1 / 40

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

aleron
Download Presentation

Na-Sodium

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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

More Related