Characteristics of the Three Acid-Base Theories...help!!

Question

Complete Table 1 by noting how each theory defines acids and bases. Also, list chemical reactions that demonstrate the action of each acid or base. For example, in the reaction HA → H A-, HA acts as an Arrhenius acid.

Table 1 Theory- Acids Bases

Arrhenius-

Brønsted-Lowry-

Lewis-

2. Which of the three theories is applicable to the greatest number of acids and bases? Explain your reasoning.

3. which theory is most important for the majority of chemistry students?

Answer 1

Arrhenius:HA → H^+ , A- introduced "disociation":an acid would split.outdated theory.plain wrong.

spontaneous

Brønsted-Lowry:HA+H2O>H3O+ , A- ,considered the interaction with the solvent,"ionization" thru H+  between  components

Lewis-same theory as Bronsted but the transfer is limited,consisted of a pair of electrons,and gives rise to a bigger molecule,with a special covalent bond>coordinative,dative.Lewis acid-base scale,in water,i think is limited(unlike pH scale>Bronsted)

2.BRONSTED,because we deal mostly with reactions which need water as solvent.H20 is not important in Lewis interactions because

of the very weak base caracter,ill defined.hidrogen bond is most preferable theory(not included as part of lewis theory)

3.BRONSTED-when explain a pair of ions forming

Lewis-to explain a bigger molecule forming-"glueing".

Hidrogen bond in water-in biochemistry;