1. Periodic Table Museum

2. HISTORY

3. John Newlands (1864) proposed an organization scheme for elements based on increasing atomic mass noticed that the properties of elements repeated every eighth element (1st and 8th, 2nd and 9th) –Example: he noticed the similar properties between Li and Na, Be and Mg, N and P –Law of Octaves – repeating (periodic) relationship every 8th element, like music notes criticized as “unscientific” and work not generally accepted

5. Dmitri Mendeleev (1869) designed the first periodic table based on: –Elements with similar properties grouped together –Increasing atomic mass –Left blank spots, predicting properties of elements that had not yet been discovered.

7. Henry Moseley Rearranged the periodic chart to its current form based on increasing atomic number elements with similar properties grouped together. –This solved problem of misplaced elements Periodic Law - when elements are arranged by increasing atomic number, there is a periodic repetition of chemical and physical properties

9. Reading the Periodic Table

10. Periodic Table Groups (or Families)– columns on the table Elements in the same group or family have similar characteristics or properties. Kr Xe Rn Ar Ne He 8A CaKScTiVCr Mn FeCoNiCuZn Ga GeAsSeBrKr Periods – rows on the table Elements in a period are not alike in properties.

11. States of Matter

12. Definite Shape (does not depend on container) Definite Volume (does not depend on container) Effect of Temperature increase Compressible (can squeeze into smaller volume) SolidYes Small expansionNo LiquidNoYesSmall/moderate expansion No Gas/ Vapor No Large expansion Yes

13. States of Matter

15. H LiBe NaMg CaK Rb Cs FrRa Ba Sr ScTiVCr Mn FeCoNiCuZnGaGeAsSeBrKr XeITeSbSnInCdAgPdRhRuTcMoNbZrY La AcRf HfTaWReOsIrPtAuHgTlPbBiPoAtRn DbSgBhHsMt LuYbTmErHoDyTbGdEuSmPmNdPrCe ThPaUNpPuAmCmBkCfEs Fm MdNoLr Ar Ne He F ClSPSiAl BCNO 1A 2A 3B4B5B6B 7B8B 1B2B 3A4A5A6A7A 8A Metals, Non-Metals, & Metalloids

16. Metals Left side of the periodic table –except H Properties: –lustrous (shiny) –good conductors of heat & electricity –malleable & ductile –solids at RT (except Hg)

17. Non-Metals Right side of table –plus H Properties: –Dull appearance –Brittle when solids –Do not conduct heat or electricity well –May be solid, liquid or gas at RT

18. Metalloids Stair step between metals and non- metals Properties in between metals and non-metals –Si: brittle but semi-conductor Many metalloids are used in computer chips to conduct electricity without conducting too much heat

19. Families

20. very reactive metals that do not occur freely in nature Slivery-white and softer than most other metals (to the point that they can be cut easily with a knife) can explode if they are exposed to water ALKALI METALS

21. They are harder, denser, and stronger than the alkali metals with higher melting points They are so reactive they are not found as free elements in nature ALKLINE EARTH METALS

22. Metals with typical metallic properties and uses Less reactive than group 1 and 2 metals – some are so unreactive that they exist in nature as free-elements Iron, cobalt, and nickel, are the only elements known to produce a magnetic field. TRANSITION METALS

23. Inner Transition Metals Wedged between groups 3 and 4 in the sixth and seventh periods The lanthanides (top) are shiny and similar in reactivity to the alkaline-earth metals. The actinides (bottom)are all radioactive and most are man-made Actinides Lanthanides

24. HALOGENS "halogen" means "salt-former" and compounds containing halogens are called "salts" Most reactive non-metals exist in all three states of matter at room temperature: Solid- Iodine, Astatine Liquid- Bromine Gas- Fluorine, Chlorine

25. NOBLE GASES Nonreactive due to their complete valence shells Do not easily gain or lose valence electrons All gases at room temperature