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- Bond Enthalpy When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to form the X2 molecule: X(g)+X(g)X2(g) a Would you predict that this reaction is exothermic or endothermic? Explain. b Is the bond enthalpy of X2 a positive or a negative quantity? Why? c Suppose H for the reaction is 500 kJ/mol. Estimate the bond enthalpy of the X2 molecule. d Another hypothetical molecular compound, Y2(g), has a bond enthalpy of 750 kJ/mol, and the molecular compound XY(g) has a bond enthalpy of 1500 kJ/mol. Using bond enthalpy information, calculate H for the following reaction. X2(g)+Y2(g)2XY(g) e Given the following information, as well as the information previously presented, predict whether or not the hypothetical ionic compound AX is likely to form. In this compound, A forms the A+ cation, and X forms the X anion. Be sure to justify your answer. Reaction: A(g)+12X2(g)AX(s)The first ionization energy of A(g) is 400 kJ/mol. The electron affinity of X(g) is 525 kJ/mol. The lattice energy of AX(s) is 100 kJ/mol. f If you predicted that no ionic compound would form from the reaction in Part e, what minimum amount of AX(s) lattice energy might lead to compound formation?Write the Lewis structure for each molecule.a. SF2 b. SiH4c. HCOOH (both O bonded to C) d. CH3SH (C and S central)Write the Lewis structure for each molecule.a. CH2O b. C2Cl4c. CH3NH2 d. CFCl3 (C central)
- a. Write a Lewis structure that obeys the octet rule for the following species. Assign the formal charge for the central atom of SO4. If multiple resonance structures exist, use one that does not involve an expanded valence. Formal charge: b. Write a Lewis structure that obeys the octet rule for the following species. Assign the formal charge for the central atom of POC13. If multiple resonance structures exist, use one that does not involve an expanded valence. Formal charge:Write the Lewis structure for each molecule or ion.a. CI4 b. N2O c. SiH4 d. Cl2COWrite the Lewis structure for each molecule.a. CH2O b. C2Cl4
- Write Lewis structures for each molecule or ion. Include reso- nance structures if necessary and assign formal charges to all atoms. If necessary, expand the octet on the central atom to lower formal charge. a. SO,2- b. HSO, c. SO3 d. BrOz8) In an exothermic reaction, the enthalpy of the reaction can be calculated by a. Subtracting the sum of all the bond energies of the products from the sum of all the bond energies of the reactants. b. Subtracting the sum of all the bond energies of the reactants from the sum of all the bond energies of the products c. Finding the sum of the enthalpies of formation of all the products and reactants together d. All of the aboveWrite the Lewis structure for each ion. Include resonance structures if necessary and assign formal charges to all atoms. If necessary, expand the octet on the central atom to lower formal charge.a. PO43- b. CN- c. SO3 2- d. ClO2 -
- a. Write a Lewis structure that obeys the octet rule for the following species. Assign the formal charge for the central atom of XeO4. If multiple resonance structures exist, use one that does not involve an expanded valence. Formal charge: b. Write a Lewis structure that obeys the octet rule for the following species. Assign the formal charge for the central atom of clO3¯. If multiple resonance structures exist, use one that does not involve an expanded valence. Formal charge:Write Lewis structures for each molecule or ion. Use expanded octets as necessary.a. ClF5 b. AsF6- c. Cl3PO d. IF55. Consider the reaction between hydrazine and hydrogen to produce ammonia, N2H4(g)+H2(g)→2NH3(g)N2H4(g)+H2(g)→2NH3(g). Use enthalpies of formation and bond enthalpies to estimate the enthalpy of the nitrogen-nitrogen bond in N2H4N2H4. (Hint: In an N2H4N2H4 molecule, each NN atom has single bonds to the adjacent NN atom and two HH atoms. In an NH3NH3 molecule, the central NN atom has single bonds to three HH atoms.)