Which of the following statements about London dispersion forces is/are true? Group of answer choices London...
Which of the following statements about London dispersion forces is/are true?
Group of answer choices
London dispersion forces are stronger between molecules of 1-butanol than between molecules of 2-methyl-2-propanol.
London dispersion forces are stronger than hydrogen bonding interactions.
both a and b
neither a nor b
How many different alkene products (counting cis and trans isomers of a compound as a single product) could be produced when 3-methyl-3-pentanol is dehydrated?
Group of answer choices
1
2
3
4
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Which of the following statements about London dispersion forces
is/are true?
Group of answer choices
London...
Classify the following mixtures of liquids into (A) those with London Dispersion forces between the two...
Classify the following mixtures of liquids into (A) those with London Dispersion forces between the two molecules (B) those with London Dispersion forces and dipole-dipole attraction between the two molecules (C) those with London Dispersion forces, dipole-dipole attraction and hydrogen bonding between the two molecules |1-propanol and 1-butanol 1,1,2,2-tetrachloroethane and ethanol methylbenzene and 1,2-dimethylbenzene trichloromethane and dichloromethane benzene and cyclohexane bromobutane and ethanol
Question 14 Which of the following is or are true? Molecules which have hydrogen bonded to...
Question 14 Which of the following is or are true? Molecules which have hydrogen bonded to F, 0, or N can undergo hydrogen-bonding London dispersion forces are the result of permanent dipoles in atoms or molecules. Bonding forces are much stronger than intermolecular forces. An intermolecular force is an attractive force that operates between molecules. London dispersion forces occur in all atoms and molecules.
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...
h of the following statements is NOT true? London dispersion forces are present in all substances but are the only significant intermolecular forces in nonpolar substances. ) The density of the l...
h of the following statements is NOT true? London dispersion forces are present in all substances but are the only significant intermolecular forces in nonpolar substances. ) The density of the liquid state of a substance is greater than the density of its gaseous state. The thermal energy in a liquid allows the atoms within molecules to completely overcome the attractions between them so they flow. Most liquids can be converted to a gas by reducing pressure and/or heating. The...
Identify the strongest intermolecular force in the compound KHSO4. Group of answer choices Ionic forces Dipole-dipole...
Identify the strongest intermolecular force in the compound KHSO4. Group of answer choices Ionic forces Dipole-dipole Hydrogen bonding Ion-dipole London dispersion forces
help please Question 3 (1.5 points) Which of the following pure liquids would have dispersion forces...
help please
Question 3 (1.5 points) Which of the following pure liquids would have dispersion forces (London forces) as its strongest intermolecular force? CH, CH, Hoc O CH Question 4 (1.5 points) Which of the following molecules has dipole-dipole interactions as it's strongest interaction? (no hydrogen bonding) You may select more than one answer. H₂ C CH 2 CH CH2 CH₂ CH2 CH₂ C H3C H2C CH3 H₂N
Given the following intermolecular attractive forces 1. Hydrogen bonding 2 Dipole-Dipole 3 London dispersion 4 Ion-dipole...
Given the following intermolecular attractive forces 1. Hydrogen bonding 2 Dipole-Dipole 3 London dispersion 4 Ion-dipole When sodium chloride dissolves in water what new attractive forces are formed between solute and solvent?
Question 12 Which of the following statements is false about CH3CH2CH3 and CH3CH2OH? Your answer: O...
Question 12 Which of the following statements is false about CH3CH2CH3 and CH3CH2OH? Your answer: O Hydrogen bonding is the only type of intermolecular forces between CH3CH2OH molecules. O (C) atom makes sp hybridization in CH3CH2CH3 molecule. o Only dispersion forces exist between CH3CH2CH3 molecules. OCH3CH2OH has stronger intermolecular forces than CH3CH2CH3. O CH3CH2CH3 molecule has tetrahedral geometry. Clear answer Back Next
Which of the following best describes London dispersion forces. Question 1 options: the intermolecular forces that...
Which of the following best describes London dispersion forces. Question 1 options: the intermolecular forces that exist when ions from an ionic compound are attracted to the dipole of polar molecules in a mixture. involves molecular orientations in which the positive end of one dipole is near the negative end of another forces that exist only between molecules that contain hydrogen atoms bonded to highly electronegative atoms such as O, N, F. Interactions between temporary dipoles cause atoms to be...
The following questions are true/false 1. The potential energy associated with London dispersion interactions decreases with...
The following questions are true/false 1. The potential energy associated with London dispersion interactions decreases with intermolecular distance as r-12 (where r is the intermolecular distance). 2. SiH4 is more polarizable than CH4. 3. In H2, the antibonding orbital formed by linear combination of two 1s orbitals has zero nodes. 4. In N2, the π bonding orbital formed by linear combination of two 2p orbitals has one node. 5. CO2 has zero total permanent dipole moment. 6. The kinetic energy...
Classify the following mixtures of liquids into (A) those with London Dispersion forces between the two molecules (B) those with London Dispersion forces and dipole-dipole attraction between the two molecules (C) those with London Dispersion forces, dipole-dipole attraction and hydrogen bonding between the two molecules |1-propanol and 1-butanol 1,1,2,2-tetrachloroethane and ethanol methylbenzene and 1,2-dimethylbenzene trichloromethane and dichloromethane benzene and cyclohexane bromobutane and ethanol
Question 14 Which of the following is or are true? Molecules which have hydrogen bonded to F, 0, or N can undergo hydrogen-bonding London dispersion forces are the result of permanent dipoles in atoms or molecules. Bonding forces are much stronger than intermolecular forces. An intermolecular force is an attractive force that operates between molecules. London dispersion forces occur in all atoms and molecules.
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...
h of the following statements is NOT true? London dispersion forces are present in all substances but are the only significant intermolecular forces in nonpolar substances. ) The density of the liquid state of a substance is greater than the density of its gaseous state. The thermal energy in a liquid allows the atoms within molecules to completely overcome the attractions between them so they flow. Most liquids can be converted to a gas by reducing pressure and/or heating. The...
help please
Question 3 (1.5 points) Which of the following pure liquids would have dispersion forces (London forces) as its strongest intermolecular force? CH, CH, Hoc O CH Question 4 (1.5 points) Which of the following molecules has dipole-dipole interactions as it's strongest interaction? (no hydrogen bonding) You may select more than one answer. H₂ C CH 2 CH CH2 CH₂ CH2 CH₂ C H3C H2C CH3 H₂N
Question 12 Which of the following statements is false about CH3CH2CH3 and CH3CH2OH? Your answer: O Hydrogen bonding is the only type of intermolecular forces between CH3CH2OH molecules. O (C) atom makes sp hybridization in CH3CH2CH3 molecule. o Only dispersion forces exist between CH3CH2CH3 molecules. OCH3CH2OH has stronger intermolecular forces than CH3CH2CH3. O CH3CH2CH3 molecule has tetrahedral geometry. Clear answer Back Next
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