Jump to content


Senior Members
  • Content Count

  • Joined

  • Last visited

Everything posted by Invader_Gir

  1. No harm no foul. Oh yes. In order to get the second nitration, higher temps, longer reaction times, would be required.
  2. I know how to name esters. That was not the question. But I did find the answer else where. They are named as alkoxycarbonyls, as in [2-(Ethoxycarbonyl)ethyl]trimethylammonium ion C2H5-C(=O)O-CH2CH2-N+(CH3)3 (positive charge on nitrogen)
  3. No need to get snippy. It isn't a carboxylic acid group either. It's an ester, that is why I said carbonyl, similar but not the same. I did take into account the electron withdrawing effects. Also, there are two equivalent meta positions, and once the first nitro group is attached, nitration may happen again at the second meta position, ie, carbon 5.
  4. I know it is an ester. How would you name this if it did not have priority and had to be named as a substituent.
  5. As of right now, the name for the following substutuent escapes me, any help would be appreciated. -C(=O)OCH3
  6. I'm fairly sure that only a few reaction conditions need to be modified. Methyl Benzoate consists of a benzene ring with an electron withdrawing carbonyl group attached. This being the case, an elevated temperature and a higher concentration of the electrophile should work. Substitution would also occur primarily meta to the carbonyl group. If multiple nitrations are required, an even higher temperature and concentration would be needed, since there is an electron withdrawing nitro group present on the ring aswell. Again that substitution would occur meta to both the carboxyl group and the existing nitro group. Hope this helps.
  7. Oh yeah, *blush* forgot about that. Thanks!
  8. Since Grignard reagents are metal organics, I figured this would be appropriate place to ask: Will Grignard reagents react with ethers? I know that they do with epoxides, but that reaction is favorable because of ring strain, but just your typical R-O-R' ethers. Thanks!
  9. If I remember correctly, you can create a sort of 'gel' by mixing the ethanol with a saturated solution of calcium acetate. Use about 1mL of the Ca(CH3COO)2 solution to 7mL of the ethanol
  10. Alright, please bear with me as I attempt to detail my proposed method of synthesizing geraniol (3,7-dimethylocta-2Z,6-dien-1-ol). Keep in mind that this is my first multistep synthesis, and with only one semester of organic. First, react ethene with bromine in carbon tetrachloride, yielding 1,2-dibromoethane. Second, react 1,2-dibromoethane with an acetylide anion, yielding 4-bromobut-1-yne. **Now this is where I have my first question...as the first molecules of the product form, would the unreacted acetylide ions displace the other bromine on the 4-bromobut-1-yne.** Let's assume that if we use a stoiciometric ratio of reactants: Third, hydrogenate the alkyne using the P-2 catalyst. This yields 4-bromobut-1-ene. **Second question, if 1 mol of hydrogen was used, would the resulting alkene react with the hydrogen that has yet to react** Assuming that it doesnt...: Fourth, conduct a hydroboration/oxidation on the 4-bromobut-1-ene, yielding 4-bromobutan-1-ol. Oxidize the bromoalcohol with pyridinium chlorochromate, yielding bromobutanal react the bromobutanal with sodium methoxide, yielding but-4-enal. React but-4-enal with Isopropyl magnesium bromide, following up with protonation with ammonium bromide. This yields 2-methylhex-5-en-2-ol. React the alkenol with Hydrogen Bromide in the presence of peroxides, yielding 5-bromo-2-methylhexan-2-ol React 5-bromo-2-methylhexan-2-ol with acetylide ion, yielding 2-methylhept-6-yn-2-ol. Hydrogenate 2-methylhept-6-yn-2-ol using P-2, yielding 2-methylhept-6-en-2-ol React the alkenol with Phosphorus Tribromide yielding 3-bromo-2-methyl-hept-6-ene. Conduct oxymercuration/demercuration, yielding 2-bromo-3-methylhept-6-ol. React alcohol with sodium methoxide, yielding 2-methylhept-2-en-6-ol. Oxidize alcohol with pyridinium chlorochromate, yielding 2-methylhept-2-en-6-one. React ketone with enolate ion of acetaldehyde, yielding geranial. Reduce the aldehyde with Lithium aluminum hydride, yielding the final product, Geraniol. Please comment on this, correct any mistakes that I (more than likely) made. I appoligize for the lack of aesthetic appearances.
  11. sodium is used to store sodium? Do you mean mineral oil?
  12. I *think* that it would be zero, since it would be a larger number divided by an even larger number....however, I am no math genius.
  13. Before starting my job at the university's chemistry stockroom, I didnt have any experience with chemical burns. That is not to say that I never had chemicals on my hands. In high school, I had concentrated sulfuric, right from the bottle, spilled on my hands, not much, but about a 1-2mL. No burn was experienced, and the acid was rinsed off. However, while working with a dilute solution of nitric acid, while making silver nitrate, I forgot to put rubber gloves on, and parts of my hands started turning white. The spots turned purple a day later, and a week later, peeled off. And, children, the moral of the story is to wear gloves when working with potentially dangerous chemicals.
  14. Is there any information that is missing? As chuinhen said, you can calculate the Ksp of AgSCN from its molar solubility. For the second question, you can do an ICE table (ICE stands for Initial Change Equilibrium), see example below. If you know your Ksp, you can just substitute these into the concentrations, Ksp=(x)(.01+x)=.01x+x^2 Then just solve for x. If I have made any mistakes, please correct me.
  15. Invader_Gir


