Question
Use the bond enthalpy data below to explain why oxygen exists as $\mathrm{O}_{2}$ molecules and not $\mathrm{O}_{\mathrm{B}}$ rings, analogous to those formed by sulfur. (Section 27.5)
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It is the change in enthalpy during the formation of one mole of a substance from its constituent elements, with all substances in their standard states. Show more…
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Use Lewis structures and other information to explain the observation that (a) the oxygen-to-oxygen bond lengths in $\mathrm{O}_{2}, \mathrm{O}_{3}$ and $\mathrm{H}_{2} \mathrm{O}_{2}$ are $121,128,$ and $148 \mathrm{pm},$ respectively. (b) the oxygen-to-oxygen bond length of $\mathrm{O}_{2}$ is $121 \mathrm{pm}$ and for $\mathrm{O}_{2}^{+}$ is $112 \mathrm{pm}$. Why is the bond length for $\mathrm{O}_{2}^{+}$ so much shorter than for $\mathrm{O}_{2} ?$
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