Draw Lewis structures for the following. Show all resonance...

Draw Lewis structures for the following. Show all resonance structures, where applicable. Carbon is the central atom in $\mathrm{OCN}^{-}$ and $\mathrm{SCN}^{-}$ a. $\mathrm{NO}_{2}^{-}, \mathrm{NO}_{3}^{-}, \mathrm{N}_{2} \mathrm{O}_{4}\left(\mathrm{N}_{2} \mathrm{O}_{4} \text { exists as } \mathrm{O}_{2} \mathrm{N}-\mathrm{NO}_{2} .\right)$ b. $\mathrm{OCN}^{-}, \mathrm{SCN}^{-}, \mathrm{N}_{3}^{-}$

Draw Lewis structures for the following. Show all resonance structures, where applicable. Carbon is the central atom in $\mathrm{OCN}^{-}$ and $\mathrm{SCN}^{-}$
a. $\mathrm{NO}_{2}^{-}, \mathrm{NO}_{3}^{-}, \mathrm{N}_{2} \mathrm{O}_{4}\left(\mathrm{N}_{2} \mathrm{O}_{4} \text { exists as } \mathrm{O}_{2} \mathrm{N}-\mathrm{NO}_{2} .\right)$
b. $\mathrm{OCN}^{-}, \mathrm{SCN}^{-}, \mathrm{N}_{3}^{-}$

Key Concepts

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 help in visualizing how electrons are arranged around atoms to form chemical bonds, and are fundamental tools in predicting molecule geometry, reactivity, and properties.

Resonance Structures

Resonance structures are multiple valid Lewis structures for a molecule that cannot be adequately represented by a single structure. They illustrate the delocalization of electrons within the molecule, showing how electron density is distributed in various ways among atoms, which contributes to the overall stability of the structure.

Octet Rule

The octet rule is a chemical rule of thumb that atoms tend to form structures in which they are surrounded by eight electrons, achieving a noble gas configuration. It is a guiding principle when constructing Lewis structures, although exceptions exist for elements that can have an expanded valence shell or for electron-deficient species.

Formal Charge

Formal charge is a bookkeeping tool used in evaluating and comparing different Lewis structure possibilities. It is calculated by assuming equal sharing of electrons in bonds, and the structure that minimizes formal charges and concentrates negative charges on more electronegative atoms is generally considered more stable.

Electron Counting

Electron counting involves adding up the total number of valence electrons from all atoms in the molecule, as well as any additional electrons due to an overall negative charge (or subtracting for a positive charge). Accurate electron counting is essential for drawing correct Lewis structures and ensuring that all electrons are accounted for in the bonding and lone pairs.

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