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Na-Sodium

Na-Sodium. Na2O- Sodium Oxide and NaCl - Sodium Chloride At standard condition- Solid Bonding and Structure: Ionic lattice Electrical Conductivity: Good conductor of electricity in molten state. Magnesium Oxide. 2Mg + O₂  2MgO Heating Magnesium in air

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Na-Sodium

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  1. Na-Sodium • Na2O- Sodium Oxide and NaCl- Sodium Chloride • At standard condition- Solid • Bonding and Structure: Ionic lattice • Electrical Conductivity: Good conductor of electricity in molten state.

  2. Magnesium Oxide • 2Mg + O₂  2MgO • Heating Magnesium in air • Physical State = Solid white powder • Forms giant ionic lattice and strong ionic bonds hold the ions together • Conducts electricity when molten • However, melting point is very high (2850°C)

  3. Magnesium Chloride • Mg + Cl₂  MgCl₂ • Physical State = Solid • Held together in a giant ionic lattice with strong ionic bonds • Conducts electricity • Ions dissociate when in molten state • Melting point is 714°C

  4. Oxides and Chlorides of Aluminum

  5. Aluminium Oxide (Al₂O₃) Physical Properties: • Solid under standard conditions, with metallic properties • Has strong bonds, ionic bonding (ionic lattice) • However, it is more covalent than usual. (All bonds are covalent to a degree) • NOTE: Aluminium Oxide is amphoteric!

  6. Electrical Conductivity: • When melted, it is a good conductor • Ionic lattice breaks, ions become free flowing • Has free moving charged particles, conducts easily Ions are held together tightly when in an ionic lattice.

  7. Aluminium Chloride (Al₂Cl₆) Physical Properties: • Physical property changes depending on the type of bonding • Can either be bonded through an ionic lattice, or a covalent bond • Empirical formula (AlCl₃), ionic lattice (has a lot of covalent properties though), is a solid • Aluminium and Chlorine do not have a strong bond • Al₂Cl₆, covalent bond (partly due to polarization). • Sublimes from AlCl₃ to Al₂Cl₆ at 180°C (gas), turns to liquid at 190°C and 2 atmospheric pressure.

  8. Electrical Conductivity: • Electrical conductivity is poor (Al₂Cl₆) • Some electrical conductivity since there is still some ionic bonding left.

  9. Silicon By TheOnlyFrankie

  10. Silicon Oxide(Dioxide)

  11. SiO2 (silicon dioxide)

  12. HIGH M.P and B.P • 16100c • 22300c

  13. Conductivity

  14. Reaction with Water?

  15. Silicon Chloride (Tetrachloride)

  16. SiCl4

  17. M.P and B.P • -70 • 58

  18. Conductivity

  19. Why Liquid? • Intermolecular (van der Waals) forces only

  20. SiCl4+2H2O ---> SiO2+4HCI • Acidic • React wildly with water (therefore It fumes with moist air) • Product -Hydrogen Chloride

  21. Phosphorus!!

  22. Oxides • P4O6 ( Tetraphosphorushexaoxide) • P4O10 (TetraphosphorusDecaoxide)

  23. P4O6 • Crystalline Solid • One Phosphorus atom bonds with 3 oxygen atoms. • Boiling Point: 173°c • Cant conduct electricity

  24. P4O10 • Crystalline Solid • One atom of phosphorus bonds with 3 oxygen atom • Boiling Point: 605°c • Cant conduct electricity

  25. Chlorides • PCl3 (Phosphorus Trichloride) • PCl5 ( Phosphorus Pentachloride)

  26. PCL3 • Liquid • It has weak Van der Waal force • One atom of phosphorus bonds with 3 chloride atoms • Cant conduct electricity ( covalent bond)

  27. PCl5 • Crystalline Solid • Cannot conduct electricity

  28. Sulfur

  29. Oxides (SO2, SO3) • covalent small gaseous molecules • Physical state is gaseous because covalent bonding has weak intermolecular forces between the molecules. • Sulfur dioxide does not conduct electricity because covalent bonding has no charges to produce current.

  30. Chlorides (S2Cl2) • covalent small liquid molecules • Physical state is liquid because covalent bonding has weak intermolecular forces between the molecules. • Sulfur chloride does not conduct electricity because covalent bonding has no charges to produce current.

  31. Chlorine properties • Oxide: • Creates Cl20, ClO2, Cl2O6, Cl207 • Creates covalent bonds • Electronegativity difference between chlorine and oxygen is 0.28 • Chloride: • Only forms Cl2

  32. Properties of oxides: Bonding • Covalent bonds are form as the electronegativity difference is small so it is not polar so there are weak inter molecular forces Cl O Electronegativity: 3.44 Electronegativity: 3.16

  33. Properties of oxides: Physical states • Cl20 and Cl02 are gases as they have weak intermolecular forces and have a low atomic mass • Cl206 and Cl2O7 are liquids as they have covalent bonds and have a higher atomic mass

  34. Properties of oxides: electrical conductivity and acidity • In the liquid state they are not electrically conductive as they do not have freely moving ions. • Chlorine forms an acid when it reacts with water. Cl207+H2O2HClO4

  35. Properties of chlorine • Chlorine bonds with itself to form Cl2 • It has covalent bonds as the electronegativity difference is 0 Cl Cl Electronegativity: 3.16 Electronegativity: 3.16

  36. Bonding change across period 3 • Group 1 to 3 are ionic bonding • Group 4 to 7 are covalent bonding • Group 4 is giant structure • Group 5 to 7 are small molecules

  37. Physical states across period 3 • Group 1 to 5 are solid • Group 6 is gaseous • Group 7 is gas/liquid

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