InterMolecular Forces!?
Q. Explain in terms of intermolecular forces why A. NH3 has a higher boiling point than CH4 B.KCL has a higher melting point than I2
Asked by HoMunCuLus - Sat Sep 23 23:33:05 2006 - - 2 Answers - 0 Comments
A. A. NH3 has hydrogen bonding while CH4 has London forces... hydrogen bonding is relatively stronger than London forces... higher IMFA means higher energy to break that force and turn the compound to its vapor phase, thus higher boiling point... B. KCl has ion-ion forces which is the strongest IMFA while I2 has London forces which is the weakest of them all... best answer?
Answered by teroy - Sat Sep 23 23:46:26 2006
Q. Explain in terms of intermolecular forces why A. NH3 has a higher boiling point than CH4 B.KCL has a higher melting point than I2
Asked by HoMunCuLus - Sat Sep 23 23:33:05 2006 - - 2 Answers - 0 Comments
A. A. NH3 has hydrogen bonding while CH4 has London forces... hydrogen bonding is relatively stronger than London forces... higher IMFA means higher energy to break that force and turn the compound to its vapor phase, thus higher boiling point... B. KCl has ion-ion forces which is the strongest IMFA while I2 has London forces which is the weakest of them all... best answer?
Answered by teroy - Sat Sep 23 23:46:26 2006
What type of intermolecular forces operate for hexane and water individually?
Q. What type of intermolecular forces operate for hexane and water individually? When they are mixed are there stronger or weaker forces operating between the two components of the mixture than within each pure liquid? And which operate for 1-butanol and water, and acetone and water.
Asked by Chelsey - Tue Feb 2 16:15:53 2010 - - 3 Answers - 0 Comments
A. Hexane C6H14 - has London dispersion forces Water-H2O has hydrogen bonds when hexane and water are mixed the intermolecular force is weak London dispersion forces When 1-butanol and water are mixed the intermolecular force is H-bonding( both have -OH groups) When acetone and water are mixed the intermolecular force is dipole-dipole attraction
Answered by halogen - Tue Feb 2 16:23:29 2010
Q. What type of intermolecular forces operate for hexane and water individually? When they are mixed are there stronger or weaker forces operating between the two components of the mixture than within each pure liquid? And which operate for 1-butanol and water, and acetone and water.
Asked by Chelsey - Tue Feb 2 16:15:53 2010 - - 3 Answers - 0 Comments
A. Hexane C6H14 - has London dispersion forces Water-H2O has hydrogen bonds when hexane and water are mixed the intermolecular force is weak London dispersion forces When 1-butanol and water are mixed the intermolecular force is H-bonding( both have -OH groups) When acetone and water are mixed the intermolecular force is dipole-dipole attraction
Answered by halogen - Tue Feb 2 16:23:29 2010
What kind of intermolecular forces exist in this situation?
Q. What kind of intermolecular forces exist between the ethyl (CH3CH2-) of the ethanol molecule and surrounding water molecules? I know for sure it's not hydrogen bonding because the OH group of ethanol participates in this, not the ethyl group. Any help would be great, thanks :)
Asked by LuLu - Sat Feb 7 20:57:54 2009 - - 1 Answers - 0 Comments
A. Van der Waals forces, aka. London dispersion forces, aka. Induced dipole/dipole forces! Take your pick on the name, they all mean the same thing. Just in case you don't know what these are, basically the theory is that when large molecules get close enough to each other, the electron clouds on each molecule will interact, causing them to tend to congregate on one side of the molecule, making it have a pseudo-positive and a pseudo-negative charge on either end. This causes them to group closer to one another.
