Determine the identity of the element with the following electron configuration. Enter the symbol of the element. [Xe] 6s^2 4f^14 5d^10 6p^2
The Correct Answer and Explanation is:
Correct Answer: Pb
The element with the electron configuration XeXeXe 6s² 4f¹⁴ 5d¹⁰ 6p² is lead, and its chemical symbol is Pb.
Explanation
To determine the identity of an element from its electron configuration, we must understand what each part of the configuration represents and how the periodic table is organized.
The configuration XeXeXe 6s² 4f¹⁴ 5d¹⁰ 6p² tells us how the electrons are distributed in the atom. The symbol XeXeXe is a shorthand that represents the electron configuration of xenon, a noble gas with an atomic number of 54. So, the configuration already accounts for the first 54 electrons.
Now we look at the remaining electrons beyond xenon:
- 6s² adds 2 electrons
- 4f¹⁴ adds 14 electrons
- 5d¹⁰ adds 10 electrons
- 6p² adds 2 electrons
Add these to xenon’s 54 electrons:
54 (from Xe) + 2 (6s²) + 14 (4f¹⁴) + 10 (5d¹⁰) + 2 (6p²) = 82 electrons
The atomic number of an element is equal to the number of protons, which is also the number of electrons in a neutral atom. Therefore, this atom has 82 electrons, meaning its atomic number is 82.
Looking at the periodic table, the element with atomic number 82 is lead, and its symbol is Pb.
Lead is in period 6 and group 14 (IVA), which matches the valence configuration 6s² 6p², characteristic of group 14 elements. The presence of filled 4f and 5d subshells is also typical for heavier elements in period 6.
This configuration shows that lead is a post-transition metal, and it is the heaviest stable element found in nature. It has applications in batteries, shielding against radiation, and historically in pipes and paints.
