what is the differ enc between intermolecular forces and intramolecular forces?
478436
Intra>>>>>>Forces among atoms of the molecule.\nInter>>>>>>Forces between a molecule and its surrounding molecules.
311625
Well, all molecules are constantly vibrating ie changing positions all the time. And yes, intermoleculer forces exsist between. Think about this: do these intermolecular forces require a meduim? This question kinda indirectly relates to the Theory of Nothingless but have a look at the nothinglesstheory website. It's quite interesting. You can find it by googling or from my source list or other resources you may come across. It kinda relates to physics more than chemistry, in  my opinion. In the universe, it began a state of nothing and now after the "Big Bang" there's "everything"... the universe is mostly made up of empty space, just like at atom being made of mostly empty space~\n\nGood question. I hope I've answered your question.
731172
ya because the intramolecular force of attraction is not compatible. Hence hydrogen bonds are not able to be form.\n\nspecial case where force of attraction are not compatibl but compound can combine with H2O: ionic compound and H2O (ion dipole interaction)
225634
None. They are two different compounds.\n\nIt looks like you want to compare a specific property of the alcohols. Please specify!
880133
There isn't a definite boundary line.  A molecule of several atoms can exhibit quantum-mechanical behavior under appropriate experimental conditions.  Of course, the heavier the molecule, the more it obeys classical mechanics as opposed to quantum mechanics.  The "correspondence principle" tells us that at a large enough scale, all processes show classical behavior.
445989
The chemical potential (or greek letter mju) of a compound is the measure of the free energy of one mole of the compound in a particular system. It is independent of the size of the system. \nit varies with concentration: mju=mju( under standard conditions) +RTln[x]\nor it is the partial Gibbs free energy: mju=G/n\nwhere G=gibbs, n= number of molecules in system. or finally \nmju of x is rate of change of free energy as the amount of x changes, at constant temperature, pressure and concentration of all other species:\nmju= (small deltaG/small delta n of x) where small delta n of x is change in x measured in moles.\n\n\nhope this helps
59242
E=MC squared. \nE is energy.\nM is mass(weight).\nC is the speed of light.\n\nForce, on the other hand, is mass times speed.
879801
Pentane\n\nIt depends on which compound has the strongest intermolecular forces. In the case of hydrocarbons the intermolecular forces that are present are dispersion forces.\nIn such cases:\n"The more branched a molecule is, the more "spherical" it is, and the smaller surface area it will have - since dispersion forces increase with surface area, the more branched molecules will have a lower boiling point. You may notice that the trend in the melting points is rather different - this is because the longer a branch is, the more potential it has to flop around and disrupt the regular crystalline lattice of frozen pentane, giving a liquid state."
255271
Yes you are correct.Different substances are different because of  their molecular structure and the constituents of each molecule. Molecules are well bound together in solids than in fluids (gases and liquids). The molecules are free in gases.\n Further the molecules are not at rest and are in vibrations.When the substance is heated  the average energy of a molecule  increases which tend to decrease the bindings of the molecules.\nGenerally by heating , a substance  chnges from solid to liquid and then to gaseous state.We call this as physical change.\nWhen the energy is  strong enough to break the  molecules into its constituent elements new compounds are produced we call it as chemical change.\nIn effect heat  has many things to do with their bondings
1021437
a) \n\nThe molecules in a substance are in constant motion. Now there are two oppposing forces on a substance. One is the intermolecular bond energy that tries to keep the molecules together. The other is the kinetic energy of the molecules that tries to push the molecules apart (these two forces work together to keep substances in equilibrium - basically keeps it from exploding or imploding in simple terms).\n\nNow, in solids, the molecules have low kinetic energy but high intermolecular bond energy(IBE). Liquids, the kinetic energy is higher and conversely the IBE is lower. Gases, the kinetic energy is high and the IBE is low (makes sense - the "bond" is weak)\n\nSo now, the kinetic energy or molecules is directly proportional to the heat applied - the hotter it is, the more kinetic energy the molecules have. Therefore when you heat it ... the kintic energy gets stronger and stronger and the IBE gets weaker and weaker until it breaks and the substance undergoes its change of state.\n\nHope this explained it well!
