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Periodic Trends

Periodic Trends. For each slide with a periodic table - copy the definition. Copy ALL of the other slides. The purpose of this exercise is for you to be able to understand 4 periodic trends and how to predict them.

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Periodic Trends

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  1. Periodic Trends • For each slide with a periodic table - copy the definition. Copy ALL of the other slides. • The purpose of this exercise is for you to be able to understand 4 periodic trends and how to predict them. • You will need to know the definitions of the trends and be able to tell me whether two atoms are bigger are smaller, or have more ionization energy, etc. (memorize the diagram with the arrows) • Place the icons at the right over the numbers indicated by the range below the icon.

  2. Bonding • More will be explained about bonding later… for now you need to know: • Covalent bonds = sharing electrons • Ionic bonds = stealing electrons

  3. H 13.6 H 13.6 If atoms love their electrons it will cost you a lot of energy to steal 1 of them. He 24.6 He 24.6 Li 5.4 Li 5.4 Be 9.3 Be 9.3 B 8.3 B 8.3 C 11.3 C 11.3 N 14.5 N 14.5 O 13.6 O 13.6 F 17.4 F 17.4 Ne 21.6 Ne 21.6 17-25 Na 5.1 Na 5.1 Mg 7.6 Mg 7.6 Al 6 Al 6 Si 8.2 Si 8.2 P 10.5 P 10.5 S 10.4 S 10.4 Cl 13 Cl 13 Ar 15.8 Ar 15.8 12.1-16.9 K 4.3 K 4.3 Ca 6.1 Ca 6.1 Ga 6 Ga 6 Ge 7.9 Ge 7.9 As 9.8 As 9.8 Se 9.8 Se 9.8 Br 11.8 Br 11.8 Kr 14 Kr 14 Rb 4.2 Rb 4.2 Sr 5.7 Sr 5.7 In 5.8 In 5.8 Sn 7.3 Sn 7.3 Sb 8.6 Sb 8.6 Te 9 Te 9 I 10.5 I 10.5 Xe 12.1 Xe 12.1 8.6-12 Cs 3.9 Cs 3.9 Ba 5.2 Ba 5.2 Tl 6.1 Tl 6.1 Pb 7.4 Pb 7.4 Bi 7.3 Bi 7.3 Po 8.4 Po 8.4 At 9.3 At 9.3 Rn 10.7 Rn 10.7 6-8.5 Fr 4.1 Fr 4.1 Ra 5.3 Ra 5.3 1st Ionization 3.9-5.8 Energy

  4. 1st Ionization Energy Helium loves its electrons because it is full and small. The closer to the right = the closer to fullness = love for electrons. Large elements have a hard time holding electrons. It would cost you a lot of energy to steal an electron from Helium. Francium would be easy to steal from. He 24.6 Fr 4.1

  5. H 2.2 H 2.2 How strongly atoms attract electrons to themselves when bonding. He He Li .98 Li .98 Be 1.57 Be 1.57 B 2.04 B 2.04 C 2.55 C 2.55 N 3.04 N 3.04 O 3.44 O 3.44 F 3.96 F 3.96 Ne Ne 3.9-4 Na .93 Na .93 Mg 1.31 Mg 1.31 Al 1.61 Al 1.61 Si 1.9 Si 1.9 P 2.1 P 2.1 S 2.5 S 2.5 Cl 3.16 Cl 3.16 Ar Ar 3.01-3.89 K .82 K .82 Ca 1 Ca 1 Ga 1.81 Ga 1.81 Ge 2.01 Ge 2.01 As 2.18 As 2.18 Se 2.55 Se 2.55 Br 2.96 Br 2.96 Kr Kr Rb .82 Rb .82 Sr .95 Sr .95 In 1.78 In 1.78 Sn 1.96 Sn 1.96 Sb 2.05 Sb 2.05 Te 2.1 Te 2.1 I 2.66 I 2.66 Xe Xe 2.01-3 Cs .79 Cs .79 Ba .89 Ba .89 Tl 1.8 Tl 1.8 Pb 1.9 Pb 1.9 Bi 1.9 Bi 1.9 Po 2 Po 2 At 2.2 At 2.2 Rn Rn 1.01-2 Fr .7 Fr .7 Ra .9 Ra .9 Electronegativity 0-1

