1. Starter S-44 A. What is Lithium’s electron configuration? B.What column of the periodic table is it in? C.What is Sodium’s electron configuration? D.What column of the periodic table is it in?

2. The Periodic Table Chapter 6

3. 6.1 Organization of the Elements Chapter 6

4. In ancient times the known elements were Gold, Silver, Copper, Iron, Lead, Tin, Mercury, Sulfur, Carbon Up until the 1700’s only 4 more had been discovered Arsenic, Antimony, Phosphorus, Zinc 6.1 Organization of the Elements

5. 1829 JW Dobereiner – puts elements in triads Sets of 3 elements with similar chemical properties 6.1 Organization of the Elements

6. 1864 John Newland – Law of Octets When elements are placed in order of atomic mass, properties seem to repeat every 8 elements 6.1 Organization of the Elements

7. 1869 – Dimitri Mendeleev – arranged by increasing atomic mass and properties The table is periodic – properties repeat 6.1 Organization of the Elements

8. 1913 – Henry Mosley – used atomic number instead of atomic mass 6.1 Organization of the Elements

9. The Periodic Law – when elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties. 6.1 Organization of the Elements

10. Period – row 7 rows 6.1 Organization of the Elements

11. Group – column 18 groups (some have names) 6.1 Organization of the Elements Alkali MetalsAlkaline Earth MetalsHalogens Noble Gases Transition Metals

12. Draw the zig-zag line on your periodic table and label the metals and nonmetals 6.1 Organization of the Elements

13. Metals Good conductors, lusterous, ductile, malleable 6.1 Organization of the Elements

14. Nonmetals Poor conductors, dull, brittle 6.1 Organization of the Elements

15. Metalloids Sometimes behaves like a metal, sometimes like a nonmetal 6.1 Organization of the Elements

16. 6.2 Classifying the Elements Chapter 6

17. Information on the periodic table Electron configuration is determined by the elements position on the periodic table 6.2 Classifying the Elements s1s1 s2s2 p1p1 p2p2 p3p3 p4p4 p5p5 p6p6 d1d1 d2d2 d3d3 d4d4 d5d5 d6d6 d7d7 d8d8 d9d9 d 10 f1f1 f2f2 f3f3 f4f4 f5f5 f6f6 f7f7 f8f8 f9f9 f 10 f 11 f 12 f 13 f 14

18. Remember 1 st s is level one, 1 st p is second, 1 st d third 1 st f fourth 6.2 Classifying the Elements s1s1 s2s2 p1p1 p2p2 p3p3 p4p4 p5p5 p6p6 d1d1 d2d2 d3d3 d4d4 d5d5 d6d6 d7d7 d8d8 d9d9 d 10 f1f1 f2f2 f3f3 f4f4 f5f5 f6f6 f7f7 f8f8 f9f9 f 10 f 11 f 12 f 13 f 14

19. 6.2 Classifying the Elements s1s1 s2s2 p1p1 p2p2 p3p3 p4p4 p5p5 p6p6 d1d1 d2d2 d3d3 d4d4 d5d5 d6d6 d7d7 d8d8 d9d9 d 10 f1f1 f2f2 f3f3 f4f4 f5f5 f6f6 f7f7 f8f8 f9f9 f 10 f 11 f 12 f 13 f 14 Noble Gas Configuration 1.Find the noble gas before the element 2.Put that element in brackets [ ] 3.Fill out the rest of the configuration using the pattern in the periodic table

20. For example Strontium (Sr) [Kr]5s 2 6.2 Classifying the Elements s1s1 s2s2 p1p1 p2p2 p3p3 p4p4 p5p5 p6p6 d1d1 d2d2 d3d3 d4d4 d5d5 d6d6 d7d7 d8d8 d9d9 d 10 f1f1 f2f2 f3f3 f4f4 f5f5 f6f6 f7f7 f8f8 f9f9 f 10 f 11 f 12 f 13 f 14 Sr

21. Germanium (Ge) [Ar]4s 2 3d 10 4p 2 6.2 Classifying the Elements s1s1 s2s2 p1p1 p2p2 p3p3 p4p4 p5p5 p6p6 d1d1 d2d2 d3d3 d4d4 d5d5 d6d6 d7d7 d8d8 d9d9 d 10 f1f1 f2f2 f3f3 f4f4 f5f5 f6f6 f7f7 f8f8 f9f9 f 10 f 11 f 12 f 13 f 14 Ge

22. Starter S-45 What are the names of the elements in 1.Group 1 2.Group 2 3.Group 3-12 4.Group 17 5.Group 18

23. 6.3 Periodic Trends Chapter 6

24. 6.3 Periodic Trends Atomic Size – The size of an atom of a particular element Increases down a group Decreases across a period Video

25. 6.3 Periodic Trends Not always an exact pattern

26. 6.3 Periodic Trends 2.Ions – charged atoms Lost (+) or gained (-) electrons Cation – lost electrons Anion – gained electrons Ion Formation Table of ionic radii

27. 6.3 Periodic Trends 3.Ionization Energy The energy required to remove an electron from an atom 1 st ionization energy – energy to remove the first electron Decrease down a group Increase across a period Ionization energy video

28. 6.3 Periodic Trends 4.Electronegativity Ability of an atom to attract electrons when the atom is in a compound Increases across periodic table Decreases down periodic table 6.3 Periodic Trends

29. 5. Density 6.3 Periodic Trends

30. 5. Melting Point 6.3 Periodic Trends

31. Main reasons for patterns 1.Increasing nuclear charge down a group and across a period more protons, larger positive charge 2.Increased shielding down a group as energy levels increase, those electrons further out, are shielded by the inner ones 6.3 Periodic Trends