Oxygen atoms can combine with ozone to form oxygen: O3(g)+O(g) → 2 O2(g) Δr H^∘=-392 k

step 1 To calculate the bond energy ozone, let us first write the Lewis structure for all the compounds

Oxygen atoms can combine with ozone to form oxygen: ...

Oxygen atoms can combine with ozone to form oxygen: $$\begin{array}{l} \mathrm{O}_{3}(\mathrm{g})+\mathrm{O}(\mathrm{g}) \rightarrow 2 \mathrm{O}_{2}(\mathrm{g}) \\ \Delta_{\mathrm{r}} H^{\circ}=-392 \mathrm{kJ} / \mathrm{mol}-\mathrm{rxn} \end{array}$$ Using $\Delta_{r} H^{\circ}$ and the bond dissociation enthalpy data in Table $8.9,$ estimate the bond dissociation enthalpy for the oxygen-oxygen bond in ozone, $\mathrm{O}_{3} .$ How does your estimate compare with the energies of an $\mathrm{O}-\mathrm{O}$ single bond and an $\mathrm{O}=\mathrm{O}$ double bond? Does the oxygenoxygen bond dissociation enthalpy in ozone correlate with its bond order?

Oxygen atoms can combine with ozone to form oxygen:
$$\begin{array}{l}
\mathrm{O}_{3}(\mathrm{g})+\mathrm{O}(\mathrm{g}) \rightarrow 2 \mathrm{O}_{2}(\mathrm{g}) \\
\Delta_{\mathrm{r}} H^{\circ}=-392 \mathrm{kJ} / \mathrm{mol}-\mathrm{rxn}
\end{array}$$
Using $\Delta_{r} H^{\circ}$ and the bond dissociation enthalpy data in Table $8.9,$ estimate the bond dissociation enthalpy for the oxygen-oxygen bond in ozone, $\mathrm{O}_{3} .$ How does your estimate compare with the energies of an $\mathrm{O}-\mathrm{O}$ single bond and an $\mathrm{O}=\mathrm{O}$ double bond? Does the oxygenoxygen bond dissociation enthalpy in ozone correlate with its bond order?

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Key Concepts

Bond Order

Bond order refers to the number of chemical bonds between a pair of atoms and is often correlated with bond strength. Higher bond orders typically indicate stronger, shorter bonds; however, discrepancies can arise in molecules with resonance or delocalized electrons, where the bond dissociation enthalpy might not scale directly with the nominal bond order.

Hess's Law

Hess's Law states that the total enthalpy change for a chemical reaction is independent of the pathway between the initial and final states. This principle allows the use of known bond dissociation enthalpies and reaction enthalpies to construct thermodynamic cycles in order to estimate unknown bond energies.

Bond Dissociation Enthalpy

Bond dissociation enthalpy is the amount of energy needed to break a specified bond in one mole of gaseous molecules and is an indicator of the bond strength. It serves as a useful measure for comparing different types of chemical bonds, such as single, double, or resonance-influenced bonds.

Reaction Enthalpy

Reaction enthalpy, often determined experimentally, represents the net energy change during a chemical reaction. It reflects the overall exothermic or endothermic nature of the reaction and can be used, alongside bond energies, to estimate unknown bond dissociation energies by applying energy conservation principles.

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