What intermolecular forces increase with the size of amides?
Q. I'm confused. Thanks!
Asked by Cheesy - Tue Mar 24 13:54:33 2009 - - 1 Answers - 0 Comments
A. As an amide increases in size the contribution of the resonance form that shows a double bond between nitrogen and the carbonyl carbon increases but this is only true as you go from very simple amides to slightly larger ones and does not continue to increase as the amide increases in size. This is an extremely important property of protein structure.
Answered by Mark R - Wed Mar 25 10:40:49 2009
Q. I'm confused. Thanks!
Asked by Cheesy - Tue Mar 24 13:54:33 2009 - - 1 Answers - 0 Comments
A. As an amide increases in size the contribution of the resonance form that shows a double bond between nitrogen and the carbonyl carbon increases but this is only true as you go from very simple amides to slightly larger ones and does not continue to increase as the amide increases in size. This is an extremely important property of protein structure.
Answered by Mark R - Wed Mar 25 10:40:49 2009
What happens to these physical properties as the strength of intermolecular forces increases?
Q. What happens to these physical properties as the strength of intermolecular forces increases? Increase or decrease? a) melting point b) vapor pressure c) boiling point d) viscosity e) surface tension
Asked by jan - Sun May 10 11:57:22 2009 - - 5 Answers - 0 Comments
A. a) increase - harder to get from solid (packed together) to liquid (free to move) b) decrease - harder to get to a gas and keep it as a gas c) increase - harder to get from gas (free) to liquid (can't move entirely freely) d) increase - particles stick together more e) increase - harder to move particles - Anonymous
Answered by Anonymous - Sun May 10 12:08:17 2009
Q. What happens to these physical properties as the strength of intermolecular forces increases? Increase or decrease? a) melting point b) vapor pressure c) boiling point d) viscosity e) surface tension
Asked by jan - Sun May 10 11:57:22 2009 - - 5 Answers - 0 Comments
A. a) increase - harder to get from solid (packed together) to liquid (free to move) b) decrease - harder to get to a gas and keep it as a gas c) increase - harder to get from gas (free) to liquid (can't move entirely freely) d) increase - particles stick together more e) increase - harder to move particles - Anonymous
Answered by Anonymous - Sun May 10 12:08:17 2009
Which of these are affected by an increase in intermolecular forces?
Q. By "these", I mean: Melting point, hardness, capillary action, conductivity, and heat of vaporization.
Asked by theweirdguy1 - Tue Mar 13 16:25:30 2007 - - 1 Answers - 0 Comments
A. Conductivity is not affected, it is concerned with the energy of electrons or ions to reach a conduction band and become mobile. Capillary action is related to the intermolecular forces between one substance and a capillary material. melting point, hardness and heat of vaporization are related to intermolecular forces within a single substance.
Answered by gaurav19671031 - Tue Mar 13 22:46:20 2007
Q. By "these", I mean: Melting point, hardness, capillary action, conductivity, and heat of vaporization.
Asked by theweirdguy1 - Tue Mar 13 16:25:30 2007 - - 1 Answers - 0 Comments
A. Conductivity is not affected, it is concerned with the energy of electrons or ions to reach a conduction band and become mobile. Capillary action is related to the intermolecular forces between one substance and a capillary material. melting point, hardness and heat of vaporization are related to intermolecular forces within a single substance.
Answered by gaurav19671031 - Tue Mar 13 22:46:20 2007
Which of these decreases as the strength of the attractive intermolecular forces increases? I give best answer?
Q. Deviations from the ideal gas law Boiling temperature Sublimation temperature Vapor pressure Also, could you briefly explain to me your choice(s)? Heat of vaporization
Asked by jake - Fri Jan 23 20:55:50 2009 - - 2 Answers - 0 Comments
A. Not deviation from ideal gas law. One of the "ideal" assumptions is that there are no intermolecular attractions. Boiling point would increase with increasing attractive forces, as those forces must be overcome to drive the molecules apart and in to the gas phase. Sublimation temperature follows the same logic as boiling point. Vapor pressure is the only property that would decrease as a function of increasing intermolecular forces. Stronger attractive forces means fewer molecules escape into the vapor phase, decreasing the overall vapor pressure.
