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Honors Chemistry

Honors Chemistry. Section 5.2 Electron Configuration and the Periodic Table. Periodic Table. Arranged in groups and periods Groups – similar chemical properties Period – length determined by # of electrons added to the shell. Blocks in the Periodic Table. S - block.

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Honors Chemistry

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  1. Honors Chemistry Section 5.2 Electron Configuration and the Periodic Table

  2. Periodic Table • Arranged in groups and periods • Groups – similar chemical properties • Period – length determined by # of electrons added to the shell.

  3. Blocks in the Periodic Table

  4. S - block • Chemically reactive metals • Group 1 more reactive than Group 2 • Group 1 – alkali metals • Configuration ns1 • Soft • Silvery • So reactive don’t exist in nature as elements • React vigorously with nonmetals • React strongly with water • As you go down the group Tmelt decreases • H not an alkali metal

  5. S – block (cont.) • Group 2 – alkaline earth metals • Configuration ns2 • Harder, denser and stronger than alkali metals • Higher melting point than alkali metals • Less reactive than alkali metals – but still not found in nature as elements • He has an alkaline earth configuration but is a noble gas

  6. Practice • Give the group, period and block of the element with the configuration [Rn] 7s1 • Give the group, period and block of the element with the configuration [He] 2s2 • How does the reactivity of [He] 2s2 compare with [He] 2s1?

  7. D-block • Fills Groups 3 to 12 • Starts filling in the 4th Period (3d) • Configuration ns2 (n-1)dx • Examples • Group 3 - ns2 (n-1)d1 • Group 12 - ns2 (n-1)d10 • D – block are metals • Called Transition Metals or Transition Elements • Good conductors of heat and electricity • Have high luster • Less reactive than alkali or alkaline earth elements • Some don’t easily form compounds (Pd, Pt, Au)

  8. Practice • What is the period, block and group of the element with the configuration [Ar] 3d10 4s1? • What is this element? • What other elements are in the same group?

  9. P - Block • Groups 13 to 18 (Except He) • S – block + P – Block = Main Group Elements • # valence electrons = Group # - 10 • Contains all metalloids • Group 17 – Halogens – most reactive nonmetals • Halogens react with metals to form salts

  10. P – Block (cont.) • Metals – harder and denser than s – block metals but softer and less dense than d – block. • Most p – block metals are not found as elements in nature. • Metalloids – brittle solids/intermediate conductivity

  11. Practice • What is the outer configuration for Group 16, Period 3? What is the name of the element? Is it a metal/nonmetal/metalloid? • What is the period block and group of the element [Kr] 4d10 5s2 5p3? What is the name of the element? Is it a metal/nonmetal/metalloid?

  12. F - Block • Between Groups 3 and 4 • In the 6th and 7th Periods • 4f and 5f are being filled • Lanthanides • Shiny • Metals • Reactivity similar to alkaline earth metals • Actinides • Radioactive • All but first 4 - synthetic

  13. Practice • For each of the following determine block, period, and group. What is the name of the element and determine if the reactivity is high or low. • [He] 2s2 2p3 • [Xe] 4f14 5d10 6s1 • [Rn] 7s1 • [Ar] 3d10 4s2 4p5

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