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The Periodic Law

The Periodic Law . Electron Configuration and the Periodic Table. The alkaline earth metals. Be. Mg + 2 H 2 O  Mg(OH) 2 + H 2 Ca + 2 H 2 O  Ca(OH) 2 + H 2. Mg. Ca. Sr. Ba. Ra. The Alkali Metals. Sodium and Water – YouTube Na + H 2 O  NaOH + H 2 Potassium and Water – YouTube

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The Periodic Law

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  1. The Periodic Law Electron Configuration and the Periodic Table

  2. The alkaline earth metals Be Mg + 2 H2O  Mg(OH)2 + H2 Ca + 2 H2O  Ca(OH)2 + H2 Mg Ca Sr Ba Ra

  3. The Alkali Metals Sodium and Water – YouTube Na + H2O  NaOH + H2 Potassium and Water – YouTube K + H2O  KOH + H2 Li Na K Rb Cs Fr

  4. Periods and Blocks of the Periodic Table Write the electron configuration for: Mg Ca F Cl 1s22s22p63s2 1s22s22p63s23p64s2 1s22s22p5 1s22s22p63s23p5

  5. Sample Problems • Without looking at the periodic table, give the group, period, and block in which the element with the electron configuration [Xe]6s2 is located. Group 2, sixth period, s-block • Without looking at the periodic table, write the electron configuration for the Group 1 element in the third period. Is this element likely to be more active or less active than the element in #1? 1s22s22p63s1; more reactive

  6. Hydrogen and Helium Hydrogen and helium are the most abundant elements in the universe. Hydrogen makes up 76 % of the mass of the universe and helium makes up 23 %. Hydrogen 1s1 • Despite the same outer configuration as the alkali metals, H has unique properties unlike any other group. Helium 1s2 • Although its configuration is similar to the alkaline earth metals, it has the properties of a noble gas due to its filled outer energy level.

  7. d-Block elements

  8. d-Block elements • d-Block elements are known as transition metals • Have common metallic properties • Conduct heat and electricity • Less reactive than alkali and alkaline earth metals • Some are very unreactive: Au, Pt, Pd, Ag

  9. d-Block elements Deviations from orbital filling: Nickel (Ni): [Ar]4s23d8 Palladium (Pd): [Kr]5s04d10 Platinum (Pt): [Xe]6s14f145d9 • In each case the sum of s and d electrons is 10

  10. d-Block elements Oxidation States • Most transition metals are multivalent Iron (Fe): [Ar]4s23d6 Iron II (Fe2+): [Ar]4s13d5 Iron III (Fe3+): [Ar]4s03d5

  11. p-Block elements • p-Block and s-block elements together are known as the main group elements. • Properties vary considerably • Includes nonmetals, metalloids, and metals

  12. p-Block elements Metalloids (semi-metals) • B, Si, Ge, As, Sb, Te, Po?, At? • Properties of both metals and nonmetals • Brittle solids • Conduct electricity Silicon

  13. p-Block Elements Metals • Al, Ga, In, Tl, Sn, Pb, Bi • Reactive and found in nature as part of compounds • Relatively stable in elemental form • Softer and less dense than d-block metals. (Pb is an exception.)

  14. p-Block Elements F Halogens • Group 17 nonmetals • Very reactive; react with most metals to form salts • one electron short of noble gas configuration • Form -1 ions Cl Br I At Uuo

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