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Electron Configuration and the Periodic Table

Chemistry Chapter 5 Section 2. Electron Configuration and the Periodic Table. Periods. http://www.bpc.edu/mathscience/chemistry/history_of_the_periodic_table.html. Periods on the periodic table Show a horizontal trend in changing properties

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Electron Configuration and the Periodic Table

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  1. Chemistry Chapter 5 Section 2 Electron Configuration and the Periodic Table

  2. Periods http://www.bpc.edu/mathscience/chemistry/history_of_the_periodic_table.html • Periods on the periodic table • Show a horizontal trend in changing properties • Show the level of outer shell electrons and orbitals filling

  3. Blocks • The periodic table can be broken into ‘blocks’ http://www.meta-synthesis.com/webbook/35_pt/pt_database.php?Button=1950-1999+Formulations

  4. S block • Groups 1 and 2 • Highest energy electron is in an s orbital • Powerful reducing agents • Group 1: Alkali metals • Soft, silvery, low melting points, not found uncombined in nature • Group 2: Alkaline Earth metals • Harder, denser, higher MP than Group 1, not found uncombined in nature

  5. Sample Problem 5-1 • Without looking at the periodic table, give the group, period and block for: [Xe]6s2 • Without looking at the periodic table, write the electron configuration of the group 1 element in the third period. Is this element likely to be more or less reactive than the previous element?

  6. D block • Transition elements • Fill d block, which is one level lower than the valence shell • Electron configuration may vary depending on half-full and totally full d orbital stablity • Properties: • Metallic luster, good conductors, may be unreactive

  7. Sample problem 5-2 • An element has the electron configuration [Kr]4d55s1. Without looking at the periodic table, identify the period, block and group in which this element is located. Then consult the periodic table to identify the element.

  8. P block • Groups 13-18 • Sometimes called main-group elements • Properties vary from metallic on left to metalloid to nonmetallic to noble gas on right • Groups within this block: • Halogens: most reactive nonmetals • Noble gases: nonreactive

  9. Sample Problem 5-3 • Without looking at the periodic table, write the outer electron configuration for the group 14 element in the second period. Then name the element and label it as metal, metalloid or nonmetal.

  10. F block • Two rows below the periodic table • F orbital 2 levels lower than valence filling • Follow Lanthanum and Actinium • Lanthanide: REE • Actinide: all radioactive

  11. Sample problem 5-4 • The electron configurations of four elements are written at the top of page 139. For each element, name the block and group in the periodic table in which it is located. Then name the element using the periodic table. Identify each element as a metal, metalloid or nonmetal. Finally, describe it as likely to be of high or low reactivity.

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