Question

determine the molecular geometry of so₂. bent trigonal pyramidal tetrahedral linear trigonal planar

Explanation:

To determine the molecular geometry of \(SO_2\), we use the VSEPR (Valence - Shell Electron - Pair Repulsion) theory.

• First, find the number of valence electrons: \(S\) has \(6\) valence electrons and each \(O\) has \(6\) valence electrons. So, for \(SO_2\), the total number of valence electrons is \(6+(2\times6)=18\).
• Then, draw the Lewis structure. \(S\) is the central atom. The Lewis structure of \(SO_2\) has \(S\) double - bonded to one \(O\) atom (\(S = O\)), single - bonded to another \(O\) atom (\(S - O\)), and a lone pair on \(S\).
• According to VSEPR, the electron - pair geometry around \(S\) is trigonal planar (because there are \(3\) electron groups: \(2\) bonding pairs and \(1\) lone pair). But when considering the molecular geometry (which ignores lone pairs in terms of the 'geometry' name but still accounts for their repulsion), the molecular geometry of \(SO_2\) is bent. The lone pair on \(S\) repels the bonding pairs, causing the \(O - S - O\) bond angle to be less than \(120^{\circ}\) (the ideal trigonal - planar bond angle).

Answer:

bent