Which element corresponds to the electron configuration [Rn] 7s^2 5f^14 6d^6?

The given electron configuration, [Rn] 7s² 5f¹⁴ 6d⁶, indicates that the element in question is in period 7 of the periodic table and contains electrons in the 7s, 5f, and 6d sublevels.

To break down the configuration:

• The [Rn] denotes the core electrons up to radon, which accounts for 86 electrons.

• The 7s² indicates there are 2 electrons in the 7s orbital.

• The 5f¹⁴ suggests that the 5f sublevel is fully occupied with its maximum of 14 electrons.

• The 6d⁶ points to 6 electrons in the 6d sublevel.

When we total these, the electron count is:

86 (from Rn) + 2 (from 7s) + 14 (from 5f) + 6 (from 6d) = 108 electrons.

The element with atomic number 108 is Hassium (Hs), which matches the provided electron configuration. This is confirmed by the fact that Hassium is a member of the transactinide series, situated in Group 8 and Period 7