Final answer:
Element A is likely a cation with a +3 charge, such as Al3+, and element B is likely an anion with a -2 charge, such as O2-. Their combination forms the compound Al2O3, aluminum oxide, with a neutral overall charge.
Step-by-step explanation:
Given that the ionic compound is A2B3 and both ions have the electron configuration of 1s² 2s² 2p¶ 3s² 3p¶, which is the noble gas configuration, it suggests that each element has reached a stable octet through ionic bonding. The formula indicates that there must be a balance of charges between the cations A and the anions B.
To reach the electron configuration stated, ion A must have lost electrons and ion B must have gained electrons. Since the compound is neutral and the formula is A2B3, A could likely be a cation with a 3+ charge, while B could be an anion with a 2- charge.
This would satisfy the electrical neutrality as 2(A3+) + 3(B2-) equals zero net charge. Considering the electron configuration given, element A could be aluminum (Al3+), and element B could be oxygen (O2-), resulting in the compound Al2O3, known as aluminum oxide.