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The instantaneous dipoles in 2 nearby rod shaped molecules are closer than those found in nearby spherical molecules. This is because rod shaped molecules have more surface area that is closer to each other. Because of this, rod shaped molecules have stronger interactions than spherical molecules. This explains why rod shaped molecules tend to have much higher boiling points than spherical molecules.
Rod shaped molecules interact more easily because of the increased surface area, and also because when they line up next to each other, their nucleus's and electrons can get closer together because in the short side of the rod, the outside of the molecule is closer to the nucleus's.
CandiceNourian1J wrote:Can someone explain the key differences between rod shaped and spherical shaped molecules?
The main thing to remember with the rod shaped molecules is that they are closer to one another and thus the strength of the LDF is greater. With the spherical shaped molecules, they are father apart form each other and thus the LDF is not as great. Think of this as a greater surface in which the two molecules can attract.
I get it now. The rod shaped molecs have greater surface area bc of more pts of interaction btwn 2 polar molecs, which causes a stronger interaction btwn the 2 molecs. therefore, a higher BP would be needed to break up the 2 molecs.
rod structures have more surface area (because they are longer and stretched out) and so they will have more areas to bond whereas a spherical structure does not have as many areas to bond. As a result, 2 rod structures are more strongly held together than two spherical structures.
Two adjacent rod shaped molecules will have more surface area in contact with each other than two spherical molecules. This is significant because London dispersion forces will have a greater effect on the rod shaped molecules.
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