Final answer:
The student is expected to use molecular simulation to determine the Lewis structure, molecular structure, and bond angles of PCl₃, resulting in a trigonal pyramidal shape and a SMILES string of 'P(Cl)(Cl)Cl'.
Step-by-step explanation:
In the context of creating and understanding complex molecules, the student is tasked with using a simulator to deduce molecular properties such as electron-group geometry, molecular structure, and bond angles. The specific example given is PCl₃, which appears to be a typo. Assuming the correct chemical is PCl₃ (phosphorus trichloride), the student would build the molecule by first creating the Lewis structure, showing one phosphorus atom covalently bonded to three chlorine atoms and one lone pair of electrons on phosphorus, indicating a trigonal pyramidal molecular structure.
The next step would involve translating the 3D structure into a SMILES (Simplified Molecular Input Line Entry System) string. For PCl₃, the SMILES string would be 'P(Cl)(Cl)Cl', which accounts for the three chlorine atoms each bonded to the central phosphorus atom. Bond angles in PCl₃ are approximately 109.5 degrees due to the trigonal pyramidal shape.