Question

The heats of combustion of two constitutional isomers are the same when estimated from average bond energies, but they are different when determined experimentally. Why?

Short answer

Answer: When estimated from average bond energies, the heats of combustion only account for the energies of specific bond types and do not consider other factors, such as molecular structure, resonance, and steric hindrance. As a result, the estimated heats of combustion for two constitutional isomers may be the same. However, when determined experimentally, these factors are taken into consideration, leading to different heats of combustion for the two isomers.

Step-by-step solution

Understand the terms involved

Constitutional isomers are compounds with the same molecular formula but differ in the connectivity of their atoms. The heats of combustion refer to the amount of heat released during the combustion of a substance.

Understand average bond energies

Average bond energies are the average values of the bond dissociation energy for a specific type of bond in a variety of molecules. These values are used to estimate the heats of combustion using the bond energy calculations. However, these average bond energies do not take into account the molecular structure, resonance, or other factors that may influence the stability of the molecule and the energy released during combustion.

Understand the factors affecting heats of combustion experimentally

Experimentally determined heats of combustion consider many factors other than just bond energies. These factors include molecular structure, resonance, steric hindrance, and other chemical factors that affect the stability of the molecule and the energy it releases during combustion.

Reason for the difference in heats of combustion

Since average bond energies only account for the energies of specific bond types and do not consider the molecular structure or other factors, the estimated heats of combustion for two constitutional isomers may be the same. However, when determined experimentally, these factors are considered, and hence the heats of combustion for two constitutional isomers are different.

Key concepts

Heats of Combustion

The heat of combustion is a measure of the energy released as heat when a compound undergoes complete combustion with oxygen. It's a vital concept in understanding chemical thermodynamics and energy changes in reactions.
When discussing constitutional isomers, these are molecules that share the same molecular formula but differ in the arrangement of atoms. Thus, their heats of combustion may appear similar if only average bond energies are considered. However, the experimental measurement often shows differences.
Several factors contribute to these differences:

• Molecular Structure: The actual spatial arrangement of atoms can affect how much energy is stored in the molecule and released during combustion.
• Resonance and Stability: Molecules with higher stability due to resonance will have different energy profiles.
• Steric Hindrance: How atoms are arranged spatially can impact how easily they react and combust.

Taking these factors into account is why experimentally determined heats of combustion can differ from theoretical predictions based only on bond energies.

Average Bond Energies

Average bond energies provide an estimate of the strength of chemical bonds in a variety of molecules. These values are derived by taking an average of the bond dissociation energies required to break a particular bond over different molecules.
Though useful, these averages carry inherent limitations:

• They don’t account for specific molecular environments, which can alter bond strength.
• Such values ignore the influence of conjugation and resonance which stabilize molecules differently.
• They provide a rough estimate and not an exact measure for the energy profile of a specific molecule.

In the context of combustion, using average bond energies helps make preliminary energy estimates, though often requires adjustments based on molecular specifics for accuracy.

Bond Dissociation Energy

Bond dissociation energy (BDE) refers to the energy required to break a specific chemical bond in a molecule to form isolated atoms. It varies widely depending on the bond and the molecular context, providing a more detailed understanding than average bond energies.

• BDEs provide insight into the strength and stability of specific bonds within unique chemical environments.
• The measurement of BDE can inform predictions about reaction pathways, particularly regarding stability and reactivity.
• Unlike average bond energies, BDE can be particularly valuable in analyzing subtle differences in constitutional isomers.

Such detailed insight is crucial when considering factors leading to differences in experimental versus theoretical heats of combustion.

Molecular Stability

Molecular stability plays a crucial role in determining chemical and physical properties, including energy release during combustion. Several elements contribute to a molecule's stability:

• Constitutional Arrangement: Atoms arranged in more stable configurations will typically release less energy upon combustion due to lesser initial potential energy.
• Resonance Effects: Resonance can greatly enhance a molecule’s stability, impacting its energy profile.
• Internal Strain and Steric Effects: Bonds that endure less strain and steric hindrance tend to be more stable, affecting both reactiveness and energy release.

Thus, although two constitutional isomers might share the same formula, diversities in stability can lead to different heats of combustion when evaluated experimentally.