Answered by Colin - Sat Feb 7 21:06:15 2009
Q. What kind of intermolecular forces exist between the ethyl (CH3CH2-) of the ethanol molecule and surrounding water molecules? I know for sure it's not hydrogen bonding because the OH group of ethanol participates in this, not the ethyl group. Any help would be great, thanks :)
Asked by LuLu - Sat Feb 7 20:57:54 2009 - - 1 Answers - 0 Comments
A. Van der Waals forces, aka. London dispersion forces, aka. Induced dipole/dipole forces! Take your pick on the name, they all mean the same thing. Just in case you don't know what these are, basically the theory is that when large molecules get close enough to each other, the electron clouds on each molecule will interact, causing them to tend to congregate on one side of the molecule, making it have a pseudo-positive and a pseudo-negative charge on either end. This causes them to group closer to one another.
Answered by Colin - Sat Feb 7 21:06:15 2009
intermolecular forces how do you determine? polarity is part how do i determine polarity of a molecule?
Q. I need help understanding intermolecular forces and a lot of it has to do with whether it is nonpolar or polar and i need help understanding how to determine whether a molecule is polar or nonpolar is there a system like one is usually nonmetal w/ metal or something i thought i learned that before?
Asked by imjustmewhatelseshouldibe - Sun Jan 28 10:03:32 2007 - - 2 Answers - 0 Comments
A. (a nonmetal and metal are ionic bonds) You need to look at a chart of the electronegativity of the elements. Subtract the electronegativity of the two atoms bonding. A difference of 0 to 0.4 is a nonpolar covelent bond. A difference of 0.5 to 1.4 is a polar covalent bond. A difference over 1.4 is an ionic bond.
Answered by physandchemteach - Sun Jan 28 10:10:06 2007
Q. I need help understanding intermolecular forces and a lot of it has to do with whether it is nonpolar or polar and i need help understanding how to determine whether a molecule is polar or nonpolar is there a system like one is usually nonmetal w/ metal or something i thought i learned that before?
Asked by imjustmewhatelseshouldibe - Sun Jan 28 10:03:32 2007 - - 2 Answers - 0 Comments
A. (a nonmetal and metal are ionic bonds) You need to look at a chart of the electronegativity of the elements. Subtract the electronegativity of the two atoms bonding. A difference of 0 to 0.4 is a nonpolar covelent bond. A difference of 0.5 to 1.4 is a polar covalent bond. A difference over 1.4 is an ionic bond.
Answered by physandchemteach - Sun Jan 28 10:10:06 2007
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
How do I test for intermolecular forces?
Q. What materials can I use to find intermolecular forces in a substance such as acetone, hexane, methanol?
Asked by Maximino - Mon Mar 23 20:13:18 2009 - - 3 Answers - 0 Comments
A. You can measure the boiling point. Generally, the higher the boiling point, the greater the intermolecular forces. Here are some methods for boiling point determination:
Answered by David H - Mon Mar 23 20:20:53 2009
Q. What materials can I use to find intermolecular forces in a substance such as acetone, hexane, methanol?
Asked by Maximino - Mon Mar 23 20:13:18 2009 - - 3 Answers - 0 Comments
A. You can measure the boiling point. Generally, the higher the boiling point, the greater the intermolecular forces. Here are some methods for boiling point determination:
Answered by David H - Mon Mar 23 20:20:53 2009
For which of the following molecules would the intermolecular forces be due mainly to London forces?
Q. For which of the following molecules would the intermolecular forces be due mainly to London forces? H2 BF3 NI3 O2 C2H5OH Thanks for the answer, and although it seemed logical, I checked it and that was wrong :(
Asked by bt_artist - Wed Nov 26 14:10:38 2008 - - 1 Answers - 0 Comments
A. What you're looking for here is a non-ionic, non-polar, non-hydrogen bonding molecule. This definitely eliminates C2H5OH, which can hydrogen bond due to its OH (alcohol) group. I would say that BF3 and NI3 are polar enough to have dipole-dipole interactions, so those are also ruled out. This leaves H2 and O2... These molecules meet the criteria that I outlined above (non-ionic, non-polar, non-hydrogen bonding), which means that their predominant force would be London Forces (aka- London Dispersion Forces). Hope that helps!
