Phosphorus pentachloride Formula: Lewis Structure (including appropriate resonance forms and formal charges) Number of valence electrons: Electron domain geometry Molecular shape: Polarity of individual bonds: Hybridization of the central atom: Bond angles: Overall polarity of molecule: Instructor initials Sulfur tetrafluoride Formula: Lewis Structure (including appropriate resonance forms and formal charges) Number of valence electrons: Electron domain geometry: Molecular shape: Polarity of individual bonds: Hybridization of the central atom: Bond angles: Overall polarity of molecule:
The Correct Answer and Explanation is :
Phosphorus Pentachloride (PCl₅)
- Formula: PCl₅
- Lewis Structure: Phosphorus (P) is the central atom, with five chlorine (Cl) atoms attached to it. Each chlorine atom forms a single bond with phosphorus, and phosphorus has an expanded octet. There are no lone pairs on phosphorus in the Lewis structure, and each chlorine has three lone pairs. The formal charges are neutral for all atoms.
- Number of Valence Electrons: Phosphorus has 5 valence electrons, and chlorine has 7 valence electrons each. Total: 5 + (5 × 7) = 40 valence electrons.
- Electron Domain Geometry: Trigonal bipyramidal (since there are five bonding pairs).
- Molecular Shape: Trigonal bipyramidal, where three chlorine atoms are positioned in the equatorial plane, and two chlorine atoms are positioned along the axial positions.
- Polarity of Individual Bonds: The P-Cl bonds are polar because of the difference in electronegativity between phosphorus and chlorine.
- Hybridization of the Central Atom: sp³d hybridization.
- Bond Angles: 90° for the axial-equatorial bonds, and 120° for the equatorial-equatorial bonds.
- Overall Polarity of the Molecule: The molecule is nonpolar because the symmetrical distribution of the chlorine atoms around the phosphorus atom results in the cancellation of the dipole moments.
Sulfur Tetrafluoride (SF₄)
- Formula: SF₄
- Lewis Structure: Sulfur (S) is the central atom, with four fluorine (F) atoms attached. There are one lone pair on sulfur. Each fluorine has three lone pairs, and sulfur has an expanded octet.
- Number of Valence Electrons: Sulfur has 6 valence electrons, and fluorine has 7 valence electrons each. Total: 6 + (4 × 7) = 34 valence electrons.
- Electron Domain Geometry: Trigonal bipyramidal (due to five electron domains, with four bonds and one lone pair).
- Molecular Shape: See-saw shape, with the lone pair occupying an equatorial position.
- Polarity of Individual Bonds: The S-F bonds are polar because of the electronegativity difference between sulfur and fluorine.
- Hybridization of the Central Atom: sp³d hybridization.
- Bond Angles: Approximately 90° between axial and equatorial bonds, and about 120° between equatorial bonds.
- Overall Polarity of the Molecule: The molecule is polar due to the asymmetry caused by the lone pair, leading to an overall dipole moment.
I’ll generate the images for both molecules now.
Here are the Lewis structures for both phosphorus pentachloride (PCl₅) and sulfur tetrafluoride (SF₄). Let me know if you need any further details!