1. Periodic Table 1

3. History of the Periodic Table 3

4. Dmitri Mendeleev 4

5. Mendeleev’s Periodic Table 5

6. Arrangement of Periodic Table Periodicity– recurrent trends seen in the elements 6

7. horizontal rows 1 - 7 Period number indicates which energy level holds the valence electrons Periods 1 2 3 4 5 6 7 7

8. Groups/Families vertical columns 1-18 elements in the same group share chemical properties Main group elements Groups 1,2 13, 14, 15, 16, 17, 18 8

9. Types of Elements 9

10. Metals Most are silver, shiny, solid, malleable, ductile & good heat/electrical conductors

11. Nonmetals Brittle (solids), dull, non-conductors, and exist in all three states (solids, liquids, gases)

12. Metalloids Elements found along the stair-step between metals and nonmetals, does NOT include Al Properties are in between metals & nonmetals Silicon (Si) is probably the most well- known metalloid.

13. Color Groups of the Periodic Table Alkali Metals Alkaline Earth Metals Transition Metals Lanthanide Series Halogens Noble Gases Actinide Series Inner Transitional Metals Also called inert gases because they do not react Metalloids 13

14. Properties and Electron Configuration Each group (column) ends with the same electron configuration. This determines many of the physical properties that the group share. 14

15. Alkali Metals with Water 15

16. Halogen 16

17. Noble Gases odorless colorless

18. Periodic Table Trends Patterns on the periodic table – Atomic Radius – Ionic Radius – Electronegativity – Ionization Energy – Reactivity 18

19. Effective Nuclear Charge (Z eff ) The relative attraction the valence electrons have for the Protons in the nucleus. Electron Shielding Effect- Inner shell electrons blocking valence electrons from the positively charged nucleus Watch this video 19 Explaining the trends

20. Atomic Radius Atomic radius is half the distance between the centers of two atoms, measured in angstroms (1x10 -10 m). 20

21. Atomic Radius Trend Atomic radius increases as you move down a group Atomic radius decreases as you move from left to right in a period 21

22. Atomic Radius Trend Across the period, the number of protons increases while the number of shielding electrons stays the same. (Z eff increases) This make the nucleus pull in the valence electrons. That makes for a smaller atom. 22

23. Atomic Radius Trend Down the group, the number of energy levels increases so the number of shielding electrons increases. The nucleus cannot pull in the valence electrons. That makes for a bigger atom. 23

24. Ionic Radius Metals lose electrons to form cations Li Li + F F-F- Nonmetals gain electrons to form anions Ionic radius is smaller than atomic radius because an energy level is lost or “shed” Ionic radius is larger than atomic radius because the electrons outnumber the protons. The nucleus has less control of the valence electrons. 24

25. Electronegativity Electronegativity is a measure of how strongly atoms attract bonding electrons to themselves An assigned number “rates” the electronegativity (from 0.7 to 4.0) – Low electronegativity = cannot attract valence electrons – High electronegativity = can attract valence electrons

26. Electronegativity Trend Electronegativity values increase as you move from left to right in any period. Biggest IE = Fluorine Smallest IE = Francium 26

27. Electronegativity Trend Within any group, electronegativity values increase as you go up. Biggest IE = Fluorine Smallest IE = Francium 27

28. Period 2 elements Large  low EN small  high EN F9pF9p Li 3p Be 4p B 5p C 6p N 7p O 8p From right to left, Z eff increases. In small atoms, the distance from the nucleus to available electrons is short, therefore the nucleus has a strong attraction (pull) for electrons. 28

29. 29 Group 17 elements small  high EN large  low EN

30. Ionization Energy Ionization Energy – the energy needed to remove the outermost electron in an atom; describes how hard it is to steal an electron from an atom Increases as you go from bottom to top in a group As you move up a group, the number of energy levels decreases. The nucleus of small atoms has a stronger hold on its electrons because they are so close. 30

31. Ionization Energy Pattern period 2 elements IE Increases as you go right in a period Larger Z eff from right to left Atom is smaller – outer electrons are closer to the nucleus 31

32. Ionization Energy Trend Increases as you go from bottom to top in a group As you move up a group, the number of energy levels decreases. The nucleus of small atoms has a stronger hold on its electrons because they are so close.

33. Metal Reactivity Trend Based on the attraction the metal has for the nonmetal’s electrons. *The most reactive metal is francium increasing metal reactivity increasing metal activity

34. Nonmetal Activity Trend Non-Metal Activity refers to how easily nonmetals gain e- to form anions *This trend does not include the noble gases, because they are non-reactive *The most reactive nonmetal is fluorine increasing nonmetal activity