Considering the bond lengths of N₂ and O₂, which statement is correct?
-
A.
Bond length of N₂ is greater than O₂.
-
B.
Bond length of O₂ is greater than N₂.
-
C.
Bond lengths of N₂ and O₂ are equal.
-
D.
Bond length of N₂ is double that of O₂.
Correct Answer:
B. Bond length of O₂ is greater than N₂.
Explanation:
The bond length of a molecule is determined by its bond order, which represents the number of chemical bonds between a pair of atoms. Nitrogen (N2) possesses a triple bond, resulting in a bond order of 3, while oxygen (O2) has a double bond, giving it a bond order of 2. Generally, a higher bond order correlates with a stronger pull between the atomic nuclei, leading to a shorter distance between them. Consequently, because nitrogen has a higher bond order than oxygen, its bond length is shorter. Therefore, the bond length of O2 is greater than that of N2.
Click below to open Discussion & Feedback
0 Issues
Please
login to comment or Report Issues.