Final answer:
The electronic configuration [Xe]4f⁷ 5d¹ 6s² indicates that the element belongs to the f-block of the periodic table, specifically within the lanthanide series.
Step-by-step explanation:
The element with the electronic configuration [Xe]4f⁷ 5d¹ 6s² belongs to the f-block of the periodic table. This can be determined by looking at the highest number 'f' orbital that electrons occupy in the given configuration. In this case, since the configuration includes 4f⁷, it indicates the presence of seven electrons in the 4f sublevel, placing this element within the f-block. Specifically, it would be part of the lanthanide series, which is known for having its 4f sublevel in the process of being filled.
Based on the general electron configuration for elements in the f-block, which is (n − 2) ƒ¹-¹⁴ns², and the fact that the f-block is located at the very bottom of the periodic table, separate from the main body, it is clear that option 4 (F) is the correct choice.
Additionally, the presence of '4f' orbitals is a significant indicator of f-block elements, as mentioned in the simplified electron configuration for larger elements like tungsten, which would be [Xe]6s² 4f⁴ 5d⁴.