A hydroxide ion, OH^-, results when a proton is removed from a H2 O molecule. The ion that resul

step 1 Let's draw the Lewis structure of the hypo peroxide ion, which is the H .O .2 minus ion, having

A hydroxide ion, OH^-, results when a proton is removed from...

A hydroxide ion, $\mathrm{OH}^{-}$, results when a proton is removed from a $\mathrm{H}_{2} \mathrm{O}$ molecule. The ion that results when a proton is removed from a $\mathrm{H}_{2} \mathrm{O}_{2}$ molecule is called a hydroperoxide ion, $\mathrm{HO}_{2}^{-}$. Write the Lewis formula for a hydroperoxide ion. Name the following ionic compounds: $\mathrm{NaHO}_{2}$ and $\mathrm{Ba}\left(\mathrm{HO}_{2}\right)_{2}$.

Key Concepts

Ionic Compound Nomenclature

Ionic compound nomenclature involves naming compounds based on the constituent cations and anions such that the overall charge of the compound is neutral. This system relies on a clear understanding of ion charges and common naming conventions, ensuring that compounds like sodium hydroperoxide and barium hydroperoxide are correctly identified and communicated in a standardized manner.

Polyatomic Ions

Polyatomic ions are ions that consist of two or more atoms covalently bonded together, carrying an overall positive or negative charge. Understanding these ions, including their structure and resonance stabilization, is important for interpreting the chemical behavior and nomenclature of compounds in which they are present.

Deprotonation and Acid-Base Reactions

Deprotonation is the process in which a proton (H+) is removed from a molecule, typically resulting in the formation of a negatively charged ion. This concept is fundamental in acid-base chemistry as it explains the formation of conjugate bases from acids, such as the transformation of water to hydroxide ion or hydrogen peroxide to hydroperoxide ion.

Lewis Structures

Lewis structures are diagrams that depict the bonding between atoms of a molecule and highlight the presence of lone pairs of electrons. They are used to illustrate the connectivity of atoms, the arrangement of shared electrons (bonds), and the distribution of unshared electrons, which is crucial for understanding molecular geometry, reactivity, and formal charge calculations.

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