Methylamine Lewis structure

Is the second step of the overall reaction for R=Me (N-methylphthalimide + hydrazine —> phthalimide hydrazide + methylamine) exothermic or endothermic Will higher temperatures accelerate or inhibit the reaction Is the structure drawn above for phthalimide hydrazide its lowest-energy form or are either the imine or diimine tautomers preferred Compare energies for the hydrazide and imine and diimine tautomers. Examine the geometry of phthalimide hydrazide and any low energy tautomer, and draw the Lewis structure(s) that best describes it. Can your Lewis structures account for the energy differences Examine electrostatic potential maps for all three molecules. Which molecule(s) are stablized by favorable electrostatic interactions Which are destabilized Can this help explain the energy differences Elaborate. 

Examine the geometry of formamide. Is the CN bond shorter than expected for a normal single bond (in methylamine), and closer to that expected for a full double bond (in methyleneimine) Is the CO bond longer than that expected in a carbonyl compound (in formaldehyde), perhaps closer to that appropriate for a single bond (in methanol) Also, compare the electrostatic potential map for formamide with those of formaldehyde and methylamine. Is the CO bond in formamide more or less polar than that in formaldehyde Is the CN bond in formamide more or less polar than that in methylamine Draw whatever Lewis structures are needed to properly describe the geometry and charge distribution of formamide. 

Write the Lewis structure of each of the following organic compounds (a) ethanol, Cl IjCLLOH, which is also called ethyl alcohol or grain alcohol (b) methylamine, CH3NH2, a putridsmelling substance formed when flesh decays (c) formic acid, HCOOH, a component of the venom injected by ants. 

Objective 12 61. Describe the information given in the following Lewis structure for methylamine,... 

Hydrogen cyanide can be catalytically reduced with hydrogen to form methylamine. Use Lewis structures and bond energies to determine for... 

A quantitative study of the s-trinitrobenzene-dimethylamine interaction in dioxane led to the conclusion that four amine molecules are involved to give a 1 4 complex (53). It was later shown that the spectroscopic data can be better accommodated by assuming three equilibria to form 1 1, 1 2, and 1 3 complexes, with the 1 3 complex responsible for most of the measured absorption. Structures comparable to those of Lewis and Seaborg were proposed for these adducts (54). A more detailed study in dioxape and chloroform (55) gave results in accord with this interpretation for the interactions of s-trinitrobenzene with methylamine, ethylamine, dimethylamine, and diethylamine. Only a 1 1 complex was observed with more bulky amines. In most cases it was possible to observe a fast reaction, probably to form a charge-transfer complex, as well as the slower reaction giving the above complexes. 

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