Answered by J - Wed Nov 26 14:50:28 2008
Q. For which of the following molecules would the intermolecular forces be due mainly to London forces? H2 BF3 NI3 O2 C2H5OH Thanks for the answer, and although it seemed logical, I checked it and that was wrong :(
Asked by bt_artist - Wed Nov 26 14:10:38 2008 - - 1 Answers - 0 Comments
A. What you're looking for here is a non-ionic, non-polar, non-hydrogen bonding molecule. This definitely eliminates C2H5OH, which can hydrogen bond due to its OH (alcohol) group. I would say that BF3 and NI3 are polar enough to have dipole-dipole interactions, so those are also ruled out. This leaves H2 and O2... These molecules meet the criteria that I outlined above (non-ionic, non-polar, non-hydrogen bonding), which means that their predominant force would be London Forces (aka- London Dispersion Forces). Hope that helps!
Answered by J - Wed Nov 26 14:50:28 2008
what happens to the intermolecular forces when a polymer reaches its glass transition temperature?
Q. i've heard that the polymer chains become more crystalline which is the reason that makes it more hard due to the greater number of intermolecular forces. However, I don't understand how it becomes more brittle? I mean it makes sense, I've seen it happen to plastics but why? in terms of intermolecular forces :P
Asked by jackinthesack - Tue Feb 23 10:04:58 2010 - - 1 Answers - 0 Comments
A. In polymers the glass transition temperature, Tg, is often expressed as the temperature at which the Gibbs free energy is such that the activation energy for the cooperative movement of 50 or so units of the polymer is exceeded. This allows molecular chains to slide past each other when a force is applied. Below the Tg, therefore, the activation energy required to allow molecular flexibility is not achieved and you have a brittle (highly inflexible) polymer.
Answered by sieg6529 - Tue Feb 23 10:16:50 2010
Q. i've heard that the polymer chains become more crystalline which is the reason that makes it more hard due to the greater number of intermolecular forces. However, I don't understand how it becomes more brittle? I mean it makes sense, I've seen it happen to plastics but why? in terms of intermolecular forces :P
Asked by jackinthesack - Tue Feb 23 10:04:58 2010 - - 1 Answers - 0 Comments
A. In polymers the glass transition temperature, Tg, is often expressed as the temperature at which the Gibbs free energy is such that the activation energy for the cooperative movement of 50 or so units of the polymer is exceeded. This allows molecular chains to slide past each other when a force is applied. Below the Tg, therefore, the activation energy required to allow molecular flexibility is not achieved and you have a brittle (highly inflexible) polymer.
Answered by sieg6529 - Tue Feb 23 10:16:50 2010
What type of intermolecular forces would you expect to be the predominant (strongest)forces in a sample of..?
Q. What type of intermolecular forces would you expect to be the predominant (strongest) forces in a sample of SrF2? 1. dipole-dipole 2. dispersion 3. ion-ion 4. hydrogen bonding 5. covalent Thanks so much!
Asked by Lauren Chandler - Tue Dec 8 10:09:48 2009 - - 1 Answers - 0 Comments
Q. What type of intermolecular forces would you expect to be the predominant (strongest) forces in a sample of SrF2? 1. dipole-dipole 2. dispersion 3. ion-ion 4. hydrogen bonding 5. covalent Thanks so much!
Asked by Lauren Chandler - Tue Dec 8 10:09:48 2009 - - 1 Answers - 0 Comments
How does one determine the intermolecular forces between these molecules?
Q. The problem is: The C-Cl bonds in CCl4 are polar covalent. What intermolecular attraction exists between CCl4 molecules? A. van der waals forces B. hydrogen bonding C. Polar covalent bonds D. dipole-dipole forces E. dipole-induced dipole foces An explanation would me much appreciated!