Answered by Chad - Fri Jan 23 21:02:10 2009
Q. Deviations from the ideal gas law Boiling temperature Sublimation temperature Vapor pressure Also, could you briefly explain to me your choice(s)? Heat of vaporization
Asked by jake - Fri Jan 23 20:55:50 2009 - - 2 Answers - 0 Comments
A. Not deviation from ideal gas law. One of the "ideal" assumptions is that there are no intermolecular attractions. Boiling point would increase with increasing attractive forces, as those forces must be overcome to drive the molecules apart and in to the gas phase. Sublimation temperature follows the same logic as boiling point. Vapor pressure is the only property that would decrease as a function of increasing intermolecular forces. Stronger attractive forces means fewer molecules escape into the vapor phase, decreasing the overall vapor pressure.
Answered by Chad - Fri Jan 23 21:02:10 2009
intermolecular forces?
Q. indicate what change if any should occur in each of the following properties as a result of the increase in the strength of intermolecular forces. a.vapor change, b.normal boiling point c. normal melting point d. surface tension e.viscosity f. heat fusion g. heat vaporization h. molecular weight
Asked by confusedkid - Wed Nov 7 16:10:14 2007 - - 1 Answers - 0 Comments
A. all except molecular weight.(h).
Answered by papastolte - Wed Nov 7 16:14:38 2007
Q. indicate what change if any should occur in each of the following properties as a result of the increase in the strength of intermolecular forces. a.vapor change, b.normal boiling point c. normal melting point d. surface tension e.viscosity f. heat fusion g. heat vaporization h. molecular weight
Asked by confusedkid - Wed Nov 7 16:10:14 2007 - - 1 Answers - 0 Comments
A. all except molecular weight.(h).
Answered by papastolte - Wed Nov 7 16:14:38 2007
Am I correct about these intermolecular forces?
Q. As intermolecular forces rise, Boiling point rises and melting point decreases As intermolecular forces increases vapor pressure increases and face surface tension increases
Asked by moviefan254 - Wed Jan 9 22:38:49 2008 - - 1 Answers - 0 Comments
A. As intermolecular forces increase, both boiling points and melting points will increase. In order to change phase (i.e. solid to liquid or liquid to gas) one must break the intermolecular forces holding molecules together. Greater intermolecular forces require higher temperatures (more energy) to break. By the same argument, vapor pressure should decrease with increasing intermolecular forces. At a given temperature, fewer molecules will be able to achieve the gas state, so the vapor pressure should be smaller.
Answered by triadspectre - Wed Jan 9 22:49:00 2008
Q. As intermolecular forces rise, Boiling point rises and melting point decreases As intermolecular forces increases vapor pressure increases and face surface tension increases
Asked by moviefan254 - Wed Jan 9 22:38:49 2008 - - 1 Answers - 0 Comments
A. As intermolecular forces increase, both boiling points and melting points will increase. In order to change phase (i.e. solid to liquid or liquid to gas) one must break the intermolecular forces holding molecules together. Greater intermolecular forces require higher temperatures (more energy) to break. By the same argument, vapor pressure should decrease with increasing intermolecular forces. At a given temperature, fewer molecules will be able to achieve the gas state, so the vapor pressure should be smaller.
Answered by triadspectre - Wed Jan 9 22:49:00 2008
List the major types of intermolecular forces of increasing strength.Is there some overlap?
