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Review Drill & Tests

Drill: Calculate the volume of hydrogen gas produced at -23 o C under 83.1 kPa pressure when 5.1 g of ammonia is decomposed. Review Drill & Tests. CHM II HW. Review PP-15 Complete the attached assignment & turn it in tomorrow. Are there any questions on previous material?. Bonding.

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Review Drill & Tests

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  1. Drill: Calculate the volume of hydrogen gas produced at -23oC under 83.1 kPa pressure when 5.1 g of ammonia is decomposed.

  2. Review Drill & Tests

  3. CHM II HW Review PP-15 Complete the attached assignment & turn it in tomorrow

  4. Are there any questions on previous material?

  5. Bonding

  6. Types of Bonds • Ionic • Covalent • Metallic

  7. Metallic Bonds • Electrons are shared by many atoms • Electrons free to move • Two or more metals

  8. Metallic Compounds • Generally high MP • Hard & lustrous • Less brittle • Conductors

  9. Metallic Bonds • No debate about metallic bonds • Easy to identify • Will not be discussed

  10. Ionic Bonds • Electrons are transferred from one atom to another creating (+) & (-) ions • Metal & nonmetal

  11. Ionic Compounds • Held together by electrostatic charge • Very high MP • Brittle

  12. Covalent Bonds • Electrons are shared by two atoms • Two nonmetals • Weaker than ionic

  13. Covalent Compounds • Low MP • Two nonmetals • Flexible • Some exceptions

  14. Network Covalent or Macromolecules • VHMP • Extremely hard

  15. Molecule • Any compound that can exist as an entity by itself

  16. Distinguishing Bonds • Distinguishing ionic & covalent bonds can be difficult, but generally determined by differenceelectronegativity

  17. Bonds Types • Ionic • Polar covalent • Non polar covalent

  18. Bond Types • Ionic: DEN > 2.0 • Covalent: DEN < 2.0 • Polar Covalent: 0.5<DEN<2.0 • Non polar covalent :DEN< 0.5 • Nothing is absolute

  19. Coordinate Covalent Bonds • A covalent bond in which the two electrons are donated by one atom

  20. Coordinate Covalent Bond H3N: BF3 H3N-BF3 H3N BF3

  21. Classify Bonds • Na-F H-Cl • C-O Mg-O • Fe-Fe

  22. Dipole • Polar bonds • Polar molecules

  23. Dipole H F d+ d-

  24. Ionic Bonding - +

  25. Covalent Bonding Occurs when electron orbitals overlap

  26. Orbitals On the board Max 2 e- per orbital

  27. Hybridization • When s, p, and/or d orbitals (electron clouds) mix to make a new type of multi-lobed orbital

  28. Hybrid Orbitals • sp dsp3 • sp2 d2sp3 • sp3

  29. Electron Cloud Repulsion • In molecules each electron cloud repels other clouds enough to spread as far apart as possible

  30. VSEPR • Valence Shell Electron Pair Repulsion • Electron pairs repel each other to spread out as much as possible

  31. Bonding OrbitalsType HybridVSEPR • 2 lobes sp AX2 • 3 lobes sp2 AX3 • 4 lobes sp3 AX4 • 5 lobes dsp3 AX5 • 6 lobes d2sp3 AX6

  32. VSEPR Orbitals

  33. Bonding Orbital Shape • 2 lobes: Linear 180o • 3 lobes: Trigonal planar 120o • 4 lobes: Tetrahedral 109.5o • 5 lobes: Hexahedral 120&180o • 6 lobes: Octahedral 90&180o

  34. Drill: Calculate the density SO2 at 47oC under 83.1 kPa Pressure:

  35. Review & Collect Drill & HW

  36. CHM II HW Review PP-15 Complete the attached assignment & turn it in tomorrow

  37. Are there any questions on previous material?

  38. Draw the Bonding Electron Dot Diagrams for Each Element

  39. Bonding Electron Dot Diagrams • Electron dot diagrams that go through 4 singles before any electrons are paired up

  40. 1A: 1 single 2A: 2 singles3A: 3 singles4A: 4 singles 5A: 1 pair & 3 singles6A: 2 pair & 2 singles7A: 3 pair & 1 single8A: 4 pair

  41. Drill: Equate each of the following: sp3 AX2 2 lobes sp AX3 4 lobes dsp3 AX4 6 lobes sp2 AX5 3 lobes d2sp3 AX6 5 lobes

  42. Drill: Classify Each type of Bond:Na-Cl Al-ClC-F H-IFe-Cr P-O

  43. Review & Collect Drill & HW

  44. CHM II HW • Review PP-15 • Lab tomorrow • Lab 6 due tomorrow • Complete the attached assignment & turn it in on Monday

  45. Lewis Dot Diagrams • Representation of valence electrons and bonds in a molecule or polyatomic ion

  46. Drawing LDDs Draw the bonding electron dot diagram for each element in the molecule with the element with the most unpaired e- near the center

  47. Drawing LDDs • If there is more than one carbon, connect the carbons by connecting single dots between one carbon & another

  48. Drawing LDDs • Connect a single dot on one atom to a single dot on another (never two on the same atom)(never connect one dot to more than one other dot)

  49. Drawing LDDs • Repeat connecting the dots until all singled dots are connected making sure to obey the octet rule if possible

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