Write the Lewis structure for each molecule or ion. c. BrO^-

Verified step by step guidance

1. Determine the total number of valence electrons in the molecule or ion. Bromine (Br) has 7 valence electrons, and oxygen (O) has 6 valence electrons. Since the ion has a negative charge, add 1 more electron.
2. Add up the valence electrons: 7 (Br) + 6 (O) + 1 (extra electron for the negative charge) = 14 valence electrons.
3. Place the least electronegative atom in the center. In this case, bromine (Br) is less electronegative than oxygen (O), so Br will be the central atom.
4. Connect the oxygen atom to the bromine atom with a single bond. This uses 2 of the 14 valence electrons, leaving 12 electrons to distribute.
5. Distribute the remaining electrons to satisfy the octet rule, starting with the outer atom (oxygen) and then the central atom (bromine). If necessary, form double bonds to ensure each atom has a complete octet.

Key Concepts

Lewis Structures

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 represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting reactivity.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in determining how atoms bond with each other. The number of valence electrons influences the molecule's structure and stability. For example, in the bromate ion (BrO^-), the total count of valence electrons must be calculated to accurately depict its Lewis structure.

Formal Charge

Formal charge is a concept used to determine the charge distribution within a molecule or ion. It is calculated based on the number of valence electrons an atom has, the number of electrons it owns in the structure, and the number of bonds it forms. Minimizing formal charges in a Lewis structure often leads to a more stable representation of the molecule.