Textbook Question
The following electron configurations represent excited states. Identify the element and write its ground-state condensed electron configuration. (b) 3Ar44s13d104p25p1
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10. Periodic Properties of the Elements
The Electron Configuration: Condensed
Multiple Choice
Which of the following condensed electron configurations represents a noble gas in its ground state?
A
[Ne]
B
[Ar] 4s^2 3d^{10} 4p^6
C
[Kr] 5s^2 4d^{10} 5p^5
D
[He] 2s^2 2p^6
Verified step by step guidance1
Recall that noble gases have completely filled valence electron shells, which correspond to stable electron configurations.
Examine each given electron configuration and identify the outermost shell electrons to determine if the shell is fully filled.
For the configuration [Ar] 4s^2 3d^{10} 4p^6, note that the 4s and 4p orbitals are fully filled, and the 3d orbitals are also completely filled, indicating a full valence shell.
For the configuration [Kr] 5s^2 4d^{10} 5p^5, observe that the 5p orbital is not fully filled (it has 5 electrons instead of 6), so this is not a noble gas configuration.
For the configuration [He] 2s^2 2p^6, check if this corresponds to a noble gas; since helium's ground state is just 1s^2, this configuration actually represents neon, which is a noble gas, but the notation is inconsistent with helium's actual configuration.
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