Multiple Choice
What is the molecular geometry of CF_4?
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12. Molecular Shapes & Valence Bond Theory
Molecular Geometry
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What is the molecular geometry of SCl_2?
A
Trigonal planar
B
Linear
C
Tetrahedral
D
Bent
Verified step by step guidance1
Determine the Lewis structure of SCl_2 by counting the total valence electrons: sulfur (S) has 6 valence electrons and each chlorine (Cl) has 7, so total electrons = 6 + 2 × 7 = 20 electrons.
Draw the skeletal structure with sulfur as the central atom bonded to two chlorine atoms, then distribute the remaining electrons to satisfy the octet rule for each atom, placing lone pairs on sulfur as needed.
Count the regions of electron density (bonding and lone pairs) around the central sulfur atom. In SCl_2, there are two bonding pairs (S–Cl bonds) and two lone pairs on sulfur, making a total of four regions of electron density.
Use the VSEPR theory to determine the electron geometry based on four regions of electron density, which corresponds to a tetrahedral electron geometry.
Since there are two lone pairs, the molecular geometry (shape) is bent (or angular), not tetrahedral, trigonal planar, or linear.
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