Use representations [A] through [I] in figure P6.16 to answer questions a-f. 272
ID: 575689 • Letter: U
Question
Use representations [A] through [I] in figure P6.16 to answer questions a-f. 272 CHAPTER 6 Intermolecular Forces ssing down on the ice is 0033, will the ice under the skate edges mel? Figure P6.12 may help you make your gas) of senon and classify the attractive forces between the xenon atoms 6.15. In Figure P6.15, ideneify the physical stane (solid, liquid, or Ethylene glycol. Ethane Helum FIGURE P6.15 6.16. Use representations [A] through I] in Figure P6.16 to answer questions a-f a. What are the intermolecular forces between the molecules in representations C, E, and G? b. Which of the nine substances has the c. Which representations are isomers of one d. Which i more soluble in water: ethylene lowest boiling point Octane Dimethyl ether G glycol or iodine? Which is more soluble in carbon tetrachloride? Explain your answers in terms of the intermolecular forces involved e. Which hydrocarbon has the higher boiling point? Which substance does not form hydrogen bonds between its molecules but can form hydrogen bonds to another molecule? Carbon tetrachloride FIGURE P6.16 UESTIONS AND PROBLEMS ndon Dispersion Forces: ey're Everywhere 6.21. Fuels from Crude Oil Petroleum mixture of mostlu l roleum (crude oil is acExplanation / Answer
a) Ethane (CH3-CH3) is non-polar, and subject only to dispersion forces. The C-O bonds of methoxymethane (dimethyl ether) (CH3-O-CH3) are polar. The geometry of the molecule is angular, resulting in an overall molecular dipole. Hence the molecule will be subject to dipole-dipole and dipole/induced dipole interactions as well as the stronger dispersion forces.Ethanol (CH3CH2OH) experiences the same types of intermolecular forces as 1,2-ethanediol but the hydrogen bonding can only occur at one site per molecule rather than two. This results in reduced interactions between molecules compared with 1,2-ethanediol but still more than in ethane and dimethyl ether which lack hydrogen bonding between their molecules.
b) As hydrogen bonding is usually the strongest of the intermolecular forces, one would expect the boiling points of these compounds to correlate with hydrogen bonding interactions present. Hence ethanol would have a lower boiling point
c) Ethanol (CH3CH2OH) and (dimethyl ether) (CH3-O-CH3) are isomers of each other. which have same molecular formula but different functional group so these are also catogaries as functional isomers.
d) Molecules containing no polar bonds include I2 and Non-polar molecules containing polar bonds include CO2, CCl4. Since I2 is non polar and CCl4 the molecule is nonpolar because the bond polarity is canceled by the symmetric tetrahedral shape. so I2 is soluble in CCl4 because like dissolves like.
e) ethylene glycol (1,2-ethanediol (OH-CH2-CH2-OH) ) due to the presence of the O-H, bonds is capable of hydrogen bonding which is usually the strongest intermolecular interaction. There are two sites for hydrogen bonding in this molecule, so this will enhance the possible hydrogen bonding interactions. This compound will of course also experience dispersion forces and dipole/dipole and dipole/induced dipole forces between molecules but the hydrogen bonding interaction would be most significant.
f) For hydrogen bonding , hydrogen must be attached to highly electronegative elements like F , O , N
and since in alkane the hydrogen is attahced to carbon , alkanes cannot form hydrogen bonding. Ethanol can form Hydrogen bonds qith other water molecules.
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.