Chapter 9: Problem 102
Arrange the following from lowest to highest ionization energy: $\mathrm{O}, \mathrm{O}_{2}, \mathrm{O}_{2}^{-}, \mathrm{O}_{2}^{+} .$ Explain your answer.
Chapter 9: Problem 102
Arrange the following from lowest to highest ionization energy: $\mathrm{O}, \mathrm{O}_{2}, \mathrm{O}_{2}^{-}, \mathrm{O}_{2}^{+} .$ Explain your answer.
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Get started for freeFor each of the following molecules or ions that contain sulfur, write the Lewis structure(s), predict the molecular structure (including bond angles), and give the expected hybrid orbitals for sulfur. $$ \begin{array}{l}{\text { a. } \mathrm{SO}_{2}} \\ {\text { b. } \mathrm{SO}_{3}}\end{array} $$ $$ \text {c} \mathrm{s}_{2} \mathrm{O}_{3}^{2-}\left[\begin{array}{c}{\mathrm{o}} \\\ {\mathrm{s}-\mathrm{s}-\mathrm{o}} \\ {\mathrm{o}} \\\ {\mathrm{o}}\end{array}\right]^{2-} $$ e. \(\mathrm{SO}_{3}^{2-}\) f. \(\mathrm{SO}_{4}^{2-}\) g. \(\mathrm{SF}_{2}\) h. \(\mathrm{SF}_{4}\) i. \(\mathrm{SF}_{6}\) j. \(\mathrm{F}_{3} \mathrm{S}-\mathrm{SF}\) k. \(\mathrm{SF}_{5}+\)
Show how two 2\(p\) atomic orbitals can combine to form a \(\sigma\) or a \(\pi\) molecular orbital.
Complete the following resonance structures for \(\mathrm{POCl}_{3}\) a. Would you predict the same molecular structure from each resonance structure? b. What is the hybridization of P in each structure? c. What orbitals can the P atom use to form the \(\pi\) bond in structure \(\mathrm{B}\) ? d. Which resonance structure would be favored on the basis of formal charges?
Using the molecular orbital model, write electron configurations for the following diatomic species and calculate the bond orders. Which ones are paramagnetic? Place the species in order of increasing bond length and bond energy. $$ \text {a} \mathrm{CN}^{+} \quad \text { b. CN } \quad \text { c. } \mathrm{CN}^{-} $$
Values of measured bond energies may vary greatly depending on the molecule studied. Consider the following reactions: $$ \begin{array}{ll}{\mathrm{NCl}_{3}(g) \longrightarrow \mathrm{NCl}_{2}(g)+\mathrm{Cl}(g)} & {\Delta H=375 \mathrm{kJ} / \mathrm{mol}} \\ {\mathrm{ONCI}(g) \longrightarrow \mathrm{NO}(g)+\mathrm{Cl}(g)} & {\Delta H=158 \mathrm{kJ} / \mathrm{mol}}\end{array} $$ Rationalize the difference in the values of \(\Delta H\) for these reactions, even though each reaction appears to involve only the breaking of one \(\mathrm{N}-\mathrm{Cl}\) bond. (Hint: Consider the bond order of the NO bond in ONCl and in NO.)
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