1 / 13

Understanding Geometry and Polarity of Covalent Compounds Using VSEPR Model

This lesson focuses on using the VSEPR (Valence Shell Electron Pair Repulsion) Model to determine the shapes and hybridizations of covalent compounds. Students will work in groups to interpret the VSEPR Model, exploring how electron repulsion influences molecular geometry. They'll predict the polarity of compounds based on the distribution of electron pairs, guided by electronegativity. The hands-on activity involves drawing Lewis Dot Structures and determining molecular shapes for various compounds like H₂O, CO₂, and NO₃⁻.

selia
Télécharger la présentation

Understanding Geometry and Polarity of Covalent Compounds Using VSEPR Model

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. Objectives • I CAN determine the geometry and hybridizations of covalent compounds based on the VSEPR Model • I CAN predict the polarity of covalent compounds using the VSEPR MOdel

  2. Investigation • Work in groups of 3-4 • Complete worksheet and shapes. STOP after every shape • 1 minute per shape

  3. Key Point 1: What is the VSEPR Model? • The VSEPR (pronounced Vesper) Model is a model that tells us a molecule’s shape • The main rule of the VSEPR model is that electrons will repel each other (negative-negative) so they must be placed as far apart as possible

  4. KP2: How do we use the VSEPR Model? • In a covalent compound, each element has a number of bonding and nonbonding pairs of electronsaround the nucleus. • For example, in H2O, Oxygen has 2 bonding pairs and 2 nonbonding (lone) pairs

  5. Bonding and nonbonding pairs of electrons are also called steric groups • Oxygen has a total of 4 steric groups

  6. KP3: Once you know the number of steric groups, you can figure out the geometry of a compound by looking at the following chart:

  7. Example: List the possible • shapes for the compounds • below: • CO2 • NH3 • PCl3 • BeBr2

  8. KP4: What does the VSEPR Model tell us about polarity? • A molecule will have a DIPOLE when the electrons spend most of their time on one side • Electrons will always spend the most time with the element that is most electronegative (highest electron affinity) • Remember: electron affinity goes UP as we move across the periodic table

  9. Example 1: Let’s look at water. First, draw the bonds in H2O with Lewis Dot Structures.

  10. Example 1: Let’s look at water. First, draw the bonds in H2O with Lewis Dot Structures. Now, figure out what SHAPE H2O will be according to the VSEPR Model: Now, which element is more electronegative? Oxygen or hydrogen? _____________________________ So, the electrons will spend more time with the ___________________ atom, and the pole will look like this:

  11. Example 2: What about CO2? First, draw LDSs: What SHAPE will CO2 be according to the VSEPR Model: Now, which element is more electronegative? Carbon or Oxygen? _____________________________ Will this element have a dipole? ____________________

  12. Example 3--CHALLENGE: What about NO3-? First, draw LDSs What shape will NO3- be according to the VSEPR Model? Now, which element is more electronegative? Nitrogen or Oxygen? _____________________________ Will this element have a dipole? ____________________

More Related