A variety of chlorine oxide fluorides and related cations and anions are known. They tend to be powerful oxidizing and fluorinating agents. \(\mathrm{FClO}_{3}\) is the most stable of this group of compounds and has been studied as an oxidizing component in rocket propellants. Draw a Lewis structure for \(\mathrm{F}_{3} \mathrm{ClO}\) , $\mathrm{F}_{2} \mathrm{ClO}_{2}^{+},\( and \)\mathrm{F}_{3} \mathrm{ClO}_{2}$ . What is the molecular structure for each species, and what is the expected hybridization of the central chlorine atom in each compound or ion?

First, let's calculate the total number of valence electrons for each compound: - F₃ClO: 7 (Cl) + 3 * 7 (F) + 6 (O) = 34 valence electrons - F₂ClO₂⁺: 7 (Cl) + 2 * 7 (F) + 2 * 6 (O) - 1 (due to the positive charge) = 33 valence electrons - F₃ClO₂: 7 (Cl) + 3 * 7 (F) + 2 * 6 (O) = 40 valence electrons

We will draw the Lewis structures for three compounds: 1. F₃ClO: Put the Cl atom in the center, and surround it by F and O atoms. Form single bonds between the Cl and F atoms and the Cl and O atoms, using up 8 valence electrons. Fill in the F and O atoms with their remaining valence electrons, which will be 6 on each F atom and 4 on the O atom (18 electrons used). Lastly, place the remaining 8 valence electrons on the Cl atom. 2. F₂ClO₂⁺: Put the Cl atom in the center, and surround it by F and O atoms. Form single bonds between Cl and F atoms, and Cl and O atoms, using up 8 valence electrons. Fill in the F and O atoms with their remaining valence electrons, which will be 6 on each F atom and 4 on each O atom (16 electrons used). Lastly, place the remaining 9 valence electrons on the Cl atom. 3. F₃ClO₂: Put the Cl atom in the center, and surround it by F and O atoms. Form single bonds between Cl and F atoms, and Cl and O atoms, using up 10 valence electrons. Fill in the F and O atoms with their remaining valence electrons, which will be 6 on each F atom and 4 on each O atom (22 electrons used). Lastly, place the remaining 8 valence electrons on the Cl atom.

1. F₃ClO: Molecular structure: Tetrahedral (four electron groups - three single bonds and one lone pair) Expected hybridization: sp³ (four electron groups) 2. F₂ClO₂⁺: Molecular structure: Trigonal bipyramidal (five electron groups - four single bonds and one lone pair) Expected hybridization: sp³d (five electron groups) 3. F₃ClO₂: Molecular structure: Octahedral (six electron groups - five single bonds and one lone pair) Expected hybridization: sp³d² (six electron groups)