Question

\(\mathrm{FClO}_{2}\) and \(\mathrm{F}_{3} \mathrm{ClO}\) can both gain a fluoride ion to form stable anions. \(\mathrm{F}_{3} \mathrm{ClO}\) and \(\mathrm{F}_{3} \mathrm{ClO}_{2}\) will both lose a fluoride ion to form stable cations. Draw the Lewis structures and describe the hybrid orbitals used by chlorine in these ions.

Short answer

In the ions \(\mathrm{F}_{2} \mathrm{ClO}_{2}^{-}\), \(\mathrm{F}_{4} \mathrm{ClO}^{-}\), \(\mathrm{F}_{2} \mathrm{ClO}^{+}\), and \(\mathrm{F}_{2} \mathrm{ClO}_{2}^{+}\), chlorine exhibits sp3, sp3d2, sp2, and sp3d hybridization, respectively. The hybrid orbitals in each ion are formed through the combination of chlorine's 3s, 3p, and 3d orbitals and are used to form single or double bonds with the surrounding atoms.

Step-by-step solution

Draw the Lewis structures of the given ions

Start with the neutral molecules, then add or remove a fluoride ion to form the anion and cation, respectively. a. Anions: For \(\mathrm{FClO}_{2}\), after adding a fluoride ion: \(\mathrm{F}_{2} \mathrm{ClO}_{2}^{-}\). For \(\mathrm{F}_{3} \mathrm{ClO}\), after adding a fluoride ion: \(\mathrm{F}_{4} \mathrm{ClO}^{-}\). b. Cations: For \(\mathrm{F}_{3} \mathrm{ClO}\) after removing a fluoride ion: \(\mathrm{F}_{2} \mathrm{ClO}^{+}\). For \(\mathrm{F}_{3} \mathrm{ClO}_{2}\) after removing a fluoride ion: \(\mathrm{F}_{2} \mathrm{ClO}_{2}^{+}\). Now, we can draw the Lewis structures for these ions.

Identify hybridization of chlorine for each ion

Determine the hybridization of chlorine in these ions by counting the number of electron groups (lone pairs, single bonds, double bonds) around the chlorine atom. a. \(\mathrm{F}_{2} \mathrm{ClO}_{2}^{-}\): Chlorine has 4 electron groups (four single bonds) - sp3 hybridization. b. \(\mathrm{F}_{4} \mathrm{ClO}^{-}\): Chlorine has 6 electron groups (six single bonds) - sp3d2 hybridization. c. \(\mathrm{F}_{2} \mathrm{ClO}^{+}\): Chlorine has 3 electron groups (three single bonds) - sp2 hybridization. d. \(\mathrm{F}_{2} \mathrm{ClO}_{2}^{+}\): Chlorine has five electron groups (three single bonds and one double bond) - sp3d hybridization.

Describe the hybrid orbitals used by chlorine in these ions

Now, we can describe the hybrid orbitals used by chlorine in these ions: a. In \(\mathrm{F}_{2} \mathrm{ClO}_{2}^{-}\) ion, chlorine is sp3 hybridized, using its 3s and three 3p orbitals to form four hybrid orbitals. These hybrid orbitals form single bonds with two fluoride and two oxygen atoms. b. In \(\mathrm{F}_{4} \mathrm{ClO}^{-}\) ion, chlorine is sp3d2 hybridized, using its 3s, three 3p, and two 3d orbitals to form six hybrid orbitals. These hybrid orbitals form single bonds with four fluoride atoms and one oxygen atom. c. In \(\mathrm{F}_{2} \mathrm{ClO}^{+}\) ion, chlorine is sp2 hybridized, using its 3s and two 3p orbitals to form three hybrid orbitals. These hybrid orbitals form single bonds with two fluoride atoms and one oxygen atom. d. In \(\mathrm{F}_{2} \mathrm{ClO}_{2}^{+}\) ion, chlorine is sp3d hybridized, using its 3s, three 3p, and one 3d orbitals to form five hybrid orbitals. These hybrid orbitals form single bonds with two fluoride atoms, a single bond with one oxygen atom, and a double bond with another oxygen atom.