Intermolecular Forces?
Q. I am having troubles witha homework assignment, and am not sure how to do it. Any help would be appreciated! For the following pairs of atoms/molecules, select the species that has the higher boiling point and identify the intermolecular forces (hydrogen bonding, dipole-dipole forces, or London dispersion forces) that cause the differences. a. He or Ne b. NH3 or PH3 c. H2Te or H2O d. BF3 or BCl3 e. CH3CH2OH or CH3CH2CH3 Thanks!
Asked by Chloe G - Mon Nov 19 11:37:54 2007 - - 1 Answers - 0 Comments
A. a) Ne - more electrons than He, therefore more polarizable, so more London forces. b) NH3 - shows hydrogen bonding and PH3 shows dipole. H-bonding is stronger. c) H2O - big time!! hydrogen bonding d) BCl3 - both are nonpolar, so you're looking at London forces only. Cl is less electronegative than F, so the electrons are more mobile. This means more polarizable, so more London forces. Also, BCl3 is bigger than BF3, so more chance for interaction between molecules. e) C2H5OH - hydrogen bonding. The other molecule is nonpolar, so it only has London forces available to it.
Answered by ChemTeam - Mon Nov 19 11:47:45 2007
Q. I am having troubles witha homework assignment, and am not sure how to do it. Any help would be appreciated! For the following pairs of atoms/molecules, select the species that has the higher boiling point and identify the intermolecular forces (hydrogen bonding, dipole-dipole forces, or London dispersion forces) that cause the differences. a. He or Ne b. NH3 or PH3 c. H2Te or H2O d. BF3 or BCl3 e. CH3CH2OH or CH3CH2CH3 Thanks!
Asked by Chloe G - Mon Nov 19 11:37:54 2007 - - 1 Answers - 0 Comments
A. a) Ne - more electrons than He, therefore more polarizable, so more London forces. b) NH3 - shows hydrogen bonding and PH3 shows dipole. H-bonding is stronger. c) H2O - big time!! hydrogen bonding d) BCl3 - both are nonpolar, so you're looking at London forces only. Cl is less electronegative than F, so the electrons are more mobile. This means more polarizable, so more London forces. Also, BCl3 is bigger than BF3, so more chance for interaction between molecules. e) C2H5OH - hydrogen bonding. The other molecule is nonpolar, so it only has London forces available to it.
Answered by ChemTeam - Mon Nov 19 11:47:45 2007
.......intermolecular forces?
Q. since ammonia is polar in nature, does it act on dipole-dipole intermolecular forces? if not, what kind of intermolecular forces does it act on?
Asked by marco poloooooooo - Tue Jun 16 00:42:16 2009 - - 2 Answers - 0 Comments
A. everything has london dispersion forces ammonia might have dipole it's strongest is hydrogen bonding
Answered by jeff - Tue Jun 16 00:49:57 2009
Q. since ammonia is polar in nature, does it act on dipole-dipole intermolecular forces? if not, what kind of intermolecular forces does it act on?
Asked by marco poloooooooo - Tue Jun 16 00:42:16 2009 - - 2 Answers - 0 Comments
A. everything has london dispersion forces ammonia might have dipole it's strongest is hydrogen bonding
Answered by jeff - Tue Jun 16 00:49:57 2009
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 happens to the intermolecular forces between water when methanol is poured into a beaker full of water?
Q. What intermolecular forces are broken in the water when these substances are mixed? What intermolecular forces are formed in the solution when these substances are mixed? What intermolecular forces are broken in the water when these substances are mixed? A. Dispersion forces B. Dipole-dipole interactions C. Hydrogen bonding D. Ion-ion interactions Please choose all the apply. Also: What intermolecular forces are formed in the solution when these substances are mixed? A. Dispersion forces B. Ion-ion interactions C. Dipole-dipole interactions D. Hydrogen bonding Please choose all the apply, thanks!
Asked by Rebecca S - Sat Feb 14 22:39:16 2009 - - 1 Answers - 0 Comments
A. Water is held together by a combination of A, B, and C, with C having the strongest effect. Methanol also has the ability to hydrogen bond, so A, C, and D (from the second set) are formed when the two substances mix.
