Which element corresponds to the electron configuration [Xe] 6s² 4f¹⁴ 5d⁶?

The electron configuration [Xe] 6s² 4f¹⁴ 5d⁶ represents an element in the transition metals section of the periodic table. To understand how this configuration leads to the correct element, we can break it down:

• The notation [Xe] indicates that the electron configuration begins from the noble gas Xenon, which accounts for the first 54 electrons.

• Following Xenon, the configuration includes 6s², indicating that there are 2 electrons in the 6s subshell.

• Next, 4f¹⁴ signifies that all 14 available positions in the 4f subshell are filled with electrons.

• Lastly, 5d⁶ shows that there are 6 electrons in the 5d subshell.

When you tally the total number of electrons, it comes to 54 (from Xenon) + 2 (from 6s) + 14 (from 4f) + 6 (from 5d) = 76. This total of 76 electrons corresponds to the atomic number of Osmium.

Osmium is known for its dense and hard characteristics, found in group 8 of the periodic table, where transition metals reside.