Multiple Choice
Which of the following represents the electron configuration of a sulfur atom (atomic number 16) in its ground state?
10. Periodic Properties of the Elements
The Electron Configuration
Multiple Choice
Which of the following is the correct electron configuration for the oxide ion, O^{2-}?
A
1s^2 2s^2 2p^5
B
1s^2 2s^2 2p^4
C
1s^2 2s^2 2p^6
D
1s^2 2s^2 2p^3
Verified step by step guidance1
Step 1: Identify the atomic number of oxygen (O), which is 8. This means a neutral oxygen atom has 8 electrons.
Step 2: Understand that the oxide ion, O^{2-}, has gained 2 extra electrons, 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: 1s, 2s, then 2p.
Step 4: Fill the 1s orbital with 2 electrons, the 2s orbital with 2 electrons, and the 2p orbitals with the remaining 6 electrons.
Step 5: Conclude that the correct electron configuration for O^{2-} is \$1s^2 2s^2 2p^6$, which corresponds to a full 2p subshell.
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