr Mn Fe Co Ni Cu 1.9 Zn 1.7 Ga Ge Nb Mo Tc Ag Cd In Sn Sb Ta W Re Hg Tl Pb Bi 1.5 - 1.9 N 3.0 O 3.5 F 4.0 Cl 3.0 - 4.0 C 2.5 S Br 2.8 I 2.5 - 2.9 2 2 Na 0.9 K 0.8 Rb Cs 0.7 Ba Fr Ra Below 1.0 3 3 3B 4B 5B 6B 7B 8B 1B 2B Period 4 4 5 5 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. 7 Hill, Petrucci, General Chemistry An Integrated Approach 2nd Edition, page 373

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