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Question
How do you express the bond strength in terms of bond order?
Solution 1
Bond strength represents the extent of bonding between two atoms forming a molecule. The larger the bond energy, the stronger is the bond and the greater is the bond order.
Solution 2
Bond strength is directly proportional to the bond order. Greater the bond order, more is the bond strength.
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RELATED QUESTIONS
Compare the relative stability of the following species and indicate their magnetic properties;
`"O"_2, "O"_2^+, "O"_2^-`(superoxide), `"O"_2^(2-)`(peroxide)
Calculate the bond order of N2, O2, `"O"_2^+`and `"O"_2^-`?
What is meant by the term bond order?
Which of the following options represents the correct bond order?
Which of the following have identical bond order?
(i) \[\ce{CN-}\]
(ii) \[\ce{NO+}\]
(iii) \[\ce{O^{-}2}\]
(iv) \[\ce{O^{2-}2}\]
Species having same bond order are:
(i) \[\ce{N2}\]
(ii) \[\ce{N^{-}2}\]
(iii) \[\ce{F^{+}2}\]
(iv) \[\ce{O^{-}2}\]
Using molecular orbital theory, compare the bond energy and magnetic character of \[\ce{O^{+}2}\] and \[\ce{O^{-}2}\] species.
What is the effect of the following processes on the bond order in \[\ce{N2}\] and \[\ce{O2}\]?
(i) \[\ce{N2 -> N^{+}2 + e-}\]
(ii) \[\ce{O2 -> O^{+}2 + e-}\]
Match the species in Column I with the bond order in Column II.
| Column I | Column II |
| (i) \[\ce{NO}\] | (a) 1.5 |
| (ii) \[\ce{CO}\] | (b) 2.0 |
| (iii) \[\ce{O^{-}2}\] | (c) 2.5 |
| (iv) \[\ce{O2}\] | (d) 3.0 |
Which of the following pair is expected to have the same bond order?
In which of the following pairs, the two species have identical bond order?
