This question involves identifying the correct molecular geometry for a given molecule. The image shows four possible molecular shapes, and you need to determine which one corresponds to the molecule in question (likely based on VSEPR theory).

VSEPR (Valence Shell Electron Pair Repulsion) theory predicts molecular geometry based on the repulsion between electron pairs in the valence shell of the central atom. The key steps are:

Step 1: Determine the steric number (SN) of the central atom. SN = number of atoms bonded to central atom + number of lone pairs on central atom.

Step 2: Use the steric number to find the electron geometry:

• SN=2: Linear
• SN=3: Trigonal planar
• SN=4: Tetrahedral
• SN=5: Trigonal bipyramidal
• SN=6: Octahedral

Step 3: Molecular geometry is determined by the positions of atoms (ignoring lone pairs). For example:

• Tetrahedral electron geometry with 4 bonded atoms: Tetrahedral molecular geometry
• Tetrahedral electron geometry with 3 bonded atoms + 1 lone pair: Trigonal pyramidal
• Tetrahedral electron geometry with 2 bonded atoms + 2 lone pairs: Bent

Without knowing the specific molecule, I can describe the four geometries shown:

1. Linear (2 atoms, 180° bond angle)
2. Trigonal planar (3 atoms, 120° bond angles)
3. Tetrahedral (4 atoms, ~109.5° bond angles)
4. Trigonal bipyramidal (5 atoms, 90° and 120° bond angles)

To solve this, you would:

1. Identify the central atom and its valence electrons
2. Count the number of bonded atoms and lone pairs
3. Determine the steric number
4. Predict the molecular geometry
5. Match with the correct option