Multiple Choice
In a molecule with a tetrahedral geometry, how many atoms are directly bonded to the central atom?
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12. Molecular Shapes & Valence Bond Theory
Molecular Geometry
Multiple Choice
What is the molecular geometry of germanium disulfide (GeS_2)?
A
Linear
B
Bent
C
Trigonal planar
D
Tetrahedral
Verified step by step guidance1
Step 1: Determine the central atom and the atoms bonded to it. In GeS_2, germanium (Ge) is the central atom bonded to two sulfur (S) atoms.
Step 2: Count the total number of valence electrons around the central atom. Germanium is in group 14 with 4 valence electrons, and each sulfur atom is in group 16 with 6 valence electrons. For GeS_2, consider the bonding and lone pairs on Ge.
Step 3: Draw the Lewis structure for GeS_2. Place Ge in the center with single or double bonds to each sulfur atom, then complete the octets of the sulfur atoms and check for lone pairs on Ge.
Step 4: Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to predict the molecular geometry. Count the regions of electron density (bonding and lone pairs) around the central Ge atom to determine the shape.
Step 5: Based on the number of bonding pairs and lone pairs, identify the molecular geometry. For GeS_2, with two bonding pairs and two lone pairs on Ge, the electron geometry is tetrahedral, but the molecular shape is bent. However, if there are no lone pairs on Ge and only two double bonds, the shape is linear. Confirm the correct structure to finalize the geometry.
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