1. Notes One Unit Nine Chapter Four Early Periodic Tables Modern Periodic Table Orbitals on The Periodic Table Elements of Life Dot Diagrams

2. Electron Shielding Explanation 12 e -1          How many e -1 for Mg ? 20 e -1 How many e -1 for Ca?               +12+20 How many protons? What is the Short-Hand element in each case? NeAr Do the nuclear protons attract or repel the e -1 ? Do the short-hand e -1 attract or repel the e -1 ?

3. Early Periodic Tables John Newland’s law(1837-1898) Organized by (a)Octaves (b) Mass Demetri Mendeleev (1834-1907) Proposed arranging elements by (a) Properties (b) Mass

4. Dobereiner and Triads From the Dobereiner’s law of triads, the atomic mass of the middle element, in this case Na, should be the arithmetic mean of Li and K. arithmetic mean of Li and K (7 + 39)/2 = 23 Elements Symbolmass LithiumLi7 SodiumNa23 PotassiumK39

5. Modern Periodic Table Organized Rows (period) Columns (Families): Alkali Metals Alkaline Earth Metals Transition Metals Rare Earth Metals Other Metals Metalloids Non-Metals Halogens Noble Gases Atomic Number (Henry Moseley 1913 X- rays) Two Main groups: Metals Nonmetals

6. Modern Periodic Table

9. Orbitals on The Periodic Table f-block d-block p-block s-block

10. Electron Configurations Most stable elements are He, Ne, Ar, Kr, Xe and Rn. Most Unstable Metals are H, Li, Na, K, Rb, Cs, Fr Most Unstable Nonmetals are F, Cl, Br, I, and At

11. Alkali Metals

12. Alkaline Earth Metals

13. Halogens

14. Noble Gases

15. Elements of Life

16. Dot Diagrams

17. Notes Two unit Nine Chapter Four Halogens Lab Observation Halogens Lab Explanation Valence Versus Kernel Electrons Electron Shielding Increasing Atomic Number Highest Energy Level Occupied Atomic Radii Ionization Energy Other Trends

18. 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← +17 ← ← ←←← ←← Ne 1s 2s 2p 3s 3p 4s 3d 4p ← ← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ← ← ←←← ←← +35 Br Ar 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p ← ← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ← ← ←←← ←← +53 I Kr Do a complete workup on each element. Bromine’s shielding(Ar) is great than Chlorine’s shielding(Ne) Bromine’s valence e -1 ’s are further from the nucleus than Chlorine’s valence e -1 ’s. Iodine’s valence e -1 ’s are even further from the nucleus and have yet greater shielding. Electronegativity 3.160 Cl 2.960 2.660 Halogen comparative Reactivity

19. 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← ← +11 Na 1s 2s 2p 3s 3p 4s 3d 4p ← ← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ← ← ←←← ←← +35 Br NaBr(aq) Colorless Solution Sodium lost an e -1 to bromine. Sodium is stable like which noble gas? neon Bromide is stable like which noble gas? krypton Halogens Lab:NaBr If chlorine comes along, what will happen? 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← +17 ← ← ←←← ←← Cl Yellow-green ← ←

20. 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← ← +11 Na 1s 2s 2p 3s 3p 4s 3d 4p ← ← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ← ← ←←← ←← +35 Br When chlorine takes the e -1 from bromide, what do we see? Chlorine(Yellow-green) turns in to chloride(colorless) 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← +17 ← ← ←←← ←← Cl Yellow-green ← ← Bromide(colorless) turns in to bromine(orange) Halogens Lab:NaBr

21. NaI(aq) Colorless Solution Halogens Lab:NaI 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← +11 Na 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p ← ← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ← ← ←←← ←← +53 I Sodium lost an e -1 to iodine. Sodium is stable like which noble gas? neon Iodide is stable like which noble gas? xenon If brome comes along, what will happen? 1s 2s 2p 3s 3p 4s 3d 4p ← ← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ← ← ←←← ←← +35 Br ←← ←

22. 1s 2s ← ← ← +3 Li 1s 2s 2p 3s ← ← ← ← ←←← ←←← ← +11 Na 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← ← +19 K 4s ← ← ←←← ←←← 1s 2s 2p 3s ← ← ← ← ←←← ←←← ← +12 Mg ← 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← ← +20 Ca 4s ← ← ←←← ←←← ← Metallic Reactivity Versus Shielding He Ne Ar Do a complete workup on each element. Which is more reactive…Li, Na or K? Why is it more reactive? Which is more reactive…Na or Mg? Why is it more reactive? (1) more shielding e -1 ’s (2) valence electrons are further from the + charge of the nucleus. (1) less protons to hold valence e -1 ’s. The e -1 ’s are lost more easily. Electronegativity 0.980 0.930 0.820 1.310 1.000

23. 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← ← 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← ← ← 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← ← ← ← 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← ← ← ←← 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← ← ← ←←← 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← ← ← ←←← ← 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← ← ← ←←← ←← 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← ← ← ←←← ←←← +11 +12 +13+14 +15+16+17 +18 Na?What is OFD for Na Mg?Al?Si?S?S?Cl?Ar? Which are the Kernel e -1 ’s for MgAl Si P?P? PSClAr Na?Mg?Al?Si?S?S?Cl?Ar?P?P? Ne Properties change due to increasing atomic # horizontally 0.9301.310 1.610 1.900 2.190 2.5803.160

24. Atomic Radii Left to Right on the periodic table What does the # of kernel e -1 ’s say about shielding’s action on atomic radii from left to right on the periodic table? How does Highest Energy Level Occupied action on atomic radii from left to right on the periodic table? Highest Energy Level Occupied does not affect size from left to right. What does this say about Increasing atomic # action on atomic radii from left to right on the periodic table? All are the 2 nd NRG in this case Increasing atomic # shrinks size. Shielding has no effect on size left to right

25. 1s 2s ← ← ← +3 Li 1s 2s 2p 3s ← ← ← ← ←←← ←←← ← +11 Na 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← ← +19 K 4s ← ← ←←← ←←← He Ne Ar Atomic Radii Top to Bottom on the periodic table What does # of kernel e -1 ’s say about shielding? How does Highest Energy Level Occupied action on size What does this say about Increasing atomic # action on atomic radii from Top to Bottom Shielding increases size Top to Bottom Highest NRG Level increases size Top to Bottom Increasing atomic # has no effect on size

26. Ionization Energy The ionization energy or ionization potential is the energy necessary to remove an electron from the neutral atom. How does ionization energy compare to atomic radii?

27. Other Trends

28. End

29. Assembly slide for K 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← +17 Cl ← ← ←←← ←← Ne

30. Iodine assembly 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p ← ← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ← ← ←←← ←← +53

31. 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p ← ← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ← ← ←←← ←← +53 I Kr 1s 2s 2p 3s 3p 4s 3d 4p ← ← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ← ← ←←← ←← +35 Br Ar 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← +17 Cl ← ← ←←← ←← Ne Assembly slide for Cl, Br and I.

32. 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 1s 2s 2p 3s ← ← ← ← ←←← ←←← ← ← ← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ← ← ←←← ←← +11+54

33. 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← +11 Na 1s 2s 2p 3s 3p 4s 3d 4p ← ← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ←←← ←←← ← ← ← ← ←←← ←← +35 Br NaCl(aq) Halogens Lab:NaBr 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← +17 ← ← ←←← ←← Cl Yellow-orange ← Colorless Solution Why does this happen? Chlorine has less shielding. It strongly attracts electron.

34. 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← ← 1s 2s 2p 3s 3p ← ← ← ← ←←← ←←← ← ← +11 +12 Na Mg