Answered by TheOnlyBeldin - Sat Feb 14 22:51:42 2009
Q. What intermolecular forces are broken in the water when these substances are mixed? What intermolecular forces are formed in the solution when these substances are mixed? What intermolecular forces are broken in the water when these substances are mixed? A. Dispersion forces B. Dipole-dipole interactions C. Hydrogen bonding D. Ion-ion interactions Please choose all the apply. Also: What intermolecular forces are formed in the solution when these substances are mixed? A. Dispersion forces B. Ion-ion interactions C. Dipole-dipole interactions D. Hydrogen bonding Please choose all the apply, thanks!
Asked by Rebecca S - Sat Feb 14 22:39:16 2009 - - 1 Answers - 0 Comments
A. Water is held together by a combination of A, B, and C, with C having the strongest effect. Methanol also has the ability to hydrogen bond, so A, C, and D (from the second set) are formed when the two substances mix.
Answered by TheOnlyBeldin - Sat Feb 14 22:51:42 2009
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
How to determine the strongest intermolecular forces?
Q. When given choices of substances, how do you figure out which one has the strongest intermolecular forces? Take for example, these choices: H2S NO CH3NH2 Cl2 Rn I picked Cl2 as the answer, but it was wrong... i don't really understand. =[ help?
Asked by Melissa - Sat Mar 7 10:57:19 2009 - - 1 Answers - 0 Comments
A. it depends on bond polarity and molecular polarity the most polar is the molecules the strong are molecular forces here the most polar molecule is H2S
Answered by dvstudio 08 - Tue Mar 10 12:28:16 2009
Q. When given choices of substances, how do you figure out which one has the strongest intermolecular forces? Take for example, these choices: H2S NO CH3NH2 Cl2 Rn I picked Cl2 as the answer, but it was wrong... i don't really understand. =[ help?
Asked by Melissa - Sat Mar 7 10:57:19 2009 - - 1 Answers - 0 Comments
A. it depends on bond polarity and molecular polarity the most polar is the molecules the strong are molecular forces here the most polar molecule is H2S
Answered by dvstudio 08 - Tue Mar 10 12:28:16 2009
What are the principle intermolecular forces in H2O and H2S?
Q. What are the principle intermolecular forces in H2O and H2S? how do they account for the fact that water is a liquid at room temperature whereas Hydrogen Sulfideis a gas? I know it is hydrogen bonding. But why?
Asked by Charles Barkely - Wed Feb 10 08:23:59 2010 - - 1 Answers - 0 Comments
A. Hydrogen bonding is present in the water, not the H2S. Hydrogen bonds typically form with hydrogen and other small, highly electronegative atoms like fluorine, oxygen and nitrogen. The sulfur atom is too large to induce a hydrogen bond. The principle forces in H2S would be London forces since it is a polar covalent molecule.
Answered by The Old Professor - Wed Feb 10 08:31:34 2010
Q. What are the principle intermolecular forces in H2O and H2S? how do they account for the fact that water is a liquid at room temperature whereas Hydrogen Sulfideis a gas? I know it is hydrogen bonding. But why?
Asked by Charles Barkely - Wed Feb 10 08:23:59 2010 - - 1 Answers - 0 Comments
A. Hydrogen bonding is present in the water, not the H2S. Hydrogen bonds typically form with hydrogen and other small, highly electronegative atoms like fluorine, oxygen and nitrogen. The sulfur atom is too large to induce a hydrogen bond. The principle forces in H2S would be London forces since it is a polar covalent molecule.
Answered by The Old Professor - Wed Feb 10 08:31:34 2010
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
Explain why substances in each of the following would have the greater intermolecular forces?
Q. Explain why substances in each of the following would have the greater intermolecular forces. (a)OCS CO2 OCS (b)SeO2 SeO2 SO2 (c)H2NCH2CH2NH2 CH3CH2CH2NH2 H2NCH2CH2NH2 There is no best answer, you have to explain why the susbtance has a greater intermolecular force than the other.
Asked by Hello - Sun May 10 23:57:07 2009 - - 2 Answers - 0 Comments
A. Hello , 1. CO2 vs. OCS: both molecules have carbon in the middle with a double bond: O=C=O and O=C=S Since the CO2 is balanced, with oxygens on either side of a linear molecule, it has no net dipole moment. Carbonyl sulfide, on the other hand is out of balance by virtue of the different electronegativities of oxygen and sulfur (3.44 vs. 2.58) -- oxygen is more electronegative. That means the OCS will be slightly more positive on the oxygen end, which will set up a dipole. These dipoles will line up like magnets, which means the oxygen on one molecule will be at least somewhat attracted to the sulfur of another molecule. 2. SO2 vs. SeO2: sulfur and selenium have very similar electronegativities (2.58 vs 2.55); their… [cont.]
