HCl H: Ci: Formula Lewis Structure Electron Pair Geometry Molecular Bond Geometry Angle Polar or Non Polar Polar H-CI H?O * H:O:H H H 109.5° Polar NH3 H:N:H N HHH 107° Polar BCL? CI: B:CI: C ?? B 120° Non-Polar CI ::::: =0 O=C=0 180° Non-Polar :9: CO? : Cl PO?³? 0: 0:0:0:1 NO? NO? CH? SO? SO?²? P ? 109.28
The Correct Answer and Explanation is:
Predicted Bond Angle of H₂S: ~92.1°
Explanation:
To determine the bond angle of hydrogen sulfide (H₂S), we utilize the Valence Shell Electron Pair Repulsion (VSEPR) theory, which predicts the three-dimensional geometry of molecules based on minimizing the electrostatic repulsion between electron pairs around a central atom.
1. Lewis Structure:
First, we draw the Lewis structure for H₂S. Sulfur (S), the central atom, is in Group 16 and has 6 valence electrons. Each hydrogen (H) atom has 1 valence electron.
Total valence electrons = 6 + 2(1) = 8.
Sulfur forms a single covalent bond with each of the two hydrogen atoms, using 4 electrons. The remaining 4 electrons are placed on the central sulfur atom as two non-bonding lone pairs.
2. Electron Pair Geometry:
According to VSEPR theory, we count the number of electron domains around the central sulfur atom. An electron domain can be a single bond, a double bond, a triple bond, or a lone pair. In H₂S, there are two single bonding pairs (S-H bonds) and two lone pairs.
Total electron domains = 2 bonding pairs + 2 lone pairs = 4 domains.
An arrangement of four electron domains results in a tetrahedral electron pair geometry. The ideal bond angle for a perfect tetrahedral shape (like in methane, CH₄)
