select the molecule that will display stronger intermolecular dipole-dipole forces?
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.
956604
Try it out in the lewis-dot diagram\n      ..        ..\nH-O-Ca-O-H\n      ..        ..
950410
Mainly H-bonding (intermolecular forces)
941271
KCl will have higher boiling point because its bond is polar.This can arise the posiibility of dipole-dipole interaction.Main factor which is determines boiling point is intermolecular forces.
223542
thermodynamic factors as well as the orientation and relative energies of the pi molecular orbitals involved.
872523
You need to specify a compound before we can tell you what its molecular geometry is!
639280
Probably because  cohesion forces (forces that bind molecules of the same type together) are stronger then adhesion forces (forces that bind molecules of the different  types together).
848068
ICl2 + should be bent like water since I will have two lone pairs and two Cl's on it.\n\nI3- will be linear\n\nSbCl6- will be octahedral
880416
TCATTG\n\nT molecules connect with A molecules\nC molecules connect with G molecules
130061
Yes, CN- has a triple bond, and N is slightly more EN than C, Remember that electronegativity increases up and to the left in the periodic table!
284075
It's fairly easy don't worry.\n\nNo need for d level splitting diagrams to answer this since we're dealing with N and F:  use the spectrochemical series to make an assumption about the ligand.  The difference in t2g and eg levels (∆o) determines whether a complex is low or high spin.  If both ligands were the same, we would have to look at the oxidation state of the ligand in the complex.\n\nHalides <  Oxygen ligands  <  Nitrogen ligands < CN- ligands\n\n   ALWAYS HIGH SPIN    ---------------            ALWAYS LOW SPIN\n\nIf ∆o > P, then a complex is low spin.  IF ∆o < P the complex is high spin.
963224
The space between the molecules
963196
Many molecules have a lot more than two. You just have to keep counting. Don't forget the green ones.
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
804164
The longer the chain the more London Dispersion forces will come into play.  There will be NO dipole-dipole, or forces based on fixed electronegativity.   There will be no hydrogen bonds.  So the only van der Waal force is the London Dispersion force based on the temporary inequality of electrons.\n\nI should mention that as the chain lengthens there are two other things that will effect the mp and bp of the hydrocarbon.  1. The increase molar mass will raise the mp and bp.  And the entanglement of the molecules as they get long will also raise the  mp and bp.
714401
LOL!\n\nLet's guess which types of molecules your homework listed.\n\nI will guess...  A water molecule.
1107805
study on intermolecular particals and there behavior