Which electron configuration corresponds to a neutral oxygen atom (atomic number 8) in the simplified orbital notation?

• A. ${\mathrm{1s}}^2{\mathrm{2s}}^1{\mathrm{2p}}^5$
• B. ${\mathrm{1s}}^2{\mathrm{2s}}^2{\mathrm{2p}}^5$
• C. ${\mathrm{1s}}^2{\mathrm{2s}}^2{\mathrm{2p}}^4$
• D. ${\mathrm{1s}}^2{\mathrm{2s}}^2{\mathrm{2p}}^3$

Answer: (C)

Verified step by step guidance

1. Identify the atomic number of oxygen, which is 8. This means a neutral oxygen atom has 8 electrons.
2. Recall the order in which electrons fill orbitals: first the 1s orbital, then the 2s orbital, and finally the 2p orbitals.
3. Fill the 1s orbital with 2 electrons, since it can hold a maximum of 2 electrons.
4. Next, fill the 2s orbital with 2 electrons, as it also holds a maximum of 2 electrons.
5. Distribute the remaining electrons (8 - 2 - 2 = 4) into the 2p orbitals, which can hold up to 6 electrons, so place 4 electrons there.