28) Define all three definitions of acids and bases giving examples of each.
Arrhenius
Acid - Contains at least one H+ ion that when diluted, will release into water. (i.e. HNO3, H2SO4)
Base - Contains at least one OH- ion that when diluted, will release into water. (i.e. KOH, Ca(OH)2)
Bronsted-Lowry
Acid - When in a reaction, will act as a H+ ion donner, ending up as the conjugate base. (i.e. HCl, H20)
Base - When in a reaction, will act as a H+ ion acceptor, resulting as the conjugate acid. (i.e. NH3, H20)
Lewis
Acid - This type of acid must act as a electron pair acceptor in a reaction. (i.e. H+, BF3)
Base - This type of base must act as a electron pair donner in a reaction. (i.e. NH3, OH-)
Very good definitions! A little expansion on the last definitions: A Lewis acid acts as an electron pair acceptor in a reaction in order to create a coordinate covalent bond. Also, a Lewis base acts as an electron pair donor in a reaction in order to create a coordinate covalent bond.Otherwise, good job and good examples!
ReplyDeleteYour definitions were very good. Just maybe you could have added a visual or picture to the Lewis definition, but otherwise good work.
ReplyDeleteGreat job Nick! You might want to go a little further and discuss how it goes from specific to a much more broad definitions. This is because when talking about the Lewis definition it does NOT mention anything about H+ ions or OH- ions. It simply means that as long it accepts or donates an electron pair it can be classified as an acid or base. However, when talking about Arrhenius it becomes a very specific definition which DOES mention that it must have an H+ and OH- ion to be considered an acid/base. Overall, great job and you might add pictures.
ReplyDeleteGood job on your blog posting. Your explanations and examples of the definetions helped a lot, the only thing that could of made it better was maybe a picture of the lewis dot defenetion.
ReplyDeleteGreat job on your definitions! They were very helpful and easy to understand. A more detailed example of the Bronsted-Lowry definitions would have been helpful, like an example showing which ions act as the acid, base, conjugate acid, and conjugate base. Otherwise, you did a really good job explaining these three types of acids and bases!
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