Recall that the bond energy determines the strength of the bond in a compound.
▪ the higher the bond energy, the higher is the energy required to break up the molecule/compound into its individual atoms
▪ higher bond energy → higher bond strength
The bond strength also determines the distance between the atoms
▪ the stronger the bonds, the closer or the smaller the distance between the atoms
▪ higher bond strength → shorter bond length
The bond length can also be determined by the type of bond between the atoms
▪ single bond (–X–X–) → longest bond length
▪ double bond (–X=X–) → shorter than a single bond
▪ triple bond (–X≡X–) → shortest bond length
▪ smaller atomic radius → shorter bond length
The Lewis Structures of the given compounds are:
Place the species below in order of the shortest to the longest nitrogen–oxygen bond.
H2NOH, N2O, NO+, NO2-, NO3-
(H2NOH exists as H2N—OH.)
Frequently Asked Questions
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Our tutors have indicated that to solve this problem you will need to apply the Bond Energy concept. If you need more Bond Energy practice, you can also practice Bond Energy practice problems.
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Based on our data, we think this problem is relevant for Professor Santhanago's class at Kean University.
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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.