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General Chemistry: Principles and Modern Applications, Loose Leaf Version (11th Edition)
- The cations O2+ and N2+ are formed when molecules of O2 and N2 are subjected to intense, high-energy solar radiation in Earths upper atmosphere. Write the electron configuration for O2+. Predict its bond order and magnetic behavior.arrow_forwardThe molecular structure shown is of one form of glucose, C6H12O6 Glucose can be oxidized to carbon dioxide and water according to the equation C6H12O6(S) + 6 O2(g)6 CO2(g) + 6 H2O(g) (a) Using the method described in Section 6-6a for estimating enthalpy changes from bond energies, estimate rH for the oxidation of this form of glucose. Make a list of all bonds broken and all bonds formed in this process. (b) Compare your result with the experimental value of 2816 kJ/mol for combustion of glucose. Why might there be a difference between this value and the one you calculated in part (a)?arrow_forwardUsing the bond dissociation enthalpies in Table 8.8, estimate the enthalpy of combustion of gaseous methane, CH4, to give water vapor and carbon dioxide gas.arrow_forward
- Write Lewis structures for CO32, HCO3, and H2CO3. When acid is added to an aqueous solution containing carbonate or bicarbonate ions, carbon dioxide gas is formed. We generally say that carbonic acid (H2C03) is unstable. Use bond energies to estimate E for the reaction (in the gas phase) H2CO3CO2+H2O Specify a possible cause for the instability of carbonic acid.arrow_forwardUsing a table of average bond enthalpies. Table 6.2 ( Sec. 6-6b), estimate the enthalpy change for the industrial synthesis of methanol by the catalyzed reaction of carbon monoxide with hydrogen.arrow_forwardFor the hypothetical cyclic square hydrogen molecular di-cation (H42+), list all electrostatic pairwise interactions including their signs and contributions to stabilising and de-stabilising the molecular structurearrow_forward
- Use the following data for magnesium fluoride to estimate ΔE for the reaction: Mg (s) + F2 (g) → MgF2 (s) ΔE = ? Lattice energy -2913 kJ/mol First ionization energy of Mg 735 kJ/mol Second ionization energy of Mg 1445 kJ/mol Electron affinity of F -328 kJ/mol Bond energy of F2 154 kJ/mol Energy of sublimation for Mg 150. kJ/molarrow_forwardConsider hypothetical elements X2 and Y2. Suppose the enthalpy of formation of the compound XY is – 84 kJ/mol, the bond energy for X2 is 105 kJ/mol, and the bond energy for Y2 is 58 kJ/mol. A)Estimate the XY bond energy, Ed, in units of kJ/mol. B)If the dissociation of a X-Y molecule were accomplished by the absorption of a single photon whose energy was exactly the quantity required, what would be its wavelength in nm? C)Would a green-light photon (λgreen=550 nm) be able to break the above X-Y bond? Explain.arrow_forwardH2 has equilibrium bond length of 0.751 Å and bond dissociation energy of 432 kJ mol21 , whereas F2 has equilibrium bond length of 1.417 Å and bond dissociation energy of 155 kJ mol21. On the same graph show qualitativesketches of the effective potential energy curve Veff for an H2 and an F2 molecule. In your solution, show the conversion from kJ mol21 to the energy of a single molecule.arrow_forward
- 2Al(s) + Fe2O3(s) = Al2O3(s) + 2Fe(s) What is the Delta H degrees for this reaction?arrow_forwardBased on average bond enthalpies, would you expect a photon capable ofdissociating a C¬Cl bond to have sufficient energy to dissociate a C¬Br bond?arrow_forwardWhich substance do you expect to have the greatest lattice energy: MgF2, CaF2, or ZrO2? Why?arrow_forward
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