Homework Answers
(c) Intermolecular hydrogen bonding is the main reason of boiling point of H2O is much higher than the H2S.
Hydrogen bonding is the main reason inspite of of low molar mass H2O should have low boiling point but due to hydrogen bonding its boiling point Rises 100 degree centigrade. Hydrogen bonding occur only in N, O, F, with highly polar HH+ charge
Answer: (C)
(d)
CH2O is a polar molecule while ethene is a non polar molecule due to polarity of CH2O it is having dipole-dipole attraction while ethene does not have dipole dipole attraction but only weak dispersion force. So show ethene has low boiling point.
Answer: (D)
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C The boiling point of H,O is much higher than the boiling point of HS. H2O...
Part A H,0 (100°C) has a higher boiling point than CH, OH (65°C). There are more...
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The boiling point of iodine (12) is much higher than the boiling point of helium (He)....
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2. Identify the strongest type of intermolecular forces in acetone, ethanol, water and hexane. (Structures listed...
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7. If an ionic bond is stronger than a dipole-dipole interaction, how can water dissolve an...
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These two molecules have an identical number of electrons. However, the boiling point of Compound B...
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Select the single best answer. Explain in terms of intermolecular forces the following: Why NaCl has...
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Arrange the compounds in order from highest to lowest boiling point.
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Use the References to access important values if needed for this question. List the following substances...
Use the References to access important values if needed for this question. List the following substances in order of increasing normal boiling points Tb, and explain your reasoning: He, HCI, HF, Nal Boiling point substance1-lowest Reason 4-highest Is an ionic compound: forces are stronger than forces between neutral molecules. Has hydrogen bonds: stronger than other dipole-dipole interactions Is polar: dipole-dipole forces are stronger than dispersion forces Is nonpolar: dispersion forces are weaker than dipole-dipole forces. HCI HF Nal Submit Answer...
Why does benzene have a much higher boiling point (80。c) than hexane (69。c), even though they...
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My answers: Not sure if they are correct. 1. a. London dispersion b. H-bonding, dipole-dipole,...
My answers: Not sure if they are correct.
1. a. London dispersion
b. H-bonding, dipole-dipole, london dispersion
c. London dispersion
d. Ionic, london disperson
2. The second one because not a lot of H+ and less acidic. Need
help understanding the meaning of the question.
3. Diethyl cannot h-bond because it does not provide intermolecular
bonding engery while 1-b. can form h-bond making strong
intermolecular bonds to take up greater engery to break
molecules.
4. Not sure...
Part A H,0 (100°C) has a higher boiling point than CH, OH (65°C). There are more hydrogen bonds between water molecules than between alcohol molecules. There are less hydrogen bonds between water molecules than between alcohol molecules. CH, OH has the higher molecular mass than H,O. There are no hydrogen bonds between alcohol molecules while there are plenty of them between water molecules. O Submit Previous Answers Request Answer X Incorrect; Try Again; 2 attempts remaining Part B H,O (100°C)...
The boiling point of iodine (12) is much higher than the boiling point of helium (He). Why? O 12 has a larger electron cloud than He, so more energy is required to overcome the stronger London Dispersion Forces. O It requires more energy to break the covalent bonds in 12 than to overcome the London Dispersion Forces between He atoms. The bonds between iodine atoms are stronger than the bonds between helium atoms and therefore harder to break. O 12...
2. Identify the strongest type of intermolecular forces in acetone, ethanol, water and hexane. (Structures listed on page 15.) Experiment 2 Intermolecular Forces There are three general types of intermolecular forces. All substances exhibit London Dispersion Forces (LDF), and they are generally the weakest of the three types. These London forces are due to the attractions between small, temporary dipoles that arise from the constant, random movement of the electrons in a substance. As molar mass increases, the size of...
These two molecules have an identical number of electrons. However, the boiling point of Compound B is much higher than that of Compound A How does chemistry rationalizelexplain this difference? CH3CH2CH2-NH2 (A) boiling pt = : 48 °C CH3CH2CH2-OH (B) boiling pt = 98°C Select one: O Compound B exhibits hydrogen-bonding forces, but Compound A does not exhibit hydrogen-bonding forces O Compound B exhibits hydrogen bonding forces but it is hydrophobic, so it does not boil easily. Because O-H is...
Select the single best answer. Explain in terms of intermolecular forces the following: Why NaCl has a higher melting point than 12 Because NaCl is soluble in water, and I, is not. Because NaCl is an ionic compound, and the ion-ion attractions are much stronger than the dispersion forces between the I, molecules. Because NaCl is a solid, and I, is a liquid. Because NaCl can form hydrogen bonds, and I cannot.
Use the References to access important values if needed for this question. List the following substances in order of increasing normal boiling points Tb, and explain your reasoning: He, HCI, HF, Nal Boiling point substance1-lowest Reason 4-highest Is an ionic compound: forces are stronger than forces between neutral molecules. Has hydrogen bonds: stronger than other dipole-dipole interactions Is polar: dipole-dipole forces are stronger than dispersion forces Is nonpolar: dispersion forces are weaker than dipole-dipole forces. HCI HF Nal Submit Answer...
My answers: Not sure if they are correct.
1. a. London dispersion
b. H-bonding, dipole-dipole, london dispersion
c. London dispersion
d. Ionic, london disperson
2. The second one because not a lot of H+ and less acidic. Need
help understanding the meaning of the question.
3. Diethyl cannot h-bond because it does not provide intermolecular
bonding engery while 1-b. can form h-bond making strong
intermolecular bonds to take up greater engery to break
molecules.
4. Not sure...
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