2. When and who? In 1869 Russian Chemist Dimitri Mendeleev and German chemist Lothar Meyer published nearly identical ways of classifying

3. But Mendeleev is generally more credited with the 1 st periodic table for 2 reasons: He published first He was better at explaining it than Meyer

4. Mendeleev also saw the “periods” Credited with publishing the first “periodic table”

5. Mendeleev got lots of credit because he left gaps for missing elements!

6. How was the periodic table of elements categorized at that time? By increasing molar mass

7. Periodic Law When the elements are arranged in increasing order by their atomic numbers, their properties repeat periodically

8. The Modern Periodic Table Organized in order of increasing atomic number

9. METALS Non-METALS METALLOIDS Left side and center Right side On the “stair step line” (Al is not included because it always acts like a metal)

10. Horizontal rows are called periods There are 7 periods HORIZONTAL ROWS

11. What do all of the elements in any given period have in common?

12. Elements within the same row (or period) are in the same energy level 1 2 3 4 5 6 7

13. Tall columns are collectively referred to as the GROUPS or FAMILIES

14. What are similarities between elements of the same group? Same number of valence electrons Same ending configuration, but different energy levels Same charge and same chemical behavior

15. Vertical columns are called groups. Elements are placed in columns by similar properties. Also called families

16. Alkali Metals Group 1

17. Alkali Metals Elements: Li, Na, K, Rb, Cs, Fr Chemical Properties: most highly reactive metals; stored in oil Physical Properties: metals, silver gray, soft, have a low density (light weight) Charge of Ions: +1 Reaction with water: 2x + H2O  2xOH + H2

18. Alkaline Earth Metals Group 2

19. Alkaline Earth Metals Elements: Be, Mg, Ca, Sr, Ba, Ra Chemical Properties: extremely reactive; kept in oil Physical Properties: shiny metals, gray silver Charge of Ions: +2 End of Electron Configuration: s 2

20. Transition Metals : short, center groups are collectively referred to as the transition elements Groups 3-12

21. Transition Metals They are given because they were believed to be chemically between metals and nonmetals Some common elements: Zn, Au, Mn, Se, Ti, Rn Charge of Ions: Variable End of Electron Configuration: d

22. Boron Family Group 13

23. Carbon Family Group 14

24. Nitrogen Family Group 15

25. Oxygen Family A.K.A. the Chalcogens Group 16

26. Halogens Group 17

27. Halogens Elements: F, Cl, Br, I, At Chemical Properties: most reactive non metals Charge of Ions: -1 End of Electron Configuration: p 5

28. Noble Gasses Group 18

29. Noble Gases Elements: He, Ne, Ar, Kr, Xe, Rn Chemical Properties: very un-reactive; do not want to bond with anything Charge of Ions: 0 End of Electron Configuration: p 6 Former Name: Inert Gases Why is this former name inappropriate to use? Because under specialized conditions, noble gases are able to bond with other elements

30. Two long rows on bottom are collectively referred to as the “inner transition metals”

31. Lanthanide Series Actinide Series

32. Lanthanide Series Elements Atomic # 58- 71 Elements: Ce, Pr, Nd, Pm, Sm, Eu, Gd, Tb, Dy, Ho, Er, Tm, Yb, Lu Located: first of the two rows below the periodic table Also classified as part of the inner transition metals Formerly named: Rare earth metals Inappropriate name because not all of them are rare

33. Lanthanide Series Actinide Series

34. Elements Atomic # 90- 103 Elements: Th, Pa, U, Np, Pu, Am, Cm, Bk, Cf, Es, Fm, Md, No, Lr Located: second of the two rows below the periodic table Also classified as part of the inner transition

35. Transuranium Elements Lab created elements Include elements 93 and higher

36. Using your own color scheme, color each group of the periodic table. Be sure to include a KEY Groups to label: Transition metals, Noble Gases, Alkali Metals, Lanthanide Series, Halogens, Alkaline Earth Metals, Actinide Series