Final answer:
BCl₃ (Boron trichloride) has an electron-pair geometry and molecular structure that is electronically identical to that of NCl₃, thereby fulfilling the criteria of an AX₃ molecular shape with three bonding pairs around the central atom.
Step-by-step explanation:
The question is asking for a compound that has an electronically identical Lewis structure to that of NCl₃. NCl₃ has a central nitrogen atom with three chlorine atoms attached and follows the octet rule.
When comparing potential candidates, we search for a compound with the same AX₃ electron-pair geometry, where the central atom has three bonding pairs and one lone pair.
Among the given options, BCl₃ (Boron trichloride) exhibits this electronic structure. For BCl₃, the central atom, boron, has three bonding pairs and no lone pairs.
However, boron is an exception to the octet rule and doesn't require a complete octet, thus making the electron-pair geometry and molecular structure identical to NCl₃, which both are AX₃.