Select the correct answer.
What is the noble gas electron configuration of bismuth (Bi)?
A. [Kr] 6s² 6p³
B. [Xe] 6s² 6p³
C. [Xe] 4/¹4 5d10 6s² 6p³
D. [kr] 5s² 5d¹0 5p6 6s² 6d¹0 6p³
E. [Xe] 6s² 5d10 6p³
The Correct Answer and Explanation is:
The correct answer is B. [Xe] 6s² 6p³.
Explanation:
Bismuth (Bi) is an element with the atomic number 83. To determine its noble gas electron configuration, we start by finding the nearest noble gas that precedes bismuth in the periodic table, which is xenon (Xe) with an atomic number of 54. The noble gas notation provides a shorthand way to express the electron configuration by encapsulating the electron arrangement of the nearest noble gas and then adding the remaining electrons.
Bismuth has a total of 83 electrons, which means its electron configuration can be built by filling up the orbitals in the order dictated by the Aufbau principle, Hund’s rule, and the Pauli exclusion principle. The electron configuration for bismuth can be derived as follows:
- Count electrons up to xenon (54 electrons):
The electron configuration of xenon is:
[ \text{Xe}: [Kr] 5s^2 4d^{10} 5p^6 ]
Here, krypton (Kr) covers the first 36 electrons. - Continuing with the next electrons:
After xenon, the next electrons fill the 6s orbital and then the 6p orbital:
- 6s² (2 electrons)
- 6p³ (3 electrons)
Combining these configurations, we arrive at:
[ \text{Bi}: [Xe] 6s^2 6p^3 ]
This configuration indicates that bismuth has two electrons in the 6s subshell and three electrons in the 6p subshell, which is characteristic of elements in group 15 of the periodic table, where bismuth is located. This also aligns with the trends in electron configuration, where elements in the same group exhibit similar valence shell configurations.
Conclusion:
The answer choice B correctly represents the noble gas electron configuration of bismuth. It accurately summarizes the distribution of bismuth’s electrons following the stable configuration of xenon, allowing for an efficient representation of its chemical behavior and properties.