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Periodic Trends in Period 3

Periodic Trends in Period 3. Chlorides and Oxides Bonding and Structure. Position of elements on the periodic table affects the type of bonding. Period 3: Chlorides. NaCl, MgCl 2 , AlCl 3 , SiCl 4 , PCl 5 increase in the number of electrons available to form bonds. increasing valence e-.

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Periodic Trends in Period 3

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  1. Periodic Trends in Period 3 Chlorides and Oxides Bonding and Structure

  2. Position of elements on the periodic table affects the type of bonding.

  3. Period 3: Chlorides • NaCl, MgCl2, AlCl3, SiCl4, PCl5 • increase in the number of electrons available to form bonds. increasingvalence e-

  4. Chlorides of Metals(NaCl, MgCl2) • ionic • high melting points • soluble in water • do not react with water • electrolytes (conduct electricity) as aqueous solutions or molten (liquid) • NaCl(aq)  Na+(aq) + Cl-(aq)

  5. Electrolyte

  6. Chlorides of Non-Metals (PCl5, PCl3) • molecular/covalent • weak van der Waal’s forces between molecules = low melting and boiling points • hydrolysis: to split by the action of water PCl3(l) + 3H2O(l)  P(OH)3(aq) + 3H+(aq) + 3Cl-(aq) • non-metal/Cl bond replaced by a non-metal/O bond

  7. non-metal chlorides (aq) conduct electricity (but not when molten) • Cl2: molecular/covalent, reacts with water in a hydrolysis reaction Cl2(g) + H2O(l)  HOCl(aq) + HCl(aq) • Al: metal, but acts like a non-metal in bonds • because of it’s high charge, small size ion

  8. Period 3 Oxides • Na2O, MgO, Al2O3, SiO2, P4O10, SO3, Cl2O7 • P4O6 SO2 Cl2Obasic acidic • reducers oxidizers • (donate e-) (accept e-)

  9. Metals: Na, Mg • ionic solids • basic • react with water to make alkaline solution Na2O(s) + H2O(l)  2Na+(aq) + 2OH-(aq)

  10. Metalloids: Al • “giant covalent lattices” • high melting/boiling points • insoluble in water • Al2O3 is amphoteric (dissolves in acid or base) • Al2O3(s) + 6H+(aq) 2Al3+(aq) + 3H2O(l) • Al2O3(s) + 2OH-(aq) 3H2O(l) + 2Al(OH)4(aq)

  11. Non-metals: Si, P, S, Cl • molecular/covalent bonding • gases, liquids, solids with low melting points • non-metal oxides react with water to produce acids P4O10(s) + 6H2O(l)  4H2PO4-(aq) + 4H+(aq)

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