Draw the skeletal structure of the product(s) for the Lewis acid-base reaction. Include lone pairs and formal charges (if applicable) on the structures. Al ΑΓ

Based on the atom connectivity shown bellow,evaluate the four resonance structure for the thiosulfate ion S2O3 ^2-. Use curved arrows to indicate how you get from one resonance structure to another. Assign formal changes to all atoms and determine which of these resonance structure is the most stable based on a formal charge analysis Explain your answer thoroughly. Look at the picture.

When it is strongly heated, ethyl diazoacetate decomposes to give nitrogen gas and a carbene. Draw a Lewis structure of the carbene.

Draw out the Lewis Structure of H3PO4, and consider its major resonance forms. Box the major resonance contributor to the hybrid. List the intermolecular forces the compound would exhibit.

(e) The mean bond enthalpy for chlorine is +242 kJ mol·l and that for fluorine is +158 kJ mol-". The enthalpy of formation of CIF (g) is 56 kJ mol·l (ii) Calculate the enthalpy of formation of, gaseous Chlorine Trifluoride, CIF3 (g), using the bond enthalpy value you obtained in part (i). (iii) The bond enthalpy of CIF3 calculated in part (ii) is likely to be different than that determined from experiment. Explain.

Estimate the enthalpy of reaction( AH), using bond enthalpy values given below 2H2(g) + 02(g) 2H20(g) ( AHO) = ? > Bond energies are given: BE (H - H)= 436 kJ/mol. BE (O=0)= 496 kJ/mol. BE (O - H)= 463 kJ/mol. A. + 367.2 kJ/mol B. + 534.1 kJ/mol C. - 484.0 kJ/mol D. - 490.2 kJ/mol

Which atom bears the formal positive charge in the hydronium ion?

(a) Compare the bond enthalpies (Table 8.3) of the carbon–carbon single, double, and triple bonds to deduce an averageπ -bond contribution to the enthalpy. What fraction ofa single bond does this quantity represent? (b) Make a similarcomparison of nitrogen–nitrogen bonds. What do youobserve? (c) Write Lewis structures of N2H4, N2H2, and N2,and determine the hybridization around nitrogen in eachcase. (d) Propose a reason for the large difference in yourobservations of parts (a) and (b).

Write the hydrolytic reaction and the equilibrium constant expression corresponding to the: (refer to the image below)

Draw the Lewis dot structure of the conjugate base of cyclopentane by assuming all the atoms in the molecule obey the octet rule. Show all lone pairs and formal charges. Do no draw resonance structures.