which of the following compounds has the smallest dipole moment? CH2Cl2, CH3Cl, CCl4, or CHCl3?
550748
CCl4...the Cl cancel each other out in the chemical arrangement.
361732
Lewis structure of CH2Br2\n\nIts identical to the lewis structure of methane but just replace two hydrogen atoms with bromine atoms (remember to add the three lone pairs around both bromine atoms).\n\nNow about polarity:\n\nThe C-Br bond is then considered to be polar. Having bromine slightly negative and carbon slightly positive. Over all the molecule is polar.\n\nSymmetry:\n\nAnd yes dibromomethane (CH2Br2) has two planes of symmetry, one horizontal and one vertical. In order to verify this, you have to look at the molecule in three dimension and not two dimentional (as drawn on a paper)
984099
I'm very surprised your book doesn't have information on VSEPR.  The acronym "VSEPR" stands for "valence shell electron pair repulsion".  Please double-check the list of topics in the back of your text.  \n\nA dipole moment in the context that you're considering is an incomplete sharing of electrons. In a covalent bond, one of the atoms involved is better at attracting & holding electrons than the other (more electronegative), so that instead of the covalent bond being perfectly shared it gets distorted to one side.  If a molecule has a dipole moment, it has more electrons (higher electron density) in one direction than in others.  One example of this is the covalently bonded acid, H-Cl.  Hydrogen is not very electronegative, but chlorine is very electronegative, so the chlorine atom does a better job holding onto the two shared electrons in the H-Cl bond.  \n\nI hope this gets you started in the right direction.  If you really can't find the info in your text, please go to a library and look at another chemistry book.
635418
CH3CH2CH2CH3 + CL2 -hV--> \nCH3CH2(CL)CHCH3 + HCL ..\n\nwhat are the ways to get the CL at the end of the chain..so that\n\nCH3CH2CH2CH2CL + 2NA + CLCH2CH2CH2CH3\n--->CH3--------CH3\n\nThat's a radical reaction, the chlorination of an alkane with chlorine in UV light. The intermediate is a carbon radical and secondary radicals are more stable than primary. There are also more secondary carbons on this molecule. So probability and reaction kinetics dictates that the primary alkyl halide will be a minor product.\n\nI guess, if this were my synthesis, I'd:\n\n1. Put the glucose in HCl to cleave the anomers it likes to make.\n\n2. Esterify the carboxlic acid with whatever's available (Fisher esterification with MeOH, for example)\n\n3. Reduce the ester with Diisobutyl aluminium hydride (DIBALH)\n\n4. React the aldehyde with 1 equivalent of Ethyl Magnesium Bromide (Grignard)\n\n5. Reduce the hydroxy groups with a Barton-McCombie deoxygenation, although I've never seen it done in a case like this.\n\nThen again:\n\nI'd go to the stockroom and save my research advisor a lot of money. :)
445447
1-chloropropane, because chlorine has a higher value of electronegativity.
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.
284634
3K4Fe(CN)6 + 4FeCl3 -> 12KCl + Fe4[Fe(CN)6]3
916374
The trichloride is a little more complicated than borane (BH3).\n\nCheck out the following:
401509
I don't know that question.\n\nI can tell you that it's an octahedral complex. The two isomers would be CIS (Both chlorides adjacent to each other) and TRANS (both chlorines opposite each other)
1135127
Since SO2 is symmetrical with the outer oxygen atoms bound at 180 degrees, I don't believe it has a dipole moment.  O3 is the same, having the oxygens on the outside, so there is no "pole," and although there is a slight 30-degree "kink" to CS2, I don't believe it has a dipole either.  I believe you need to actually have hydrogen present for a hydrogen bond to occur... these are all gases, and are therefore not bound to anything in this gaseous form.
985077
chlorine, Cl2, bromine, Br2, or iodine, I2 or fluorine
2963
Carbon tetrachloride.  You could also call it tetrachloromethane.
961365
ch3cooh is Ethel alcohol.\n\nNa cl is salt.\n\nSalt is the better conductor, and the higher concentration of .2 moles is the better conductor.\n\nWilliam
737669
Bond energy (in kJ/mol)\n\nF-F:158\nCl-Cl: 244\nBr-Br-:193\nI-I: 151\n\nHence, in order of decreasing bond strength:\nCl-Cl => Br-Br => (F-F) =>  I-I\nFluorine is an anomaly.\n\nBond strength decreases from chlorine to iodine as down the group, the atomic size becomes larger and thus the valence electron orbitals become more diffused, causing the overlap of orbitals to become less effective. Therefore the halogen-halogen bond becomes weaker from chlorine to iodine.\n\nFluorine is an exception due to its extremely small size. The F-F bond length is so short that the lone pairs of electrons on the fluorine atoms repel each other and weakens the F-F bond.\n\nI hope that answers your question.
264077
Right off the bat without looking up anything, I would say CH4 has the lowest boiling point.  Why?  Well, it is the least complex molecule of them all.  Additionally, it is symmetric, therefore non polar.  Since it is the smallest and least complex, it really doesn't have a dipole-dipole interaction such as the other larger molecules, requiring either a lot more pressure to cause condensation or a removal of a lot of heat to really bring it to a low temperature.  Furthermore, there isn't any entanglements when two or more molecules collide, which the larger hydrocarbons are prone to because they have comparatively longer chains.
452453
No, we don't use the electronegativity chart; instead we draw the full structure of the molecule and then see which 'pulling of bonds' cancel each other. \nIn the molecule AsF3, since As has 5 outer most electrons(in group 5), each F is bonded to As with a single covalent bond. Hence, the shape of the molecule becomes trigonal pyramidal, with 3 bond pairs (with 3 F atoms) and 1 lone pair. The 3 bond pairs pull the electrons towards themselves in the lower plane, while the 1 lone pair pulls at the top. The pulling effect of the 2 F atoms at the 2 sides cancel out  because the pulling effect is the same for both F atoms; however, the pulling effect of the lone pair at the top and the 1 F bond pair at the bottom will not cancel, because it is not from the same atom/species. Hence the overall dipole moment( dipole moment = charge x distance) does not cancel out, so the molecule is polar, with some charge distribution remaining due to the unequal pulling effect.\n\nIn CF3Cl, the shape is tetrahedral, with the 3 Cl atoms and 1 F atom bonded by single covalent bonds to the central C atom. The bond pairs spread out with the 3 Cl atoms pulling at the bottom and the 1 F atom pulling at the top. The pulling effect of the 2 Cl atoms at the sides cancels out, but that of the F atom at the top and the Cl atom at the bottom does not, as the pullin effect of 2 different atoms is different. Hence, as before, overall dipole does not cancel and the molecule is hence polar.
596849
2 - Potassium Chloride\n\nIt has, by far, the weakest covalency of all those listed, and therefore breaks apart most readily.