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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. H 13.6 H 13.6 How much love do atoms have for their electrons? Lots of love = lots of energy is needed to give up electrons for Ionic Bonds. 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

  3. 1st Ionization Energy Helium loves its electrons. It would take a lot for it to give them up to make an ionic bond He 24.6 Francium does not really like its electrons. It will give them up easily. Fr 4.1

  4. H 2.2 H 2.2 How strong do atoms hold on to their electrons when sharing them in covalent bonds? Lots of strength = holds electrons closer to them when “sharing.” 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

  5. Electronegativity He Helium is noble. It does not share. Fluorine holds its electrons very close. It does not share well, but does share. F 3.96 Fr .7 Francium does not hold its electrons strong enough so it actually loses them. This leads to Ionic Bonds forming.

  6. H 37 H 37 Each row of the Periodic Table represents an energy level around the atom. So lower is bigger. Memorize that farther left is bigger. 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

  7. 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

  8. The left side loses electrons and the right side gains electrons. More electrons repel further from the protons in the nucleus making the right side bigger. Atoms are also bigger further down on the chart. 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

  9. Ionic Radii Helium is noble… It does not make ions because it does not want to lose its electrons. He Carbon loses 4 electrons making it small C 15 Astatine gains 3 electrons and is pretty low making it big As 222 Fr 194 Francium gains 1 electron and is high up making it medium.

  10. QuestionsCopy the following and paste it on your wiki to answer 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

  11. Ionization Energy = energy to lose the outermost (valence) electron – Helium only has two electrons, so that outer electron is close to the nucleus and is strongly attracted to the nucleus – Francium has a lot of electrons so that outer electron is far from the nucleus and is weakly attracted to the nucleus • Electronegativity – similarly the electrons shared by fluorine would be closer to the nucleus than francium so fluorine holds onto the electrons harder – it is a mix of effective nuclear charge, shielding, and atomic radius • Atomic Radii – two trends – vertically the electrons go into shells further from the nucleus so it makes a new layer, like the layers of an onion – horizontally the electrons go into the same shell, so no new layers, but also more protons from left to right so the nucleus can pull harder on the layers making them closer and smaller • Ionic Radii – decent rule of thumb- adding electrons makes elements bigger as they repel each other and removing electrons makes elements smaller as there is less repulsion between the electrons

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