4 posts • Page 1 of 1
Hi everyone! As I an studying for the final, I am just a little confused on evaluating Bronsted Acids and Bases, and how those compare to Lewis Acids and Bases. I often think to myself about how a compound will affect the H+ or OH- concentration, but I mix up how to identify a Bronsted B/A and Lewis B/A. Could someone give me a basic overview on how to approach evaluating what makes an acid and base according to Lewis and Bronsted acids and bases? Thank you so much!
Lewis bases will donate an electron pair to a compound while Bronsted bases will accept a proton (H+). On the other hand, Lewis acids will accept a donated electron pair while Bronsted Acids will donate a proton. When looking at specifically Bronsted Bases and Acids, Bronsted bases when added to water will take away a proton from water (remember they are proton acceptors), resulting in the formation of OH-. This will raise the solutions pH. The opposite is true for Bronsted Acids, which will donate a proton to water when mixed, creating H3O+ molecules. THis will lower the pH of a solution. Depending on the situation, Bronsted Bases and Acids can either be Lewis bases or acids. For Lewis Bases and acids, look specifically at the electron pair, and whether one is being donated or accepted. Hope this helps!
Lewis acid accepts electron while Lewis base donate electron. Bronsted acid donate proton(H+) while Bronsted base accept protons(H+).In water, Bronsted acid will therefore donate a proton to H2O making it a H3O+, thus making the solution more acidic(lower pH), while Bronsted acid will take away the proton from H2O forming OH-, thus making the solution more basic.
Who is online
Users browsing this forum: No registered users and 1 guest