Which compound in each of the following pairs would you expect to have the greater dipole moment ? Why?
CHCl3 or CCl3F
So now, what about between CHCl3 and CCl3f, okay? So I'm going to go ahead and paste our table down again, right? Our chem 7 with our trans here, but guys we actually do need to worry about geometry here, so I'm going to go ahead and draw this out, we have our carbon in the middle, let's say we have our hydrogen at top and then we've got a planar chlorine a wedge chlorine and a dash chlorine. Now, the next one would look something like this, we can go ahead and put our F at the top, our Cl down here, our Cl on the wedge and then I'm going to dash another Cl, okay? So, really what we see here is that we've got a net dipole pulling down, right? Our net dipole looks like that, going toward the chlorines in the middle of the chlorines and then over here well actually we still have that net dipole pulling down but we've got that one fluorine on top, right? That's going to be subtracting from that vector, okay? So we're going to get, for exaggeration here, to make it more clear, we're going to have a vector about that size. So, actually even though we've got that fluorine and you might be thinking, okay? Great we got the most electronegative atom there in addition to our three chlorines, I'm going to, you're actually not going to end up with a more polar molecule, right? this guy is actually more polar, so this one wins. Alright, so let's move on.
Which of the below molecules has no net dipole moment?
For the following molecules, use the dipole moment symbol to show the direction of the molecular dipole moment in all molecules that have an overall molecular dipole. Note for this one you do NOT need to draw the individual bond dipole moments, just the overall molecular dipole moment,
Based on the electronegativities of C, H, and Cl, would you expect the Cl3CCCH molecule to be polar or nonpolar? A molecule is polar if the vector sum of its bond dipole moments is not equal to zero. A molecule is nonpolar if the vector sum of its bond dipole moments is equal to zero. Pauling electronegativity values are listed in the periodic table on the last page of this handout.
A. Polar molecule
B. Nonpolar molecule
Which pair of elements listed below would be expected to form an ionic bond rather than a covalent bond?
A. C–Mg B. C–Li C. Al–Cl D. H–F E. O–Na
F. More than one pair, but not all of them, would form ionic bonds rather than covalent bonds.
G. All of these pairs would form ionic bonds.
H. None of these pairs would form ionic bonds.
Circle the molecule with the smallest dipole moment.
Which compound is less polar?
Five pairs of atoms are listed below with dipole moments. Pick the correct ones (maximum of two).
Which of the following molecules is polar (hint: It has a molecular dipole)