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Why do some ionic compounds have some solubility in water . . . - Socratic For sodium chloride, these intramolecular or interparticle interactons, are compensated for by the making of ion-dipole bonds when sodium chloride dissolves in water, and the water dipoles solvate the individual ions; we write N a+(aq) to represent this, a shorthand for [N a(OH 2)6]+
Question #8cf1f + Example - Socratic You should probably go through each type of intermolecular force, and see if it is there The order of precedence for each type of intermolecular force is: hydrogen bond permanent dipole-dipole interactions London forces The most powerful types of intermolecular force are the ones with the greatest ionic character These will occur between atoms with the greatest difference in
Question #0df6a - Socratic Polar molecules interact with each other by strong attractive dipole-dipole interactions whether polar molecules interact with non-polar molecules through dipole- induced dipole interactions ( a weak dipole induced subject to charge of a dipole similar to the way a permanent magnet induces a temporary magnetism on a metal )
Why is #n-C_10 H_22# boiling point higher than #Br_2 . . . - Socratic Decane has a very slight dipole, whereas bromine has no dipole Carbon and hydrogen have approximately a 0 35 difference in electronegativity This is a demonstration of how negligible dispersion forces are when there are also dipole-dipole interactions There may be other reasons, which I'm open to hearing!
Site Map - Dipoles Questions and Videos | Socratic Does H20 have permanent dipole dipole forces as well as hydrogen bonding? How would you determine if polar bond is ion-ion, dipole-dipole, dispersion forces or hydrogen bonds? What are the intermolecular forces of CHF3, OF2, HF, and CF4? What is the difference between hydrogen bonds and dipole dipole interaction?
How can a dipole exist? How can the two charges stay stable . . . - Socratic For an electric dipole to exist an external electric field is required Two charges alone (one positive and one negative) will not be stable This is because the charges will attract one another, so the distance between them will decrease over time If the charges are in an external electric field, then the dipole may be stable as there is the possibility of zero net force acting on each
Question #d4d89 - Socratic Ideality assumes minimal interaction between the gaseous particles For hydrogen chloride, a potent intermolecular force can operates: hydrogen bonding, in that the hydrogen is bound to a strongly electronegative chlorine to give the −δCl − H δ+ dipole, which can act intermolecularly Possibly the best metric with which to compare this is the boiling point of the gases: helium has a
Question #8e98a - Socratic This gives an individual CH_3Cl molecule a side that is more negative than the other, otherwise known as a dipole moment Since every CH_3Cl molecule is like this, the CH_3Cl molecules can form stronger bonds with each other, having the partially negative end of one molecule form bonds with the partially positive end of another molecule
Which is strongest lewis acid and why bf3 or bh2? - Socratic BH_2 is unknown If you mean BBr_3, this is the strongest Lewis acid known , For BF_3, while the stackrel(+delta)B-stackrel(delta-)F dipole is certainly polar, the electrons in the lone pair orbitals on fluorine, are the right shape and the right symmetry to donate to an empty "p-orbital" on boron On the other hand, the lone pair electrons on bromine in BBr_3 are larger and more diffuse
Questions asked by Pankaj Solanki - Socratic What is the magnitude of the electric dipole moment of this system? Three point charges of +2q, -q and -q are placed at the corners A, B and C of an equilateral triangle ABC of side ‘x’ What is the magnitude of the electric dipole moment of this system?