Question

Order the anionic compounds from the most basic to least basic? 3) 1) 2) Magnify Select One Strongest base Second strongest Match With B 3) Weakest base C 2)

PLEASE EXPLAIN! I NEED HELP. IT WOULD MEAN A LOT.

Answer 1

Greater the tendency of a compound to donate its electrons, greater is its basicity. Oxygen is more electronegative than carbon and would be less susceptible to donate its electron density, therefore, compound (3) is least basic. Compound (2) is less basic than compound (1) as electron density on the carbon can be delocalized on the benzene ring due to conjugation, thereby decreasing its basicity. Therefore, compound (1) is the strongest base. The order of basicity is shown as follows: 3) Strongest base Second strongest Weakest base Sulfur is greater in size than Oxygen so it can easily accommodate electrons around it and therefore would be least basic. Between nitrogen and oxygen, oxygen is more electronegative than oxygen so is less basic. The order of basicity is shown as follows: Strongest base Second strongest Weakest base Among the given molecules, compound (3) is most basic as the free electrons on nitrogen are easily available for donation. In both compounds (1) and (2), the lone pair on nitrogen undergoes delocalization; in (1) the delocalization takes place over oxygen atom and (2) the delocalization of lone pair takes place on benzene ring. Therefore, compound (1) is least basic. The order of basicity is shown as follows: NH2 NH2 Strongest base Second strongest Weakest base

Oxygen is most electronegative among carbon and nitrogen therefore, compound (3) would be least basic. In between nitrogen and carbon, nitrogen is more electronegative, so it is less susceptible towards electron donation. Therefore, compound (1) would be more basic. The order of basicity is shown as follows: NH Strongest base Second strongest Weakest base