Multiple Choice
Which of the following represents the electron configuration of S^{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 oxide ion (O^{2-})?
A
1s^2 2s^2 2p^6
B
1s^2 2s^2 2p^4
C
1s^2 2s^2 2p^5
D
1s^2 2s^2 2p^3
Verified step by step guidance1
Step 1: Identify the atomic number of oxygen (O). Oxygen has an atomic number of 8, which means a neutral oxygen atom has 8 electrons.
Step 2: Understand that the oxide ion (O^{2-}) has gained 2 extra electrons compared to the neutral oxygen atom, so the total number of electrons is 8 + 2 = 10.
Step 3: Write the electron configuration for 10 electrons by filling the orbitals in order of increasing energy: first the 1s orbital, then 2s, and then 2p orbitals.
Step 4: Recall the maximum number of electrons each subshell can hold: 1s can hold 2, 2s can hold 2, and 2p can hold 6 electrons.
Step 5: Combine these to write the full electron configuration for O^{2-} as \$1s^{2} 2s^{2} 2p^{6}$, which corresponds to a filled 2p subshell.
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