Question:
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:
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:
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:
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Remember: Higher bond order implies stronger bonds and shorter bond lengths; a bond order of zero means the molecule is unstable.
Updated On: May 10, 2025
- Both Statement I and Statement II are false
- Statement I is true but Statement II is false
- Statement I is false but Statement II is true
- Both Statement I and Statement II are true
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The Correct Option is A
Solution and Explanation
Statement I: Bond order is an indicator of stability in molecules. A bond order of zero means there is no bond formation between the two atoms, hence the molecule cannot exist in a stable form.
Therefore, this statement is false.
Statement II: As bond order increases, the number of bonding electrons increases, strengthening the bond and pulling the atoms closer together.
Thus, bond length decreases with increasing bond order. Hence, this statement is also false.
Thus, both the statements are incorrect.
Therefore, this statement is false.
Statement II: As bond order increases, the number of bonding electrons increases, strengthening the bond and pulling the atoms closer together.
Thus, bond length decreases with increasing bond order. Hence, this statement is also false.
Thus, both the statements are incorrect.
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