1 / 17

Periodic Table

Periodic Table. A Work in Progress. History. 1817 German chemist Johann Dobereiner Triads of similar chemical properties 1864 John Newlands – English Law of Octaves 1869 Dmitri Mendeleev – Russian Cards, left holes where he thought elements should be Dutch Anton van den Broek

jacob
Télécharger la présentation

Periodic Table

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Periodic Table A Work in Progress

  2. History • 1817 German chemist Johann Dobereiner • Triads of similar chemical properties • 1864 John Newlands – English • Law of Octaves • 1869 Dmitri Mendeleev – Russian • Cards, left holes where he thought elements should be • Dutch Anton van den Broek • arranged according to charge, not mass

  3. Organization • Periods – ROWS • properties change gradually • Group (family) – COLUMNS • have similar properties

  4. Key to the Periodic Table • Element name • Atomic number (Whole #, element ID) • Symbol • Atomic mass (weighted average of isotopes) • State of matter

  5. Metals • Solids (except mercury) • Luster (shiny) • Conducts heat, electricity • Maleable (easily shaped) • Ductile (can be shaped into wire)

  6. Non-metals • Gases or brittle solids • Poor conductors of electricity • Only 17

  7. Metalloids - Semimetals • Some properties of metals/nonmetals

  8. Groups (Columns) • Representative elements – groups 1-2, 13-18 (some metals, metalloids, non-metals) • Transition elements – groups 3-12 – metals • Inner transition elements – inside bottom 2 rows – lanthanide, actinide series

  9. Group 1 Alkali Metals • Far left column on PT • Silvery solids • Low density • React violently with water, burns skin • Never found in pure form in nature • Forms +1 ions

  10. Group 2 Alkaline Earth Metals • 2nd column from left • Denser, harder, higher melting points • Not as reactive as alkali metals • Burn different colors – fireworks! • Forms +2 ions

  11. Groups 13-16 • BCNO – large family, diverse • Similar bonding characteristics • Group 13 – Boron family • Group 14 – carbon family • Group 15 – Nitrogen group • Group 16 – Oxygen family • Forms -2 ions

  12. Halogens • Group 17 • Forms salts/ -1 ions • Poisonous • Very reactive • Not found in pure form in nature • When bonded to Carbon, destroys ozone layer

  13. Noble Gases • Far right of PT • Gases • Light up when electrical current goes through • Don’t react • Outer energy levels filled • Group 18

  14. Transition Metals • Groups 3-12 • Conduct heat, electricity • Combine with oxygen different ways • Dissolve in acid (except gold) • Higher melting points than other elements

  15. Inner Transition Metals • Lanthanides • Soft, silvery metals • Spark when struck • Actinides • all radioactive • Some synthetic

  16. Energy Levels • 2 • 8 • 8 • 18 • 18 • 32 • 32

  17. Valance Electrons • In outer incomplete energy level • Used to bond with other atoms • Shown in electron dot diagrams

More Related