1 / 20

VSEPR Theory: Molecular Shapes & Polarity

Learn about Valence Shell Electron Pair Repulsion (VSEPR) theory to understand how molecular shapes are determined based on electron pair repulsion. Explore examples of linear, bent, trigonal, pyramidal, and tetrahedral shapes, and differentiate between polar and non-polar molecules. Discover how to draw electron dot diagrams and build molecular models.

jaredlucas
Download Presentation

VSEPR Theory: Molecular Shapes & Polarity

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. Molecular Shapes

  2. What is VSEPR?

  3. VSEPR • Valence Shell Electron Pair Repulsion • The main idea is that electrons don’t like to hang around near each other because they repel each other. As a result, the atoms in a molecule tend to separate as far as they can because their bonds repel each other.

  4. Shapes Linear Lone pairs : 0 A Lone Pair is a pair of electrons that are not involved with bonding

  5. Shapes Bent Lone pairs : 2

  6. Shapes Trigonal Planar Lone pairs : 0 This shape is typically formed with Boron. Boron is an exception to the octet rule and can be happy with only 6 valence electrons.

  7. Shapes Trigonal Pyrimidal Lone pairs : 1

  8. Shapes Tetrahedral Lone pairs : 0

  9. Recap • Linear = 0 lone pairs • Bent = 2 lone pairs • Trigonal Planar = 0 lone pairs • Trigonal Pyramidal = 1 lone pair • Tetrahedral = 0 lone pairs

  10. Polar covalent molecules: A type of bond that forms when electrons are not shared equally (nonsymmetrical) • Non polar molecules: A type of bond that forms when electrons are shared equally (symmetrical)

  11. Polarity • Go back to page 6 and for each shape, include the following examples of when the shape is polar and non polar.

  12. Shapes Linear can be Non-Polar OR Polar depending on if the outside atoms are similar or different. Linear Nonsymmetrical Polar Symmetrical Non-Polar

  13. Shapes Bent This molecule is NOT symmetrical horizontally. Always Nonsymmetrical Polar

  14. Shapes Trigonal Planar can be Non-Polar OR Polar depending on if the outside atoms are similar or different. Trigonal Planar Nonsymmetrical Polar Symmetrical Non-Polar

  15. Shapes This molecule is NOT symmetrical horizontally. Trigonal Pyrimidal Lone pairs : 1 Always Nonsymmetrical Polar

  16. Shapes Tetrahedral can be Non-Polar OR Polar depending on if the outside atoms are similar or different. Tetrahedral Nonsymmetrical Polar Symmetrical Non-Polar

  17. Molecular Model Lab

  18. Molecular Model Lab • On the next page in the Unit 6 Packet. • You will draw electron dot diagrams, and then build the molecules using the plastic models. • All of the holes need to be filled. • Use the longer “bendy” ones to make double bonds. • Each kit should have the exact number of atoms in order to make all of the molecules without having to take any apart. • Next Slide has the Color Key

  19. Color Codes • White = hydrogen • Red = oxygen • Black = carbon • Blue = nitrogen • Green = chlorine

  20. When you finish… In the space below the chart, draw these and determine the shape and polarity of these molecules without building them. • BF3 • CF4 • N2 • H2S • CS2 • C2H2

More Related