Identify each chemical species as an Arrhenius acid or base, a Brønsted-Lowry acid or base or a Lewis?

Question

In Table 2, identify each chemical species as an Arrhenius acid or base, a Brønsted-Lowry acid or base, or a Lewis acid or base. Some species may fit the definitions for more than one of the theories. Use a check mark to indicate all applicable answers.

Here is the table

Please help, I have NO IDEA what to do

http://tinypic.com/view.php?pic=2mqiz44&s=4

Answer 1

let me add on to the previous answer. With bronsted lowry keep in mind...to be a base it just needs to be able to accept a proton with its electron pair. Such examples are NH3, or So3 2 minus, or pretty much any polyatomic ion with a negative charge on it since it has free electrons to pluck  off a hydrogen. While Arrhenius bases are bronsted bases, it does not work the other way around. Arrhenius bases need to have an OH minus in solution to accept the proton, which is DEFINATELY not what a bronsted base is.

Most importantly if something is a Bronsted base it is ALWAYS a lewis base, and vice versa! Lewis bases just have to do with having that free electron pair to donate and pluck off that proton.

As for acids, ALL Arrhenius acids are bronsted acids, and all bronsted acids still need ot have a proton to donate like arrhenius( not exactly the same since arrhenius said it must be in water) That just has to do with giving up a proton. A lewis acid is VERY different  than a bronsted acid. It just needs to have a vacant orbital to accept an electron. Common acids include aluminum trichloride, and especially metal cations with posiitve charges, they can definately accept electrons.  this will hopefully make your homework easier good luck!

Answer 2

the arrhenius definition of acids and bases are based off the exchange of H+ and OH- ions. it's the narrowest definition...an acid must be able to give up an H+ and a base must be able to receive that H+ with an OH-.

the Bronsted-lowry definition is based solely on the exchange of the H+ ion...the acid gives and the base receives...this definition is a little more broad and the bases do not need to have an OH-

lastly, the Lewis definition is based on the exchange of electron pairs....this is the broadest definition of acids and bases....they don't even have to have an H+. the acid gives the electron pair and the base receives it.

the end.