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Ch.8 - Basic Concepts of Chemical Bonding
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 14th EditionCh.8 - Basic Concepts of Chemical Bonding문제 53c
8장, 문제 53c

(c) What would you predict for the lengths of the bonds in NO2- relative to N¬O single bonds and double bonds?

검증된 단계별 안내
1
Understand the structure of the nitrite ion (NO2-). It consists of a nitrogen atom bonded to two oxygen atoms, with one of these bonds being a double bond and the other a single bond, due to resonance.
Recognize that resonance in NO2- means that the actual structure is a hybrid of the two resonance forms, where the double bond and single bond are averaged over the two N-O bonds.
Recall that in resonance structures, the bond lengths are intermediate between the lengths of a single bond and a double bond. This is because the electron density is delocalized over the entire molecule.
Compare the bond lengths: A typical N-O single bond is longer than a typical N-O double bond. Therefore, the bond lengths in NO2- will be shorter than a single bond but longer than a double bond.
Conclude that the bond lengths in NO2- are equal due to resonance and are intermediate between the lengths of a N-O single bond and a N-O double bond.

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주요 개념

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Bond Order

Bond order is a measure of the number of chemical bonds between a pair of atoms. It is calculated as the difference between the number of bonding electrons and the number of antibonding electrons, divided by two. In the case of nitrogen dioxide (NO2) and its anion (NO2-), the bond order helps predict the bond lengths, as higher bond orders typically correlate with shorter bond lengths due to increased electron density between the bonded atoms.
추천 영상:
가이드 코스
00:36
Average Bond Order

Resonance Structures

Resonance structures are different ways of drawing the same molecule that illustrate the delocalization of electrons. In NO2-, resonance indicates that the actual structure is a hybrid of these forms, leading to bond lengths that are intermediate between single and double bonds. This concept is crucial for understanding the bond lengths in NO2- as it affects the distribution of electron density and the effective bond order.
추천 영상:
가이드 코스
01:42
Resonance Structures

Bond Length Trends

Bond length is influenced by the type of bond formed between atoms; single bonds are generally longer than double bonds due to the increased electron sharing in double bonds. In NO2-, the bond lengths can be predicted to be shorter than a typical N-O single bond but longer than a double bond, reflecting the resonance and partial double bond character present in the anion.
추천 영상:
가이드 코스
00:38
Periodic Trends
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