Acids & Bases: Arrhenius, Brønsted-Lowry, and Lewis

Click For Summary

Discussion Overview

The discussion revolves around the definitions and examples of acids and bases according to the Arrhenius, Brønsted-Lowry, and Lewis theories. Participants are attempting to complete a table that outlines these definitions and provide chemical reactions that illustrate each theory's concepts. The scope includes conceptual understanding and application of these theories in chemistry.

Discussion Character

  • Conceptual clarification
  • Debate/contested
  • Homework-related

Main Points Raised

  • One participant seeks clarification on the definitions of acids and bases according to the three theories, noting confusion about the symbols used in their initial answers.
  • Some participants explain that the Arrhenius definition involves proton transfer, while the Brønsted-Lowry definition focuses on the contribution to hydronium concentration in water.
  • Another participant suggests that the Lewis definition is broader, encompassing electron pair donation and acceptance, which may apply to more acids and bases than the other two definitions.
  • There is a discussion about the limitations of the Arrhenius theory, which requires acids to be in aqueous solution, and the variability of Lewis acids.
  • Participants express uncertainty about how to provide examples for the Brønsted-Lowry theory and whether it matters which reactions are listed for acids and bases.
  • One participant acknowledges a misunderstanding and seeks further resources to clarify their confusion regarding chemical formulas and definitions.

Areas of Agreement / Disagreement

Participants express differing views on the applicability of the three theories, with some arguing that the Lewis theory is more general, while others highlight the limitations of Arrhenius and Brønsted-Lowry definitions. The discussion remains unresolved regarding which theory is most applicable to a broader range of acids and bases.

Contextual Notes

Participants mention confusion over specific chemical reactions and the symbols used in their examples. There is also uncertainty about the definitions and applications of the theories, indicating a need for further clarification and understanding.

AngelShare
Messages
208
Reaction score
0
Problem: 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.

Firstly, I'd like to check my answers for the chemical reactions part.

Arrhenius:

Acids- HA --> H+ + A-
Bases- XOH --> X+ + OH-

Bronsted-Lowry:

Acids- ?
Bases- ?

This is all that was listed:

HCl + H2O <===> H3O+ + Cl-

HNO3 + H2O <===> H3O+ + NO3-

HC2H3O2 + H2O <===> H3O+ + C2H3O2-

NH3 + H2O <===> NH4+ + OH-

I don't really understand them though...

Lewis:

Acids- HNO3 => H+1 + NO3-1
Bases- ?

To be honest, I don't really understand what I'm doing. :blushing: I started reading what I was assigned but I got stuck on Bronsted-Lowry's theory so I took out the book my public school loaned me. Since this is a new chapter, I started off reading the basics and worked my way up to the three theories mentioned on my lesson page. Doing so only manged to confuse me more because now I'm wondering where the "A" and "X" are coming from in my first answer.

Maybe someone could explain this to me or give me some sites?:smile:
 
Physics news on Phys.org
:rolleyes: Um...
 
the arhenius definition refers to proton transfer, bronsted to the acid/base contribution to the hydronium concetration in water (pH), the lewis definition is defined by the acid being the acceptor of the lone pair electrons that are donated by the base to form a coordinate covalent bond.

Usually in the lewis definition the bases are denoted as "B" with the lone pair component, the acid is a times denoted as A and the resulting adduct is A-B
 
The browsted lowry theory is an acid base definition in respect to proton transfer. an acid is class as a solution that :bugeye: under normal conditions will donate protons. a base being the opposite is one that will accept protons.:smile:
 
GCT said:
the arhenius definition refers to proton transfer, bronsted to the acid/base contribution to the hydronium concetration in water (pH)
I believe you've got these interchanged.
 
Perhaps, it's just that the op suggested that the info was from the text, and accordingly he/she had denoted those characteristics for Bronsted and Arrehnius respectively. My internet connection is desparately slow at the moment, so I'm going to need to update myself with a text when I have the time.
 
AngelShare said:
Maybe someone could explain this to me or give me some sites?:smile:

http://www.nyu.edu/classes/tuckerman/honors.chem/lectures/lecture_21/node1.html
 
Last edited by a moderator:
yeah, my mistake, sorry about that.
 
The site I was given seems to be rather good this time so I think the misunderstanding is all on me this round.:smile: I'm just not very good with formulas and understanding what's going on. For some reason, when I look at the formulas I have written down, my mind goes blank. I haven't the slightest idea of what I'm looking at.:redface:
 
  • #10
And oh, what am I to do for the Bronsted-Lowry theory? Does it really matter which chemical reaction I list for what because I believe I have to put one for the acid side of the chart as well as the base?:smile:
 
  • #11
Which of the three theories is applicable to the greatest number of acids and bases? Explain your reasoning.

Lewis? I'm scanning over the Chemistry section of Southwestern's Volume Library and that's the only one it mentions.

"A more general definition for acids and bases is called Lewis acids and bases."

Does it simply fill in the holes the other two couldn't?
 
  • #12
yep, it's the lewis definition and yes to the second.
 
  • #13
How am I supposed to know what's what?:bugeye:

Write chemical formulas representing each of the six types of compounds listed below.

I may have overlooked this but I haven't the slightest idea of how I'm to just start naming examples that haven't already been used.:redface:
 
  • #14
AngelShare said:
How am I supposed to know what's what?:bugeye:

Write chemical formulas representing each of the six types of compounds listed below.
What compounds are you referring to?
 
  • #15
Arrhenius acid
Arrhenius base
Brønsted-Lowry acid
Brønsted-Lowry base
Lewis acid
Lewis base
 
  • #16
Which of the three theories is applicable to the greatest number of acids and bases? Explain your reasoning.

Lewis's theory is applicable to the greatest number of acids and bases because Arrhenius and Bronsted-Lowry's theories limit acid/base reactions to a transfer of hydrogen ions while Lewis's includes electrons.

Right, wrong? :smile:
 
  • #17
"Arrhenius acids are limited by having to be in aqeous solution. Lewis acids can be a "real stretch" sometimes and are not nearly as typical as Bronsted-Lowry acids."

That's the response I got... I'm to resubmit my work and fix number two up but I can't simply reword that so I've been searching around for info. I can't seem to find exactly what I'm looking for though.
 

Similar threads

Chemistry How does Bronsted-Lowry definition of base apply to NaOH exactly?
  • · Replies 5 ·
Replies
5
Views
3K
Is this a Brønsted–Lowry acid–base reaction?
  • · Replies 2 ·
Replies
2
Views
2K
Need help with (Acids and Bases) high school exam
  • · Replies 2 ·
Replies
2
Views
2K
MHB HSO4^-1 as Arrhenius & Bronsted-Lowry Acid/Base
  • · Replies 1 ·
Replies
1
Views
3K
Is BH3 a Lewis Base in Reaction with NH3?
  • · Replies 5 ·
Replies
5
Views
3K
How Do Acids and Bases Interact in Reactions?
  • · Replies 1 ·
Replies
1
Views
5K
How does a buffer actually work?
  • · Replies 1 ·
Replies
1
Views
2K
CH3NH2 in the Bronsted-Lowry Theory
  • · Replies 7 ·
Replies
7
Views
35K
Carbon Dioxide and Water: Lewis Base or Bronsted-Lowry Base?
  • · Replies 5 ·
Replies
5
Views
7K
Acid-Base Reactions: Did the Solutions Neutralize Each Other? | Homework Help
  • · Replies 2 ·
Replies
2
Views
3K