The barrier to C-C bond rotation in bromoethane is 15 kJ/mol. What energy can you assign to an H-Br eclipsing interaction? Use strain energy increments from the table below in your calculation. (Specify units, kJ/mol; Calculate to nearest 0.1 energy units) Interaction H→ H eclipsed H→ CH3 eclipsed CH3 CH3 eclipsed CH3 CH3 gauche Cause Torsional strain Mostly torsional strain Torsional and steric strain Steric strain (kJ/mol) Energy cost 4.0 6.0 11.0 3.8 (kcal/mol) 1.0 1.4 2.6 0.9
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- Using the following bond energies, calculate the molar heat of hydrogenation, AHhydrogenation CH=CH(g) + 2H₂(g) →→→ CH₂CH₂(g) Bond Bond Strength (kJ/mol) C-C 348 839 411 432 || C=C C-H H-H kJ/molCalculate strain energy for the conformer pictured below, using strain energy increments from the table. Strain Energy for Alkanes Interaction / Compound kJ/mol H: H eclipsing 4.0 H: CH3 eclipsing CH3 CH3 eclipsing gauche butane H Strain energy = cyclopropane cyclobutane cyclopentane cycloheptane cyclooctane (Calculate your answer to the nearest 0.1 energy unit, and be sure to specify units, kJ/mol or kcal/mol. The answer is case sensitive.) H CH3 ball & stick V + labels 5.8 11.0 3.8 115 H kcal/mol 110 26.0 26.2 40.5 1.0 1.4 2.6 0.9 27.5 26.3 6.2 6.3 9.7Calculate strain energy for the conformer pictured below, using strain energy increments from the table Strain Energy for Alkanes \table[[Interaction / 1 Compound,k-ol, kca-ol m H3C. J m H CH3 CH3 CH3 H
- The average bond energy (enthalpy) for a C=CC=C double bond is 614 kJ/molkJ/mol and that of a C−CC−C single bond is 348 kJ/molkJ/mol. Estimate the energy needed to break only the ππ bond of the double bond of 2-butene. Express your answer numerically in joules per molecule.Select the bonds in the 3D representation of methyl urethane below that are multiple bonds. (Hint: Consider the number of bonds attached to an atom in the image compared to the normal valence of that atom. In a valid structure, the number of bonds to an atom will equal the valence of that atom.) • Gray = C: white = H; red = 0; blue = N; dark green = Cl; brown = Br; light green = F; purple = 1; yellow = S: orange = P. • Double click to select bonds. You can zoom in and out using the mouse scroll wheel (or pinch to zoom on touch screens). ●Estimate the strain energy of the following 2,3-dimethylbutane conformation. Use strain energy increments from the table given in the question, and be sure to specify your units, e.g.kJ/mol. Calculate energy to the nearest 0.1 energy unit. Strain Energy Increments strain CH3 Ø CH3 H. H CH3 The strain energy is Interaction HH eclipsing H→ CH3 eclipsing CH3 CH3 eclipsing CH3 CH3 gauche → → kJ/mol kcal/mol 4.0 6.0 11.0 3.8 1.0 1.4 2.6 0.9
- The general values for steric and torsional strain are provided. Use these values to calculate the amount of strain in the molecule in the box. လင်းလင်းခြင်း H3C CH3 H CH3/CH3 gauche 3.8 kJ/mol steric strain H/H eclipsed bond 4 kJ/mol torsional strain CH3/H eclipsed bond 5.6 kJ/mol torsional strain CH3 CH3 eclipsed 11 kJ/mol torsional & steric strain H CH3 H H -CH3 H 1 2 4 7 LO 00 +/- 5 8 kJ/mol 3 6 9 0 C x 100Estimate the heat released when 1-butene(CH3CH2CHCH2) reacts with bromine to give CH3CH2CHBrCH2Br. Bond enthalpies are CH : 412 kJ/mol; CC : 348 kJ/mol;CC : 612 kJ/mol; CBr : 276 kJ/mol;BrBr : 193 kJ/mol. 1.317 kJ/mol 2.507 kJ/mol 3.95 kJ/mol 4.288 kJ/mol 5.181 kJ/molYour chemistry professor draws a number of molecules on the board: (1) CH4 ; (2) H2C=CH2 ; (3) H2C=C=CH2 ; and (4) H2C=C=C=CH2. You muse about all the molecules that chemists draw on a two-dimensional board and wonder which ones are actually planar, existing basically as they appear on the board, and which ones are not plane but rather three-dimensional. Answer the following questions. What is the geometry and hybridization of the carbon in CH4? What is the geometry and hybridization of each central carbon atom in the remaining molecules? Draw each molecule showing the bonds and identify each bond in all the molecules as s or p. What are the specific orbital overlaps (i.e., sp3-sp3) that are in each of the molecules? What are the bond angles for each central atom in each molecule? Which molecules are planar and which are non-planar?
- Your chemistry professor draws a number of molecules on the board: (1) CH4 ; (2) H2C=CH2 ; (3) H2C=C=CH2 ; and (4) H2C=C=C=CH2. You muse about all the molecules that chemists draw on a two-dimensional board and wonder which ones are actually planar, existing basically as they appear on the board, and which ones are not plane but rather three-dimensional. Answer ALL of the following questions. What are the specific orbital overlaps (i.e., sp3-sp3) that are in each of the molecules? What are the bond angles for each central atom in each molecule? Which molecules are planar and which are non-planar?Haloethanes (CH3CH2X, X = Cl, Br, I) have similar barriers to rotation (13.4–15.5 kJ/mol) despite the fact that the size of the halogen increases, Cl ? Br ? I. Offer an explanation.Rank the conformations of 1,2-dichloroethane in terms of stability. Draw a plot of potential energy versus rotation for the C-C bond in 1,2-dichloroethane. Do your calculations for conformations of 1,2-dichloroethane agree with the plot you predict?