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It doesn't. Oxygen must gain (or borrow) two electrons to complete its outer shell since it has only 6 electrons in its valence shell.

Oxygen is atomic #8 in the Periodic Table, meaning it has 8 electrons. The first shell of an element needs only 2 electrons to be stable and relatively unreactive. Shells (energy levels) beyond the first need 8 electrons to be stable, but oxygen has only 6 left because 2 were used in the first shell. Therefore, oxygen needs 2 more to complete its outer (valence) shell.

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14y ago
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5mo ago

Oxygen achieves a full outer electron shell by gaining two electrons, which allows it to reach a stable electron configuration similar to noble gases. This stability is energetically favorable for oxygen as it reduces the overall energy of the atom. Additionally, gaining two electrons allows oxygen to form more stable compounds with other elements.

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Q: WHY does it make sense that oxygen achieved full shell by gaining electron?
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