A diatomic molecule with a triple covalent bond is O2.
The correct answer and explanation is:
Actually, the molecule O2 (oxygen) does not have a triple covalent bond. O2 has a double covalent bond between the two oxygen atoms.
In a diatomic molecule like O2, the two oxygen atoms share electrons to achieve a stable electron configuration, usually by forming covalent bonds. A single covalent bond involves the sharing of one pair of electrons between two atoms. In O2, each oxygen atom contributes two electrons, and these two pairs of electrons form a double covalent bond, making the total number of shared electrons four.
A triple covalent bond, as seen in nitrogen gas (N2), involves the sharing of three pairs of electrons (six electrons in total). This bond is stronger and shorter than a double bond due to the additional shared electrons. In contrast, the double bond in O2 is relatively weaker and longer than a triple bond.
The bond strength and length are a result of the type of overlap between atomic orbitals. In O2, the two oxygen atoms each have a half-filled p-orbital, and these orbitals overlap to form a bonding molecular orbital. This overlap accounts for the double bond.
In summary, O2 has a double covalent bond, not a triple bond. A triple bond is characteristic of molecules like nitrogen (N2), where three pairs of electrons are shared between the two atoms.