is GaI3 polar or non polar ......is AsF5 polar or nonpolar...?
352077
Thanks NeuroProf.\n\nThe molecule AsF5 is trigonal bipyramidal in shape. First lay out all the bond pairs in that shape and then see if the 'pulling effect' of all the bonds cancel each other. Here, there are 3 bond pairs (of Cl) at the corners of the triangle, 1 bond pair at the bottom and 1 at the top. The Cl at the top pulls electrons and the pulling effect is cancelled by the one at the bottom. Considering the 3 bond pairs left in the middle, 2 are angled at 120 degress and one is at 90 degrees to the top and bottom bond pair. So the pulling effect of the 2 pairs is cancelled by the one at 90 degrees. Overall dipole cancels out and there is no charge distribution, so the molecule is non-polar.\n\nIn BrF4- (with square planar shape), the pulling effect of the lone pair at the top is cancelled by that of the lone pair at the bottom. This leaves 4 F atoms arranged at the corners of the square in the middle. The pulling effect(dipole) of 2 diagonal F atoms will cancel because they are in the same plane and are the same atoms. Hence all the 4 dipoles cancel out and that of the lone pairs too, so the molecule is non-polar.\n\nIn GaI3, the 3 I atoms are arranged in a trigonal planar manner. The dipole of the 2 I atoms at the sides will cancel, but the I atom at the top is not paired with any other atom at the bottom, so the dipole cannot cancel out. Since overall dipole moment is not equal to zero, the molecule is polar.\n\nAre you sure the molecule is SbF6- and not SeF6? If it's SbF6 then the shape will be square bipyramidal or octahedral (similar to BrF4-). The dipole of the 2 F atoms at the top and bottom will cancel and that of 2 diagonal F atoms will cancel and overall dipole will be zero, so the molecule will be non-polar.
822762
Both CH3F and CF4 are tetrahedrons, but due to the substitution each has a different symmetry (C4v and Td respectively), as a rule the lower the symmetry the higher the polarity of the molecule. Actually, any Td (fully substituted tetrahedron), Oh (fully substituted octahedron), D4h (fully substituted square planar), D3h (fully substituted trigonal bi-pyramidal) will be non-polar molecules. This is due to the cancellation of the dipole moments.\n\nThus in order of the strongest dipole moment the answer is\n\nCH3F > CF4 (C3v < Td)\nXeO3 > XeO4 (C2v < D4h)\nSO2 > CO2 (C2v < D(inf)H)\nCOCl2 > BF3 (C2v < D3h)\n\nIf you are having a hard time understanding the Schoedinger group types, try a 3D modeling program (eg Spartan Build or ChemDraw 3D) to see the differences in the symmetry of the molecules.\n\nI hope that this helps. Please feel free to contact me if you have any further questions.\n\nKen
486231
NaOH is ionic.\n\nAll has to do with electronegativity and the difference between the two species bonded to each other.  If the electronegativity difference is less than 0.5, the bond is considered to be fairly non-polar.  Between 0.5 and 1.5 is usually a polar bond, greater than 1.5 usually means that there will be charge separation and the bond will be ionic.\n\nFor either polar or non-polar bonds, you need to know the geometry of the molecule and determine whether the sum of the individual dipoles in the molecule will cancel (vector sum).  If they do, the molecule is non-polar.  If they don't, it is.  For instance, water is polar as its polar bonds do not cancel geometrically, but CH4 is non-polar, even though each of its bonds is polar.
957540
You have three types of bonds (essentially)\n\nYou have ionic, non polar covalent, and polar covalent.  Each has a strength in bonding.\n\nIonic is the strongest.  These will have the highest melting points (just try to melt salt for instance).  The non polar covalent bonds tend to be liquids or gases at room temperature (very low melting points).  Examples of these would be Methane , Benzene, ethane etc.\n\nPolar covalent bonds have a stronger pull on the electrons and therefore tend to be higher in melting point than non polar and lower than ionic.
912679
PCl3 has the same shape as NH3 (tetrahedral with P in the center, the 3 Cl at the 3 corners and a lone pair at the fourth corner) So the polar covalent bonds don't cancel out each other\n\nSO3 is planar trigonal and thus the dipole moments cancel out each other and it is non-polar\n\nCF4 has a tetrahedral shape and since all bonds are the same they cancel each others dipole moment;the molecule is nonpolar\n\nCH2F2 has the approximately the same shape as CF4, but since not all bonds are the same their angle is a bit different and the sum of the dipole moments is not zero; thus the molecule is polar\n\nSO2 is a bent molecule (because of the sulphur's lone pair), think of it in a way as water with S in the place of O and O in the place of H so it is polar.\n\nCO2 is a linear molecule (O=C=O) so the dipole moments of the two identical polar bonds cancel out each other; the molecule is nonpolar\n\nO=C=S has different polar bonds, so although they have opposite directions the result will be a slight dipole moment, so the molecule is polar.\n\nIn all your questions you have to compare a polar and a nonpolar molecule. Of course the one with the strongest dipole-dipole interactions in each case is the polar molecule.
852794
dobereiner's like that mendeleev guy right? if my memory is right, all  of the elements above have similar chemical properties, that's why he placed them in his "triads". This means that all of them act similarly. Remember that it is the VALENCE electrons that causes the specific reaction of an element. So, as all three elemnts have the same number of valence electrons, they act similarly.
