a) CH3(CH2)29CH3, a component found in paraffin wax is a solid at room temperature while octane is a liquid.
Interpretation:
The observation that, CH3(CH2)29CH3, a component found in paraffin wax is a solid at room temperature while octane is a liquid is to be explained.
Concept introduction:
Even in non polar molecules, the attractive dispersion forces are possible, caused by temporary dipoles arising due to the costant change in electon distribution wihin the molecule. These temporary dipoles, though have a fleeting existence are constantly changing. But their cumulative effect may be strong enough to hold the molecule close together so that a substance can be a solid or liquid.
To explain:
The observation that, CH3(CH2)29CH3, a component found in paraffin wax is a solid at room temperature while octane is a liquid.
b) CH3CH2CH2OH has a higher boiling point than CH4
Interpretation:
The observation CH3CH2CH2OH has a higher boiling point than CH4.
Concept introduction:
An attractive interaction between a hydrogen bonded to an electronegative oxygen or nitrogen atom and an unshared electron pair on another oxygen or nitrogrn atom is termed as hydrogen bonding. It is a very strong dipole-dipole interaction that leads to molecular association. These molecules associated through hydrogen bonding will have a high boiling point.
To explain:
The observation CH3CH2CH2OH has a higher boiling point than CH4.
c) CH3CO2H, which is found in vinegar, will dissolve in water but not in oil- for simplicity you may assume oil is CH3(CH2)4CH3
Interpretation:
The observation that CH3CO2H, which is found in vinegar, will dissolve in water but not in oil with molecular formula CH3(CH2)4CH3.
Concept introduction:
Like dissolves like. A polar molecule will dissolve in another polar solvent. The solubility can also be explained using the formation of hydrogen bonding between the two substances.
Want to see the full answer?
Check out a sample textbook solutionChapter 2 Solutions
Study Guide with Student Solutions Manual for McMurry's Organic Chemistry, 9th
- 6. Ethanoic acid (CH3COOH) has a much lower vapor pressure than ethanol (CH3CH2OH). What is the most reasonable explanation? (A) The polarizability of two oxygen atoms increases the London forces of attraction in ethanoic acid compared with ethanol. (B) Hydrogen bonding in ethanoic acid is the strongest attractive force and is mainly responsible for the observed data. (C) Both ethanol and ethanoic acid have an – OH, so the difference is the dipole of the second oxygen that increases the attractive forces. (D) Ethanol has an - OH group and can hydrogen bond; therefore, the London forces must cause the effect.arrow_forwardAcetone [(CH3)2CO] is widely used as an industrial solvent.(a) Draw the Lewis structure for the acetone molecule andpredict the geometry around each carbon atom. (b) Is theacetone molecule polar or nonpolar? (c) What kinds ofintermolecular attractive forces exist between acetone molecules?(d) 1-Propanol (CH3CH2CH2OH) has a molecularweight that is very similar to that of acetone, yet acetoneboils at 56.5 °C and 1-propanol boils at 97.2 °C. Explain thedifference.arrow_forwardArrange the following acids in the increasing order of their solubility in water: p-ClC6H4COOH, CH3COOH, CH3(CH2)3COOHarrow_forward
- Which type of intermolecular force accounts for each of these differences? (a) CH3OH boils at 65 °C; CH3SH boils at 6 °C. (b) Xe is a liquid at atmospheric pressure and 120 K, whereas Ar is a gas under the same conditions. (c) Kr, atomic weight 84 amu, boils at 120.9 K, whereas Cl2, molecular weight about 71 amu, boils at 238 K. (d) Acetone boils at 56 °C, whereas 2-methylpropane boils at -12 °C. CH3 CH3 O C CH3 CH3 CH3 CH Acetone 2-Methylpropanearrow_forwardWhich of these molecules exhibits only the London dispersion forces (LDF) of interactions? (A) H2O (B) CO2 (C) SO2 (D) N2Oarrow_forwardIn degrees C, what is the approximate boiling point of (CH3CH2)2O?arrow_forward
- Chemistry 1. Glycerol, CH2(OH)CH(OH)CH2OH, has a 3 carbon chain with -OH groups coming off of each carbon. This thick, syrup like liquid is used in anti-freeze and as a food additive. Hexaoctane, C18H38, is a greasy wax-like solid at room temperature. Using this information rank molecules in order of increasing boiling point and justify your answer: PCl2F, H2O, SeS3, MgS, Glycerol, CH4, CaS, PF2Cl, Hexaoctane, Nearrow_forwardAll compounds in a chemical series have the same commonality of structure, therefore the same predominant IMF. Using concepts of intermolecular forces, please explain thetrends of decreasing ΔTwith increasing molar mass within a chemical series.arrow_forward(a) What atoms must a molecule contain to participatein hydrogen bonding with other molecules of the samekind? (b) Which of the following molecules can formhydrogen bonds with other molecules of the same kind:CH3F, CH3NH2, CH3OH, CH3Br?arrow_forward
- 7The substance with the lowest known boiling point (4 K) is helium, an atomic element that has two electrons. Hydrogen is a diatomic molecule and also has two electrons, but its boiling point is significantly higher, at 20.28 K. (a) What is the dominant intermolecular force between a pair of helium atoms and a pair of H2 molecules? (b) Why do you think H2 has a higher boiling point?arrow_forwardWhich compound would have the lowest boiling point? I OV ||| O IV OII OI IV OH II OH V SOH Ш -OHarrow_forward(a) 4. Identify the intermolecular forces which can operate between molecules of the following pure compounds: (b) N. (c) Numbering N. (d) 5. For the compounds in the previous question, what intermolecular forces would operate between the compound and water?arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning