Methyl amine is more basic than trimethyl amine because it is more stable. Basicity is based on the stability of a compound as well as the availability of the hydrogens present. With three methyl groups are far more unstable than one methyl group on a nitrogen, since all of the protons are pushing away from one another.
ethylamine is more basic than dimethylamine because the former one allows nitrogen atom to take reaction without any hindrance(prevention) of this reaction to occur.The later one has methyl groups on both sides of nitrogen atom,these groups hind nitrogen atom from reacting weth electrophiles.Remember nitrogen determine reactivity of amines.
In what amine is the nitrogen bonded to two carbon atoms? A 2 carbon amine is ethyl amine C2H5NH2 I have a way to remember the prefixes for organic molecules with a straight line,1C, 2 C, 3 C, and 4C organic molecules. The prefixes are methyl-, ethyl-, propyl-, and butyl-. "ME EAT PEANUT BUTTER". The molecules with more C's -C- methyl -C-C- ethyl -C-C-C- propyl -C-C-C-C- butyl (long u sound) ethyl amine ...H..H ….!...! H-C-C-N-H …!...!...! ...H..H.H
3-methyl amine, aka methyl amine, conatins N-H bonds (polar covalent bonds). Ethane contains only C-H bonds (non-polar covalent bonds). Since the N-H bonds are polar and Nitrogen being more electronegative (ability to attract electrons), it has a slighly negative charge by pulling the elecrons from the hydrogen it is bonded to, giving the Hydrogen a slighly positive charge. The positive H's of one molecule will be attracted to the negative N's of another molecule. This is the force that 'holds' the molecules close to each other. This is why it takes more kinetic energy (temperature) to convert it to a gas than ethane, which essentially has no charge and subsequently very little attraction to other ethane molecules.
Historically, methyl-methyl ester. More modernly, the compound is called methyl methanoate.
Because in Benzylamine : the unshared lone pair of electron on nitrogen atom isavailable >.. But in n-ethyl aniline: the unshared lone pair of electron is not available and enter resonance with benzene ring .(Villa)
Because methyl is an electron pumping group and It pumps electrons to Amine group to make it basic, But Ammonia has no influence from any basic groups. Therefore compared to Methyl-Amine, Ammonia is less basic
You have to state more precisely WHERE the second methyl-group and the amine-group is situated before this Q. can be answered.
ethylamine is more basic than dimethylamine because the former one allows nitrogen atom to take reaction without any hindrance(prevention) of this reaction to occur.The later one has methyl groups on both sides of nitrogen atom,these groups hind nitrogen atom from reacting weth electrophiles.Remember nitrogen determine reactivity of amines.
Pyridine itself (unsubstituted) is basic due to presence of lone pare of electron on nitrogen atom which is not involved in aromatic character , methyl at 4th (Para) position is electron donor due to hyper-conjugation so electrons density at nitrogen becomes increase so 4-methyl pyridine is more basic as compare to unsubstituted pyridine.
In what amine is the nitrogen bonded to two carbon atoms? A 2 carbon amine is ethyl amine C2H5NH2 I have a way to remember the prefixes for organic molecules with a straight line,1C, 2 C, 3 C, and 4C organic molecules. The prefixes are methyl-, ethyl-, propyl-, and butyl-. "ME EAT PEANUT BUTTER". The molecules with more C's -C- methyl -C-C- ethyl -C-C-C- propyl -C-C-C-C- butyl (long u sound) ethyl amine ...H..H ….!...! H-C-C-N-H …!...!...! ...H..H.H
3-methyl amine, aka methyl amine, conatins N-H bonds (polar covalent bonds). Ethane contains only C-H bonds (non-polar covalent bonds). Since the N-H bonds are polar and Nitrogen being more electronegative (ability to attract electrons), it has a slighly negative charge by pulling the elecrons from the hydrogen it is bonded to, giving the Hydrogen a slighly positive charge. The positive H's of one molecule will be attracted to the negative N's of another molecule. This is the force that 'holds' the molecules close to each other. This is why it takes more kinetic energy (temperature) to convert it to a gas than ethane, which essentially has no charge and subsequently very little attraction to other ethane molecules.
You add one more amine into it !
in basic medium m-nitrobenzoic acid reacts with methanol to form methyl m-nitrobenzoate
There are more than 20 stuctural isomers of hexene C6H12, including various branched (cis and trans) and cyclic compounds (eg. cyclohexane, methyl-cylopentane, 1,1-dimethyl-cyclobutane, 1,2-dimethyl-cyclobutane, 1,3-dimethyl-cyclobutane, and some other, maybe not stable, propyl/methyl-ethyl/trimethyl-cyclopropanes) Some of them also count for optical isomerism (eg. 3*-methyl-1-pentene)
yes methyl chloride is more reactive.
Methyl mercury is more toxic
Historically, methyl-methyl ester. More modernly, the compound is called methyl methanoate.