When an atom loses a proton in an acid–base reaction, its formal charge is decreased by one. Thinking about the equation for calculating formal charge, explain this observation in your own words.

Verified step by step guidance

1. Identify the formula for calculating formal charge: \( \text{Formal Charge} = \text{Valence Electrons} - \text{Non-bonding Electrons} - \frac{1}{2} \times \text{Bonding Electrons} \).
2. Consider what happens when an atom loses a proton (H⁺) in an acid-base reaction. The proton is essentially a hydrogen ion without electrons.
3. When the proton is lost, the atom retains its electrons, specifically the bonding electrons that were shared with the hydrogen.
4. Since the atom retains the bonding electrons, the number of non-bonding electrons increases, while the number of bonding electrons effectively decreases.
5. According to the formal charge formula, an increase in non-bonding electrons or a decrease in bonding electrons results in a decrease in the formal charge by one unit.

Key Concepts

Formal Charge

Formal charge is a theoretical charge assigned to an atom in a molecule, calculated using the formula: Formal Charge = Valence Electrons - (Non-bonding Electrons + 1/2 Bonding Electrons). It helps in understanding the distribution of electrons in a molecule and predicting the stability of different resonance structures.

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In these reactions, acids donate protons while bases accept them. The loss of a proton by an atom during such a reaction directly affects its formal charge, as the atom's overall electron count changes, leading to a decrease in its positive charge.

Proton Loss and Charge Change

When an atom loses a proton, it effectively reduces its positive charge because protons are positively charged particles. This loss alters the balance of protons and electrons around the atom, resulting in a decrease in formal charge by one unit, which reflects a more stable electronic configuration.