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- Ethanol can be made by the reaction of ethylene and water: H2C=CH2(g) + H2O(g) CH3CH2OH(g) Use bond dissociation enthalpies to estimate the enthalpy change in this reaction. Compare the value obtained to the value calculated from enthalpies of formation.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 Lewis structures for the following molecules or ions: (a) SbH3 (b) XeF2 (c) Se8 (a cyclic molecule with a ring of eight Se atoms)
- The compound oxygen difluoride is quite reactive, giving oxygen and HF when treated with water: OF2(g) + H2O(g) O2(g) + 2 HF(g) rH = 318 kl/mol-rxn Using bond dissociation enthalpies, calculate the bond dissociation enthalpy of the OF bond in OF2.Write Lewis structures and predict whether each of the following is polar or nonpolar. a. HOCN (exists as HOCN) b. COS c. XeF2 d. CF2Cl2 e. SeF6 f. H2CO (C is the central atom.)Which of the following is most likely a covalent compound? A1203 b SF4 KF CaC12
- Explain formation of covalent bonds in the following chemical compounds (using three theories). NH KF Ar2, C:Br Hz , BeCl2.Identify the most polar bond in each molecule. (To answer this question you may consult the table of electronegativity values in the table below.) 1A 2A Li Be 1.0 1.5 Na Mg 0.9 1.2 3B 4B 5B 6B 7B 2: CHBRCIF K Ca Sc Ti V Cr Mn Fe 0.8 1.0 1.3 1.5 1.6 1.6 1.5 1.8 Rb Sr Y 0.8 1.0 1.2 1: (CH3)3CCI Zr Nb Mo 1.4 1.6 1.8 <1.0 1.0-1.4 H 2.1 1.5-1.9 2.0-2.4 8B Co 1.8 1B 2B Ni Cu Zn 1.8 1.9 1.6 3A B 2.0 2.5-2.9 3.0-4.0 Al 1.5 Ga 1.6 Te Ru Rh Pd Ag Cd In 1.9 2.2 2.2 2.2 1.9 1.7 1.7 4A 5A 6A 7A с 0 2.5 3.0 3.5 F 4.0 Si 1.8 2.1 P S 2.5 Ge As Se 1.8 2.0 2.4 Sn 1.8 Sb Te 1.9 2.1 At Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po 0.7 0.9 1.1 1.3 1.5 1.7 1.9 2.2 2.2 2.2 2.4 1.9 1.8 1.8 1.9 2.0 2.2 CI 3.0 Br 2.8 I 2.5 Write the symbols for the two atoms involved in the bond, separated by a hyphen, i.e. O-H (note that the answer is case-sensitive).Decreasing electronegativity- 1.0 Na Mg 0.9 1.2 Be 1.5 K Ca 0.8 1.0 Rb Sr 0.8 1.0 Cs Ba 0.7 Fr 0.7 table. Sc 1.3 Y 1.2 0.9 10-1.2 H IN Ra Ac 0.9 11 2.1 Ti 1.5 La-Lu Hf 1.3 Zr Nb 1.4 1.6 V 1.6 1.3 Ta 1.5 Pa 14 Increasing electronegativity Cr 1.6 Mo 1.8 14 Mn Fe Co 1.5 1.8 1.9 Tc 1.9 W Re Os 1.7 1.9 2.2 Ru 2.2 Np-No 14-13 Rh 2.2 2.2 1.9 Pd 2.2 Cu 1.9 Ag 1.9 Pt Au 2.2 2.4 Zn 16 Cd 17 Hg 19 B 20 AI 15 Ga 16 In 17 с 2.5 SI 18 Ge 18 Sn 18 TI Pb 18 19 N 3.0 2.1 As 2.0 Sb 1.9 Bi 19 3.5 2.5 Se 2.4 Te 2.1 Po 2.0 Figure 7.6 The electronegativity values derived by Pauling follow predictable periodic trends, with the higher electronegativities toward the upper right of the periodic F 4.0 CI 3.0 Br 2.8 I 2.5 At 2.2