26. What type of bond promotes the solubility of alcohols in water?A. Hydrogen bondsB. Dipole-dipole bondsC. Covalent bondsD. Van der Waals forces27. The dehydration of ethyl alcohol primarily yieldsA. EthyleneB. EthanalC. Ethanoic acidD. Ethane28. In general, the boiling point of primary alcohol isthe boiling point of a linear ether of the same carbonchain length.A. Greater thanB. Lower thanC. Equal toD. Stronger than29. Ethyl alcohol and dimethyl ether are isomers. However, they differ in their dipole moment. Which statement is TRUE?A. Dimethyl ether has a lower dipole moment than ethyl alcohol.B. Ethyl alcohol has a lower dipole moment than dimethyl ether.C. Dimethyl ether has a greater bond dipole than ethyl alcohol.D. Ethyl alcohol has a greater bond dipole than dimethyl ether.30. Based on molecular structure, alcohol molecules and ether molecules are analogues of water. This implies that both.molecules can form hydrogen bonds with water molecules. Which statement is FALSE?A. Alcohol molecules are hydrogen bond donors.B. Ether molecules are hydrogen bond acceptors.C. Alcohol molecules are hydrogen bond acceptors.D. Ether molecules are hydrogen bond donors.

26. Option (a) Alcohols are soluble in water. This is due to the hydroxyl group in the…

26. What type of bond promotes the solubility of alcohols in water? A. Hydrogen bonds B. Dipole-dipole bonds C. Covalent bonds D. Van der Waals forces 27. The dehydration of ethyl alcohol primarily yields A. Ethylene B. Ethanal C. Ethanoic acid D. Ethane 28. In general, the boiling point of primary alcohol is chain length. A. Greater than B. Lower than C. Equal to D. Stronger than the boiling point of a linear ether of the same carbon

26. What type of bond promotes the solubility of alcohols in water? A. Hydrogen bonds B. Dipole-dipole bonds C. Covalent bonds D. Van der Waals forces 27. The dehydration of ethyl alcohol primarily yields A. Ethylene B. Ethanal C. Ethanoic acid D. Ethane 28. In general, the boiling point of primary alcohol is chain length. A. Greater than B. Lower than C. Equal to D. Stronger than the boiling point of a linear ether of the same carbon

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter9: Liquids, Solids, And Materials

Section: Chapter Questions

Problem 104QRT: Consider this information regarding two compounds. Thallium azide: yellow crystalline solid; melting...

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Arrange the compounds of each group in order of increasing boiling point. a. ethanol, 1-propanol, methanol b. butane, ethylene glycol, 1-propanol
Consider this information regarding two compounds. Thallium azide: yellow crystalline solid; melting point = 330 C; slightly soluble in water, more soluble in hot water; insoluble in ethanol or diethyl ether. Camphene: colorless, cubic crystals; melting point = 51 C; boiling point = 159 C; insoluble in water; moderately soluble in ethanol; soluble in diethyl ether. (a) Is camphene an ionic or molecular compound? Explain your answer. (b) Is thallium azide an ionic or molecular compound? Explain your answer.
12. Normal boiling point of ethanol (C2H5OH) is 78 °C, and of propanol (C3H;OH) is 97 °C. a. Explain the reason for the difference in boiling points of these two alcohols. b. When the underline methyl group in propanol, CH3CH2CH2OH, is replaced with a hydroxyl group (HOCH2CH2OH), boiling point of the molecule increases to 197 °C. Explain the reason for observed increase in the boiling point.
12. Normal boiling point of ethanol (C2H5OH) is 78 °C, and of propanol (C3H;OH) is 97 °c. a. Explain the reason for the difference in boiling points of these two alcohols. b. When the underline methyl group in propanol, CH3CH2CH2OH, is replaced with a hydroxyl group (HOCH CH2OH), boiling point of the molecule increases to 197 °C. Explain the reason for observed increase in the boiling point.
Why do alcohols have boiling points much higher than hydrocarbons of similar molecular weight? a. Alcohols have greater van der Waals attraction forces.b. Alcohol molecules have greater molecular symmetry.c. Hydrogen bonds must be broken in the process of volatilization.d. Alcohols must overcome greater ionic forces in the process of volatilization.
Why is the boiling point of the aldehyde greater than that of the alkane? Why is the boiling point of alcohol the highest? Explain why the solubility of aldehydes and alcohols falls as the molecules get bigger.
Molecule Type Boiling point (°C) CH3CH2CH3 Alkane -42 CH3CHO Aldehyde +21 CH3CH2OH Alcohol +78 i. Why is the boiling point of the aldehyde greater than that of the alkane?ii. Why is the boiling point of alcohol the highest?iii. Explain why the solubility of aldehydes and alcohols falls as the molecules get bigger.
4. What type of bond promotes solubility of alcohols in water? A. Hydrogen bonds B. Dipole-dipole bonds C. Covalent bonds D. Van der Waals forces
1. Volatile impurities usually decrease the boiling point of the liquid.TRUE or FALSE 2. Solid organic compounds with weak cohesive forces exhibit higher melting points. TRUE or FALSE 3. What is the intermolecular forces of attraction present in the following organic compounds; 1-propanol, 2-butanol and ethanol
1. On average there are _______ hydrogen bonds per molecule in water at room temperature a. 1 b. 2 c. 3 d. 4 e. 5 2. On average, there are ______ hydrogen bonds per molecule in ice. a. 1 b. 2 c. 3 d. 4 e. 5 3. Which of the following alcohols would be most soluble in water? a. methanol (CH3OH) b. ethanol (CH3CH2OH) c. butanol (CH3CH2CH2CH2OH) d. octanol (CH3[CH2]6CH2OH) e. phenol (benzyl-OH) 4. Hydrophobic interactions a. are stronger than covalent bonds b. are responsible for the surface tension of water c. can hold two ions together d. are the major force forming lipid (hydrocarbon) bilayers
At 25°C, the vapor pressure of diethyl ether, (CH3CH2)2O, is higher than the vaporpressure of its isomer n-butanol, CH3CH2CH2CH2OH, becausea. diethyl ether has a higher density than n-butanol.b. diethyl ether has weaker intermolecular forces than n-butanol.c. diethyl ether has a lower critical temperature than n-butanol.d. diethyl ether has a higher surface tension than n-butanol.e. diethyl ether has a smaller molar mass than n-butanol.
VI. Arrange the following compounds according to increasing solubility in water. Write only the letters. 1. A. CH3(CH2)2 OCH3 B. D. (CH3)2CHCH₂NH2 CH3(CH2)16C-OH C. CH3 CH₂2CH3