Why does oxygen carry the positive F.C in [CH3OH2]+?

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The discussion centers on determining the Lewis structure for [CH3OH2]+, where oxygen carries a positive formal charge despite its higher electronegativity compared to carbon. The participant notes that their initial assumption was for carbon to have an incomplete octet and thus the positive charge, but this was not feasible. They highlight the electronegativity difference between carbon and oxygen, which is 0.9, indicating a polar covalent bond. The conversation also touches on the conventional rule that the most electronegative atom should bear the negative formal charge. Ultimately, the focus is on understanding the formal charge distribution in the molecule.
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Homework Statement


Find the lewis structure for [CH3OH2]+

Homework Equations


n/a

The Attempt at a Solution


I found the lewis structure to have a positive formal charge on the oxygen. I'm not sure why the oxygen would have the + f.c. since it is much more electronegative than fairly neutral carbon. I initially wanted carbon to have an incomplete octet, so it would carry the + charge, but that did not work.
 
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I just looked up the electronegativity difference (Pauling scale) for Carbon and oxygen=0.9

So... this would be a polar covalent bond.

However, basic lewis structure rules say that the most electronegative atom should carry the negative formal charge. Right?
 
Start with CH3OH, then look for a lone pair which can hold H+.
 

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