[ostudent]

I understand that formal charge is a charge associated with an atom when it doesn't exhibit the expected # of valence e-.

However, how can you assume that the middle carbon isn't donating 2 of its valence electrons to the bond here rather than the oxygen having an extra electron?

The picture is incorrect, struggling with formatting. It should be just 'O' with a formal charge -1, not HO.


Very appreciative for feedback...

[ostudent]

Here, sorry, I found the way to upload the image.

[Babcock_Hall]

I understand that formal charge is a charge associated with an atom when it doesn't exhibit the expected # of valence e-.

I do not agree with your first sentence.  For example oxygen can have formal charges of -1, 0, and +1 in situations in which it has an octet of electrons.  It may help to think of formal charge as a bookkeeping device that assumes that electrons in a bond are shared equally.  It is not strictly true (we know that electrons are not shared exactly equally), but that does not matter as long as we apply this idea consistently.  I am not sure whether or not this answers your question.

[ostudent]

Thank you. Your redefining makes it much clearer.