Consider the following chemical species: H ₂ O , SF ₄ , I ₃^- , and BrF ₅ . Identify the species that possesses the maximum number of lone pairs of electrons on its central atom, and select its correct molecular shape.

Step-by-step solution

First, determine the number of lone pairs on the central atom for each given species: 1. H ₂ O : The central oxygen atom has 6 valence electrons. It forms 2 single bonds with hydrogen atoms, leaving 4 non-bonding electrons, which corresponds to 2 lone pairs. 2. SF ₄ : The central sulphur atom has 6 valence electrons. It forms 4 single bonds with fluorine atoms, leaving 2 non-bonding electrons, which corresponds to 1 lone pair. 3. I ₃^- : The central iodine atom has 7 valence electrons, plus 1 electron from the nega