Numerical VSEpr Theory

This video is a practical guide to applying the VSEPR (Valence Shell Electron Pair Repulsion) theory to predict the molecular geometry and bond angles of various compounds. The instructor explains the process by examining the electron configuration of the central atom, identifying the number of valence electrons, and accounting for both bonding and lone pairs. Examples Practiced: Carbon Tetrachloride (CCl4): Geometry: The central carbon atom has 4 bonding pairs and 0 lone pairs, resulting in a Tetrahedral shape (0:44 - 3:58). Bond Angle: Approximately 109.5 degrees. Phosphorus Trichloride (PCl3): Geometry: The central phosphorus atom has 3 bonding pairs and 1 lone pair, leading to a Trigonal Pyramidal shape (4:15 - 7:33). Bond Angle: Approximately 107 degrees. Hydrogen Sulfide (H2S): Geometry: The central sulfur atom has 2 bonding pairs and 2 lone pairs, resulting in a V-shape (bent geometry) (7:46 - 10:29). Bond Angle: Approximately 104 degrees. The instructor emphasizes that while all these molecules have four electron pairs around the central atom, the repulsion difference between lone pairs and bonding pairs is what fundamentally dictates the unique shape and bond angle for each molecule. Subscribe for more Videos ‪@CBA_Notebook‬ #cbanotebook #chemistry #chemicalbonding #VSPERtheory #bonding #h2s #pcl3