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Periodic Table

Physical Science. Periodic Table. Early Attempts. In the 1800’s, chemists tried to organize the elements using their chemical and physical properties They laid the foundation for the modern periodic table

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Periodic Table

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  1. Physical Science Periodic Table

  2. Early Attempts • In the 1800’s, chemists tried to organize the elements using their chemical and physical properties • They laid the foundation for the modern periodic table • Some chemists notices that certain properties repeated every eighth element, but this only worked for the first twenty elements • Early tables organized the elements by their atomic mass, this presented some issues with elements such as • Ar and K • Co and Ni • Te and I • Th and Pa • By the early 1900’s the table was arranged in order of Atomic Number rather than mass, the way it is today

  3. B) Dmitri Mendeleev • Father of the Periodic Table • Published in 1869 a table with the elements arranged by atomic mass • Left gaps for elements that had not been discovered yet • Because his predictions about unknown elements were so darn close, he is credited with the creation of the periodic table

  4. Predictions About the Undiscovered Element- Germanium

  5. Sculpture of Mendeleev in Slovakia- Talk about getting your Nerd On!!!!!

  6. C) Periodic Table Geography • Horizontal Rows on the table are called Periods • Periods represent energy levels in an atom • Vertical Columns on the table are called Families or Groups • Each element in a family has the same number of valence electrons • Elements in a group have similar chemical and physical properties Periodic Law- says that when arranged by atomic number that certain traits occur periodically, thus creating families, certain family have particular names

  7. Group 1 – Alkali Metals * highly reactive metals that do not occur freely in nature -must be stored either in wax or oil to protect * 1 valence electron in the outermost shell * often soft metals, but are good conductors of electricity and heat *malleable and ductile *low melting points *form very strong basic solutions Group 2- Akaline Earth Metals *also highly reactive metals * 2 valence electrons in the outermost shell * called earth metals because of their extremely high melting points *burn reddish colors in flame tests

  8. Groups 3-12 Transition Metals *38 elements total *Good conductors, malleable and ductile * these elements the gain or lose electrons differently based upon the particular chemical reaction

  9. Group 17 –Halogens *non-metallic *seven valence electrons *elements are found in three different phases-solids, liquids and gas *highly reactive, found in lots of compounds

  10. Group 18 – Noble Gases *not very reactive *8 valence electrons in outermost shell, making them stable *all of them are gasses

  11. Groups 14-16 – Non-metals also include groups 17-18 *Poor conductors of heat and electricity *very brittle, dull colored *can be solids or liquids *tend to form acidic solutions *lower densities than metals *are highly electronegative, tend to steal electrons from other atoms Metalloids – line the transition between metals and non-metals *have properties similar to both metals and non-metals *elements 5, 14, 32, 33, 51, 52, 84, 85

  12. Rare Earth Elements * compose the lanthanide and actinide series -the two lonely rows at the bottom *total of 30 elements *are all metals *most are man-made *highly electrically conductive *mainly formed in complex minerals, which made them seem rare

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