2. alkaline earths halogens  Elements with similar chemical behavior are in the same group.  Elements of Group 1 are.  Elements of Group 2 are  Elements of Group 17 are the.  Elements of Group 18 are the. noble gases alkali metals Copyright 2007 Pearson Benjamin Cummings. All rights reserved.

3. 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

4. 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. Copyright 2007 Pearson Benjamin Cummings. All rights reserved. H1H1 Li 3 Na 11 K 19 Rb 37 Cs 55 Fr 87 1

5. 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

6. 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. Copyright 2007 Pearson Benjamin Cummings. All rights reserved. Be 4 Ca 20 Sr 38 Ba 56 Ra 88 Mg 12 2

7. 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

8. 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. Copyright 2007 Pearson Benjamin Cummings. All rights reserved. F9F9 Cl 17 Br 35 I 53 At 85 17 Fluorine F 19.0 F 2 pale-yellow gas -187.0 Chlorine Cl 35.5 Cl 2 greenish-yellow gas -34.5 Bromine Br 79.9 Br 2 red-brown liquid 58.0 Iodine I 126.9 I 2 black solid (m.p.113 o C) 184.0 Element At. Mass Normal Form at STP b.p., o C Astatine At (210)

9. 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

10. 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. Copyright © 2007 Pearson Benjamin Cummings. All rights reserved. He 2 Ne 10 Ar 18 Kr 36 Xe 54 Rn 86 18

11. 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

12. 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. 2. +6, in which all six valence electrons are lost to give the closed-shell electron configuration of the preceding noble gas. 3. +4, in which only the four np electrons are lost to give a filled ns 2 subshell. Copyright © 2007 Pearson Benjamin Cummings. All rights reserved. O8O8 S 16 Se 34 Te 52 Po 84 16

13. 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

14. 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. Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.

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 Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.

16. 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

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 La

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 La

19. 1 2 3 4 5 6 1 2 3 4 5 6 7 Be 1.5 Al 1.5 Si 1.8 Ti 1.5 V 1.6 Cr 1.6 Mn 1.5 Fe 1.8 Co 1.8 Ni 1.8 Cu 1.9 Zn 1.7 Ga 1.6 Ge 1.8 Nb 1.6 Mo 1.8 Tc 1.9 Ag 1.9 Cd 1.7 In 1.7 Sn 1.8 Sb 1.9 Ta 1.5 W 1.7 Re 1.9 Hg 1.9 Tl 1.8 Pb 1.8 Bi 1.9 1.5 - 1.9 N 3.0 O 3.5 F 4.0 Cl 3.0 3.0 - 4.0 C 2.5 S 2.5 Br 2.8 I 2.5 2.5 - 2.9 Na 0.9 K 0.8 Rb 0.8 Cs 0.7 Ba 0.9 Fr 0.7 Ra 0.9 Below 1.0 H 2.1 B 2.0 P 2.1 As 2.0 Se 2.4 Ru 2.2 Rh 2.2 Pd 2.2 Te 2.1 Os 2.2 Ir 2.2 Pt 2.2 Au 2.4 Po 2.0 At 2.2 2.0 - 2.4 Period Actinides: 1.3 - 1.5 Li 1.0 Ca 1.0 Sc 1.3 Sr 1.0 Y 1.2 Zr 1.4 Hf 1.3 Mg 1.2 La 1.1 Ac 1.1 1.0 - 1.4 Lanthanides: 1.1 - 1.3     1A 2A 3B 4B 5B 6B 7B 1B 2B 3A 4A 5A 6A 7A 8A Hill, Petrucci, General Chemistry An Integrated Approach 2 nd Edition, page 373 8B

20. Li Na K Rb Cs Cl S P Si Al Br Se As Ge Ga I Te SbSn 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 IA IIA IIIA IVA VA VIA VIIA = 1 Angstrom

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

22. Li Na K Rb Cs Cl S P Si Al Br Se As Ge Ga I Te SbSn 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 IA IIA IIIA IVA VA VIA VIIA = 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 Li 1+ Be 2+ Na 1+ Mg 2+ Ba 2+ Sr 2+ Ca 2+ K 1+ Rb 1+ Cs 1+ Cl 1- N 3- O 2- F 1- S 2- Se 2- Br 1- Te 2- I 1- Al 3+ Ga 3+ In 3+ Tl 3+ Ionic Radii

23. 1 2 3 4 5 6 1 2 3 4 5 6 7 Be 900 Al 578 Si 787 Ti 659 V 651 Cr 653 Mn 717 Fe 762 Co 760 Ni 737 Cu 746 Zn 906 Ga 579 Ge 762 Nb 652 Mo 684 Tc 702 Ag 731 Cd 868 In 558 Sn 709 Sb 834 Ta 761 W 770 Re 760 Hg 1007 Tl 589 Pb 716 Bi 703 N 1402 O 1314 F 1681 Cl 1251 C 1086 S 1000 Br 1140 I 1008 Na 496 K 419 Rb 403 Cs 376 Ba 503 Fr -- Ra 509 H 1312 B 801 P 1012 As 947 Se 941 Ru 710 Rh 720 Pd 804 Te 869 Os 839 Ir 878 Pt 868 Au 890 Po 812 At -- Period Actinide series Li 520 Ca 590 Sc 633 Sr 550 Y 600 Zr 640 Hf 659 Mg 738 La 538 Ac 490 Lanthanide series     Group 1 2 3 4 5 6 7 11 12 13 14 15 16 17 18 9 Ne 2081 Ar 1521 Kr 1351 Xe 1170 Rn 1038 He 2372 Rf -- Db -- Sg -- Bh -- Hs -- Mt -- 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 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 -- Ds -- Uub -- Uut -- Uuq -- Uup -- Uuu -- Uuo -- Mg 738 Symbol First Ionization Energy (kJ/mol) 810

24. Ionic size (cations) Ionic size (anions) decreases Shielding is constant Atomic radius decreases Ionization energy increases Electronegativity increases Nuclear charge increases Shielding increases Atomic radius increases Ionic size increases Ionization energy decreases Electronegativity decreases 1A 2A3A4A 5A 6A7A 0