Multiple Choice
Which element in the ground state has exactly 3 electrons in the 2p sublevel?
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10. Periodic Properties of the Elements
The Electron Configuration
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Which of the following represents the noble gas electron configuration of bismuth (Bi)?
A
[Rn] 6s^{2} 6p^{3}
B
[Xe] 4f^{14} 5d^{10} 6s^{2} 6p^{5}
C
[Kr] 4d^{10} 5s^{2} 5p^{6} 6s^{2} 6p^{3}
D
[Xe] 4f^{14} 5d^{10} 6s^{2} 6p^{3}
Verified step by step guidance1
Identify the atomic number of bismuth (Bi), which is 83. This tells us how many electrons the neutral atom has.
Recall that the noble gas electron configuration uses the electron configuration of the nearest noble gas with fewer electrons as a starting point, followed by the additional electrons needed to reach the element in question.
Determine the noble gas preceding bismuth in the periodic table. Since bismuth has 83 electrons, find the noble gas with an atomic number less than 83 but closest to it. This is xenon (Xe) with atomic number 54.
Write the electron configuration starting from [Xe], then add the electrons in the 4f, 5d, 6s, and 6p orbitals to reach a total of 83 electrons. This includes filling the 4f^{14} and 5d^{10} subshells, then adding 6s^{2} and 6p^{3} electrons.
Compare the given options to this configuration. The correct noble gas configuration for bismuth is [Xe] 4f^{14} 5d^{10} 6s^{2} 6p^{3}.
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