How many unpaired electrons does oxygen have?

Two unpaired electrons.

Think of an oxygen atom like a small hotel with rooms that hold electrons; the first two floors are full and cozy, but the third floor, the two p rooms, has four guests who arrange themselves to be as comfortable as possible. The p level has three rooms and four electrons, so one room gets a pair while the other two rooms each have a single electron; those two single electrons are unpaired. In ground state oxygen the arrangement follows Hund’s rule, which means electrons occupy separate rooms first with the same spin before pairing up, so you end up with two unpaired electrons in the two singly occupied p orbitals.

A common mistake is thinking that all electrons must be paired, but atoms with partially filled orbitals often have unpaired electrons; remember to draw each p orbital separately and place one electron in each before pairing. Another confusion is miscounting electrons because of core electrons in lower shells, so focus on the valence p electrons when deciding unpaired counts. If you forget Hund’s rule, you might pair too early and get the wrong number, so always place single electrons in each degenerate orbital first.

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Oxygen Ground-State: 2 Unpaired Electrons

1. First two shells are full
2. 2p level has three orbitals
3. Four electrons occupy those orbitals
4. One orbital gets a pair
5. Two orbitals have single electrons
6. Follow Hund’s rule for placement

Common Mistakes Counting Oxygen Electrons

1. Assuming all electrons pair
2. Miscounting valence electrons
3. Ignoring Hund’s rule

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