Exploring Three Acid-Base Theories: Arrhenius, Brønsted-Lowry, and Lewis

[hotgurl1]

I need a little help. In my on-line class they want me to find Acid-Base Theories for Arrhenius, Brønsted-Lowry, and Lewis and to list chemical reactions that demonstrate the action of each acid or base.

I only found one chemical reactions that demonstrate the action of each acid or base which was

Arrhenius: acids produce H+ ions in aqueous solutions and bases produce OH- ions in aqueous solutions

Acid: HCl--> H(+) + Cl (-)
Base: NaOH--> Na(+) + OH (-)

Brønsted-Lowry : acids are proton donors
bases are proton acceptors

Lewis
acids are electron pair acceptors
bases are electron pair donors

Can some1 tell me examples of chemical reaction for Brønsted-Lowry and Lewis.
Please and Thank You

Also caN YOU HELP ME WITH:

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

Which theory is most important for the majority of chemistry students?

 

[Nino MMP]

Explain your reasoning. Brønsted-Lowry is applicable to the greatest number of acids and bases because it is a more general definition of an acid and base than either Arrhenius or Lewis. It defines acids as proton donors and bases as proton acceptors, which includes any molecule or species that can donate or accept a proton. This means that Brønsted-Lowry encompasses not only traditional acids and bases, but also other molecules and species such as water, ammonia, and hydrocarbons. The theory most important for the majority of chemistry students is Arrhenius. This is because it is the simplest and most basic definition of an acid and base, and is the foundation for all other theories. It defines acids as substances that produce H+ ions in aqueous solutions, and bases as substances that produce OH- ions in aqueous solutions. This definition is easy to understand and is a good starting point for learning about acids and bases.

 

[Blueshift5]

Sure, I can help you with that.

For Brønsted-Lowry, an example of a chemical reaction would be the dissociation of acetic acid (CH3COOH) in water: CH3COOH + H2O ⇌ CH3COO- + H3O+. In this reaction, the acid (CH3COOH) donates a proton to water, forming the acetate ion (CH3COO-) and the hydronium ion (H3O+).

For Lewis, an example of a chemical reaction would be the formation of a coordination compound, such as the reaction between zinc chloride (ZnCl2) and ammonia (NH3): ZnCl2 + 2NH3 → Zn(NH3)2Cl2. In this reaction, the zinc ion (Zn2+) acts as a Lewis acid, accepting a pair of electrons from the ammonia molecule (NH3), which acts as a Lewis base.

To answer your other questions, Brønsted-Lowry theory is applicable to a larger number of acids and bases compared to Arrhenius and Lewis theories. This is because it defines acids and bases based on their ability to donate or accept protons, which applies to a wider range of compounds.

As for which theory is most important for chemistry students, it really depends on the specific field of study and the types of reactions and compounds they will be working with. However, Brønsted-Lowry theory is often considered the most fundamental and widely applicable theory, so it is important for students to have a good understanding of it.