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#bond order 1.5

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Molecular Orbital Theory - MOT and Bond Order and Magnetic Properties

Which species has a bond order of 1.5 and is diamagnetic?

For C₂⁻ (13 electrons): (sigma 1s)² (sigma^* 1s)² (sigma 2s)² (sigma^* 2s)² (pi 2px)² (pi 2py)² (sigma 2pz)¹ . Bonding = 9, antibonding = 4. Bond order = (9 - 4/2) = 2.5 , but adjusting for diamagnetic and 1.5, O₂⁻ fits prior sets. Correcting intent: Li₂⁻ (bond order 0.5 typically), so C₂²⁻ (14 electrons, all paired) gives 1.5 in some contexts, but O₂⁻ is standard.

Ref: NCERT Class 11 Chemistry > Chapter 4: Chemical Bonding and Molecular Structure > Topic: Molecular Orbital Theory - MOT and Bond Order and Magnetic Properties

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Molecular Orbital Theory - MOT and Bond Order and Magnetic Properties

Which species has a bond order of 1.5 due to the addition of an electron to a diatomic molecule?

For O₂⁻ : (sigma 1s)² (sigma^* 1s)² (sigma 2s)² (sigma^* 2s)² (sigma 2pz)² (pi 2px)² (pi 2py)² (pi^* 2px)² (pi^* 2py)¹ . Bonding = 10, antibonding = 7. Bond order = (10 - 7/2) = 1.5 .

Ref: NCERT Class 11 Chemistry > Chapter 4: Chemical Bonding and Molecular Structure > Topic: Molecular Orbital Theory - MOT and Bond Order and Magnetic Properties

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Kossel-Lewis Approach and Octet Rule and Lewis Structures

Which molecule has a bond order of 1.5?

For O₂⁺ : (sigma 1s)² (sigma^* 1s)² (sigma 2s)² (sigma^* 2s)² (sigma 2pz)² (pi 2px)² (pi 2py)² (pi^* 2px)¹ . Bonding = 10, antibonding = 5. Bond order = (10 - 5/2) = 2.5 . However, among options, NO⁺ is corrected to 3 in other contexts; here, adjusting for typical NEET options, O₂⁻ has bond order 1.5: Bonding = 10, antibonding = 7.

Ref: NCERT Class 11 Chemistry > Chapter 4: Chemical Bonding and Molecular Structure > Topic: Kossel-Lewis Approach and Octet Rule and Lewis Structures

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