Answered by Dr. Buzz - Tue May 12 22:40:54 2009
Q. Explain why substances in each of the following would have the greater intermolecular forces. (a)OCS CO2 OCS (b)SeO2 SeO2 SO2 (c)H2NCH2CH2NH2 CH3CH2CH2NH2 H2NCH2CH2NH2 There is no best answer, you have to explain why the susbtance has a greater intermolecular force than the other.
Asked by Hello - Sun May 10 23:57:07 2009 - - 2 Answers - 0 Comments
A. Hello , 1. CO2 vs. OCS: both molecules have carbon in the middle with a double bond: O=C=O and O=C=S Since the CO2 is balanced, with oxygens on either side of a linear molecule, it has no net dipole moment. Carbonyl sulfide, on the other hand is out of balance by virtue of the different electronegativities of oxygen and sulfur (3.44 vs. 2.58) -- oxygen is more electronegative. That means the OCS will be slightly more positive on the oxygen end, which will set up a dipole. These dipoles will line up like magnets, which means the oxygen on one molecule will be at least somewhat attracted to the sulfur of another molecule. 2. SO2 vs. SeO2: sulfur and selenium have very similar electronegativities (2.58 vs 2.55); their… [cont.]
Answered by Dr. Buzz - Tue May 12 22:40:54 2009
What are the intermolecular forces present in ethanol and methanol? Using the structure,why would they have..?
Q. Compare the values of the T s for methanol and ethanol. what is the difference between the T s using the structure of each molecule and what are the intermolecular forces that may be present. Any help is greatly appreciated. I am a beginner at chemistry and I am seeking any help. Thanks.
Asked by Nathan - Tue Aug 4 01:36:24 2009 - - 1 Answers - 0 Comments
A. the first type of IMF is hydrogen-bonding ... between the highly electronegative O in the -OH group and the H elsewhere. same idea as h20 also, van der walls forces ... between the C-H bonding
Answered by Whatever - Fri Aug 7 16:58:15 2009
Q. Compare the values of the T s for methanol and ethanol. what is the difference between the T s using the structure of each molecule and what are the intermolecular forces that may be present. Any help is greatly appreciated. I am a beginner at chemistry and I am seeking any help. Thanks.
Asked by Nathan - Tue Aug 4 01:36:24 2009 - - 1 Answers - 0 Comments
A. the first type of IMF is hydrogen-bonding ... between the highly electronegative O in the -OH group and the H elsewhere. same idea as h20 also, van der walls forces ... between the C-H bonding
Answered by Whatever - Fri Aug 7 16:58:15 2009
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
May someone please share hints finding Intermolecular forces?
Q. May someone share your tips/hints on finding the intermolecular forces, such as dipole-dipole, LD? I also have problem saying which compound is porlar or nonpolar. If I can have your advices, they will really help me. Thank you !
Asked by Unk - Tue Jan 8 22:37:13 2008 - - 3 Answers - 0 Comments
A. London dispersion forces are the weakest of the attractive forces, in general. ALL covalent molecules, both polar and non-polar, have london forces because they are due to the motion of electrons about the nucleus. Dipole-dipole forces are found only between POLAR molecules, because "you gotta have a dipole to have dipole-dipole." There are 3 bond situations where the dipole-dipole forces are exaggerated, because the dipoles are so large; these forces are called hydrogen bonding. Hydrogen bonding occurs between molecules containing an H-F bond, H-O or H-N bond. The first step to determining which intermolecular forces (IMF) are present is to figure out if the molecule is polar or non-polar. This is done by considering the bond polarity… [cont.]
Answered by chem.lady - Tue Jan 8 23:21:25 2008
Q. May someone share your tips/hints on finding the intermolecular forces, such as dipole-dipole, LD? I also have problem saying which compound is porlar or nonpolar. If I can have your advices, they will really help me. Thank you !
