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Assuming that Hund's rule is violated, the bond order and magnetic nature of the diatomic molecule B2 is
(2010, Single Option Correct Type)
- a)1 and diamagnetic
- b)0 and diamagnetic
- c)1 and paramagnetic
- d)0 and paramagnetic
Correct answer is option 'A'. Can you explain this answer?
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Verified Answer
Assuming that Hund's rule is violated, the bond order and magnetic...
For molecules lighter than O2, the increasing ord er order of energies of molecular orbitals is :
Where, π2py and π2pz are degenerate molecular orbitals, first singly occupied and then pairing starts if Hund’s rule is obeyed. If Hund’s rule is violated in B2, electronic arrangement would be :
No unpaired electron-diamagnetic.
Most Upvoted Answer
Assuming that Hund's rule is violated, the bond order and magnetic...
To determine the bond order and magnetic nature of the diatomic molecule B2, we need to consider the electronic configuration of the molecule.
The atomic number of boron is 5, so the electronic configuration of a single boron atom is 1s^2 2s^2 2p^1. When two boron atoms combine to form a diatomic molecule, they share their valence electrons to form molecular orbitals.
- Hund's Rule violation:
Hund's Rule states that electrons occupy orbitals of the same energy level singly before pairing up. However, in the case of boron, the 2p orbital is not completely filled in the ground state configuration. This violates Hund's Rule as the electrons should first occupy separate orbitals before pairing up.
- Formation of molecular orbitals:
When two boron atoms combine, they form molecular orbitals by combining their atomic orbitals. The 2s orbitals of each boron atom combine to form two molecular orbitals: one bonding (σ) and one antibonding (σ*). The 2p orbitals also combine to form two molecular orbitals: one bonding (π) and one antibonding (π*).
- Bond order calculation:
The bond order is given by the difference between the number of bonding and antibonding electrons divided by 2. In the case of B2, the molecular orbital diagram can be represented as:
σ2s^2 σ*2s^2 π2p^2 π*2p^0
The number of bonding electrons is 4 (2 from σ2s and 2 from π2p), and the number of antibonding electrons is 2 (from σ*2s). Therefore, the bond order is (4 - 2) / 2 = 1.
- Magnetic nature:
Diamagnetic substances have all their electrons paired up, while paramagnetic substances have unpaired electrons.
Since the bond order is 1, this indicates that there are unpaired electrons in the molecule. Therefore, the diatomic molecule B2 is paramagnetic.
- Conclusion:
The correct answer is option A: The bond order of B2 is 1, and it is paramagnetic.
The atomic number of boron is 5, so the electronic configuration of a single boron atom is 1s^2 2s^2 2p^1. When two boron atoms combine to form a diatomic molecule, they share their valence electrons to form molecular orbitals.
- Hund's Rule violation:
Hund's Rule states that electrons occupy orbitals of the same energy level singly before pairing up. However, in the case of boron, the 2p orbital is not completely filled in the ground state configuration. This violates Hund's Rule as the electrons should first occupy separate orbitals before pairing up.
- Formation of molecular orbitals:
When two boron atoms combine, they form molecular orbitals by combining their atomic orbitals. The 2s orbitals of each boron atom combine to form two molecular orbitals: one bonding (σ) and one antibonding (σ*). The 2p orbitals also combine to form two molecular orbitals: one bonding (π) and one antibonding (π*).
- Bond order calculation:
The bond order is given by the difference between the number of bonding and antibonding electrons divided by 2. In the case of B2, the molecular orbital diagram can be represented as:
σ2s^2 σ*2s^2 π2p^2 π*2p^0
The number of bonding electrons is 4 (2 from σ2s and 2 from π2p), and the number of antibonding electrons is 2 (from σ*2s). Therefore, the bond order is (4 - 2) / 2 = 1.
- Magnetic nature:
Diamagnetic substances have all their electrons paired up, while paramagnetic substances have unpaired electrons.
Since the bond order is 1, this indicates that there are unpaired electrons in the molecule. Therefore, the diatomic molecule B2 is paramagnetic.
- Conclusion:
The correct answer is option A: The bond order of B2 is 1, and it is paramagnetic.
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Community Answer
Assuming that Hund's rule is violated, the bond order and magnetic...
For molecules lighter than O2, the increasing ord er order of energies of molecular orbitals is :
Where, π2py and π2pz are degenerate molecular orbitals, first singly occupied and then pairing starts if Hund’s rule is obeyed. If Hund’s rule is violated in B2, electronic arrangement would be :
No unpaired electron-diamagnetic.
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Assuming that Hund's rule is violated, the bond order and magnetic nature of the diatomic molecule B2 is(2010, Single Option Correct Type)a)1 and diamagneticb)0 and diamagneticc)1 and paramagneticd)0 and paramagneticCorrect answer is option 'A'. Can you explain this answer?
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