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Understanding the Periodic Table: Groups, Periods, and Element Properties

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The periodic table organizes elements into groups and periods based on their electron configurations and properties. Elements in the same group share similar characteristics due to having the same number of valence electrons, affecting their bonding behavior. For example, group 2 elements like beryllium and magnesium each have 2 outer shell electrons. Additionally, elements in the same period have the same number of electron shells, such as potassium and iron, both in period 4. This classification helps predict element behavior and reactions, aiding in the understanding of chemistry.

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Understanding the Periodic Table: Groups, Periods, and Element Properties

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  1. Vertically intoGroups Horizontally IntoPeriods Elements are arranged:

  2. Why?

  3. If you looked at one atom of every element in a group you would see…

  4. Each atom has the same number of electrons in it’s outermost shell. • An example…

  5. The group 2 atoms all have 2 electrons in their outer shells Be (Beryllium) Atom Mg (Magnesium) Atom

  6. The number of outer or “valence” electrons in an atom effects the way an atom bonds. • The way an atom bonds determines many properties of the element. • This is why elements within a group usually have similar properties.

  7. If you looked at an atom from each element in a period you would see…

  8. Each atom has the same number of electron holding shells. An example…

  9. The period 4 atoms each have 4 electroncontaining shells 4th Shell K (Potassium) Atom Kr (Krypton) Atom Fe (Iron) Atom

  10. Each group has distinct properties • The periodic Table is divided into several groups based on the properties of different atoms.

  11. http://www.lyon.edu/webdata/Users/DMcDowell/GenChem/alkalishow.htmlhttp://www.lyon.edu/webdata/Users/DMcDowell/GenChem/alkalishow.html Alkali Metals Soft, silvery colored metals Very reactive!!!

  12. Alkali Metals reacting with water: • Li (Lithium) • Na (Sodium) • K (Potassium) • Rb (Rubidium) • Cs (Cesium) What would you expect from Francium?!?!

  13. Alkaline Earth Metals Silvery-White Metals Fairly reactive Many are found in rocks in the earth’s crust

  14. Transition Metals Most are good Conductors of electricity Malleable (easily bent/hammered into wires or sheets)

  15. How many things can you think of that have Transition Metals in them?

  16. Metalloids lie on either side of these “stairsteps” They share properties with both metals and non-metals Si (Silicon) and Ge (Germanium) are very important “semi-conductors”

  17. What are semiconductors used in?

  18. Nonmetals Brittle Do not conduct electricity

  19. Halogens Most are Poisonous Fairly reactive

  20. Chlorine Gas was used as a chemical weapon during World War I. It was used by the Nazis in World War II.

  21. Noble Gases Unreactive Gases at room temperature

  22. Jellyfish lamps made with noble gases artist- Eric Ehlenberger

  23. Colors Noble Gases produce in lamp tubes: • Ne (Neon): orange-red • Hg (Mercury): light blue • Ar (Argon): pale lavender • He (Helium): pale peach • Kr (Krypton):pale silver • Xe (Xenon): pale, deep blue

  24. Lanthanide Series Actinide Series

  25. http://www.bookrags.com/periodictable/

  26. Quiz • The symbol Au represents which element on the periodic table? • A. silver • B. gold • C. mercury • D the element of surprise

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