Q. List the major types of intermolecular forces of increasing strength.Is there some overlap?
Asked by star_hwrd - Mon Nov 12 09:43:21 2007 - - 1 Answers - 0 Comments
A. generally speaking ionic interaction (pos w/ neg) > hydrogen bonding > dipole-dipole > van der waals forces will trend is this order but there is no fixed physical law
Answered by ferrous lad - Mon Nov 12 09:52:12 2007
Q. List the major types of intermolecular forces of increasing strength.Is there some overlap?
Asked by star_hwrd - Mon Nov 12 09:43:21 2007 - - 1 Answers - 0 Comments
A. generally speaking ionic interaction (pos w/ neg) > hydrogen bonding > dipole-dipole > van der waals forces will trend is this order but there is no fixed physical law
Answered by ferrous lad - Mon Nov 12 09:52:12 2007
I f we increase the molecular weight in a single compound, would any of the intermolecular forces change?
Q. I f we increase the molecular weight in a single compound, would any of the intermolecular forces change?
Asked by tasha7987 - Sat Feb 25 20:01:37 2006 - - 1 Answers - 0 Comments
A. Not necessarily. Simply changing the actual weight of the compound would not affect the three main types of intermolecular forces (LDF, DD, hydrogen). Heavier compounds do have higher boiling points simply because the molecular weight is higher, requiring more energy to change the state of the molecule.
Answered by JohnnyWash1 - Sun Feb 26 00:13:52 2006
Q. I f we increase the molecular weight in a single compound, would any of the intermolecular forces change?
Asked by tasha7987 - Sat Feb 25 20:01:37 2006 - - 1 Answers - 0 Comments
A. Not necessarily. Simply changing the actual weight of the compound would not affect the three main types of intermolecular forces (LDF, DD, hydrogen). Heavier compounds do have higher boiling points simply because the molecular weight is higher, requiring more energy to change the state of the molecule.
Answered by JohnnyWash1 - Sun Feb 26 00:13:52 2006
Explain which intermolecular forces are affected by increasing the temperature of a protein?
Q. Explain which intermolecular forces are affected by increasing the temperature of a protein?
Asked by 2 ears, 1 mouth - Thu May 7 13:59:14 2009 - - 2 Answers - 0 Comments
A. Hydrogen bonding. proteins get their shape by hydrogen bonding, so heat increases the kinetic energy of the molecules and denatures it
Answered by Brews - Thu May 7 14:02:53 2009
Q. Explain which intermolecular forces are affected by increasing the temperature of a protein?
Asked by 2 ears, 1 mouth - Thu May 7 13:59:14 2009 - - 2 Answers - 0 Comments
A. Hydrogen bonding. proteins get their shape by hydrogen bonding, so heat increases the kinetic energy of the molecules and denatures it
Answered by Brews - Thu May 7 14:02:53 2009
Would you expect these to increase, decrease, or no change?
Q. Answer each of the following questions. (Select I-Increase, D-Decrease, N-Not change. If the first is I and the rest D, enter IDDD). A) The vapor pressure will ... if the surface area increases. B) The equilibrium vapor pressure will ... when the temperature of the liquid is raised. C) If the intermolecular forces decrease in going from one liquid to another, the normal boiling point will ...? D) If the intermolecular forces increase in going from one liquid to another, the equilibrium vapor pressure will ...?
Asked by blah!!! - Wed Apr 8 10:37:35 2009 - - 3 Answers - 0 Comments
Q. Answer each of the following questions. (Select I-Increase, D-Decrease, N-Not change. If the first is I and the rest D, enter IDDD). A) The vapor pressure will ... if the surface area increases. B) The equilibrium vapor pressure will ... when the temperature of the liquid is raised. C) If the intermolecular forces decrease in going from one liquid to another, the normal boiling point will ...? D) If the intermolecular forces increase in going from one liquid to another, the equilibrium vapor pressure will ...?
Asked by blah!!! - Wed Apr 8 10:37:35 2009 - - 3 Answers - 0 Comments
What are the types of intermolecular forces that act between molecules of hydrocarbons used in fuels?
