Final answer:
The statement that NaNH2 is too strong a base for the dehydrohalogenation of a geminal dihalide is true. Dimethylamine is stronger than methylamine, and its conjugate acid is weaker due to better stabilization of the positive charge. The statement is true.
Step-by-step explanation:
Regarding the true or false question of whether NaNH2 is too strong a base to perform dehydrohalogenation of a geminal dihalide, the statement is true. Sodium amide (NaNH2) is a very strong base, often too strong to selectively dehydrohalogenate geminal dihalides without deprotonating other acidic protons present in the molecule.
Comparing the base strength, methylamine (CH3NH2) and dimethylamine ((CH3)2NH), the dimethylamine is the stronger base because it has two electron-donating methyl groups that increase the electron density on the nitrogen, making it more able to accept a proton. Conversely, among the conjugate acids (CH3)2NH₂+ is the weaker acid because the positive charge is better stabilized by the electron-donating effects of the two methyl groups, compared to CH3NH3+, which has only one such group.
In the context of acidity and base strength, the acidity of compounds increases down the group in the periodic table, and across a period, the acidity increases with increasing electronegativity. An example of a strong base given in one of the provided extracts is Mg(OH)2, while NH2- is mentioned as a strong base that completely dissociates in water to form hydroxide ions.