Determine the electron geometry for the carbon disulfide molecule, CS₂. 

• A. Linear
• B. Bent
• C. Trigonal planar
• D. Tetrahedral

Answer: (A)

Verified step by step guidance

1. Step 1: Draw the Lewis structure of CS\_2. Carbon (C) is the central atom bonded to two sulfur (S) atoms. Each sulfur atom forms a double bond with carbon, and each sulfur has two lone pairs of electrons, as shown in the image.
2. Step 2: Count the regions of electron density around the central carbon atom. Each double bond counts as one region of electron density. Since there are two double bonds, there are two regions of electron density around carbon.
3. Step 3: Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to determine the electron geometry. Two regions of electron density around the central atom will arrange themselves as far apart as possible, which is 180° apart.
4. Step 4: Based on the arrangement of two electron regions, the electron geometry is linear.
5. Step 5: Confirm that there are no lone pairs on the central atom that would alter the geometry. Since carbon has no lone pairs in CS\_2, the molecular geometry is also linear.