Q. And do they, if at all, increase the hydrocarbons capability as a fuel?
Asked by Riszle - Tue Mar 31 12:29:16 2009 - - 1 Answers - 0 Comments
A. Only weak van der waals forces exist between hydrocarbons. Because there are only weak forces, the boiling point of hydrocarbons is much lower than similar polar molecules. This often makes them gases or liquids e.g. methane, ethane, propane and butane are all gases. I suppose the reason this makes them good fuels is it takes less energy to break the intermolecular interactions and so ignites more easily.
Answered by Griffin - Tue Mar 31 12:41:31 2009
Q. And do they, if at all, increase the hydrocarbons capability as a fuel?
Asked by Riszle - Tue Mar 31 12:29:16 2009 - - 1 Answers - 0 Comments
A. Only weak van der waals forces exist between hydrocarbons. Because there are only weak forces, the boiling point of hydrocarbons is much lower than similar polar molecules. This often makes them gases or liquids e.g. methane, ethane, propane and butane are all gases. I suppose the reason this makes them good fuels is it takes less energy to break the intermolecular interactions and so ignites more easily.
Answered by Griffin - Tue Mar 31 12:41:31 2009
Which of the following statements is true regarding intermolecular forces?
Q. a. They act only between oppositely charged ions b. They are stronger than chemical bonds. c. They act over short increase d. They increase as molecules get farther apart. 2. A dipole-dipole force is strongest when the molecules are a. far apart b. non polar c. strongly polar d. large 3. As dip-dipole forces increase, melting points a. increase b. decrease c. remain the same d. cannot be predicted Water's relatively high boiling points is the result of a. Covalent bonding b. hydrogen bonding. c. ionic bonding d. London Forces
Asked by bashir442003 - Sun Mar 29 21:16:26 2009 - - 1 Answers - 0 Comments
A. I think answer C in question #1 is supposed to read: They act over short distances. The word "increase" there obviously does not make any sense. The correct answer for #1 is my version of C. #2. they are strongest when the molecules are strongly polar. #3. As the dipole-dipole forces increase, the melting points increase. Answer A. (stronger attraction means more energy is needed to get the molecules away from each other). #4. B. Hydrogen Bonding
Answered by Cian - Sun Mar 29 21:50:33 2009
Q. a. They act only between oppositely charged ions b. They are stronger than chemical bonds. c. They act over short increase d. They increase as molecules get farther apart. 2. A dipole-dipole force is strongest when the molecules are a. far apart b. non polar c. strongly polar d. large 3. As dip-dipole forces increase, melting points a. increase b. decrease c. remain the same d. cannot be predicted Water's relatively high boiling points is the result of a. Covalent bonding b. hydrogen bonding. c. ionic bonding d. London Forces
Asked by bashir442003 - Sun Mar 29 21:16:26 2009 - - 1 Answers - 0 Comments
A. I think answer C in question #1 is supposed to read: They act over short distances. The word "increase" there obviously does not make any sense. The correct answer for #1 is my version of C. #2. they are strongest when the molecules are strongly polar. #3. As the dipole-dipole forces increase, the melting points increase. Answer A. (stronger attraction means more energy is needed to get the molecules away from each other). #4. B. Hydrogen Bonding
Answered by Cian - Sun Mar 29 21:50:33 2009
Chemistry help!!! Intermolecular forces!!?
Q. Place the following compounds in order of increasing strength of intermolecular forces. CO2 F2 NH2CH3 Also, how do i figure it out?? I'm desperate!! Thank you!!
Asked by phys - Sun Dec 7 00:13:38 2008 - - 2 Answers - 0 Comments
A. F2 is non-polar, therefore it only has dispersion forces. CO2 is polar, and is a molecule, therefore it has both dispersion forces and dipole-dipole forces. NH2CH3 is polar and has an NH pairing, which gives it a Hydrogen bond, therefore it has dispersion forces, dipole-dipole forces and Hydrogen bonding, making it the strongest the three intermolecular forces.
