1. Quiz review Lewis Structures, VSEPR shape, polarity, and IMFs Get started!

2. Draw the Lewis Structure for…. Once you have drawn a Lewis Structure, click on the molecule to check your answer and complete the rest of the questions

3. What is its shape? tetrahedral angular linear

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5. Angular…Very good! What is the polarity? Polar Nonpolar

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7. Polar…Very good! What is its principal IMF? London Dispersion London Dispersion Dipole - Dipole Dipole - Dipole Hydrogen Bonding Hydrogen Bonding

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9. Dipole-Dipole…Very good! This molecule is angular because it has 4 e- pairs around the central atom, 2 atoms bonded to it, and 2 lone pairs. It is polar because it is angular with two lone pairs. Since it is polar, it will have a dipole-dipole IMF Back to Lewis Structures Back to Lewis Structures

10. What is its shape? Trigonal planar Trigonal planar Pyramidal Tetrahedral

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12. Trigonal Planar…Very good! What is the polarity? Polar Nonpolar

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14. Nonpolar…Very good! What is its principal IMF? London Dispersion London Dispersion Dipole - Dipole Dipole - Dipole Hydrogen Bonding Hydrogen Bonding

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16. London Dispersion…Very good! This molecule is trigonal planar because it has 3 e- pairs around the central atom, 3 atoms bonded to it, and 0 lone pairs. It is nonpolar and therefore will experience london dispersion intermolecular forces. Back to Lewis Structures Back to Lewis Structures

17. What is its shape? tetrahedral octahedral pyramidal

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19. Octahedral…Very good! What is the polarity? Polar Nonpolar

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21. Nonpolar…Very good! What is its principal IMF? London Dispersion London Dispersion Dipole - Dipole Dipole - Dipole Hydrogen Bonding Hydrogen Bonding

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23. London Dispersion…Very good! This molecule is octahedral because it has 6 e- pairs around the central atom, 6 atoms bonded to it, and 0 lone pairs. It is nonpolar so it will experience london dispersion intermolecular forces. Back to Lewis Structures Back to Lewis Structures

24. What is its shape? tetrahedral angular square planar

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26. Tetrahedral…Very good! What is the polarity? Polar Nonpolar

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28. Nonpolar…Very good! What is its principal IMF? London Dispersion London Dispersion Dipole - Dipole Dipole - Dipole Hydrogen Bonding Hydrogen Bonding

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30. London Dispersion…Very good! This molecule is angular because it has 4 e- pairs around the central atom, 4 atoms bonded to it, and 0 lone pairs. Since it is nonpolar it will experience london dispersion intermolecular forces. Back to Lewis Structures Back to Lewis Structures

31. What is its shape? tetrahedral pyramidal see saw

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33. See Saw…Very good! What is the polarity? Polar Nonpolar

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35. Polar…Very good! What is its principal IMF? London Dispersion London Dispersion Dipole - Dipole Dipole - Dipole Hydrogen Bonding Hydrogen Bonding

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37. Dipole-Dipole…Very good! This molecule is see saw shape because it has 5 e- pairs around the central atom, 4 atoms bonded to it, and 1 lone pairs. It is polar because it has one lone pair which will distort the shape. Since it is polar, it will have a dipole- dipole IMF Back to Lewis Structures Back to Lewis Structures

38. What is its shape? tetrahedral trigonal planar pyramidal

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40. Trigonal planar…Very good! What is the polarity? Polar Nonpolar

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42. Nonpolar…Very good! What is its principal IMF? London Dispersion London Dispersion Dipole - Dipole Dipole - Dipole Hydrogen Bonding Hydrogen Bonding

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44. London Dispersion…Very good! This molecule is trigonal planar because it has 4 e- pairs around the central atom, 3 atoms bonded to it, and 0 lone pairs. It is polar because it is angular with two lone pairs. Since it is polar, it will have a dipole-dipole IMF Back to Lewis Structures Back to Lewis Structures **It is also ok to determine shape by saying 3 electron regions, 3 atoms bonded to it, and 0 lone pairs. You get the same answer

45. What is its shape? Square planar Pyramidal Octahedral

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47. Square Planar…Very good! What is the polarity? Polar Nonpolar

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49. Nonpolar…Very good! What is its principal IMF? London Dispersion London Dispersion Dipole - Dipole Dipole - Dipole Hydrogen Bonding Hydrogen Bonding

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51. London Dispersion…Very good! This molecule is square planar because it has 6 e- pairs around the central atom, 4 atoms bonded to it, and 2 lone pairs. Although it has lone pairs, it is nonpolar because it is one of the exceptions. The fluorines cancel each other out, as do the lone pair in this specific shape. Since it is nonpolar it experiences london dispersion intermolecular forces. Back to Lewis Structures Back to Lewis Structures

52. What is its shape? see saw angular linear

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54. Linear…Very good! What is the polarity? Polar Nonpolar

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56. Nonpolar…Very good! What is its principal IMF? London Dispersion London Dispersion Dipole - Dipole Dipole - Dipole Hydrogen Bonding Hydrogen Bonding

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58. London Dispersion…Very good! This molecule is linear because it has 5 e- pairs around the central atom, 2 atoms bonded to it, and 3 lone pairs. Although it has lone pairs, this is one of the exceptions and is nonpolar since the lone pairs are on the same plane and cancel each other out. Since is it nonpolar, it will experience london dispersion intermolecular forces. Back to Lewis Structures Back to Lewis Structures

59. What is its shape? angular trigonal planar linear

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61. Angular…Very good! What is the polarity? Polar Nonpolar

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63. Polar…Very good! What is its principal IMF? London Dispersion London Dispersion Dipole - Dipole Dipole - Dipole Hydrogen Bonding Hydrogen Bonding

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65. Dipole-Dipole…Very good! This molecule is angular because it has 4 e- pairs around the central atom, 2 atoms bonded to it, and 1 lone pair. It is polar because it is angular with a lone pair. Since it is polar, it will have a dipole-dipole IMF Back to Lewis Structures Back to Lewis Structures

66. Remember for any acid with an oxygen (starts with H and has an O), the hydrogen is bonded to one of the oxygen atoms What is its shape? tetrahedral angular trigonal planar

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68. Trigonal planar…Very good! What is the polarity? Polar Nonpolar

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70. Polar…Very good! What is its principal IMF? London Dispersion London Dispersion Dipole - Dipole Dipole - Dipole Hydrogen Bonding Hydrogen Bonding

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72. Hydrogen bonding…Very good! This molecule is trigonal planar because it has 4 e- pairs around the central atom, 3 atoms bonded to it, and 0 lone pairs. It is polar because all of the electrons around the central atom are not pulled equally because of the -OH group. Since it is polar and there is an oxygen atom covalently bonded to a hydrogen atom, this molecule will experience hydrogen bonding Back to Lewis Structures Back to Lewis Structures **It is also ok to determine shape by saying 3 electron regions, 3 atoms bonded to it, and 0 lone pairs. You get the same answer