1. What is Bond Order?

Bond order is a measurement of the number of electron pairs shared between two atoms in a chemical bond. For O₂ (oxygen molecule), the bond order helps determine its stability and magnetic properties.

2. How Does the Calculator Work?

The calculator uses the molecular orbital theory formula:

For O₂ specifically:

• Total valence electrons: 12 (6 from each oxygen atom)
• Bonding electrons: 8 (σ2s², σ*2s², σ2p², π2p⁴)
• Antibonding electrons: 4 (π*2p²)
• Bond order = (8 - 4)/2 = 2

Explanation: Higher bond order indicates stronger and shorter bonds. O₂ has a bond order of 2, representing a double bond.

3. Importance of Bond Order Calculation

Details: Bond order helps predict bond length, bond energy, and magnetic properties (paramagnetism in O₂ due to unpaired electrons).

4. Using the Calculator

Tips: Enter the number of bonding and antibonding electrons based on molecular orbital configuration. For O₂, these are typically 8 and 4 respectively.

5. Frequently Asked Questions (FAQ)

Q1: Why is O₂ paramagnetic despite being a stable molecule?
A: The molecular orbital diagram shows two unpaired electrons in the π* antibonding orbitals, making O₂ paramagnetic.

Q2: What does bond order tell us about bond strength?
A: Higher bond order means stronger bonds (more shared electron pairs) and shorter bond lengths.

Q3: Can bond order be a fraction?
A: Yes, in molecules like O₂⁻ (superoxide) the bond order is 1.5, indicating intermediate strength between single and double bonds.

Q4: How does bond order relate to molecular vibrations?
A: Higher bond order correlates with higher vibrational frequencies (stronger bonds vibrate faster).

Q5: What's the bond order in O₂⁺?
A: Removing one antibonding electron increases bond order to 2.5, making the bond stronger than in neutral O₂.