Which element has the electron configuration: [Xe] 4f14 5d10 6s2 6p3? _
The Correct Answer and Explanation is:
Correct Answer: Bi (Bismuth)
The given electron configuration is:
[Xe] 4f¹⁴ 5d¹⁰ 6s² 6p³
This configuration shows the distribution of electrons in the atomic orbitals of an element, starting from the core configuration of xenon (Xe), which has 54 electrons. The rest of the configuration describes electrons beyond xenon:
- 4f¹⁴: These 14 electrons fill the 4f subshell, characteristic of the lanthanide series.
- 5d¹⁰: These 10 electrons fill the 5d subshell, found in the transition metals.
- 6s²: These 2 electrons fill the 6s subshell.
- 6p³: These 3 electrons are in the outermost p-orbital of the sixth period.
Adding all the electrons:
- Xenon core: 54 electrons
- 4f¹⁴: 14 electrons
- 5d¹⁰: 10 electrons
- 6s²: 2 electrons
- 6p³: 3 electrons
Total = 54 + 14 + 10 + 2 + 3 = 83 electrons
An element with 83 electrons is Bismuth, which has the atomic number 83.
Bismuth is a post-transition metal located in group 15 and period 6 of the periodic table. It is in the same group as nitrogen, phosphorus, arsenic, and antimony, and like them, it has five valence electrons (two in the s-orbital and three in the p-orbital). This valence structure allows Bismuth to commonly form +3 oxidation states in compounds.
Bismuth is a heavy, brittle metal with low toxicity compared to other heavy metals, making it useful in medical applications like Pepto-Bismol. It is also known for its colorful oxide layers and unique crystal shapes when cooled slowly. The full electron configuration helps chemists understand its chemical behavior and position in the periodic table.