327488
hi,\n\nas i remember:\n\n - molecules behave as rigid objects (spheres, if you like)that move according to newtonian physics\n\n -  collisions between molecule/molecule and molecule/container are perfectly elastic (i.e. energy is conserved in all collisions)\n\n  - the size of the particle is much less than their typical separation (i.e. collisions are infrequent).  this leads to the related feature that there are no long-range interactions betweeen molecules.\n\n - the average kinetic energy of a collection of molecules is a function of only the temperature.
879729
Please see my answer to your previous question for more details.\n\nThe more unshared pairs of e-, the more distortion in the geometry of the molecule.
862864
H3C-CH2-CH2-CH3\nion-ion bonds: not an ion\nion-dipole bonds: not an ion and no dipole\ndipole-dipole bonds: butane is nonpolar, so no dipole\nHydrogen bonds: does not contain H bonded to F,O, or N\n\ntherefore the only intramolecular bonds remaining are the weakest of the weak - london dispersion forces (aka Van Der Waals). These are randomly induced dipole attractions that happen when the electrons that move around randomly just happen to have a higher concentration at one end of the molecule. This causes dipoles to form in adjacent molecules, which induce dipoles in molecules next to them. these forces are very weak, but still play a part in raising the boiling point of butane.
314032
Well, that's a very general question, and it's open for textbooks worth of information.\n\nMolecules are made of atoms, which all have different properties depending on the electrons present in their valence shells.  Interactions of molecules can be very simple or extremely complex.  Currently I have an organic chemistry textbook which is about 5 lbs in weight and is 1500 pages long, and all that it contains are rules for reactions between different functional groups of molecules.  \nScientists have discovered a lot about molecules--and this is why we have such advanced medicinal technologies that we have developed.  Any pill you take was formed because scientists and pharmaceutical companies learned about reactions between specific molecules.  \nThere is really a lot more to tell, but I'll stop here in order to keep it brief.
1187079
Boiling point depends on the strength of the intermolecular forces. Following is the list of them all with their strength and when they occur. \nnetwork covalent (strongest) with only diamond or SiO2\nIonic (ionic compound, 2nd strongest) like Na-Cl etc. Gets stronger with smaller sizes. \nHydrogen bonding (N, O, F with H) 3 rd strongest. \nDipole dipole (when there is a polar molecule) 4 th strongest, gets stronger with more polarity. \nLondon dispersion weakest. Stronger with more mass. \n\na NH3of the first two. Because NH3 has hydrogen bonding (only if you have N, O, or F with hydrogen) while PH3 has regular dipole dipole (based on polarity), which is weaker than NH3. \nNow in this one its c because if you draw their Lewis diagrams out c molecule has on O----H bond while d doesn't. That hydrogen bond is strong enough to make c stronger. As other than that they only have London dispersion force, (which are found in non polar molecules, and they get stronger as atomic mass gets higher). \ne and f both have the London dispersion force that I talked about earlier cause they both are non polar. So f has greater mass so f has higher boiling point. \ng because HCl has polarity (dipole dipole forces) which are stronger than F2 which is non polar and has London dispersion forces (they are the weakest).
194193
van der Waals forces are weak intermolecular forces between molecules that don't have a permanent charge or dipole moment.  They are electromagetic in nature.\n\nThe way they work, simplified, is like this. There are several ways atoms and molecules of a substance can be bonded to each other. Some atoms and molecules have an electric charge.  They are called ions.  Opposite charges attract, so oppositely charged ions are attracted to each other, and thus the ions become linked together. \n\nOther molecules are formed when atoms share electrons.  These are called covalent bonds.\n\nStill other molecules have no overall net charge, but are formed in such a way that they are polarized, i.e. they have a part that is more positive, and a part that is more negative.  The positive part of one molecule is attracted to the negative parts of other molecules.\n\nAnd still other atoms and molecules have no overall charge, and are not permanently polarized, but because of the way their electron "clouds" interact with the electron clouds of other molecules, they can become temporarily polarized.  When that happens, just as in polar molecules the unlike parts of the molecules or atoms are attracted to each other.  This weak attractions are referred to as van der Waals forces.
986647
ionic = ionic crystal\npolar-covalent = molecule with dipole bond\nnonpolar-covalent = molecule w/ no dipole bond