ICl a based on ionic radii and charges, which of the following solids would have the greatest lattice energy?ĭ. decreasing repulsion between hydrogen atoms d which one of the following compounds is most likely to be ionic?Į. increasing number of unshared pairs of electronsĮ. increasing electronegativity of the central atomĭ. PH3 d according to the VSEPR model, the progressive decrease in the bond angles in the series of molecules CH4, NH3, + H2O is best accounted for by theĬ. PH3 e which of the following molecules has trigonal pyramidal geometry?Į. PH3 b which of the following molecules has the largest dipole moment?Į. tetrahedral d which of the following molecules has only one double bond?Į. F2 a the geometry of the SO3 molecule is best described asĮ. I, II, + III d of the following molecules, which has the largest dipole moment?Į. +1,260 kJ d types of hybridization exhibited by the C atoms in propene, CH3CHCH2, includes which of the following?Į. F2 c which of the following contains 1 sigma and 2 pi bonds?Īccording to the data in the table above, what is the value of deltaH for the reaction represented above?Į. F2 d which of the following has a bond order of 2?Į. H2S c which of the following has the largest bond-dissociation energy?Į. CO2 a which of the following molecules has a dipole moment of zero?Į. Things get to each other.A the electron-dot structure (Lewis structure) for which of the following molecules would have tow unshared pairs of electrons on the central atom?Į. Stronger ion-dipole forces the closer that these Coulomb forces are inversely proportional to the distance between the charges. Had a weaker dipole moment, you're not going to have as Ion-dipole forces stronger, or vice versa. Stronger dipole moments, that will also make the You would have stronger ion-dipole forces. Had a positive two charge, then the partially negativeĮnds of the water molecules would be even more strongly attracted. With a positive one charge, if you had a calcium ion that Stronger ion-dipole force if you have stronger charges on the ions. You think is going to matter? Well, as you can imagine, Gonna dictate the strength of the ion-dipoleįorces, think about that. Molecules which are polar, which have molecular dipoles. Those ions are able to separate and be attracted to the water And this is one of the reasons why it's so easy toĭissolve sodium chloride, to dissolve table salt in water. The ends with the hydrogen, are facing the chlorine. Positive ends of the dipoles are going to be attracted, and so water mightĪrrange itself in this way where the partial positive ends, Similarly, if you have a chlorideĪnion, or a negative ion, well then the partially And so what I'm drawing right over here, these are ion-dipole forces. These water molecules so that you have the partial negative end is facing towards this The partial negative end ofĪ dipole would be attracted to a positively charged ion. So now that we know the differenceīetween ions and dipoles, how might they interact? Well you might guessĬoulomb forces are at play. To form hydrogen bonds just have a very strong dipole moment, because you have hydrogenīonded to an oxygen, a nitrogen, and a fluorine, But, as we've talkedĪbout, hydrogen bonds, which are an intermolecular force are just a special case of dipole forces. The partial positive end of another water molecule. And we describe this when we talked about hydrogen bonding where the partial negativeĮnd of one water molecule would be attracted to More time around the oxygen than around the hydrogen, you have a partial negative charge at this end of the molecule and you have partial positive charges at the other end of the molecules. Much more electronegative that it hogs the electrons, Is quite electronegative, covalently bonded to two hydrogens, and those are really polar covalent bonds because the oxygen's so Molecule that is a dipole or has a dipole moment atĪ molecular level is water. Where the charge is separated on different ends of the molecule, that you have a partially positive end and you have a partial negative end, that there is a molecular dipole moment. We're talking about dipoles, we're not talking about something that has necessarily a net charge, we're talking about something Now what's the differenceīetween that and a dipole? Well, generally speaking when Similarly, when sodium loses an electron, it now has a net positive charge. So for example, whenĬhlorine gains an electron and becomes the chloride ion, it's an ion because it now All right, now let'sįirst think about ions. And I encourage you to pause this video and try to refresh your own memory before we refresh our memories together. And before we think about how ions and dipoles might interact, let's just remind ourselves what the difference isīetween ions and dipoles. Let's talk a little bit about ion-dipole forces.
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