  6. Electronegativity Small elements can attract electrons more easily because their positive nucleus is closer. Elements on the right want more electrons until the last Group because they are full. Noble gases like Helium is therefore unreactive. Fluorine attracts electrons the most and Francium the least. F 3.96 Fr .7

  7. H 37 H 37 Atoms get bigger as you go down and to the left. He 31 He 31 31-80 Li 152 Li 152 Be 112 Be 112 B 85 B 85 C 77 C 77 N 75 N 75 O 73 O 73 F 72 F 72 Ne 71 Ne 71 81-100 Na 186 Na 186 Mg 160 Mg 160 Al 143 Al 143 Si 118 Si 118 P 110 P 110 S 103 S 103 Cl 100 Cl 100 Ar 98 Ar 98 101-159 K 227 K 227 Ca 197 Ca 197 Ga 135 Ga 135 Ge 122 Ge 122 As 120 As 120 Se 119 Se 119 Br 114 Br 114 Kr 112 Kr 112 Rb 248 Rb 248 Sr 215 Sr 215 In 167 In 167 Sn 140 Sn 140 Sb 140 Sb 140 Te 142 Te 142 I 133 I 133 Xe 131 Xe 131 160-269 Cs 265 Cs 265 Ba 215 Ba 215 Tl 170 Tl 170 Pb 146 Pb 146 Bi 150 Bi 150 Po 168 Po 168 At 140 At 140 Rn 140 Rn 140 Fr 282 Fr 282 Ra 223 Ra 223 Atomic Radii 270-300

  8. Atomic Radii He 31 Helium is the smallest because it has the least energy levels and is farthest to the right Francium is big because it has the most energy levels and is farthest to the left. Fr 282

  9. Ions are atoms that have gained or lost electrons. Their size depends on how big they were and whether or not they have gained or lost electrons. H H He He 15-40 Li 76 Li 76 Be 31 Be 31 B 20 B 20 C 15 C 15 N 146 N 146 O 140 O 140 F 133 F 133 Ne Ne 41-60 Na 102 Na 102 Mg 72 Mg 72 Al 54 Al 54 Si 41 Si 41 P 212 P 212 S 184 S 184 Cl 181 Cl 181 Ar Ar 61-100 K 138 K 138 Ca 100 Ca 100 Ga 62 Ga 62 Ge 53 Ge 53 As 222 As 222 Se 198 Se 198 Br 195 Br 195 Kr Kr Rb 152 Rb 152 Sr 118 Sr 118 In 81 In 81 Sn 71 Sn 71 Sb 62 Sb 62 Te 221 Te 221 I 220 I 220 Xe Xe 101-170 Cs 167 Cs 167 Ba 135 Ba 135 Tl 95 Tl 95 Pb 84 Pb 84 Bi 74 Bi 74 Po Po At At Rn Rn Fr 194 Fr 194 Ra Ra 171-200 Ionic Radii

  10. Ionic Radii He The left side loses electrons and the right side gains electrons. Carbon is the smallest and looses the most, so its ion is the smallest. As you go down and to the left toward Francium, it gets bigger. It continues to get bigger from the top right down and to the left toward Arsenic which is the biggest. Noble Gases don’t make ions. C 15 As 222 Fr 194

  11. QuestionsCopy the following and paste it on a wiki titled 10-1 Periodic Trends. Answer the questions there. ATOMIC RADIUS - Rank the following from smallest to largest atomic radius. 1. Li, C, F 2. Li, Na, K 3. Ge, P, O 4. C, N, Al 5. Al, Cl, Ga 6. Describe the periodic trend IONIC RADIUS - Rank the following from smallest to largest ionic radius. 7. Mg2+, Si4-, S2- 8. Mg2+, Ca2+, Ba2+ 9. F-, Cl-, Br- 10. Ba2+, Cu2+, Zn2+ 11. Si4-, P3-, O2- 12. Describe the periodic trend IONIZATION ENERGY - Rank the following from lowest to highest ionization energy. 13. Mg, Si, S 14. Mg, Ca, Ba 15. F, Cl, Br 16. Ba, Cu, Ne 17. e. Si, P, He 18. Describe the periodic trend ELECTRONEGATIVITY - Rank the following from lowest to highest electronegativity 19. Li, C, N 20. C, O, Ne 21. Si, P, O 22. K, Mg, P 23. S, F, He 24. Describe the periodic trend

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