1 / 53

Chemical Bonding

Chemical Bonding. Shape Lab. 1) One structural isomer only. i) water, H 2 O . shape: angular. END = O – H = 3.5 – 2.1 = 1.4 polar covalent bond bond dipoles exist, molecule is asymmetrical dipoles do not cancel molecule is polar. ii) methane, CH 4. Shape: Tetrahedral

callum-brooks
Download Presentation

Chemical Bonding

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. Chemical Bonding Shape Lab

  2. 1) One structural isomer only

  3. i) water, H2O • shape: angular

  4. END = O – H = 3.5 – 2.1 = 1.4 • polar covalent bond • bond dipoles exist, • molecule is asymmetrical • dipoles do not cancel • molecule is polar

  5. ii) methane, CH4

  6. Shape: Tetrahedral • END = C – H = 2.5 – 2.1 = 0.4 • polar covalent bond • bond dipoles exist, • molecule is symmetrical • the forces cancel • molecule is non-polar

  7. iii) methanol, CH3OH

  8. Shape: Tetrahedral about C Angular about O • END = C – H = 2.5 – 2.1 = 0.4 • END = C – O = 2.5 – 3.5 = 1.0 • END = O – H = 3.5 – 2.1 = 1.4 • all bonds are polar covalent • bond dipoles exist • molecule is not symmetrical because different atoms are bonded to the C and the O is angular • the forces do not cancel • molecule is polar

  9. iv) carbon tetrachloride, CCl4

  10. Shape: Tetrahedral • END = C – Cl = 2.5 – 3.0 = 0.5 • polar covalent bond • bond dipoles exist • molecule is symmetrical • the forces cancel • molecule is non-polar

  11. v) ammonia, NH3

  12. Shape: Trigonal pyramidal • END = N - H = 3.0 – 2.1 = 0.9 • polar covalent bond • bond dipoles exist, • molecule is asymmetrical • dipoles do not cancel • molecule is polar

  13. vi) hydrazine, N2H4

  14. Shape: Trigonal pyramidal about each N • END = N - H = 3.0 – 2.1 = 0.9 • END = N – N = 3.0 – 3.0 = 0.0 • N – H is polar covalent bond • N – N is covalent bond • bond dipoles exist, • molecule is asymmetrical • dipoles do not cancel • molecule is polar

  15. vii) hydrogen sulfide, H2S

  16. Shape: Angular • END = S – H = 2.5 – 2.1 = 0.4 • polar covalent bond • bond dipoles exist, • molecule is asymmetrical • dipoles do not cancel • molecule is polar

  17. viii) nitrogen triiodide, NI3

  18. Shape: Trigonal pyramidal • END = N - I = 3.0 – 2.5 = 0.4 • polar covalent bond • bond dipoles exist, • molecule is asymmetrical • dipoles do not cancel • molecule is polar

  19. ix) hydrogen peroxide, H2O2

  20. Shape: Angular about each O • END = O – H = 3.5 – 2.1 = 1.4 • polar covalent bond • bond dipoles exist, • molecule is asymmetrical • dipoles do not cancel • molecule is polar

  21. x) chlorine, Cl2

  22. Shape: only 2 atoms (linear) END: Cl – Cl = 3.0 – 3.0 = 0.0 covalent bond no bond dipoles exist, so molecule is non-polar

  23. 2) Double and triple bonds (use the springs)

  24. i) carbon dioxide, CO2

  25. Shape: Linear (bonded to 2 atoms with no lone pairs) • END = C – O = 2.5 – 3.5 = 1.0 • END = C – C = 2.5 – 2.5 = 0.0 • C – O is polar covalent bond • bond dipoles exist • molecule is symmetrical • the forces cancel • molecule is non-polar

  26. ii) nitrogen, N2

  27. Shape: only 2 atoms (linear) • END: N – N = 3.0 – 3.0 = 0.0 • covalent bond • no bond dipoles exist • molecule is non-polar

  28. iii) oxygen, O2

  29. Shape: only 2 atoms • END: O – O = 3.5 – 3.5 = 0.0 • covalent bond • no bond dipoles exist • molecule is non-polar

  30. iv) ethyne, C2H2

  31. Shape: Linear (each C bonded to 2 atoms with no lone pairs) • END = C – H = 2.5 – 2.1 = 0.4 • END = C – C = 2.5 – 2.5 = 0.0 • C – H is polar covalent bond, • C - C is covalent • bond dipoles exist • molecule is symmetrical • the forces cancel • molecule is non-polar

  32. v) hydrogen cyanide, HCN

  33. Shape: Linear (C bonded to 2 atoms with no lone pairs) • END = C – H = 2.5 – 2.1 = 0.4 • END = C – N = 2.5 – 3.0 = 0.5 • both are polar covalent bonds • bond dipoles exist • molecule is symmetrical but the C is bonded to 2 different atoms • the forces do not cancel • molecule is polar

  34. vi) carbon disulfide, CS2

  35. Shape: Linear (bonded to 2 atoms with no lone pairs) • END = C – S = 2.5 – 2.5 = 0.0 • END = C – C = 2.5 – 2.5 = 0.0 • both are covalent bonds • no bond dipoles exist • molecule is non-polar

  36. vii) methanal, CH2O

  37. Shape: Trigonal planar (bonded to 3 atoms with no lone pairs) • END = C – O = 2.5 – 3.5 = 1.0 • END = C – H = 2.5 – 2.1 = 0.4 • both are polar covalent bonds • bond dipoles exist • molecule is symmetrical but the C is bonded to 2 different atoms • the forces do not cancel • molecule is polar

  38. viii) ethene, C2H4

  39. Shape: Planar trigonal (each C bonded to 3 atoms with no lone pairs) • END = C – H = 2.5 – 2.1 = 0.4 • END = C – C = 2.5 – 2.5 = 0.0 • C – H is polar covalent bond • bond dipoles exist • molecule is symmetrical • the forces cancel • molecule is non-polar

  40. 3) Special Compounds

  41. i) beryllium hydride, BeH2

  42. Shape: Linear END: Be – H = 1.5 – 2.1 = 0.6 polar covalent bond bond dipoles exist molecule is symmetrical the forces cancel molecule is non-polar

  43. ii) boron trichloride, BCl3

  44. Shape: Planar trigonal • END: B – Cl = 2.0 – 3.0 = 1.0 • polar covalent bond • bond dipoles exist • molecule is symmetrical • the forces cancel • molecule is non-polar

  45. iii) phosphorus pentabromide, PBr5

  46. Shape: Trigonal bipyramidal • END: P – Br = 2.1 – 2.8 = 0.7 • polar covalent bond • bond dipoles exist • molecule is symmetrical • the forces cancel • molecule is non-polar

  47. iv) sulfur hexachloride, SCl6

  48. Shape: Octahedral • END: S – Cl = 2.5 – 3.0 = 0.5 • polar covalent bond • bond dipoles exist • molecule is symmetrical • the forces cancel • molecule is non-polar

  49. v) cyclohexane, C6H12

More Related