General chemistry chapter 7,8 , and 9

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1. Compare the bond enthalpy of F2 with the energy change for the following process: F2(g) → F+(g) + F-(g) Which is the preferred dissociation for F2, energetically speaking? (Specifics!!!) 2. What is the binding energy (in J/mol or kJ/mol) of an electron in a metal whose threshold frequency for photoelectrons is 2.50  1014 /s? 3. A common way of initiating certain chemical reactions with light involves the generation of free halogen atoms in solution. If DH for the reaction Cl2(g) → 2Cl(g) is 242.8 kJ/mol, what is the longest wavelength of light that will produce free chlorine atoms in solution? 4. Write Lewis structures for the following molecules and ions: a. b. c. d. e. f. NCl3 OCS H2O2 CH3COOCNCH3CH2NH3+ 5. What are the products of the following reactions? a. 2Al(s) + 6H+(aq) → b. 2 Li(s) + 2H2O(l) → c. SO2(g) + H2O(l) → 6. What is the ground-state electron configuration for______? a. S-2 b. Ca+2 c. Cu(I) d. Cr+3 7. Use the bond enthalpy data given to estimate the heat released when 6.50 g of nitrogen gas reacts with excess hydrogen gas to form ammonia at 25C. BE(NN) = 941.4 kJ/mol BE(H–H) = 436.4 kJ/mol BE(N–H) = 393 kJ/mol 8. Give the four quantum numbers for the following: a. Cr+3 b. Cu(I) 9. Use the Born-Haber cycle to calculate the lattice energy of MgO (s) given the following data: H(sublimation) Mg = 130 kJ/mol I1 (Mg) = 738.1 kJ/mol I2 (Mg) = 1450 kJ/mol Bond energy (O=O) = 498.7 kJ/mol EA (O) = 141 kJ/mol EA (O–) = –780 kJ/mol H (MgO(s)) = –601.8 kJ/mol 10. The standard enthalpy of formation of ammonia at 25C is –46.3 kJ/mol. Estimate the N–H bond enthalpy at this temperature. (Given: BE(NN) = 941.4 kJ/mol, BE(H–H) = 436.4 kJ/mol)
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