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Sulfur Dioxide, which is also know as Sulphur Dioxide, is entity of bond between sulfur and oxygen atoms. It is known as formula written as SO2. Here we will provide an explanation of SO2 molecular Geometry, SO2 Electron Geometry, SO2 bond angle, and SO2 Lewis Structure.
How to find SO 2 molecular geometry using VSEPR theory is not very difficult using these three steps. Step 1: Draw the Lewis structure for SO 2 using an easy method where you calculate the total valence of electrons in molecule to determine the Lewis structure. You can look at atoms like puzzle pieces where you are trying to fit together electrons SO that everyone that needs an octet has one. In this example, sulfur is the central atom. Oxygen atoms will come off each side of sulfur. For each oxygen to have octet, there must be double bonds between sulfur and oxygen atoms. Sulfur will have two double bonds and a lone pair, for a total of 18 electrons. Sulfur in this molecule is hypervalent. = Number of central atoms X = Number of surrounding atoms E = Number of lone pairs on the central atom based on the Lewis structure above AXE notation would be AX 2 E 1, meaning there are a total of three substituents coming off of the central atom. Step 3: Use VSEPR table to determine SO 2 electron geometry: three substituents are trigonal planar. While electron geometry is trigonal planar, SO 2 molecular geometry is bent. The bond angle for this molecule is 120 0.
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