Asked by Graham D - Sun May 18 15:05:30 2008 - - 3 Answers - 0 Comments
A. With all due respect I believe the previous two posters to be incorrect. Please read on. Yes, but even if the C-Cl bonds are polar, the symmetry of the molecule means that all of the individual dipole moments cancel out to give a zero net dipole moment for the compound. Therefore the only van der Waals force that exists for CCl4 is London dispersion forces. All compounds in every substance exhibit London dispersion forces. In some cases they may be small compared to hydrogen bonding or dipole-dipole interactions, or even covalent network bonds. But in the case of CCl4 there are no other IMF's, and so London dispersion forces are it. By the way, (A) is a bit problematic because van der Waals forces encompass all of the various kids… [cont.]
Answered by pisgahchemist - Sun May 18 15:24:36 2008
Q. The problem is: The C-Cl bonds in CCl4 are polar covalent. What intermolecular attraction exists between CCl4 molecules? A. van der waals forces B. hydrogen bonding C. Polar covalent bonds D. dipole-dipole forces E. dipole-induced dipole foces An explanation would me much appreciated!
Asked by Graham D - Sun May 18 15:05:30 2008 - - 3 Answers - 0 Comments
A. With all due respect I believe the previous two posters to be incorrect. Please read on. Yes, but even if the C-Cl bonds are polar, the symmetry of the molecule means that all of the individual dipole moments cancel out to give a zero net dipole moment for the compound. Therefore the only van der Waals force that exists for CCl4 is London dispersion forces. All compounds in every substance exhibit London dispersion forces. In some cases they may be small compared to hydrogen bonding or dipole-dipole interactions, or even covalent network bonds. But in the case of CCl4 there are no other IMF's, and so London dispersion forces are it. By the way, (A) is a bit problematic because van der Waals forces encompass all of the various kids… [cont.]
Answered by pisgahchemist - Sun May 18 15:24:36 2008
Why do some alcohols have stronger intermolecular forces than others?
Q. For example, methanol has stronger forces than ethanol, 1 propanol, and 1-butanol. Why? What causes it to have stronger intermolecular forces? (plz provide ur source).
Asked by Meh - Fri Oct 23 21:41:44 2009 - - 1 Answers - 0 Comments
A. The hydroxyl group is what gives strong hydrogen bonding. The hydroxyl group makes up a bigger percent of methanol's total size than the others you mentioned (since methanol is so small).
Answered by E - Fri Oct 23 22:21:37 2009
Q. For example, methanol has stronger forces than ethanol, 1 propanol, and 1-butanol. Why? What causes it to have stronger intermolecular forces? (plz provide ur source).
Asked by Meh - Fri Oct 23 21:41:44 2009 - - 1 Answers - 0 Comments
A. The hydroxyl group is what gives strong hydrogen bonding. The hydroxyl group makes up a bigger percent of methanol's total size than the others you mentioned (since methanol is so small).
Answered by E - Fri Oct 23 22:21:37 2009
In which of the following are intermolecular forces the strongest and which has lowest boiling point?
Q. hexane cyclohexane 2-methylpentane out of these three compounds: 1. which one has the strongest intermolecular forces? 2. which one has the lowest boiling point?
Asked by melanie - Mon Jul 6 01:13:24 2009 - - 2 Answers - 0 Comments
A. cyclohexane boiling point is 80.74 degrees Celsius, hexane is 69 C*, 2-methylpentane is 60C*! Thats one answer!
Answered by BloodDimond85 - Mon Jul 6 01:43:46 2009
Q. hexane cyclohexane 2-methylpentane out of these three compounds: 1. which one has the strongest intermolecular forces? 2. which one has the lowest boiling point?
Asked by melanie - Mon Jul 6 01:13:24 2009 - - 2 Answers - 0 Comments
A. cyclohexane boiling point is 80.74 degrees Celsius, hexane is 69 C*, 2-methylpentane is 60C*! Thats one answer!
Answered by BloodDimond85 - Mon Jul 6 01:43:46 2009
Can you help me with my intermolecular forces lab?