Asked by Unk - Tue Jan 8 22:37:13 2008 - - 3 Answers - 0 Comments
A. London dispersion forces are the weakest of the attractive forces, in general. ALL covalent molecules, both polar and non-polar, have london forces because they are due to the motion of electrons about the nucleus. Dipole-dipole forces are found only between POLAR molecules, because "you gotta have a dipole to have dipole-dipole." There are 3 bond situations where the dipole-dipole forces are exaggerated, because the dipoles are so large; these forces are called hydrogen bonding. Hydrogen bonding occurs between molecules containing an H-F bond, H-O or H-N bond. The first step to determining which intermolecular forces (IMF) are present is to figure out if the molecule is polar or non-polar. This is done by considering the bond polarity… [cont.]
Answered by chem.lady - Tue Jan 8 23:21:25 2008
Predicting the types of intermolecular forces?
Q. I need to predict which types of intermolecular forces would be on each of these molecules (dipole-dipole, hydrogen, or dispersion). 1. NH3 I thought it might be dipole-dipole, hydrogen, and dispersion, but I'm not sure if it is a polar molecule. 2. C3H4 I thought it would be all of them once again, but I'm not sure if it is polar or if it's hydrogen since it's bonded to carbon and not a halogen, nitrogen, oxygen, etc. Thanks for your help!
Asked by Steven M - Thu Feb 21 18:31:21 2008 - - 2 Answers - 0 Comments
A. Hydrogen bonding occurs when you have hydrogen bonded to O,N, or F, which are very electronegative. The large difference between the electronegativity of hydrogen and O,N or F produces a highly polar covalent bond where H is partially positve and O, N or F is partially negatve. So now you have an electrostatic attraction between the partially positive hydrogen in one atom and the partially negative of the O,N or F in another molecule which makes a strong dipole dipole attraction called a hydrogen bond. That being said... NH3 has hydrogen bonding. The second one is nonpolar, no hydrogen bonding since H is not bonded to O,N or F. So it is dispersion forces.
Answered by unknown - Thu Feb 21 18:56:03 2008
Q. I need to predict which types of intermolecular forces would be on each of these molecules (dipole-dipole, hydrogen, or dispersion). 1. NH3 I thought it might be dipole-dipole, hydrogen, and dispersion, but I'm not sure if it is a polar molecule. 2. C3H4 I thought it would be all of them once again, but I'm not sure if it is polar or if it's hydrogen since it's bonded to carbon and not a halogen, nitrogen, oxygen, etc. Thanks for your help!
Asked by Steven M - Thu Feb 21 18:31:21 2008 - - 2 Answers - 0 Comments
A. Hydrogen bonding occurs when you have hydrogen bonded to O,N, or F, which are very electronegative. The large difference between the electronegativity of hydrogen and O,N or F produces a highly polar covalent bond where H is partially positve and O, N or F is partially negatve. So now you have an electrostatic attraction between the partially positive hydrogen in one atom and the partially negative of the O,N or F in another molecule which makes a strong dipole dipole attraction called a hydrogen bond. That being said... NH3 has hydrogen bonding. The second one is nonpolar, no hydrogen bonding since H is not bonded to O,N or F. So it is dispersion forces.
Answered by unknown - Thu Feb 21 18:56:03 2008
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
what kind of intermolecular forces are responsible for the aggregation of hemoglobin molecules?
Q. what kind of intermolecular forces are responsible for the aggregation of hemoglobin molecules that leads to sickle cell anemia?
Asked by afif_maxim - Wed Jul 25 05:35:43 2007 - - 1 Answers - 0 Comments
A. Hydrogen bonds.
Answered by Gervald F - Wed Jul 25 07:13:10 2007
Q. what kind of intermolecular forces are responsible for the aggregation of hemoglobin molecules that leads to sickle cell anemia?
Asked by afif_maxim - Wed Jul 25 05:35:43 2007 - - 1 Answers - 0 Comments
A. Hydrogen bonds.
Answered by Gervald F - Wed Jul 25 07:13:10 2007
Can someone please help with intermolecular forces?
Q. > The greater the number of carbon atoms in a higher alcohol, the less easily the alcohol will mix with water.< Now I know its to do with intermolecular forces, but why do lower alcohols mix easily with water whereas higher alcohols do not?
Asked by yellowbird555 - Fri Sep 19 12:41:03 2008 - - 2 Answers - 0 Comments
A. Alcohols are essentially hydrocarbons with an OH group at the end. In general chain hydrocarbons don't mix well with water because water is very polar and hydrocarbons are not. Water can form hydrogen bonds with itself, but not the hydrocarbon, so it bonds with itself preferentially, rejecting the hydorarbon. The -OH group at the end, however is very polar and it by itself mixes very well with water. Water can form hydrogen bonds with it. The variation in miscibility is due to the fact that for small-chain alcohols, the -OH group makes up a significant percentage of the molecule, and dominates the behaviour. For long-chain alcohols, the hydrocarbon chain is "most" of the molecule, so the substance behaves closer to a pure hydrocarbon. [cont.]
