Consider the following chemical species: I ₃^-, SF ₄, XeF ₄ , and BrF ₃ . Identify the species that possesses the maximum number of lone pairs of electrons on its central atom. What is the hybridization and molecular geometry of this species?

Step-by-step solution

First, determine the number of lone pairs on the central atom for each species. 1. I ₃^- : The central I atom has 7 valence electrons. Adding 1 electron for the negative charge gives 8 electrons. It forms 2 single bonds with the other two iodine atoms. Number of lone pairs = 8 - 2 2 = 3 . 2. SF ₄ : Central S atom has 6 valence electrons. It forms 4 single bonds. Number of lone pairs = 6 - 4 2 = 1 . 3. XeF ₄ : Central Xe atom has 8 valence electrons. It forms 4 single bonds. Number of lone pairs = 8 - 4 2 = 2 . 4. B