![]() ![]() The shape of the compound is bent due to the presence of lone pairs in oxygen. SO2 (sulfur dioxide) has the same lewis structure, same resonance structures, and again all of the atoms are sp2-hybridized with one delocalized electron pair, and it leads to the same geometry: trigonal planar (120 degrees) and bent (slightly less than 120 degrees). NO2 has Trigonal planner geometry with bent shape. Nitrogen Dioxide (NO2) is a covalent compound that is composed of a central nitrogen atom single bonded to an oxygen atom and a double bond with another oxygen atom. The major resonance structure has one double bond. N2O Preparation Methods There are several methods for making nitrous oxide. Did you get this If not, check your bonds. The valence electrons of N and O are five and six, respectively. A central atom is the one that forms the most number of bonds. The N2O molecular geometry is covalently bonded by nitrogen (N) and oxygen (O) atoms. ![]() Therefore the bond angle should be slightly less than 120 degrees. Our molecule NO2 contains two oxygen atoms and one nitrogen atom. All of the atoms are sp2-hybridized (+1 delocalized electron pair), which means the electron group geometry is trigonal planar (120 degrees in between bonds), and the molecular geometry is bent. Here's the way I approached it: After drawing the lewis structure of NO2- (nitrite), you can see that there are 2 resonance structures. In every way I look at it, both molecules have the same structure with the same bond angle. Which of these bonds has the biggest bond angle? Our chemistry teacher gave us a list of test questions to prepare ourselves for an upcoming exam, but I fail to find the answer to this one question.Įxplain the structure of NO2- and SO2- by using the VSEPR theory. ![]()
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