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Can someone explain why the electron geometry for the ONF is trigonal planar and not linear? There are two bonding regions in the Lewis structure and according to the lecture, two bonding regions will create a linear structure.
You must remember to take into account the area of electron density present due to the lone pair of nitrogen. Nitrogen has 5 valence electrons. It uses 1 to make a covalent bond with fluorine and 2 to make a covalent bond with oxygen. After using 3, it has 2 remaining. These two create a trigonal planar structure of electron density for the molecule. The shape itself, however, is bent.
When predicting molecular shape we have to take into account the number of electron densities that the molecule has. Nitrogen is the central atom and it bonds to oxygen with a double bond and fluorine with a single bond. Since that only give nitrogen 6 shared electrons, nitrogen also has a lone pair of electrons. This creates 3 electron densities, thus leading to the trigonal planar shape of the molecule. But when naming molecular shapes we only take into account the atoms present so since the long electron pair is not an atom we disregard it when naming, therefore the shape of ONF is bent.
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