Q. We floated yen on liquid water. I need to know if yen is more or less dense than water and explain the difference with atomic models. Also, I need to know the intermolecular forces (all of them) for water, isopropanol, and acetone). This is a lot, but any help is appreciated.
Asked by Robert Moran - Mon Feb 2 21:03:19 2009 - - 1 Answers - 0 Comments
A. if its floats on it that means that it is less dense as each molecule weighs less. the intermolecules forces in water are hydrogen bonds (which is why it has a high boiling point isoproanol and acetone are just van der Waals for all i know i hope this helps
Answered by George - Thu Feb 5 08:37:08 2009
Q. We floated yen on liquid water. I need to know if yen is more or less dense than water and explain the difference with atomic models. Also, I need to know the intermolecular forces (all of them) for water, isopropanol, and acetone). This is a lot, but any help is appreciated.
Asked by Robert Moran - Mon Feb 2 21:03:19 2009 - - 1 Answers - 0 Comments
A. if its floats on it that means that it is less dense as each molecule weighs less. the intermolecules forces in water are hydrogen bonds (which is why it has a high boiling point isoproanol and acetone are just van der Waals for all i know i hope this helps
Answered by George - Thu Feb 5 08:37:08 2009
Using the concepts of how kinetic energy is related to temperature and intermolecular forces...?
Q. Using the concepts of how kinetic energy is related to temperature and intermolecular forces, explain why the temperature must level off until the phase change is complete. please helpp.
Asked by confuzzled - Sun Feb 24 23:26:47 2008 - - 1 Answers - 0 Comments
A. mmm...Kinetic energy will cure what ails ya...lol Kinetic energy can be best understood by examples that demonstrate how it is transformed from other forms of energy and to the other forms. For example, a cyclist will use chemical energy that was provided by food to accelerate a bicycle to a chosen speed. This speed can be maintained without further work, except to overcome air-resistance and friction. The energy has been converted into the energy of motion, known as kinetic energy but the process is not completely efficient and heat is also produced within the cyclist. The kinetic energy in the moving bicycle and the cyclist can be converted to other forms. For example, the cyclist could encounter a hill just high enough to coast up, so… [cont.]
Answered by **wj25** - Sun Feb 24 23:34:28 2008
Q. Using the concepts of how kinetic energy is related to temperature and intermolecular forces, explain why the temperature must level off until the phase change is complete. please helpp.
Asked by confuzzled - Sun Feb 24 23:26:47 2008 - - 1 Answers - 0 Comments
A. mmm...Kinetic energy will cure what ails ya...lol Kinetic energy can be best understood by examples that demonstrate how it is transformed from other forms of energy and to the other forms. For example, a cyclist will use chemical energy that was provided by food to accelerate a bicycle to a chosen speed. This speed can be maintained without further work, except to overcome air-resistance and friction. The energy has been converted into the energy of motion, known as kinetic energy but the process is not completely efficient and heat is also produced within the cyclist. The kinetic energy in the moving bicycle and the cyclist can be converted to other forms. For example, the cyclist could encounter a hill just high enough to coast up, so… [cont.]
Answered by **wj25** - Sun Feb 24 23:34:28 2008
are there intermolecular forces between ions in a lattice or giant covalent structures?
Q. i presume because they are not molecules means they don't have IM forces - they are just many atoms or ions held together. does this mean that something like diamond's inability to dissolve in water comes from the need to break strong covalent bonds, rather than to overcome an intermolecular force like in other substances?
Asked by SB1 - Mon May 11 19:07:55 2009 - - 1 Answers - 0 Comments
A. you're correct that diamonds don't dissolve because of strong covalent bonds instead of intermolecular forces. however, remember that all things, everything, have London Dispersion Forces. It's just that you don't really see it's effect unless the molecule is small and can move around.
Answered by anoman5000 - Mon May 11 19:15:23 2009
Q. i presume because they are not molecules means they don't have IM forces - they are just many atoms or ions held together. does this mean that something like diamond's inability to dissolve in water comes from the need to break strong covalent bonds, rather than to overcome an intermolecular force like in other substances?
