Chapter 8: Q9 E (page 446)
Why is the concept of hybridization required in valence bond theory?
Hybridization is necessary to determine the molecular geometry of complex.
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Calculate the bond order for an ion with this configuration: \({\left( {{{\bf{\sigma }}_{{\bf{2s}}}}} \right)^{\bf{2}}}{\left( {{\bf{\sigma }}_{{\bf{2s}}}^{\bf{*}}} \right)^{\bf{2}}}{\left( {{{\bf{\sigma }}_{{\bf{2px}}}}} \right)^{\bf{2}}}{\left( {{{\bf{\pi }}_{{\bf{2py}}}}{\bf{,}}{{\bf{\pi }}_{{\bf{2pz}}}}} \right)^{\bf{4}}}{\left( {{\bf{\pi }}_{{\bf{2py}}}^{\bf{*}}{\bf{,\pi }}_{{\bf{2pz}}}^{\bf{*}}} \right)^{\bf{3}}}\).
The main component of air is N2. From the molecular orbital diagram of N2, predict its bond order and whether it is diamagnetic or paramagnetic.
Explain why N22+ is diamagnetic, while O24+, which has the same number of valence electrons, is paramagnetic.
Draw a curve that describes the energy of a system with H and CI atoms at varying distances. Then, find the minimum energy of this curve two ways.
(a) Use the bond energy found in Table 8.1 to calculate the energy for one single HCl bond (Hint: How many bonds are in a mole?)
(b) Use the enthalpy of reaction and the bond energies for \({{\rm{H}}_{\rm{2}}}\)and \({\rm{C}}{{\rm{l}}_{\rm{2}}}\)to solve for the energy of one mole of \({\rm{HCl}}\)bonds.
\({{\text{H}}_{\text{2}}}{\text{(g) + C}}{{\text{l}}_{\text{2}}}{\text{(g)}} \rightleftharpoons {\text{2HCl(g)}}\) ฮHยฐrxn = โ184.7 kJ/mol
Another acid in acid rain is nitric acid, HNO3, which is produced by the reaction of nitrogen dioxide, NO2, with atmospheric water vapor. What is the hybridization of the nitrogen atom in NO2? (Note: the lone electron on nitrogen occupies a hybridized orbital just as a lone pair would.)
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