Why does the oxygen atom in H3O+ have a positive formal charge?

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SUMMARY

The discussion centers on the formal charge of the oxygen atom in the hydronium ion (H3O+) and its implications in acid-base chemistry. The oxygen atom in H3O+ carries a formal charge of +1 due to the presence of three hydrogen atoms, each contributing a +1 charge, while oxygen's typical valence is -2. This leads to the conclusion that acids dissociate in water to form H3O+ and OH-, and the Brønsted-Lowry theory defines acids as proton donors, not acceptors.

PREREQUISITES
  • Understanding of acid-base theories, specifically Brønsted-Lowry theory
  • Knowledge of formal charge calculations in molecular structures
  • Familiarity with the concept of electronegativity and its implications in chemical bonding
  • Basic principles of acid dissociation in aqueous solutions
NEXT STEPS
  • Research the Brønsted-Lowry theory of acids and bases
  • Study formal charge calculations in organic chemistry
  • Explore the concept of electronegativity and its role in molecular polarity
  • Investigate the process of acid dissociation in water and its effects on pH
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Chemistry students, educators, and professionals interested in acid-base reactions and molecular structure analysis.

semc
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Acid dissociates in water to form H3O+ and OH- but the formal charge on the oxygen atom in H3O+ is +1. Shouldn't the oxygen atom have a negative formal charge since it is more electronegative than hydrogen atom?
 
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semc said:
Acid dissociates in water to form H3O+ and OH- but the formal charge on the oxygen atom in H3O+ is +1. Shouldn't the oxygen atom have a negative formal charge since it is more electronegative than hydrogen atom?

Acids don't dissociate into H3O+ and OH-, formal charge of oxygen in H3O+ is not +1 - so I have no idea what you are asking about.

-2 + 3*(+1) = +1
 
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I meant to ask the acid dissociation in water into H+ and A-. So I wanted to ask why this is so. Why can't the acid accept the proton. Is this just because of the definition of acid?
 
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