In chemical bonding, the Bond Order indicates the number of chemical bonds existing between a pair of atoms. A higher bond order means the bond is stronger, shorter, and more stable.
According to both the simple Lewis structure and the advanced Molecular Orbital (MO) Theory, the bond order of the Oxygen molecule (O₂) is 2.
Molecule: O₂ (Diatomic Oxygen).
Total Electrons: 16.
Bond Order: 2 (indicates a double bond).
Formula: (Bonding Electrons - Antibonding Electrons) / 2.
Magnetic Nature: Paramagnetic (due to 2 unpaired electrons in antibonding orbitals).
An oxygen atom has 6 valence electrons. To achieve a stable octet (8 electrons), two oxygen atoms must share two pairs of electrons with each other. This creates a double bond (O=O). Since there is a double bond connecting the two atoms, the bond order is simply 2.
For competitive exams (like JEE or NEET), you must calculate bond order using MO Theory. Formula: Bond Order = (Number of Bonding Electrons - Number of Antibonding Electrons) / 2
The MO Theory configuration reveals something the Lewis structure cannot. In the highest energy orbitals (π2px¹ and π2py¹), there are two unpaired electrons. Because of these unpaired electrons, liquid oxygen is actually attracted to a magnetic field. This property is called paramagnetism.
The bond order of the O2 molecule is 2, which corresponds to the double bond between the two oxygen atoms.
Subtract the number of antibonding electrons from the number of bonding electrons, and divide the result by 2.
O2 is paramagnetic. Molecular Orbital Theory shows that it contains two unpaired electrons in its anti-bonding pi orbitals.
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