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Given below are two statements:Statement I: A hypothetical diatomic molecule with bond order zero is quite stable.Statement II: As bond order increases, the bond length increases.In the light of the above statements, choose the most appropriate answer from the options given below:

  1. A
    Both Statement I and Statement II are true
  2. B
    Both Statement I and Statement II are false
  3. C
    Statement I is true but Statement II is false
  4. D
    Statement I is false but Statement II is true

Solution & Step-by-step Explanation

1. Statement I is false: A bond order of zero means no net bonding forces exist between the atoms, so the molecule is unstable and does not exist (e.g., ).2. Statement II is false: Bond order is inversely proportional to bond length. As bond order increases (single double triple), the bond length decreases.

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Given below are two statements:Statement I: A hypothetical diatomic molecule with bond order zero is quite stable.Statement II: As bond order increases, the bond length increases.In the light of the above statements, choose the most appropriate answer from the options given below:
A
Both Statement I and Statement II are true
B
Both Statement I and Statement II are false
C
Statement I is true but Statement II is false
D
Statement I is false but Statement II is true

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Chemical BondingMolecular Orbital TheoryBond Order

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