Answered by IIwintermuteII - Sun Dec 7 00:26:47 2008
Q. Place the following compounds in order of increasing strength of intermolecular forces. CO2 F2 NH2CH3 Also, how do i figure it out?? I'm desperate!! Thank you!!
Asked by phys - Sun Dec 7 00:13:38 2008 - - 2 Answers - 0 Comments
A. F2 is non-polar, therefore it only has dispersion forces. CO2 is polar, and is a molecule, therefore it has both dispersion forces and dipole-dipole forces. NH2CH3 is polar and has an NH pairing, which gives it a Hydrogen bond, therefore it has dispersion forces, dipole-dipole forces and Hydrogen bonding, making it the strongest the three intermolecular forces.
Answered by IIwintermuteII - Sun Dec 7 00:26:47 2008
which is stronger intermolecular force- london forces or dipole-dipole?
Q. i've found so many different sources arguing each way - is one always stronger or does it just depend on the molecule? i thought dipole-dipole would be stronger but the fact that the boiling point of the hydrogen halides increases with increasing number of electrons from Cl to I suggests that increasing london forces are more important than the loss of dipole-dipole forces. is this an exception or are london forces always stronger?
Asked by SB1 - Mon May 25 19:27:51 2009 - - 3 Answers - 0 Comments
Q. i've found so many different sources arguing each way - is one always stronger or does it just depend on the molecule? i thought dipole-dipole would be stronger but the fact that the boiling point of the hydrogen halides increases with increasing number of electrons from Cl to I suggests that increasing london forces are more important than the loss of dipole-dipole forces. is this an exception or are london forces always stronger?
Asked by SB1 - Mon May 25 19:27:51 2009 - - 3 Answers - 0 Comments
Intermolecular forces and boiling points?
Q. 1.) Based upon the strength of the intermolecular attraction and the relative molecular masses, rank the following in order of increasing boiling point from lowest to highest. A) PH3 B) AsH3 C) SbH3 D) NH3 2.) Does the following increase or decrease? A) If the intermolecular forces decrease in going from one liquid to another, the equilibrium vapor pressure will ...? B) The vapor pressure will ... if the surface area increases. C) The equilibrium vapor pressure will ... when the temperature of the liquid is lowered. D) If the intermolecular forces decrease in going from one liquid to another, the normal boiling point will ...?
Asked by alabamian_girl - Sun Apr 12 22:33:11 2009 - - 1 Answers - 0 Comments
A. Visit these sites to learn more about chemistry formulas and concepts that can help you in regards to your problem:
Answered by Dhan Noon - Thu Apr 16 21:47:21 2009
Q. 1.) Based upon the strength of the intermolecular attraction and the relative molecular masses, rank the following in order of increasing boiling point from lowest to highest. A) PH3 B) AsH3 C) SbH3 D) NH3 2.) Does the following increase or decrease? A) If the intermolecular forces decrease in going from one liquid to another, the equilibrium vapor pressure will ...? B) The vapor pressure will ... if the surface area increases. C) The equilibrium vapor pressure will ... when the temperature of the liquid is lowered. D) If the intermolecular forces decrease in going from one liquid to another, the normal boiling point will ...?
Asked by alabamian_girl - Sun Apr 12 22:33:11 2009 - - 1 Answers - 0 Comments
A. Visit these sites to learn more about chemistry formulas and concepts that can help you in regards to your problem:
Answered by Dhan Noon - Thu Apr 16 21:47:21 2009
Viscosity increases with increased intermolecular force?
