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Ch.8 - Basic Concepts of Chemical Bonding
Brown - Chemistry: The Central Science 14th Edition
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Tutti i libri di testoBrown 14th EditionCh.8 - Basic Concepts of Chemical BondingProblema 55
Capitolo 8, Problema 55

Predict the ordering, from shortest to longest, of the bond lengths in CO, CO2, and CO32- .

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Identify the types of bonds in each molecule or ion. CO has a triple bond, CO2 has two double bonds between carbon and oxygen, and CO32- (carbonate ion) has resonance structures typically represented with one double bond and two single bonds between carbon and oxygen.
Recall that generally, triple bonds are shorter than double bonds, and double bonds are shorter than single bonds due to the increasing number of shared electrons pulling the bonded atoms closer together.
Consider the effect of resonance in CO32-. Resonance can cause the actual bond lengths to be an average of the different forms, potentially making the bonds in CO32- shorter than a typical single bond but not as short as a double bond.
Compare the bond types and the effects of resonance to predict the relative bond lengths. Since CO has a triple bond, it should have the shortest bond length. CO2 with double bonds should have a longer bond length than CO but shorter than CO32-.
Order the molecules and ion from shortest to longest bond length based on the analysis: CO (shortest), CO2, CO32- (longest).

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Bond Length

Bond length is the distance between the nuclei of two bonded atoms. It is influenced by the type of bond (single, double, or triple) and the size of the atoms involved. Generally, shorter bonds correspond to stronger interactions between atoms, while longer bonds indicate weaker interactions.
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Average Bond Order

Bond Order

Bond order refers to the number of chemical bonds between a pair of atoms. It is calculated as the difference between the number of bonding and antibonding electrons divided by two. Higher bond orders typically result in shorter bond lengths due to increased electron density between the nuclei, leading to stronger attractions.
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Average Bond Order

Resonance Structures

Resonance structures are different ways of drawing the same molecule that illustrate the delocalization of electrons. In molecules like CO3^2-, resonance indicates that the actual bond lengths are an average of the different structures. This delocalization can affect bond lengths, making them longer than expected for a single bond but shorter than for a double bond.
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Resonance Structures
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Domanda del libro di testo

Consider the formate ion, HCO2-, which is the anion formed when formic acid loses an H+ ion. The H and the two O atoms are bonded to the central C atom. (c) Would you predict that the C—O bond lengths in the formate ion would be longer or shorter relative to those in CO2?

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Domanda del libro di testo

Mothballs are composed of naphthalene, C10H8, a molecule that consists of two six-membered rings of carbon fused along an edge, as shown in this incomplete Lewis structure:(a) Draw all of the resonance structures of naphthalene. How many are there?

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

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Based on Lewis structures, predict the ordering, from shortest to longest, of N¬O bond lengths in NO+, NO2-, and NO3-.

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Domanda del libro di testo

Consider the formate ion, HCO2-, which is the anion formed when formic acid loses an H+ ion. The H and the two O atoms are bonded to the central C atom. (b) Are resonance structures needed to describe the structure?

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