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2. 2 Who developed the Periodic Table? Dimitri Mendeleev – (Russian Chemist) In 1871 developed the first Periodic Table with 63 elements that were known at the time. He found that as the atomic mass increased, a repeating patterns of properties developed.

3. 3 Rearranging Table Henry Moseley- English scientist In 1913 he rearranged the periodic table by the atomic number and chemical properties. This is the periodic table we use today

4. 4 and COLUMNS called GROUPS or FAMILIES. Mendeleev arranged these elements into ROWS called PERIODS… Arrangement of the Periodic Table

5. 5 You can think about it like this… You have to use a PERIOD at the end of a sentence……..that goes left to right. And a COLUMN holds up the porch on the house where your GROUP / FAMILY gather.

6. 6 Periods represent the number of rings. Energy Level 2: Li, Be, B, C, N, O, F & Ne Locate them on your periodic table These outer ring is called Valence Shell or energy level 2 nd Row = 2 Rings electron

7. 7 4 3 5 6 7 1 2 This is period number 3 Which means it has 3 energy levels This is period number 3 Which means it has 3 energy levels Period #’s run down the side of the Periodic Table.

8. 8 The Group Numbers run on top Of the Periodic Table This is group 1 the alkali group. Families have similar but not identical characteristics 1 IA 2 IIA 18 VIIIA 17 VIIA 15 VA 16 VIA 14 IVA 13 IIIA

9. 9 Metals Non-Metals Transition Metals Inner Transition Metals Metalloids

10. 10 Properties of Metals Good conductors of heat and electricity Malleable, Ductile Have Luster High melting & boiling points High density Mostly solids – except for Hg (liquid) Fr Left of the STAIRS

11. 11 Properties of Nonmetals Poor conductors of heat and electricity Dull, Brittle Low melting and boiling points Most are GASES, some SOLIDS, and only 1 Liquid - Bromine Right of the STAIRS F

12. 12 Properties of Metalloids Conduct…not as well as TRUE metals Shiny or dull Have other properties of metals and nonmetals All Solids Touch the STAIRS

13. 13 Characteristics  Group IA or 1  Has 1 Valence electron  Make salts such as NaCl and KCl  Lithium - Treatment for bi-polar disorder  Highly reactive

14. 14 Characteristics  Group IIA or 2  Has 2 Valence electrons  Gemstones and fireworks  Magnesium burns brightly.  Calcium makes bones strong.  Makes strong and light materials-planes, cars

15. 15 Characteristics  Group VIIA or 17  Has 7 Valence electrons  Cl - is the most abundant, used in bleach  Br - used as dyes in cosmetics  I - (shiny gray) used to make thyroxin.  Highly reactive group of Non-Metals

16. 16 Characteristics  Group VIIIA or 18  Have 2 or 8 Valence electrons  Uses: Neon lights, laser lights...  Most Stable Group of Elements  Normally don’t mix with other compounds

17. 17  Group 1, IA but not an Alkali Metal  Has 1 Valence Electron  Used in everything from water to acids and bases.  Most abundant element  Acts more like a Metal than a Non-Metal  Has properties of both Alkali Metals & Halogens Characteristics

18. 18 Characteristics  Groups 3 through 12 or IIIB to IIB  Has 1 or 2 valence electrons  Iron, copper, and silver are examples  Makes gemstones  From Left to Right –gain properties of Non-Metals  Less active than alkali metals and alkaline earth metals

19. 19 Inner Transition Elements Lanthanide seriesLanthanide series Elements 57-71 1 or 2 valence electrons Actinide Series Elements 89-103 1 or 2 valence electrons All are radioactive Most are synthetic (man-made)