Q. Viscosity increases with increased intermolecular force because the molecules attract each other strongly which hinders the flow. True or False
Asked by deanjp - Mon Jul 6 20:19:26 2009 - - 1 Answers - 0 Comments
A. True.
Answered by Steve B - Wed Jul 8 23:11:42 2009
Q. Viscosity increases with increased intermolecular force because the molecules attract each other strongly which hinders the flow. True or False
Asked by deanjp - Mon Jul 6 20:19:26 2009 - - 1 Answers - 0 Comments
A. True.
Answered by Steve B - Wed Jul 8 23:11:42 2009
----Intermolecular Forces I NEED HELP!!!!!!!!!!!!!!------?
Q. 1. State the predominant intermolecular forces in each compound. methyl alcohol ethyl alcohol acetone water 2. Why does acetone have a lower boiling point than the rest? 3. Why does water have a high boiling point than the alcohols? 4. If you kept increasing the length of the carbon chain in the alcohols, would the boiling point increase infinitely ? Explain why or why not.
Asked by Soojin - Tue May 12 19:16:59 2009 - - 1 Answers - 0 Comments
Q. 1. State the predominant intermolecular forces in each compound. methyl alcohol ethyl alcohol acetone water 2. Why does acetone have a lower boiling point than the rest? 3. Why does water have a high boiling point than the alcohols? 4. If you kept increasing the length of the carbon chain in the alcohols, would the boiling point increase infinitely ? Explain why or why not.
Asked by Soojin - Tue May 12 19:16:59 2009 - - 1 Answers - 0 Comments
Intermolecular forces and vapor pressure?
Q. Answer each of the following questions. Select I-Increase, D-Decrease, N-Not change. A) The normal boiling point will ... if the intermolecular forces get larger. B) If the intermolecular forces decrease in going from one liquid to another, the equilibrium vapor pressure will ...? C) The vapor pressure will ... if the surface area increases. D) If the temperature of a liquid is raised, the equilibrium vapor pressure will ...? this is what i figured out: A. increase B. decrease C. not change D. decrease what am i doing wrong? maybe i just don't understand the relationship between equilibrium vapor pressure and temperature?
Asked by Jane - Thu Dec 10 11:44:01 2009 - - 1 Answers - 0 Comments
A. The vapor pressure of a substance is directly proportional to the number of molecules of that substance that are in the gas phase. In order to get into the gas phase, the attractive intermolecular forces that hold the substance together in the condensed phase (liquid or solid) must be overcome by the thermal (kinetic) energy of the molecules. The higher the temperature, the greater the kinetic energy of the molecules and the greater is the fraction of them with enough energy to escape into the vapor. That leads to the answer for D: D. increase The stronger the intermolecular (attractive) forces are, the more energy that is required to overcome them, hence a higher temperature is required to get to1.0 atm. vapor pressure. Therefore,… [cont.]
Answered by Timothy - Sun Dec 13 21:23:01 2009
Q. Answer each of the following questions. Select I-Increase, D-Decrease, N-Not change. A) The normal boiling point will ... if the intermolecular forces get larger. B) If the intermolecular forces decrease in going from one liquid to another, the equilibrium vapor pressure will ...? C) The vapor pressure will ... if the surface area increases. D) If the temperature of a liquid is raised, the equilibrium vapor pressure will ...? this is what i figured out: A. increase B. decrease C. not change D. decrease what am i doing wrong? maybe i just don't understand the relationship between equilibrium vapor pressure and temperature?
Asked by Jane - Thu Dec 10 11:44:01 2009 - - 1 Answers - 0 Comments
A. The vapor pressure of a substance is directly proportional to the number of molecules of that substance that are in the gas phase. In order to get into the gas phase, the attractive intermolecular forces that hold the substance together in the condensed phase (liquid or solid) must be overcome by the thermal (kinetic) energy of the molecules. The higher the temperature, the greater the kinetic energy of the molecules and the greater is the fraction of them with enough energy to escape into the vapor. That leads to the answer for D: D. increase The stronger the intermolecular (attractive) forces are, the more energy that is required to overcome them, hence a higher temperature is required to get to1.0 atm. vapor pressure. Therefore,… [cont.]
