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This means that the atoms have a steric number equal to #2#, which implies that they are #"sp"# hybridized.Īccording to VSEPR Theory, this molecule falls into the #"AX"# category, i.e. In this case, one triple bond and one lone pair will amount to two regions of electron density. So, pick one of the two nitrogen atoms and count how many regions of electron density surround it - this is called the steric number. a single, double, or triple bond - they all count as one region of electron density.There are regions in molecules that have high. Polarity of molecule results from non-symmetrical sharing of valence electron, creating a region of unequal charges in molecule. Can be used as content for research and analysis. Remember, a region of electron density is Collected from the entire web and summarized to include only the most important parts of it. Now, molecular geometry is all about regions of electron density, that is, about how many regions of electron density surround a given atom. The remaining #4# valence electrons will be distributed as lone pairs, one of each nitrogen atom. This will account for #3 xx 2 = 6# of the molecule's #10# valence electrons. Therefore, you must draw a triple bond between the two nitrogen atoms. This tells you that in order for both nitrogen atoms to have a complete octet, each must share three electrons with the other. This means that the nitrogen molecule will have a total of #10# valence electrons, #5# from each of the two nitrogen atoms.Īnother important thing to realize about the fact that nitrogen has #5# valence electrons is that it needs #3# more to complete its octet. Nitrogen is located in period 2, group 15 of the periodic table, which tells you that it has #5# valence electrons.
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Start by calculating how many valence electrons you'd get for a molecule of nitrogen gas, #"N"_2#. In order to be able to determine the molecular geometry of a given compound, you need to first draw its Lewis structure.