AP Chemistry - Electronegativity, Electron and Molecular geometry, hybridization, sigma/pi bonds

18 flashcards · Other · by luckydog789 (harrison holbrook)

1. Electron Geometry: Linear Molecular Geometry: Linear Bond Angle(s): 180 Polarity (if all bonds are polar): Non-polar Hybridization: sp

   2 Bonding, 0 Non-bonding

2. Electron Geometry: Trigonal Planar Molecular Geometry: Bent Bond Angle(s): <120 Polarity (if all bonds are polar): Polar Hybridization: sp2

   2 Bonding, 1 Non-bonding

3. Electron Geometry: Trigonal Planar Molecular Geometry: Trigonal Planar Bond Angle(s): 120 Polarity (if all bonds are polar): Non-polar Hybridization: sp2

   3 Bonding, 0 Non-bonding

4. Electron Geometry: Tetrahedral Molecular Geometry: Bent Bond Angle(s): <109.5 Polarity (if all bonds are polar): Polar Hybridization: sp3

   2 Bonding, 2 Non-bonding

5. Electron Geometry: Tetrahedral Molecular Geometry: Trigonal Pyramidal Bond Angle(s): <109.5 Polarity (if all bonds are polar): Polar Hybridization: sp3

   3 Bonding, 1 Non-bonding

6. Electron Geometry: Tetrahedral Molecular Geometry: Tetrahedral Bond Angle(s): 109.5 Polarity (if all bonds are polar): Non-polar Hybridization: sp3

   4 Bonding, 0 Non-bonding

7. Electron Geometry: Trigonal Bipyramidal Molecular Geometry: Linear Bond Angle(s): 180 Polarity (if all bonds are polar): Non-polar Hybridization: sp3d

   2 Bonding, 3 Non-bonding

8. Electron Geometry: Trigonal Bipyramidal Molecular Geometry: T-Shaped Bond Angle(s): 90,180 Polarity (if all bonds are polar): Polar Hybridization: sp3d

   3 Bonding, 2 Non-bonding

9. Electron Geometry: Trigonal Bipyramidal Molecular Geometry: Saw horse Bond Angle(s): 90,120,180 Polarity (if all bonds are polar): Polar Hybridization: sp3d

   4 Bonding, 1 Non-bonding

10. Electron Geometry: Trigonal Bipyramidal Molecular Geometry: Trigonal Bipyramidal Bond Angle(s): 90,120,180 Polarity (if all bonds are polar): Non-polar Hybridization: sp3d

    5 Bonding, 0 Non-bonding

11. Electron Geometry: Octahedral Molecular Geometry: Square Planar Bond Angle(s): 90,180 Polarity (if all bonds are polar): Non-polar Hybridization: sp3d2

    4 Bonding, 2 Non-bonding

12. Electron Geometry: Octahedral Molecular Geometry: Square Pyramidal Bond Angle(s): 90,180 Polarity (if all bonds are polar): Polar Hybridization: sp3d2

    5 Bonding, 1 Non-bonding

13. Electron Geometry: Octahedral Molecular Geometry: Octahedral Bond Angle(s): 90,180 Polarity (if all bonds are polar): Non-polar Hybridization: sp3d2

    6 Bonding, 0 Non-bonding

14. Non-polar covalent electronegativity difference: 0

15. Polar covalent electronegativity difference: 0<x<1.7

16. Ionic electronegativity difference: >1.7

17. To find hybridization, count the number of electron domains on the central atom, then use that number to find hybridization. Ex: 1 →\to→ s 2 →\to→ sp 3 →\to→ sp2 4 →\to→ sp3 5 →\to→ sp3d 6 →\to→ sp3d2 Etc...

18. Sigma/Pi Bonds Single bond = 1 sigma bond 0 pi bond Double bond = 1 sigma bond 1 pi bond Triple bond = 1 sigma bond 2 pi bond ...