Problem 15
What is the hybridization of the carbon atom in phosgene, \(\mathrm{Cl}_{2}\) CO? Give a complete description of the \(\sigma\) and \pi bonding in this molecule.
Problem 16
What is the hybridization of the carbon atoms in benzene, \(\overline{\mathrm{C}_{6} \mathrm{H}_{6}}\) ? Describe the \(\sigma\) and \(\pi\) bonding in this compound.
Problem 17
What is the electron-pair and molecular geometry around the central \(S\) atom in thionyl chloride, \(\operatorname{SOCl}_{2} ?\) What is the hybridization of sulfur in this compound?
Problem 18
What is the electron-pair and molecular geometry around the central \(\mathrm{S}\) atom in sulfury \(\mathrm{chloride}, \mathrm{SO}_{2} \mathrm{Cl}_{2} ?\) What is the hybridization of sulfur in this compound?
Problem 24
Platinum hexafluoride is an extremely strong oxidizing agent. It can even oxidize oxygen, its reaction with \(\mathrm{O}_{2}\) giving \(\mathrm{O}_{2}^{+} \mathrm{PtF}_{6}^{-}\). Sketch the molecular orbital energy Level diagram for the \(\mathrm{O}_{2}^{+}\) ion. How many net \(\sigma\) and \(\pi\) bonds does the ion have? What is the oxygen-oxygen bond order? How has the bond order changed on taking away electrons from \(\mathbf{O}_{2}\) to obtain \(\mathbf{O}_{2}^{+}\) ? Is the \(\mathbf{O}_{2}^{+}\) ion paramagnetic?
Problem 25
When sodium and oxygen react, one of the products obtained is sodium peroxide, \(\mathrm{Na}_{2} \mathrm{O}_{2}\). The anion in this compound is the peroxide ion, \(\mathbf{O}_{2}^{2-} .\) Write the electron configuration for this ion in molecular orbital terms, and then compare it with the electron configuration of the \(\mathbf{O}_{2}\) molecule with respect to the following criteria: (a) magnetic character (b) net number of \(\sigma\) and \(\pi\) bonds (c) bond order (d) oxygen-oxygen bond length
Problem 28
Consider the following list of small molecules and ions: \(\mathrm{C}_{2}, \mathrm{O}_{2}^{-}, \mathrm{CN}^{-}, \mathrm{O}_{2}, \mathrm{CO}, \mathrm{NO}, \mathrm{NO}^{+}, \mathrm{C}_{2}^{2-}, \mathrm{OF}^{-} .\) Identify (a) all species that have a bond order of 3 (b) all species that are paramagnetic (c) species that have a fractional bond order
Problem 34
Sketch the Lewis structures of \(\mathrm{C} 1 \mathrm{F}_{2}^{+}\) and \(\mathrm{C} \mathrm{AF}_{2}^{-} .\) What are the electron-pair and molecular geometrics of each ion? Do both have the same \(\mathbf{F}-\mathbf{C} \mathbf{7}-\mathbf{F}\) angle? What hybrid orbital set is used by \(\mathrm{G}\) in each ion?
Problem 35
Sketch the resonance structures for the nitrite ion, \(\mathrm{NO}_{2}^{-} .\) Describe the electron-pair and molecular geometries of the ion. From these geometries, decide on the O-N-O bond angle, the average NO bond order, and the \(\mathrm{N}\) atom hybridization.
Problem 37
Sketch the resonance structures for the \(\mathrm{N}_{2} \mathrm{O}\) molecule. Is the hybridization of the N atoms the same or different in each structure? Describe the orbitals involved in bond formation by the central \(\mathrm{N}\) atom.
