Multiple Choice
Which of the following represents the ground-state electron configuration of the oxide ion, O^{2-}?
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10. Periodic Properties of the Elements
The Electron Configuration: Ions
Multiple Choice
Which of the following is the correct electron configuration for the Ca^{2+} ion?
A
1s^2 2s^2 2p^6 3s^2 3p^6
B
1s^2 2s^2 2p^6 3s^2 3p^4
C
1s^2 2s^2 2p^6 3s^2 3p^6 3d^2
D
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2
Verified step by step guidance1
Identify the atomic number of calcium (Ca), which is 20. This means a neutral calcium atom has 20 electrons.
Write the electron configuration for neutral calcium by filling orbitals in order of increasing energy: \$1s^2 2s^2 2p^6 3s^2 3p^6 4s^2$.
Recognize that the Ca\(^{2+}\) ion has lost 2 electrons compared to the neutral atom, so it has 18 electrons.
Remove the 2 electrons from the highest energy level first, which is the 4s orbital, resulting in the electron configuration for Ca\(^{2+}\): \$1s^2 2s^2 2p^6 3s^2 3p^6$.
Confirm that this configuration corresponds to the electron configuration of the noble gas argon, indicating a stable, filled shell arrangement.
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