Draw a Lewis structure for a resonance form of each ion with...

Draw a Lewis structure for a resonance form of each ion with the lowest possible formal charges, show the charges, and give oxidation numbers of the atoms:
(a) $\mathrm{BrO}_{3}^{-} ;$ (b) $\mathrm{SO}_{3}^{2-}$

Key Concepts

Resonance Structures

Resonance structures are multiple valid Lewis structures for a single molecule or ion that differ only in the positions of the electrons, not the positions of the atoms. They are used to represent the delocalization of electrons that cannot be adequately described by a single classical structure, thereby providing a more accurate depiction of the electron distribution within the species.

Oxidation Numbers

Oxidation numbers are theoretical charges assigned to atoms in a molecule or ion assuming that the bonding electrons are completely transferred to the more electronegative atom. They are useful for understanding electron distribution in compounds, balancing redox reactions, and providing insight into the oxidation state of an atom, which reflects its tendency to gain or lose electrons in chemical transformations.

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms of a molecule and the lone pairs of electrons that may exist. They are drawn by placing dots around element symbols to denote valence electrons and connecting atoms with lines to indicate bonds, thus offering a simplified visualization of how electrons are arranged within a molecule or ion.

Formal Charges

Formal charges are a bookkeeping tool used to estimate the charge distribution within a molecule or ion based on Lewis structures. By comparing the number of valence electrons in an isolated atom with the number of electrons assigned to it in the molecule (including half of the bonding electrons), formal charges help identify the most stable or favorable resonance structure, typically the one with the lowest formal charges on atoms.

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