By the Br phi nsted-Lowry definition, acids are proton donors and bases are prot
ID: 773768 • Letter: B
Question
By the Br phi nsted-Lowry definition, acids are proton donors and bases are proton acceptors. By the Lewis definition, acids are electron-pair acceptors, and bases are electron-pair donors. For bases, the two definitions are equivalent such that all Lewis bases are Br phi nsted-Lowry bases and vice versa. However, it is possible to have a Lewis acid that is not a Br phi nsted-Lowry acid. This is because Lewis acids include molecules and cations that have a vacant valence orbital, regardless of whether they have a proton to donate. Common examples of Lewis acids (that are not Br phi nsted-Lowry acids) are metal ions, such as Al3+ and Cu2+ The following is an example of a Lewis acid-base reaction: Cu2+ + 4NH3 rightarrow CU(NH3)42+ donates the electron pair to Cu2+ Therefore, is a Lewis base, and Cu2+ is a Lewis acid. Classify each of the following as a Lewis acid or a Lewis base. Drag the appropriate items to their respective bins.Explanation / Answer
lewis acids:Ag+,CH3NH2,SiO2,AlCl3. each are e- acceptors
lewis bases: OH-,Br-, each are e- donors
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.