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Hydrogen fluoride has a dipole moment of 1.83 D; its boiling point is
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- Two isomers of 1,2-dichloroethene are known. One has a dipole moment of 2.4 D; the other has zero dipole moment. Draw the two isomers, and explain why one has zero dipole moment. CHCl“CHCl 1,2-dichloroethenearrow_forwardArrange the following alkyl halides in order of increasing boiling point:(CH 3)3Br, (CH 3)2CH C(CH3) 2Br, (CH 3) 2CHBr, CH 3CH 2F.arrow_forwardThe dipole moment of trans 1,2-dichloroethane is less than the cis – isomer. Explain.arrow_forward
- Why does styrene have a higher boiling point, 145 °C, than isopropanol, 83 °C? Explain your answer by indicating the types and relative strengths of intermolecular forces present in each compound (see the line structures given below). HO styrene dipole moment = 0.13 D isopropanol dipole moment = 1.66 Darrow_forwardThere are three different dichloroethylenes (molecular for-mula C₂H₂Cl₂), which we can designate X, Y, and Z. CompoundX has no dipole moment, but compound Z does. Compounds Xand Z each combine with hydrogen to give the same product:C₂H₂Cl₂ (X or Z) +H₂→ClCH2-CH2Cl What are the structures of X, Y, and Z? Would you expect com-pound Y to have a dipole momenarrow_forward11. Which statement is true of the carbon-carbon bonds in benzene? (a) They are identical to the carbon-carbon bonds in cyclohexane. (b) They are identical to the carbon-carbon bonds in cyclohexene. (c) They are half-way between a double and single bond. (d) They are easily broken in chemical reactions. (e) They are all double bonds. ct Copyright O 2002 McGraw-Hill Ryerson Limited Name: Class:arrow_forward
- Formaldehyde, H2C=O, is known to all biologists because of its usefulness as a tissue preservative. When pure, formaldehyde trimerizes to give trioxane, C3H6O3, which, surprisingly enough, has no carbonyl groups. Only one monobromo derivative (C3H5BrO3) of trioxane is possible. Propose a structure for trioxane.arrow_forwardTwo useful organic compounds that contain Cl atoms are vinyl chloride (CH2 = CHCI) and chloroethane (CH;CH;CI). Vinyl chloride is the starting material used to prepare poly (vinyl chloride), a plastic used in insulation, pipes, and bottles. Chloroethane (ethyl chloride) is a local anesthetic. Why is the C- Cl bond of vinyl chloride stronger than the C– CIl bond in chloroethane.arrow_forwardDraw Lewis structures and condensed structural formulas for the four alcohols with the molecular formula C4H10O. Classify each alcohol as primary, secondary, or tertiary. (Hint: First consider the connectivity of the four carbon atoms; they can be bonded either four in a chain or three in a chain with the fourth carbon as a branch on the middle carbon. Then consider the points at which the iOH group can be bonded to each carbon chain.)arrow_forward
- 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.arrow_forwardTrue or false: (a) The C¬C bonds in benzene are all the samelength and correspond to typical single C¬C bond lengths.(b) The C¬C bond in acetylene, HCCH, is longer than theaverage C¬C bond length in benzene.arrow_forwardAlcohols A, B, and C all have the composition C4H10O. Molecules of alcohol A contain a branched carbon chain and can be oxidized to an aldehyde; molecules of alcohol B contain a linear carbon chain and can be oxidizedto a ketone; and molecules of alcohol C can be oxidized to neither an aldehyde nor a ketone. Write the Lewis structures of these molecules.arrow_forward