    If you know the concentration of the ions in the solution, and the Ksp of the compounds in question that may form, you can predict if a precipitate will form.
  16. I've converted most of the left over silver to AgCl. Is there anyway to then convert this to silver nitrate? Or is there way to convert silver sulfate to silver nitrate. I was thinking about trying to dissolve them in concentrated ammonia solution to make the Tollens reagent again, then reduce the ion to silver metal and just add nitric. Would this work? Or would so little dissolve that it would be futile? Thanks
  17. Oh oh! I know what that says! And its true!
  18. Just a follow up question...after performing this experiment, a greyish sediment was collected via vacuum filtration. What is this compound...is there any silver in this? Would adding nitric acid make silver nitrate, so we could do the experiment again? Also, a buddy and I are making a chess table with this stuff, so the black spots are mirrored. What tape would be good to use to keep some of the squares clean. Tried a sample with painters tape, with tollerable results. Thanks again
  19. That would be awesome akapr. Dookiedog@gmail.com
  20. Is there such a thing? A book that contains numerous syntheses. Google is a good resourse, but I would like to know if a hard bound copy exists. Thanks.
  21. In response to YT: Yes this compound does exist. There was a presentation at my college a few weeks ago about how scent functions. The presenter had an array of different esters and things that had distinct smells. This one in particular caught my fancy, since it had the aroma of cotton candy. I was hoping to fix me up some, but whatever. Thanks for all the replies!
  22. It's ok if the name is over my head, could you please still tell me what the name is? And I may not have taken organic chemistry yet, but that doesn't mean I haven't read any books =P. Thanks
  23. Could someone help me with naming the attached organic molecule. Sorry for the crappy diagrahm, but I did my best. Would the parent compound be Toluene? Would the name be 2-Hydroxy-3-Oxy-Oxytoluene? I have yet to take organic yet, so I have very basic knowledge of organic nomenclature. Thank you very much.
  24. Alright thanks. But the lab manual I have calles for Potassium Hydroxide instead of Sodium.
  25. In this reaction, a solution of silver nitrate, potassium hydroxide, glucose, and a little ammonia are put into a flask. The flask is swirled, and the glucose reduces the silver ions and they are deposited on the wall of the flask. This reaction is a little more detailed than that, but I just wanted to give a little backround. Any ways, the question: Could sodium hydroxide be used in place of the posassium hydroxide. Thanks
  • Create New...

Important Information

We have placed cookies on your device to help make this website better. You can adjust your cookie settings, otherwise we'll assume you're okay to continue.