Which molecule in each pair(See the whole question) has the greater dipole moment?
956449
1.) ClO2, because the O=Cl=O angle is 90deg whereas O=S=O is linear, 180deg\n2.) HCl, because Cl is more electronegative than Br\n3.) SCl2, because the Cl-S-Cl angle is 90deg, whereas Cl-Be-Cl is linear, 180deg\n4.) AsF3, because As sits at the top of a tripod of F atoms, whereas AsF5 is symmetrical.
273309
wat r u ppl talking about....u ppl r absolutely wrong.....its alkynes n i am 100% sure about\n\nthey r more reactive becoz of there triple bonds...\n\n\n2 ppl in a row a row giving a wrong answer can confuse a person completely
965017
You need to know the number of valence electrons.  Carbon, for example, would want to pair with 4 other atoms.  If there were fewer atoms attached as in CH2O (only 3 attached to the carbon) then one of the atoms must be double bonded.  In this case it is the oxygen that would have the double bond.  You could deduce the approximate shape from the number of bonds.  It would be slightly distorted by the slight negative polarity of the oxygen atom.  Shape of a molecule is a complicated issue that I glossed over.
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.
950410
Mainly H-bonding (intermolecular forces)
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
762737
the C has four bonded pairs, leaving 3 lone pairs on each F\n\n4 bonded pairs\n6 lone pairs
809957
The most polar bond will be between the atoms with the greatest difference in electronegativity.\n\nF2 has bond that is not polar since the electrons are equally shared between the two identical atoms. The electronegativity series is As<S<Br<F so the biggest difference is between As and F and the most polar bond is in AsF3.\n\nAs belongs to the same family as N. Thus in AsF3 it forms 3 single bonds and also has 1 lone pair. So the electron-group arrangement is tetrahedral but since there are only 3 identical bonds there will be a net dipole moment.\n\nI already explained why F2 has no dipole moment\n\nBrF3 has trigonal bipyramid electron group arrangment (3 bonds+2 lone pairs) but not corners are occupied by identical atoms (2 have lone pairs of Br) so the dipole moments do not cancel out and the molecule has a net dipole moment\n\nSF4 has again trigonal bipyramid electron group arrangement(4 bonds + 1 lone pair) with one lone pair at one of the corners so it has a net dipole moment\n\nSF6 has octahedral electron group arrangement (6 single bonds)\nand since all corners have F atoms the dipole moments of the bonds cancel each other and the molecule has no net dipole moment.
963196
Many molecules have a lot more than two. You just have to keep counting. Don't forget the green ones.
878681
Molecules exist in different shapes. Many of the physical & chemical prpoerties of molecules arise due to the different shapes.\n\nSome of the common geometrical shapes are trigonal, planar, tetra hedral etc.The VSEPR theory provides a simple treatment for predicting the shapes of polyatomic molecules. The theory was originally proposed by Sigdwick and Powell in 1940. \n\nIn case of molecules with central atom having one or more lone pairs VSEPR treatment is as follows: In these type of molecules, both lone and bonded pairs of electrons are present. The lone pairs are localised on the central atom, & bonded pairs are shared between the two atoms. Consequently, the lone pair of electrons occupy more space as compared to the bonding pair. This causes great repulsion between lone pair of electrons.\n\nThese repulsion effectscause deviations in the predicted bond angles in molecules. \n\nThe descending order of repulsion interaction is lp - lp > lp - bp > bp - bp\n\nlp - lone pair\nbp - bonded pair
786962
If the molecule has O,N,F,or Cl then most likely it is polar.  Look at the periodic chart and remember that the elements in the upper right are the most electronegative, so they want electrons.  When these elements are in a compound with other atoms such as C and H they will pull electrons closer making a dipole moment.  \n\nThe only real trick is looking at the geometry of the molecule, if there is more than one electronegative atom pulling in opposite directions then the dipole is canceld.  Such as O=C=O which is liniar.\n\nLook at an electronegativity chart you will see what I mean
627227
The carbonyl double bond is between atoms of different electronegativity, resulting in an electron deficite at the weaker atom (C) and a surplus at the stronger atom (O) along the bond.\n\nStill, the carbon-carbon double bond also does create a dipol (or rather quadrupol) moment:\n\nThe carbon and all other bonded atoms lie in a plane. The double bond electrons are distributed: 2 to the direct bond between the atoms, 2 to the overlapping P-orbitals. This creates a slight electron deficite in the plane of the bond and a slight electron surplus above and below, which is what makes double bonds more reactive than single bonds.
158656
Unable to guesstimate.  You're talking biological macromolecules, most likely.  They would probably have carbon, hydrogen, nitrogen, oxygen, sulfur, phosphorus, and perhals a halogen or two.  And maybe even a metal ion or two thrown in for good measure.
826844
H\n |    \nC=O:  (You need 2 lone pairs on Oxygen)\n |   \nH\n\nIt doesnt get much better than that :)
223542
thermodynamic factors as well as the orientation and relative energies of the pi molecular orbitals involved.
503103
No - methanol, ammonium\nYes - formic acid, sulfur troxide\nKinda - carbonate, nitrate, chlorate (all can be drawn as resonance structures, so the bonds aren't quite single and aren't quite double)
867785
Dipole moment is a vector quantity. It is the vectorial sum of all the bond moments in the molecule. \n\nIf the molecule is symmetrical and the bond moments are cancelled by each other then the dipole moment is zero.\n\nIn case of SO3, the dipole moment is zero because the molecule is trigonal planar.\n\nWhereas the BrF5 is square pyramidal and hence has some dipole moment. The Flourine present above the square plane causes this dipole moment.