Asked by SB1 - Mon May 11 19:07:55 2009 - - 1 Answers - 0 Comments
A. you're correct that diamonds don't dissolve because of strong covalent bonds instead of intermolecular forces. however, remember that all things, everything, have London Dispersion Forces. It's just that you don't really see it's effect unless the molecule is small and can move around.
Answered by anoman5000 - Mon May 11 19:15:23 2009
Why do we assume that gas particles experience no intermolecular forces?
Q. a. because its true. b. because gas particles move too quickly to experience intermolecular forces for very long. c. because gas particles are usually a long distance from one another. d. more than one of the above.
Asked by Sarah J - Sun Jan 11 10:31:11 2009 - - 2 Answers - 0 Comments
A. B and C, so D.
Answered by Colin - Sun Jan 11 10:38:38 2009
Q. a. because its true. b. because gas particles move too quickly to experience intermolecular forces for very long. c. because gas particles are usually a long distance from one another. d. more than one of the above.
Asked by Sarah J - Sun Jan 11 10:31:11 2009 - - 2 Answers - 0 Comments
A. B and C, so D.
Answered by Colin - Sun Jan 11 10:38:38 2009
What combination of intermolecular forces will result in a solution where a large amount of solute dissolves?
Q. strong/weak solute-solute intermolecular forces and either strong/weak solute-solvent intermolecular forces? I think that its weak solute-solute and strong solute-solvent.
Asked by Allen - Sat Jul 4 12:14:49 2009 - - 1 Answers - 0 Comments
Q. strong/weak solute-solute intermolecular forces and either strong/weak solute-solvent intermolecular forces? I think that its weak solute-solute and strong solute-solvent.
Asked by Allen - Sat Jul 4 12:14:49 2009 - - 1 Answers - 0 Comments
Which of the following properties indicates the presence of strong intermolecular forces in a liquid?
Q. Which of the following properties indicates the presence of strong intermolecular forces in a liquid? a low heat of vaporization a low critical temperature a low vapor pressure a low boiling point None of the above.
Asked by MB - Sun Apr 13 02:13:29 2008 - - 3 Answers - 0 Comments
A. A low vapor pressure. If there are strong intermolecular forces, that means that a lot of heat is required in order to break the bonds in the liquid form; thus, there will be fewer molecules converting into gas molecules leading to a low vapor pressure. It can't be a low heat of vaporization because that means the forces are weak; same goes for critical temperature and boiling point. Therefore, your answer is C. [Answer: see above]
Answered by /\/ ? - Sun Apr 13 02:17:48 2008
Q. Which of the following properties indicates the presence of strong intermolecular forces in a liquid? a low heat of vaporization a low critical temperature a low vapor pressure a low boiling point None of the above.
Asked by MB - Sun Apr 13 02:13:29 2008 - - 3 Answers - 0 Comments
A. A low vapor pressure. If there are strong intermolecular forces, that means that a lot of heat is required in order to break the bonds in the liquid form; thus, there will be fewer molecules converting into gas molecules leading to a low vapor pressure. It can't be a low heat of vaporization because that means the forces are weak; same goes for critical temperature and boiling point. Therefore, your answer is C. [Answer: see above]
Answered by /\/ ? - Sun Apr 13 02:17:48 2008
Predict which substance in each of the following pairs would have the stronger intermolecular forces?
