Consider the molecule PF₄Cl. (a) Draw a Lewis structure for the molecule, and predict its electron-domain geometry.

Verified step by step guidance

1. Step 1: Count the total number of valence electrons available for the molecule PF4Cl. Phosphorus (P) has 5 valence electrons, each fluorine (F) has 7 valence electrons, and chlorine (Cl) also has 7 valence electrons. Calculate the sum of these electrons.
2. Step 2: Determine the central atom. Phosphorus (P) is typically the central atom because it is less electronegative than fluorine and chlorine.
3. Step 3: Arrange the fluorine and chlorine atoms around the central phosphorus atom. Connect each of these atoms to phosphorus with a single bond, using 2 electrons per bond.
4. Step 4: Distribute the remaining valence electrons to complete the octets of the surrounding atoms (fluorine and chlorine) first, and then place any remaining electrons on the central phosphorus atom.
5. Step 5: Predict the electron-domain geometry. Count the number of electron domains (bonding and non-bonding pairs) around the central phosphorus atom to determine the geometry using VSEPR theory. PF4Cl has 5 electron domains, which corresponds to a trigonal bipyramidal electron-domain geometry.