Please explain why each option is true/false. Need explanation specfically for i
ID: 792937 • Letter: P
Question
Please explain why each option is true/false.
Need explanation specfically for iv and vi.
The answer is suppose to be C.
Indicate the false statement below: Compounds 1 and 3 form a classical Lewis add / Lewis base pair Compound 4 is less acidic than compound 5 Compound 3 can act as a Bromated base but not as a Lewis base Compounds 2 and 3 are both good bases Compound 2 will not react with compound 4 Compound 5 would not react with a strong acid i and iv iii and vi ii, iii and v i, iii and iv ii and viExplanation / Answer
1)compound 4 is more acidic because a carboxylic acid is stronger,b/c the OH group has H- bondage
2)cant act as a bronstead base because it is no longer able to H and by definition a lewis base can be a bronsted base but bronstead base cant be a lewis base
3) will react as the H is a good leaving group (list of good leaving groups online)
iv) look at the pKa values for the aacids if it has a high pKa for acid then it will be a god base and vise versa ex) carboxylic is very acidic so it conjugate base will be weak stong acid bad base, weak acid strong base
vi) it wont react with a strong acid because it its self is a strong acid and in the reaction wont work as there will be no base present to accept the electrons in donates as usually for the reaction to occure there needs to be a base