Dipole-Dipole?

Question

Do tetrahedral structures have dipole-dipole interaction? If so, how?

Answer 1

Imagine CCl4
Each bond is polar because there is a big difference between the electronegativity of Cl and H. However the sum of the dipole moment of all the bonds is zero, because of the geometry but also because the bonds (and thus their dipole moments) are identical.

Imagine CH2Cl2
The geometry is again tetrahedral but now not all bonds are identical. The dipole moment for the C-H bonds is much smaller than that of C-Cl. So now the sum of these vectors is not going to be 0. It is going to be a new vector (can't really draw it here) but it will be a dipole (at one end it will have partial negative charge and at the other partial positive).

Have a look at

http://dwb.unl.edu/Teacher/NSF/C06/C06Links/www.uis.edu/7Etrammell/organic/introduction/polarity.htm

The interaction will be between 2 molecular dipoles, based on the spatial position of the total dipole moment of each molecule.

Answer 2

I don't think so. I think dipole-dipole interactions are interactions between a dipole of one molecule to dipole of another molecule.

so, a tetrahedral can't have dipole-dipole interaction within the own molecule but it can have one with another molecule as long it has a dipole.

Answer 3

right here is my advice: look for advice from a typical chemistry e book (heavily). which could help you recognize a thank you to foretell whether the geometry is bent or not. unquestionably, you look on the molecule and are available up with what that is geometry could be if each lone pair of electrons grow to be bonded to a various atom. as an occasion, H2O has 2 lone pairs of electrons, which if bonded, could provide you a tetrahedral geometry. Then think of which you do away with the atom on the right of the tetrahedron, leaving a lone pair at the back of. next you do away with yet another atom, leaving yet another lone pair at the back of. The configuration of the remainder 3 atoms is bent. See? With CO2, you have not have been given any lone pairs, so the configuration is in simple terms linear. you may then be waiting to work out that, because of the fact that CO2 is linear, the two oxygens pull electrons in opposite instructions, cancelling out one yet another's dipoles, leaving no internet dipole. whether, with water, there is not any such symmetry and for this reason a internet dipole. this is this dipole that makes water a polar molecule, alongside with the reality that there is a super difference in electronegativity between oxygen and hydrogen. you're unlikely to be waiting to hit upon the dipole 2nd of a molecule straight away, yet like I reported, you may look for advice from a typical chemistry textbook.