883229
PCl5, or phosphorus pentachloride, has a trigonal bipyramidal structure. A photo of the structure of this molecule is shown below:\n\nhttp://en.wikipedia.org/wiki/Phosphorus_pentachloride\n\nBrF5, or bromine pentafluoride, has a square pyramidal structure: a link to this molecule is shown below as well:\n\nhttp://www.chemistry.ccsu.edu/crundwell/Galleries/VSEPR/brf5.html\n\nBecause PCl5 has a trigonal bipyramidal structure, there is no net dipole moment since the molecule is symmetric around the central phosphorus atom.\n\nBrF5, on the other hand, does have a dipole moment due to the asymmetric structure. The absence of a sixth fluorine atom prevents the structure from becoming octahedral, which would be symmetrical in the structure of BrF6.\n\nSo in short, the differences between the two are as follows:\n\nPCl5=no dipole moment\nBrF5=dipole moment\n\nHope this helps!
833912
hmm...do i detect a slight hint of webassign?\n\nammonium chloride(NH1+ and Cl1-) that should tell you enough.\n\nAnd for polyethylene, let's just say it's non-polar...how much does that help? (provided that hydrogen bonding is a special form of dipole-dipole, and dipole moments only happen in polar molecule)
441135
polar means that the electron cloud is not even, and yields a slight negative charge to one side, and postive charge to the other side, it is call a dipo moment.\n\nNon polar means that the electron cloud is evenly balanced and no dipo moment is formed.\n\nNaCl, table salt is polar, and will go into solution with a polar solvent such as water.\n\nMethane, CH4 is non polar and will not go into solution with a polar solvent, but will with a non-polar solvent.\n\nThis is matters alot in chemistry, since electron reactions are the bases for all chemical bonds and reactions.\n\nRead more , and you will understand better, good luck
686965
migs is correct.\n\nFor just a qualitative identification of functional groups, IR is the best for organic (and some inorganic) compounds. You load it in and, a few minutes later, you have a spectrum that tells you what groups you have. (assuming your compound is reasonably pure)
308551
Xavier is dead wrong. NH4+ is tetrahedral. Most of his answer applies to NH3, which is trigonal pyramidal, and not the same thing as NH4+.\n\nPolar molecules have a large net electrical dipole moment. In a sense, the dipole moment tells you how close you are to becoming an ionic compound. If there is no net dipole moment, the compound is completely non-polar. On the other extreme, if it's an ionic compound, it's completely polar.\n\nLook carefully at your question. NH4+ is an ion, not a molecule, and the terms "polar" and "non-polar" don't really apply to ions. The reason is that ions must be part of an ionic compound, and the ionic compound would be considered polar by definition. For example, (NH4)Cl is an ionic compound and therefore very polar, but asking whether NH4+ is polar is no different than asking whether Cl- is polar.\n\nA couple of good textbooks for further information and examples would be "Organic Chemistry" by Solomons and "Organic Chemistry" by Peter Vollhardt.
664759
It's Ionic if thats what you were looking for because sodium is an alkali metal (group 1) and Iodine is a halogen (group 17). Iodine forms an I- ion (this is an anion) and Na forms an Na+ ion (a cation) so they combine on a 1:1 ratio and the formula is NaI
844446
AsF3=Arsenic tri fluoride\nAg2CO3=silver carbonate\nFeSO4=Iron[II] Sulfate\nP5O10=Phosphorus Di oxide or penta phosphorus deca oxide\nPb(OH)4=Lead Hydroxide
363162
When you ask about the formula that is a pretty broad question.  The only formula I know is the balanced compound formula which is Ga2(SO4)3, direct combination formula which is 2Ga + 3S04 --> Ga2(SO4)3, or the decomposition formula which is, Ga2(SO4)3 --> 2Ga + 3S04.  If this isn't what you wanted I'm sorry, if you want you can email me and be more specific.
451415
i think it is a polar covalent bond\nI used to remember why but I'm not in Chemistry anymore...\nHeres a website.. Look at Example #3\nhttp://users.rcn.com/jkimball.ma.ultranet/BiologyPages/E/Electronegativity.html#covalent_bond\nAnd another http://academic.brooklyn.cuny.edu/biology/bio4fv/page/polar_c.htm\nhope its not too late
1099257
There are different grades of polarity.  Polarity is hard to tell by simply looking at a molecule, since there is a lot of spooky stuff happening at the quantum level.  Some polar molecules are more polar than others.  If you have an -OH group in an organic molecule (polar) then you have a somewhat polar molecule.  Not as polar as say, water.  Water is extremely polar.  Polar molecules include\n\nNaCl (salt), H2O (water)\n\nNon-polar molecules include\n\nCl2 (chlorine gas), H2 (natural hydrogen), O2 (atmospheric oxygen)\n\nHowever some molecules you would expect to be extremely polar based on oxidation states are NOT, like HCl (hydrochloric acid)  where the Cl shares electrons with its hydrogen neighbor.  So generally by looking at a molecule you can't really tell.  But there are some guidelines.\n\n1.  Diatomic bonds (as found in naturally occuring oxygen, nitrogren, etc, i.e. O2, N2) are non-polar.\n2.  Organic molecules are generally non-polar (there are exceptions:  some soaps, ketones, alcohols, organic salts)\n3.  Non-organic salts are polar\n4.  An alcohols polarity DECREASES when you add more chains.  I.E.  methyl alcohol is MORE polar than ethyl alcohol, which is more polar than isopropyl alcohol.  Extremely long chain alcohols even with an -OH group are essentially non-polar.
855087
Ca2+=[Ar]\nMg2+=[Ne]\nI-=[Xe]\nF-=[Ne]