Q. Predict which substance in each of the following pairs would have the stronger intermolecular forces. Explain. (b) SeO2 SO2 (c) CH3CH2CH2NH2 H2NCH2CH2NH2 (e) CH3OH H2CO
Asked by Hello - Mon May 11 22:07:11 2009 - - 3 Answers - 0 Comments
A. Hello , 1. SO2 vs. SeO2: sulfur and selenium have very similar electronegativities (2.58 vs 2.55); their interactions with oxygen would be quite similar insofar as the polarity of their bonds. However, by virtue of its size (and therefore having a more diffuse electron cloud), selenium is more polarizable than sulfur. That means that as it nears a more electronegative element or group (such as the oxygen end of another molecule), the selenium end will distort to become more electropositive than sulfur will. ***SeO2*** 2. CH3CH2CH2NH2 vs. H2NCH2CH2NH2: both are amines, but the first has a single amine group, while the second has two amine groups. When you consider hydrogen bonding (the attractive force between one electronegative… [cont.]
Answered by Dr. Buzz - Tue May 12 22:50:41 2009
Q. Predict which substance in each of the following pairs would have the stronger intermolecular forces. Explain. (b) SeO2 SO2 (c) CH3CH2CH2NH2 H2NCH2CH2NH2 (e) CH3OH H2CO
Asked by Hello - Mon May 11 22:07:11 2009 - - 3 Answers - 0 Comments
A. Hello , 1. SO2 vs. SeO2: sulfur and selenium have very similar electronegativities (2.58 vs 2.55); their interactions with oxygen would be quite similar insofar as the polarity of their bonds. However, by virtue of its size (and therefore having a more diffuse electron cloud), selenium is more polarizable than sulfur. That means that as it nears a more electronegative element or group (such as the oxygen end of another molecule), the selenium end will distort to become more electropositive than sulfur will. ***SeO2*** 2. CH3CH2CH2NH2 vs. H2NCH2CH2NH2: both are amines, but the first has a single amine group, while the second has two amine groups. When you consider hydrogen bonding (the attractive force between one electronegative… [cont.]
Answered by Dr. Buzz - Tue May 12 22:50:41 2009
Is the strength of intermolecular forces determined by the bond strenghts within the individual molecules?
Q. Is the strength of intermolecular forces determined by the bond strenghts within the individual molecules?
Asked by Hansol - Tue Jan 19 21:41:19 2010 - - 1 Answers - 0 Comments
A. Not exactly. There are several factors the determine the strength of intermolecular forces. The only situation that intramolecular forces determine it is when we have a situation like this: Say O-H --- N-H and O-H--- O-H. The broken likes represent intermolecular attraction. The second interaction is expected to be stronger. In either case, the H attached to the O is less available for intermolecular bonding because O is very electronegative. Then N is even less electronegative that O so the intermolecular bond is even weaker because the H is more attracted to the O. Unlike in the second O, there seems to be a tug of war between the two O's. This reasoning is not always true especially for non polar compounds. In this case,… [cont.]
Answered by Melissa B - Tue Jan 19 22:00:12 2010
Q. Is the strength of intermolecular forces determined by the bond strenghts within the individual molecules?
Asked by Hansol - Tue Jan 19 21:41:19 2010 - - 1 Answers - 0 Comments
A. Not exactly. There are several factors the determine the strength of intermolecular forces. The only situation that intramolecular forces determine it is when we have a situation like this: Say O-H --- N-H and O-H--- O-H. The broken likes represent intermolecular attraction. The second interaction is expected to be stronger. In either case, the H attached to the O is less available for intermolecular bonding because O is very electronegative. Then N is even less electronegative that O so the intermolecular bond is even weaker because the H is more attracted to the O. Unlike in the second O, there seems to be a tug of war between the two O's. This reasoning is not always true especially for non polar compounds. In this case,… [cont.]
Answered by Melissa B - Tue Jan 19 22:00:12 2010
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SaharaReporters.com Just echoes from intermediate science, intermolecular forces are the forces of attraction that exist between molecules in a compound. These forces cause and ...
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On the Fabrics Acetate Arnel Viscose and cotton These four fabrics all have similar structures They form an intricate laticework with few polar sites These fabrics did not hold dye at all well due to
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What type of . intermolecular forces. operate for hexane and water individually? When they are mixed are there stronger or weaker forces operating between the two components of the mixture than within each pure liquid? ...
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