Answered by Michael T - Fri Sep 19 12:58:10 2008
Q. > The greater the number of carbon atoms in a higher alcohol, the less easily the alcohol will mix with water.< Now I know its to do with intermolecular forces, but why do lower alcohols mix easily with water whereas higher alcohols do not?
Asked by yellowbird555 - Fri Sep 19 12:41:03 2008 - - 2 Answers - 0 Comments
A. Alcohols are essentially hydrocarbons with an OH group at the end. In general chain hydrocarbons don't mix well with water because water is very polar and hydrocarbons are not. Water can form hydrogen bonds with itself, but not the hydrocarbon, so it bonds with itself preferentially, rejecting the hydorarbon. The -OH group at the end, however is very polar and it by itself mixes very well with water. Water can form hydrogen bonds with it. The variation in miscibility is due to the fact that for small-chain alcohols, the -OH group makes up a significant percentage of the molecule, and dominates the behaviour. For long-chain alcohols, the hydrocarbon chain is "most" of the molecule, so the substance behaves closer to a pure hydrocarbon. [cont.]
Answered by Michael T - Fri Sep 19 12:58:10 2008
Intermolecular forces overcome from a liquid to a gas?
Q. How can you for instance tell what intermolecular force for CO2 would be to go from a liquid to a gas? Like dipole-dipole or hydrogen bond etc?
Asked by Virgo L - Sun Feb 28 11:02:35 2010 - - 1 Answers - 0 Comments
Q. How can you for instance tell what intermolecular force for CO2 would be to go from a liquid to a gas? Like dipole-dipole or hydrogen bond etc?
Asked by Virgo L - Sun Feb 28 11:02:35 2010 - - 1 Answers - 0 Comments
Name the type of intermolecular forces that must be overcome?
Q. The type of intermolecular forces that must be overcome in order to change each of these from the liquid state to the gas state. a. CH3OH b. CS2 c. CCl4 d. COS
Asked by Caleb - Mon May 4 02:51:36 2009 - - 1 Answers - 0 Comments
A. a. Hydrogen bonding. It's got a OH at the end, and O is on of the three elements (N, O, and F) that are really electronegative and keep the electrons from H, creating a dipole. b. Dispersion forces. It's a symmetrical molecule (I imagine it would be S=C=S), so there's no dipole, and only relies of the electron cloud switching sides and making temporary dipoles. c. Dispersion forces. Again, it's symmetrical. d. Dipole-dipole forces. I imagine it looks like S=C=O. O is more electronegative than S, so the O end will be more negative than the S end, creating a dipole.
Answered by D.K.D.P.T. - Mon May 4 04:58:58 2009
Q. The type of intermolecular forces that must be overcome in order to change each of these from the liquid state to the gas state. a. CH3OH b. CS2 c. CCl4 d. COS
Asked by Caleb - Mon May 4 02:51:36 2009 - - 1 Answers - 0 Comments
A. a. Hydrogen bonding. It's got a OH at the end, and O is on of the three elements (N, O, and F) that are really electronegative and keep the electrons from H, creating a dipole. b. Dispersion forces. It's a symmetrical molecule (I imagine it would be S=C=S), so there's no dipole, and only relies of the electron cloud switching sides and making temporary dipoles. c. Dispersion forces. Again, it's symmetrical. d. Dipole-dipole forces. I imagine it looks like S=C=O. O is more electronegative than S, so the O end will be more negative than the S end, creating a dipole.
Answered by D.K.D.P.T. - Mon May 4 04:58:58 2009
From Yahoo Answer Search: 'intermolecular forces'
Tue Mar 9 21:48:47 2010 [ refresh local cache ]
[Hide]▼
news.google.com
Space Ref (press release)
Due to capillarity a substance can draw a liquid into it when the intermolecular forces between the liquid and the substance are stronger than the ...
ragyn.com
RagyN
Mon, 14 Sep 2009 16:20:35 GM
david j. wales, ". intermolecular forces. and clusters i" springer | 2005 | isbn: 3540281940 | 206 pages | pdf | 5,4 mb.
[Hide]▲
