An element X with electronic configuration 1s22s22p 63s 23p5combines with another element Y with the configuration 1s2s22p23s33p5. What is the formula of th...

To determine the formula of the compound formed between elements X and Y, we need to find out the number of electrons that each element can gain or lose to form ions. Element X has 7 valence electrons and needs to gain one electron to achieve the stable configuration of the nearest noble gas, which is 3s₂3p₆. Thus, element X can form an anion with a charge of -1, which is denoted by X^-. Element Y has 5 valence electrons and needs to gain three electrons to achieve the stable configuration of the nearest noble gas, which is 3s₂3p₆. Thus, element Y can form an anion with a charge of -3, which is denoted by Y^3-. To form a compound, the total positive charge must balance the total negative charge. The least common multiple of 1 and 3 is 3, so we need three X^- ions to balance two Y^3- ions. Therefore, the formula of the compound formed is X₃Y₂. So, the correct option is: XY₂.