Which is more basic nh3 or CH3NH2?

The CH3NH2 is more basic than ammonia. It is because the CH3NH2 has methyl group which is usually an election releasing group. It has +l effect of the methyl group. For this electrons are more concentrated over Hydrogen.

Which one of the following is most basic NH2 NH2 CH3?

(CH₃)₂NH is most basic most basic among all others. Basicity is the ability of the atom to donate its lone pair of electrons.

Which is more basic NH2 or NH?

Answer: Answer:This is due to the electron donating effect of alkyl groups which increase the electron density on nitrogen. This makes the lone pair on nitrogen more available for donation, and tertiary amines are the strongest bases. Hence the more R groups the amine has, the more basic it is.

Why is NH2 most basic?

The amide anion (NH2-) is much, much more basic than the chloride anion (Cl-). This is because of their conjugate acids. Strong acids have weak conjugate bases and weak acids have stronger conjugate bases. The conjugate acid of Cl- is HCl, a very strong acid called hydrochloric acid.

Which is more basic CH3NH2 or CH3 3n?

(CH3)3N is more basic because greater number of alkyl groups increase the magnitude of +I effect so increase the basicity.

Is NH2 stronger base than F?

Fluorine is the most electronegative, so F- (fluoride ion) is the least willing to donate electrons (the weakest base). Overall, the electronegativity order is C (2.5) < N (3.0) < O (3.5) < F (4.0), so the order of basicity is -CH3 (strongest base) > -NH2 > HO- > F-.

Which of the following amine is most basic?

Aliphatic amines are more basic than aromatic amines thus methylamine is most basic. Electron donating groups increase the basicity whereas electron withdrawing groups decrease the basicity of the aromatic amines. Thus p-methoxyaniline is more basic than aniline which is further more basic than p-nitroaniline.

Which of the following are stronger bases than CH3NH2?

d : The increasing order of basicity of the given compounds is CH32NH > CH3NH2 > CH33N > C6H5NH2 Due to the +I effect of alkyl groups the electron density on nitrogen increases and thus the availability of the lone pair of electrons to proton increases and hence the basicity of amines also increases.

Which amine is less basic?

Basicity of amines can be explained on the basis of availability of electron density on N-atom for protonation. Because of the +I effect, alkyl group increases the electron density on N-atom in alkyl amines. However, aniline is less basic because phenyl group exerts −I effect, ie, it withdraws electrons.