Which element is associated with the configuration [Xe] 6s^2 4f^14 5d^10?

The electron configuration [Xe] 6s² 4f¹⁴ 5d¹⁰ indicates that the element in question has completely filled orbitals beyond the xenon core, specifically filling the 6s, 4f, and 5d subshells.

This configuration reveals that we are looking at an element in the d-block of the periodic table, particularly one that is also a transition metal. The 4f subshell has 14 electrons, which is characteristic of lanthanides, and the 5d subshell holds 10 electrons, typical for elements that follow the lanthanides.

To identify the element, consider its position on the periodic table. The configuration corresponds to mercury, which is located in group 12 and period 6. Specifically, mercury has an atomic number of 80, and its electron configuration is correctly represented by [Xe] 6s² 4f¹⁴ 5d¹⁰, confirming it as the element associated with this electron configuration.

Other elements such as vanadium, lead, and osmium have different configurations and would not fit the provided description. Vanadium specifically has a much simpler configuration and is in period 4, while lead would