Oxygen typically forms two covalent bonds. This is because an oxygen atom has six valence electrons, meaning it needs two more electrons to achieve a stable octet (eight electrons in its outermost shell). By forming two covalent bonds, oxygen shares two pairs of electrons with other atoms, fulfilling the octet rule.
Examples of Oxygen Covalent Bonds:
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Water (H₂O): Oxygen forms two single covalent bonds with two hydrogen atoms. Each hydrogen atom shares one electron with the oxygen atom, completing oxygen's octet and each hydrogen atom's duet (two electrons).
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Oxygen gas (O₂): Two oxygen atoms form a double covalent bond, sharing two pairs of electrons to achieve a stable octet for each atom.
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Carbon dioxide (CO₂): Oxygen forms two double covalent bonds with a carbon atom. Each oxygen atom shares two pairs of electrons with the carbon atom.
Several references support this:
- "Oxygen and other atoms in group 6A (16) obtain an octet by forming two covalent bonds." [Reference 1, Reference 3]
- "Oxygen atoms require 2 electrons; hence form 2 bonds." [Reference 2]
- "Like hydrogen, oxygen exists in its elemental state as a diatomic molecule. Each oxygen has 6 electrons and so need to share to more and so makes two bonds with..." [Reference 4]
- "In the formation of water, an oxygen atom has two unpaired electrons... " [Reference 6]
- "Oxygen has 6 electrons (2 pairs and 2 singles)..." [Reference 7]
- "To achieve a full outer shell, oxygen would need 8 electrons..." [Reference 10]
It's important to note that while oxygen typically forms two covalent bonds, there are exceptions in certain unusual chemical environments or compounds. However, the most common and prevalent number of covalent bonds formed by oxygen is two.
