dipole moment explanation?
964289
The reason or this dipole moment is the presence of a lone pair electrons on the sulfur atom.  Sulfur has 6 valence electron.  4 participates in bonding with 4 F atoms and 2 lone pair gives a dipole moment for the molecule.  I am not sure how to calculate the dipole moment but I think you use 4 bonding electrons and 2 non bonding electrns in the formula.\nhope this helps - Stella
969369
The rapid tumbling in solution of molecules modulates the electric quarupole interaction this causes rapid relaxation of the nucleus. Rapid relaxation implies that T2 will be short the FID will be short and so the lines will be broad.\nIn some compounds the quadrupole moment may be so big that molecular motion may not average it to zero also leading to broadening.
224170
please (2 pdf documents)\nhttp://physics.angelo.edu/~dbixler/phys3444lab4new.pdf\nhttp://physics.angelo.edu/~dbixler/phys3444lab8.pdf
837121
Hmmm.. The one affecting the boiling point is the intermolecular force..\nAs you can see, most of the compound here is polar. \n\nTherefore all you have to do is if the compound is consisted only of 2 elements (Group 17), you'll have to calculate the electronegativity difference. The more difference between them, the boiling will increase as well.\n\nIf there is more than 2 atoms in a molecule, you'll have to see the dipole moment magnitude (a.k.a polarity). The higher the magnitude, the higher the boiling point will be.\n\n\npeace\nvixklen
953238
It is true for individual bonds, but not for molecules.\nThe dipole moment of the molecule will depend on the geometry of the polar covalent bonds. E.g. CF4 has 4 polar bonds but they arranged so that the sum of their dipole moments is zero and the molecule has actually no dipole moment.
276224
these guys do it much better than i can:\n\nhttp://hyperphysics.phy-astr.gsu.edu/Hbase/class/phscilab/kundt2.html
30976
to explain how two electrons can be near each other
790902
moment1 (torque) =0.500 x 20.0 = 10.0Nm\nmoment2 = F x (1.60-0.50) = 1.1F\nHere, F means the vertical component of the 35.0N force. [When you draw a rectangle whose diagonally opposite corners touch a line which denotes the force vector, you will see that it has a vertical component (length) and a horizontal component (breadth)] This is because moment is derived from F x d, where F is perpendicular to d.\n\nSO, after drawing a diagram, F = 35cos 30\nWith this, you can find the net torque, depending on which force is producing a torque in which direction (CW or CCW). \n\nHope this helps=)
943195
It has been many years since I even cracked the book on crystal field theory, but I refreshed myself a bit here:\n\nhttp://www.unine.ch/chim/chw/Chapter%204.html\n\nBasically, the difference in splitting (delta value) decreases as you go down a group and increases by about 50% as you add positive charge on a metal cation. Other factors are covered on that page as well. Thanks for the reminder that I took a graduate inorganic chemistry class once back in the early 90's! I assure you that, at one time, I actually understood it, but I haven't used it in so long...well, you get the picture!\n\nP.S. (I had forgotten that it replaced VB theory, which I was supposed to teach my students but ran out of time!)
938015
It's not exactly a binding force like the strong.  I haven't run across any way it affects orbiting electrons.  See the reference for some info.  But it seems to me like a force without an identity.  Its range is extremely short.
975119
Okay now you're getting into physics or something here, so I have absolutely no idea!\n\nBut it might have something to do with.......oh yeah, ions, that's it! Ions......
733675
the oxygen atom is much more electronegative than the hydrogens, meaning that it draws the electrons toward it more than the h's do.  this causes a dipole moment, meaning that the molecule, even though it is neutral overall, has areas where there is a greater electron density than other areas of the molecule.  the shared electrons spend a disproptionaltely high amount of time around the oxygen than they do around the hydrogens, making the oxygen a negatively charged region and the hydrogens a positively charged region
4764
You can't balance it because you don't know what it yields.\n\n\nP.S. This needs to be in the chemistry category. You really must not know much about chemistry and physics.
697038
This is kinda hard to draw on here...\n......_\nK--Br|\n......_\n\nThe lines around Br represent 2 electrons, and the -- represents a bond...ignore the periods
606035
Fluctuating dipole bond: Weak electric dipole bonding can take place among atoms due to an instantaneous asymmetrical distribution of electron densities around their nuclei. This type of bonding is termed fluctuation since the electron\ndensity is continuously changing.\nPermanent dipole bonds: Weak intermolecular bonds are formed between molecules which possess permanent dipoles. A dipole exists in a molecule if there is asymmetry in its electron density distribution.
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.
797314
this guy explains it as easily as can be explained\n\nhttp://www.newton.dep.anl.gov/askasci/chem99/chem99297.htm