Shapes of Molecules (VSEPR Theory)

Learn how to predict the shapes of molecules using the VSEPR (Valence Shell Electron Pair Repulsion) theory. In this video, we'll explore how the shape of simple molecules varies depending on the central atom's number of bonds and lone pairs of electrons. We'll cover key molecular shapes including linear, non-linear (bent), trigonal planar, trigonal pyramidal, tetrahedral, square planar, see-saw, and octahedral. Examples are given for all. Perfect for AQA, OCR (A), Edexcel, CIE, and IB Chemistry students, this guide will help you master molecular geometry for your exams! Recap: 00:26 Bond Angles: 01:19 Lone Pair Repulsion: 04:01 Shapes (VSEPR Theory): 05:31 CO2 - Carbon Dioxide EXAMPLE: 10:48 BF3 - Boron Trifluoride EXAMPLE: 11:11 H2O - Water EXAMPLE: 11:37 CH4 - Methane EXAMPLE: 12:21 NH3 - Ammonia EXAMPLE: 12:41 BF5 - Boron Pentafluoride EXAMPLE: 13:23 SF6 - Sulfur Hexafluoride EXAMPLE: 13:50 How shapes can change: 14:11 Summary: 15:01 Thank you for watching - if you found the video useful, please like and subscribe!