Chemistry Semester 1 Final Exam Answers

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  These two pi bonds are not conjugated. We usually think of the geometry of a nitrogen with three single bonds as trigonal pyramidal e. This is a tradeoff: the slightly increased strain of the eclipsed N-H bonds is made up for by a decrease in...

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  For the image above, the crucial concept here is just the partial double bond character. Not crucial for the rest of the discussion. The reactivity of an alkene can be modified dramatically through the attachment of various groups. To take just one...

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  It was only in that it was finally made as its conjugate acid through a clever route by the lab of Brian Stoltz at Caltech. The X-ray crystal structure bears witness to the lack of conjugation in this amide. The C-N bond length is 1. However, this simplistic approach can only take us so far. Two quick examples, because this post has gone on long enough. First: Conjugation And Color If you saw this post on how bleach works , you learned that as we lengthen the conjugation length, we change the wavelength at which molecules absorb light. Some very brightly coloured molecules such as carotene, chlorophyll and lycopene all have very long conjugated double bonds. For instance, lycopene is responsible for the red colour of tomatoes.

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  If we remove the double bonds, we remove the colour. Why would the number of double bonds have an influence on this? Resonance fails to illuminate this subject. If you treat butadiene with the molecule to its right methyl maleate you obtain a new product containing a six membered ring. Interestingly, if you treat ethene with the same molecule, nothing happens except if you treat it with UV light. Then you get a 4-membered ring, but I digress. Next Up: Molecular Orbital Theory What will help us answer these questions, as well as many others going forward is a concept called molecular orbital theory.

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  Thanks to Tom Struble for all his help with this post. Notes A-1,2 strain is the reason why tetra-tert-butylethylene has not yet been synthesized. The pi bonds are not conjugated. Look at the orbitals comprising the two pi bonds. They are at right angles to each other and cannot overlap. The peaks can usually be made to coalesce by heating the sample probe. This stands in contrast to, say, different chair forms of cyclohexane, which generally can still interconvert at room temperature and coalesce to a single peak.

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