Benzene is a non-polar molecule
It forms a very polar covalent bond between the hydrogen and the carbon and a completely covalent, nonpolar bond forms between the carbon and carbon bond
Forces placed on this molecule when attracted to an identical molecule:
London Dispersion- a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles; the bond is extremely weak and very temporary; the electron distribution is very uneven and gives one side an occasional or the other will gain a small excess of electron density
Benzene is a great chemical. It is formed from both natural processes and human activities. The natural sources of benzene include volcanoes and forest fires. Benzene is also a natural part of crude oil, gasoline, and cigarette smoke. Benzene is very widely used in the United States and ranks in the top 20 chemicals for production volume. Benzene is a colorless, flammable, liquid aromatic hydrocarbon. Some industries use benzene to make other chemicals that are used to make plastics, resins, and nylon and synthetic fibers. Benzene is also used to make some types of lubricants, rubbers, dyes, detergents, drugs, and pesticides. It is also an industrial solvent and additive in gasoline. It is a great chemical that all companies should look into using. It is also known as benzine or benzol.
I like this blog's appearance. The colors really contrast and it is easy to read. My only suggestion would be to make the text a little bit larger. This might make it a little bit easier to read, but it is still fine as it is. I don't really understand the picture because it looks like there is are ten electrons on some of the carbons but I think that might just be me. I think that it might have been better if she drew it herself, however, the angles are obviously accurate, and the polarity of the bonds is also correct. I agree that the molecule is non-polar and would only be attracted to itself by London dispersion, which she did a great job of explaining. The ad is very well-written. I think the best part is that she made it very clear that there are many uses for benzene, and she gave many examples to make her point. I would definitely look into using benzene because it seems to be such a versatile chemical. However, I think it would have been helpful to give some kind of caption to the ad to set it off from the earlier section of basic information. Overall, it was definitely a good ad and a good presentation with accurate information.
ReplyDeleteThe appearance of this blog is good and it is easy to focus on the information. The molecule has accurate bond angles, but I cannot figure out the bonds between the carbon atoms. They look like they would be triple bonds but then that would make each carbon have ten electrons. It is correct to say that this is a non-polar molecule because no side is more negative or positive than another. The intermolecular forces are correct and are well explained. The ad does a good job describing the molecules properties and if I owned a company I would buy this chemical.
ReplyDelete1. The appearance of the page is nicely displayed. It is easy to read and follow. The background is very cute and the colors complimentary.
ReplyDelete2. The molecule appears to be drawn correctly. Although you may want to think about adding color nest time the bonds appear to be correct as well.
3. I agree the molecule is non-polar with the positive forces of the Hydrogens canceling out the positive Carbon atoms.
4. The only intermolecular forces in this molecule can be London Dispersion as stated.
5. Finally I think you did a fantastic job with the ad. You not only gave its uses but also its properties. I just wanted to go out and buy some of this chemical.
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