What is the molecular structure for each of the following molecules or ions? a. \(\mathrm{OCl}_{2}\) b. \(\mathrm{ClO}_{4}-\) c. \(\mathrm{ICl}_{5}\) d. \(\mathrm{PF}_{6}-\)

First, identify the central atom in each molecule or ion. Then, count the total number of electron groups around it, including bonded atoms and lone pairs of electrons. a. \(\mathrm{OCl}_2\) - Central atom: O - Electron groups: 2 (two Cl atoms) b. \(\mathrm{ClO}_4^-\) - Central atom: Cl - Electron groups: 4 (four O atoms) c. \(\mathrm{ICl}_5\) - Central atom: I - Electron groups: 5 (five Cl atoms) d. \(\mathrm{PF}_6^-\) - Central atom: P - Electron groups: 6 (six F atoms)

Use the number of electron groups to determine the electron geometry according to the VSEPR theory. a. \(\mathrm{OCl}_2\) - Electron geometry: Linear b. \(\mathrm{ClO}_4^-\) - Electron geometry: Tetrahedral c. \(\mathrm{ICl}_5\) - Electron geometry: Trigonal bipyramidal d. \(\mathrm{PF}_6^-\) - Electron geometry: Octahedral

In some cases, the electron geometry is different from the molecular geometry. If there are lone pairs on the central atom, adjust the geometry accordingly. a. \(\mathrm{OCl}_2\) - Molecular geometry: Bent - Explanation: There are two lone pairs on the Oxygen atom. b. \(\mathrm{ClO}_4^-\) - Molecular geometry: Tetrahedral - Explanation: No lone pairs on the central Chlorine atom. c. \(\mathrm{ICl}_5\) - Molecular geometry: Square pyramidal - Explanation: No lone pairs on the central Iodine atom. d. \(\mathrm{PF}_6^-\) - Molecular geometry: Octahedral - Explanation: No lone pairs on the central Phosphorus atom. Thus, the molecular structures are as follows: a. \(\mathrm{OCl}_2\): Bent b. \(\mathrm{ClO}_4^-\): Tetrahedral c. \(\mathrm{ICl}_5\): Square pyramidal d. \(\mathrm{PF}_6^-\): Octahedral