Basic Chemistry

Arrhenius, Bronsted-Lowry, and Lewis Acids and Bases in Organic Chemistry 

Before know acid base theories you must know about acid base

Acids and base

Acid and base

An acid is a chemical compound that can donate a hydrogen ion (H+) to another substance. In other words, acids are substances that release positively charged hydrogen ions when they are dissolved in water. Common examples of acids include hydrochloric acid (HCl), sulfuric acid (H2SO4), and acetic acid (CH3COOH).

A base, on the other hand, is a chemical compound that can accept a hydrogen ion (H+) from another substance, or it can donate a negatively charged hydroxide ion (OH-) to another substance. In other words, bases are substances that release negatively charged hydroxide ions when they are dissolved in water. Common examples of bases include sodium hydroxide (NaOH), potassium hydroxide (KOH), and ammonia (NH3).

Acids have a sour taste and can corrode metals. They also turn blue litmus paper red, and have a pH below 7. Strong acids can be very corrosive and dangerous to handle.

Bases, on the other hand, have a bitter taste and are slippery to the touch. They can also dissolve fats and oils. Bases turn red litmus paper blue, and have a pH above 7. Strong bases can be caustic and also pose hazards if not handled carefully.

In chemistry, acid-base reactions play a crucial role in many processes, such as the digestion of food, the functioning of batteries, and the regulation of blood pH in the human body. Acids and bases can also react with each other to form a buffer solution, which helps to maintain a stable pH in certain biological systems.

Acids and bases can neutralize each other when they react, producing a salt and water. This reaction is known as neutralization. The strength of an acid or base is measured on a pH scale, which ranges from 0 (very acidic) to 14 (very basic or alkaline). A pH of 7 is considered neutral.

Acids and bases play important roles in many aspects of our daily lives. Here are some examples:

1. Cooking: Acids such as lemon juice, vinegar, and yogurt are often used in cooking to add flavor and tenderize meat. Bases such as baking soda are used to leaven baked goods like bread and cakes.

2. 1. Cleaning: Many cleaning products contain acids or bases. For example, vinegar and lemon juice are often used as natural cleaning agents due to their acidic properties, while bleach and ammonia are strong bases used in cleaning products.

   2. Personal care: Acids such as salicylic acid are used in skin care products to exfoliate and treat acne. Bases like sodium hydroxide are used in hair relaxers to break down the protein structure of hair and make it more manageable.

Acid and Base Theories

Arrhenius, Bronsted-Lowry, and Lewis Acids and Bases in Organic Chemistry explain very easily
In organic chemistry, there are three common theories used to explain acids and bases: Arrhenius theory, Bronsted-Lowry theory, and Lewis theory.
According to this theory, an acid is a substance that produces hydrogen ions (H+) when dissolved in water, while a base is a substance that produces hydroxide ions (OH-) when dissolved in water. For example, HCl is an acid because it produces H+ ions in water, while NaOH is a base because it produces OH- ions in water. However, this theory is limited to aqueous solutions and does not apply to non-aqueous solvents or gas-phase reactions.
This theory defines an acid as a substance that donates a proton (H+) to another substance, while a base is a substance that accepts a proton (H+). For example, in the reaction HCl + H2O -> H3O+ + Cl-, HCl is the acid because it donates a proton to water (which acts as the base) to form hydronium ion (H3O+). Similarly, NH3 is a base because it accepts a proton from water to form NH4+ ion. This theory is more general than Arrhenius theory, as it applies to both aqueous and non-aqueous solutions.
According to Lewis theory, an acid is a substance that accepts an electron pair, while a base is a substance that donates an electron pair. This theory is more general than both Arrhenius and Bronsted-Lowry theories because it applies to both aqueous and non-aqueous solutions, as well as gas-phase reactions. For example, in the reaction between BF3 and NH3, BF3 acts as an acid because it accepts a lone pair of electrons from NH3 (which acts as a base) to form a covalent bond between the two species.

1. Arrhenius Theory:

2. Bronsted-Lowry Theory:

3. Lewis Theory:

In summary, Arrhenius theory describes acids and bases based on their behavior in aqueous solutions, while Bronsted-Lowry theory describes them based on their ability to donate or accept protons. Lewis theory defines them based on their ability to donate or accept electron pairs, and is the most general theory of the three.

Can you give example all theories by and diagram how shift electrons

1. Arrhenius Theory: Example: HCl + H2O → H3O+ + Cl- In this reaction, HCl donates a proton to water (acting as a base), forming hydronium ion (H3O+). The Cl- ion is left behind as the conjugate base of HCl.

Diagram: HCl + H2O ⇌ H3O+ + Cl- ↓ ↓ Donates H+ Accepts H+

2. Bronsted-Lowry Theory: Example: NH3 + H2O → NH4+ + OH- In this reaction, NH3 acts as a base and accepts a proton from water (acting as an acid), forming NH4+ ion. The OH- ion is left behind as the conjugate base of water.

Diagram: NH3 + H2O ⇌ NH4+ + OH- ↓ ↓ Accepts H+ Donates H+

3. Lewis Theory: Example: BF3 + NH3 → BF3NH3 In this reaction, BF3 acts as an acid and accepts a lone pair of electrons from NH3 (acting as a base), forming a coordinate covalent bond between the two species.

Diagram: BF3 + NH3 → BF3NH3 ↓ ↓ Accepts e- Donates e-

As an organic chemistry student you will find yourself faced with acid/based questions again and again.

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1. Arrhenius Theory: Example: HCl + H2O → H3O+ + Cl- In this reaction, HCl donates a proton to water (acting as a base), forming hydronium ion (H3O+). The Cl- ion is left behind as the conjugate base of HCl.

Diagram: HCl + H2O ⇌ H3O+ + Cl- ↓ ↓ Donates H+ Accepts H+

2. Bronsted-Lowry Theory: Example: NH3 + H2O → NH4+ + OH- In this reaction, NH3 acts as a base and accepts a proton from water (acting as an acid), forming NH4+ ion. The OH- ion is left behind as the conjugate base of water.

Diagram: NH3 + H2O ⇌ NH4+ + OH- ↓ ↓ Accepts H+ Donates H+

3. Lewis Theory: Example: BF3 + NH3 → BF3NH3 In this reaction, BF3 acts as an acid and accepts a lone pair of electrons from NH3 (acting as a base), forming a coordinate covalent bond between the two species.

Diagram: BF3 + NH3 → BF3NH3 ↓ ↓ Accepts e- Donates electron

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