The Lewis structures for perchlorate, sulfurous acid, and hydronium ion can be represented as follows:
1. Perchlorate ( ClO4^-)
The Lewis structure for perchlorate features a chlorine atom centrally located and bonded to four oxygen atoms. One of these bonds is a double bond with one oxygen, while the others are single bonds. Additionally, perchlorate carries a -1 charge due to an unshared electron that contributes to the overall structure.
2. Sulfurous Acid (H2SO3)
The Lewis structure of sulfurous acid displays a sulfur atom at the center with four total bonds – one to each of the two hydroxyl (OH) groups and two to oxygen atoms. Importantly, one of the sulfur-oxygen bonds is a double bond. This structure accounts for the interactions and valence of sulfur, resulting in a stable configuration.
3. Hydronium Ion (H3O+)
The Lewis structure for the hydronium ion shows a central oxygen atom bonded to three hydrogen atoms, with an additional pair of electrons contributing to the positive charge of the ion. The presence of this extra electron pair leads to a complete octet for oxygen, creating a stable molecule.
