Structure
The molecule C3H6O, also known as Acetone, is Triangular Planar. Its Lewis Structure is:
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| This atom is an AX3 or a Triangular Planar because there are no unshared pairs on the central atom and the central atom has three other atoms haning off of it. The central carbon shares a double bond with the Oxygen and a single bond with the other Carbons. The two other carbons share three single bonds with three Hydrogens each. Bond Angles  The red ball represents Oxygen. The black balls represent Carbon. The white ball repsesent the Hydrogens. The molecule is a triangular planar molecule so the bond angles on C3H6O are 120 degrees. Polarity of the Molecule and its Bonds Molecule Polarity Acetone is a polar molecule. First of all, there is a double bond between the central carbon and the oxgen. The oxygen has two unshared electron pairs which make that end of the molecule highly negative. The bonds between the central Carbon to the other Carbons are single. Those Carbons both have bonds with three Hydrogens, which have a positive charge. The uneven distribution of charges througout the molecule makes it polar. Bond Polarity/Electronegativity C-----H 2.5-2.2---> 0.3 This bond is very covalent O----C 3.5-2.5---> 1.0 This bond is moderately covalent Attractive Forces If one Acetone came next to another Acetone there would be two attractive forces. These are: London Dispersion Forces:An electrostatic attraction between the poitive end of a dipole and the negative end of another dipole. Dipole-Dipole Forces:A weak force of attraction between two molecules created by temporary dipoles caused by elections moving around two atoms. This happens with all molecule because electrons are constantly moving This molecule is not attracted to another molecule of Acetone by hydrogen bonding because although there are hydrogen molecules they are not bonded to an Oxygen, Flourine or Nitrogen. Hydrogen Bonding: A special case of dipole-dipole where a covalent bond occurs between a hydrogen of one molecule and a Oxygen, Nitrogen or Fluorine of a different molecule. However, if this molecule came across a molecule such as HF there would be hydrogen bonding because the Hydrogen of Acetone would form a bond with the Flourine of HF. |
I like the appearance of this blog becasue it is easy to read and get all the information from. It is easy to access and read. Your information about acetone is completely accurate. You gave good general information at the beginning and then went into the more complicated information later which was very good. You were accurate in saying that the molecule is triangular planar in an AX3 form. Also, you were right saying that acetone is polar because of the negative oxygen with an unpaired pair of electrons and the positice hydogrens, making the moelcule have an uneven distribution.
ReplyDeleteYou were accurate in finding the intermolecular forces of acetone as well. It has hydrogen bonding possible in other cases but not between two molecules of acetone. It does have london dispersion forces and dipole dipole forces. This is because of the attraction bewteen the positive and negative ends of the molecule and also because of the distribution of electrons on the molecule that make it temporarily negative or positive.
Lastly, I thought the ad was sucessful in giving all the information needed about acetone but be careful giving information on how dangerous it is as well. I thought it was ver informative and I did not know acetone was in nail polish remover, which was very cool to learn. Overall, I thought this was a very good blog.
--Sam Travelyn
Overall Appearance: The general appearance of this blog is very nice. It is simple and does not distract or take away from the very important information you gathered on your molecule. Everything is very organized and easy to find. I like how you put your ad at the top of the blog to really capture the readers attention and make want to read more.
ReplyDelete-Kaleigh Crowell Period A
You correctly identified your molecule as polar. One end is positive ( due to the H's) and another end is negative (due to the O). Your bond polarity findings are also accurate in saying both bonds are covalent and that the bond between O and C is a little less covalent then C and H.
ReplyDelete-Kaleigh Crowell Period A
Intermolecular forces: You correctly identified your intermolecular forces. London dispersion is obviously present and dipole-dipole as well do to the positive and negative ends of the molecule. What i found interesting was that hydrogen bonding, as you stated, is in fact not a force in this molecule due to the covalent bond with the carbon atoms leaving it without a positive charge to bond to the oxygen.
ReplyDelete-Kaleigh Crowell Period A
Accuracy of Molecule: Your lewis structure and 3D picture are very accurate. The double bond between Carbon and Oxygen is clearly shown in both structures and the angles are seen in the bottom one as well. This structure is correctly identified as an AX3 and your angles are correct. The information in this blog has proven to be accurate and very enlightening, well done!
ReplyDelete-Kaleigh Crowell Period A
The general appearance of this webpage is appealing and easy to read. The color choices fit well together, along with the font style and type. The brightness of this ad is attractive and helps to sell the product. All images are nicely designed making them easy to read and follow. The layout of information was done so in a order that made sense and impelled the reader to continue.
ReplyDelete-Marissa Salvati, Period C
The molecules shape, bond angles and AX form where explain fully and accurately. The molecule, being a AX3 Triangular Planar was mentioned multiple times and explained so that anyone could understand. Along with the shape the correct bond angle or 120 was expressed and displayed in a picture. All required fields of information where provided in an easy to follow manner.
ReplyDeleteThe molecule is polar, and this reasoning is explained thoroughly. The electronegativity was not only correct by easy to follow. I like the way you showed your results, instead of in paragraph form you listed them in a easier was to follow.
ReplyDeleteThe forces of attraction where stated correctly. I like the way that you not only gave the forces, but then provided a definition. It was also informative that you included the definition of hydrogen bonding, but explained why it didn't work between to acetone molecules because neither F, O, or N where present.
ReplyDeleteUseful info . Thanks for sharing.
ReplyDelete- Mr Acetate
Thank you for the further info about Acetone! It's quite helpful though :)
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ReplyDeleteDo we need to consider acetone as a polyatomic ion? I came across a question that required knowledge of the chemical formula of acetone in order to draw its Lewis structure and derive certain information from it. While I understand that we should be familiar with the acetate ion (C2H3O2-), I'm uncertain if we also need to know the specifics of acetone (C3H6O). I'm a bit concerned now, as I'm wondering if I need to memorize more polyatomic ions than I initially thought. The question only mentioned acetone without providing any additional context or formula. If it's allowed, I can share the question or perhaps send it via private message. I wanted to seek your thoughts on this matter.