Write the Lewis structure for each molecule (octet rule not followed). b. NO₂

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent valence electrons and lines to indicate bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting reactivity.

The octet rule is a chemical rule of thumb that states atoms tend to bond in such a way that they each have eight electrons in their valence shell, achieving a stable electron configuration similar to that of noble gases. However, some molecules, like NO2, do not follow this rule, leading to exceptions that require careful consideration of electron distribution and formal charges.

Formal charge is a concept used to determine the distribution of electrons in a molecule and assess the stability of a Lewis structure. It is calculated by taking the number of valence electrons of an atom, subtracting the number of non-bonding electrons, and half the number of bonding electrons. A lower formal charge on atoms generally indicates a more stable structure, especially in cases where the octet rule is not followed.