What element matches the electron configuration [Xe] 6s^2 4f^14 5d^10 6p^5?

The electron configuration given is [Xe] 6s² 4f¹⁴ 5d¹⁰ 6p⁵, which indicates that the element has filled subshells (4f and 5d) along with additional electrons in the 6s and 6p orbitals. To analyze this configuration, we can break it down:

• The [Xe] represents the electron configuration of xenon, which accounts for the first 54 electrons.

• The 6s² indicates that the element has 2 electrons in the 6s subshell.

• The 4f¹⁴ indicates that there are 14 electrons fully occupying the 4f subshell.

• The 5d¹⁰ signifies that there are 10 electrons in the 5d subshell.

• Finally, the 6p⁵ shows that there are 5 electrons in the 6p subshell.

To find the total number of electrons, we can add these together: 54 (from xenon) + 2 (from 6s) + 14 (from 4f) + 10 (from 5d) + 5 (from 6p) equals 85