H is 0
O is 0
F is +1
O is -1
Some things to remember about formal charges. +3 is MOST uncommon so do a reality check to make sure you did it right.
Second point. How did you come up with these numbers. Here is a site to help you with formal charges. Let me know if I can help. This site, I think, makes it far to complicated. I think there is an easier way to do it. But take a look at it, anyway. http://www.cartage.org.lb/en/themes/sciences/chemistry/Inorganicchemistry/Informationbonding/bondingindex/FormalCharge/FormalCharge.htm
Here is a site that I think is a little simpler at explaining formal charges.
hmmm, how is that possible? I calculated it to be 0, 0, 0, 0. Just to make sure, H is singly bonded to oxygen which is singly bonded to fluorine, which is double bonded to oxygen, right?
Hmm, can you explain?
FC = valence e - lone pair e- 1/2bonded e.
FC for hydrogen = 1-0-1 = 0
FC for oxygen = 6-4-2 = 0
FC for fluorine = 7-4-3=0
FC for oxygen = 6-4-2=0
NVM! I violated an octet rule! hah!. DrBob, you're rite
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