Organic Chemistry
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Explain:
a. Why does ethyl alcohol (78 °C) boils at a higher temperature than ethylamine (16 °C)?
b. Why does dimethylamine (7 °C) boils at a higher temperature than dimethyl ether (-24 °C)?
Despite having a high melting point, ionic compounds like sodium carbonate are quite soluble in water. Explain why.
Show the intermolecular hydrogen bonding between two molecules of methanol and the intermolecular hydrogen bonding between two molecules of methylamine.
Between the given substances, dipropyl ether and hexan-1-ol, which one exhibits a higher boiling point?
Determine the atoms that act as hydrogen bond donors and acceptors in the molecule below.
Determine which compound has the higher boiling point for each of the following pairs: CH3OCH3 or CH3CH2OH, and CH3CH2CH3 or CH3CH2CH2CH3. Explain.
Determine which molecule is expected to have a higher boiling point in the given pair and explain your reasoning.
Predict which one of the given compounds has a stronger dipole moment and which one has a higher boiling point.
Rank the following isomers from the one with the lowest boiling point to the one with the highest boiling point. Explain your answer.
Identify the compounds which can form intermolecular hydrogen bonds.
a. CH3CH2OH
b. (CH3)2NH
c. (CH3)3N
Consider the molecule shown below:
Identify the hydrogen bond acceptors and the hydrogen bond donors in the structure.
Dipropyl ether and 1-hexanol are isomers. The two compounds have similar solubilities in water but have very different boiling points. Account for this observation.
Explain why benzene melts at a higher temperature even though it has a smaller molecular weight than toluene. Consider the possible interactions between molecules based on their shapes.
The two N-containing isomers below have a boiling point difference of 19.0 °C. Meanwhile, the two O-containing isomers have a boiling point difference of 83.2 °C. The two N-containing isomers have a much smaller boiling point difference than the two O-containing isomers. Explain this observation.
Explain why 1-heptanol boils at a higher temperature compared to 4-heptanol.
From the two compounds below, which has a lower net dipole? Which is expected to have a lower boiling point?
Determine which compound has the higher boiling point for each of the following pairs: CH3CH2CH2CH3 or (CH3)2CHCH3, and CH3CH2CH2CH3 or CH3CH2CH2CH2Cl. Explain.
Determine which compound you expect to have the higher boiling point for each of the following pairs: (CH3)3C-CH2-C(CH3)3 or (CH3)2CH-CH2CH2CH2-CH(CH3)2, CH3(CH2)5CH3 or CH3(CH2)4CH2OH, and CH3OCH3 or CH3CH2OH. Explain your reasoning.
Determine which of the following compounds, cis-2,3-dibromobut-2-ene or trans-2,3-dibromobut-2-ene, has a higher boiling point, and which has zero dipole moment.
Explain why pyrrole (129 °C) boils at a higher temperature than N-methyl pyrrole (112 °C).
Which of the two given molecules would have the higher melting point and why?
Determine which of the following two compounds has the higher boiling point. Explain why that compound has the higher boiling point. 1-bromopropane and 1-chloropropane.
Identify: (i) compounds that can form intermolecular hydrogen bonds; (ii) compounds that can form hydrogen bonds with water; (iii) compounds which you think are soluble in water. CH3(CH2)2CH3, CH2=CH-CH3, CH3CHO and CH3COOH.
Arrange the given compounds in decreasing order of their boiling points (from highest to lowest).
Determine which compound has the higher boiling point for each of the following pairs: (i): 3-methylpiperidine or 1,3-dimethylpyrrolidine, and (ii): 2,4-dimethylpyrrolidine or 4-methylpyrrolidin-2-one. Explain.
List these three compounds from the one with the lowest boiling point to the one with the highest boiling point. Pentane, propane and butane.
Illustrate the hydrogen bonding present in propan-2-ol.
Which of the following substances, 1-bromohexane or 1-chlorohexane, has a higher boiling point?
Determine which of the two molecules below will have a lower melting point:
Indicate the atoms that act as hydrogen bond donors and acceptors in the given molecule.
Illustrate the hydrogen bonding that exists between (i) two molecules of triethylamine ((CH 3CH2)3N) and one molecule of water (H2O) and (ii) one molecule of ethoxyethane (CH 3CH2OCH2CH3) and two molecules of water (H 2O). Use dashes or broken lines to show the interactions.
Choose the molecules that would form a hydrogen bond to methanol.
i. CH3CH2CH2OCH2CH2CH2OH
ii. CH3CH2CH2N(CH3)2
iii. CH3CH2CH2Cl
Determine the smallest possible straight-chain alkane that is liquid at 37 °C.
Determine which molecule has:
(i) a higher density between hexane and nonane.
(ii) a higher boiling point between tert-butyl alcohol and tert-butylamine.
(iii) a lower boiling point between octylamine or di-tert-butylamine.
Which of the substances listed below can form hydrogen bonds with methanol?
(i) CH3(CH2)2F
(ii) CH3(CH2)3SCH3
(iii) CH3(CH2)3N(CH3)2
(iv) CH3CH2COOH
Explain the difference in boiling points in the following pairs of compounds:
i. The boiling point of ethanol (78 °C) is lower than methanediol (192 °C).
ii. The boiling point of ethanamine (17°C) is lower than ethanol (78 °C).
Identify the compound that has the higher boiling point between each pair:
i. chlorocyclobutane or chlorocyclohexane
ii. 1-bromohexane or 1-bromo-2,3-dimethylbutane
Among the compounds in the table below, identify the largest alkane, the largest terminal alkene, and the largest terminal alkyne that are gases at room temperature.
Consider the following compounds with their corresponding boiling points:
i. Explain why the two amides have a much larger boiling point difference than the two amines.
ii. Explain why they have higher boiling points than any of the other four compounds.
Which compound in each pair has a higher boiling point?
Contrary to expectation, upon the addition of the 4th Cl to methane, the boiling point suddenly becomes very low. Provide an explanation as to why this is the case.
Consider the following pair of compounds:
Predict which will have a higher boiling/melting point.
Determine the (i) compounds that can form intermolecular hydrogen bonds, (ii) compounds that can form hydrogen bonds with water, and (iii) compounds that are likely to be soluble in water.
CH3OH, C2H5Cl, CH3CH2OH, and CH3COCH3