Answered by Timothy - Sun Dec 13 21:23:01 2009
intermolecular forces question?
Q. what IM forces are present in acetone, glycerin, pentane, 1-pentanol, and water? rank them in increasing relative strength of IM forces..and why?
Asked by nomad - Sun Nov 8 14:55:06 2009 - - 1 Answers - 0 Comments
A. First of all, ALL molecules have the weak London dispersion forces. Acetone: somewhat polar so it has dipole-dipole forces. Glycerin: also called glycerol, it has three -OH groups so it has hydrogen bonding, the strongest of the three forces. Pentane: nonpolar; has only weak London forces. 1-pentanol: has one -OH group, but hydrogen bonding ability is overshadowed by the nonpolar five-carbon chain (insoluble in H2O) Water: very polar, shows very strong H bonding. Ranked from lowest to highest: pentane < 1-pentanol < acetone < water < glycerol? I'm a little unsure about the order of glycerol and water. Glycerol is more polar (dipole moment = 2.7 vs water at 1.8) but glycerol is a much larger molecule (molar mass = 92 vs 18 for H2O).
Answered by HPV - Sun Nov 8 15:10:50 2009
Q. what IM forces are present in acetone, glycerin, pentane, 1-pentanol, and water? rank them in increasing relative strength of IM forces..and why?
Asked by nomad - Sun Nov 8 14:55:06 2009 - - 1 Answers - 0 Comments
A. First of all, ALL molecules have the weak London dispersion forces. Acetone: somewhat polar so it has dipole-dipole forces. Glycerin: also called glycerol, it has three -OH groups so it has hydrogen bonding, the strongest of the three forces. Pentane: nonpolar; has only weak London forces. 1-pentanol: has one -OH group, but hydrogen bonding ability is overshadowed by the nonpolar five-carbon chain (insoluble in H2O) Water: very polar, shows very strong H bonding. Ranked from lowest to highest: pentane < 1-pentanol < acetone < water < glycerol? I'm a little unsure about the order of glycerol and water. Glycerol is more polar (dipole moment = 2.7 vs water at 1.8) but glycerol is a much larger molecule (molar mass = 92 vs 18 for H2O).
Answered by HPV - Sun Nov 8 15:10:50 2009
Help! this is a chemistry question regarding intermolecular forces?
Q. How do you rank the following solutions in terms of increasing magnitude of solute-solvent interaction and indicate the principal type of interaction in each case: (a) KCl in water; (b) CH2Cl2 in benzene, C6H6; (c) acetone, (CH3)2CO, in water.
Asked by mashedpotatomonk - Wed Jan 2 19:47:51 2008 - - 3 Answers - 0 Comments
A. b dipole-dipole c hydrogen bonding a ion-dipole
Answered by pinochleplayer115 - Wed Jan 2 19:54:53 2008
Q. How do you rank the following solutions in terms of increasing magnitude of solute-solvent interaction and indicate the principal type of interaction in each case: (a) KCl in water; (b) CH2Cl2 in benzene, C6H6; (c) acetone, (CH3)2CO, in water.
Asked by mashedpotatomonk - Wed Jan 2 19:47:51 2008 - - 3 Answers - 0 Comments
A. b dipole-dipole c hydrogen bonding a ion-dipole
Answered by pinochleplayer115 - Wed Jan 2 19:54:53 2008
From Yahoo Answer Search: 'intermolecular forces increase'
Thu Mar 4 07:48:26 2010 [ refresh local cache ]
[Hide]▼
lhsblogs.typepad.com
Veronica Cook
hu, 23 Apr 2009 19:41:55 GM
but we know they do! van der waal's . intermolecular forces. . at high temperatures with lots of ke, these weak . forces. have little effect. at low temperatures (near the substance's boiling point), the . intermolecular forces. matter. ...
[Hide]▲
