Question:
Which of the following statement is incorrect about bond order?
Which of the following statement is incorrect about bond order?
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Triple bond (BO=3) has highest bond enthalpy and shortest bond length compared to double (BO=2) or single (BO=1) bond.
Updated On: Apr 24, 2026
- Bond order is the number of bonds between the two atoms in a molecule.
- Isoelectronic molecules and ions have identical bond orders.
- Bond enthalpy decreases with increase in bond order.
- Bond length decreases with increase in bond order.
- Bond enthalpy increases with increase in bond order.
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Verified By Collegedunia
The Correct Option is C
Solution and Explanation
Step 1: Understanding the Concept:
Bond order indicates bond strength. Higher bond order means shorter bond length and higher bond enthalpy.
Step 2: Detailed Explanation:
(A) Correct: Bond order = (Nb - Na)/2.
(B) Correct: Isoelectronic species have same electronic configuration, hence same bond order.
(C) Incorrect: Bond enthalpy increases with bond order.
(D) Correct: Bond length decreases as bond order increases.
(E) Correct: Bond enthalpy increases with bond order.
Step 3: Final Answer:
The incorrect statement is that bond enthalpy decreases with increase in bond order.
Bond order indicates bond strength. Higher bond order means shorter bond length and higher bond enthalpy.
Step 2: Detailed Explanation:
(A) Correct: Bond order = (Nb - Na)/2.
(B) Correct: Isoelectronic species have same electronic configuration, hence same bond order.
(C) Incorrect: Bond enthalpy increases with bond order.
(D) Correct: Bond length decreases as bond order increases.
(E) Correct: Bond enthalpy increases with bond order.
Step 3: Final Answer:
The incorrect statement is that bond enthalpy decreases with increase in bond order.
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