Chemistry SL
6
Chapters
243
Notes
Chapter 1 - Models Of The Particulate Nature Of Matter
Chapter 2 - Models Of Bonding & Structure
Chapter 3 - Classification Of Matter
Chapter 4 - What Drives Chemical Reactions?
Chapter 5 - How Much, How Fast & How Far?
Chapter 6 - What Are The Mechanisms Of Chemical Change?
Chemistry SL
Chapter 6 - What Are The Mechanisms Of Chemical Change?
Explore Acids & Bases: Reactivity Properties
498 words
3 mins read
Last edited on 5th Nov 2024
Table of content
Properties of Acids 🍋
- Definition
- Brønsted–Lowry Acids have at least one exchangeable (weakly bound) hydrogen atom.
- They dissociate in water to form H+ (Hydronium) ions.
- Example: Hydrogen chloride HCl.
- Examples and Real-World Analogy
- Think of acids like a lemon (citric acid)! They contain hydrogen ions that can detach or "squeeze out," much like lemon juice!
- Exchangeable Hydrogen
- Usually bonds with electronegative atoms like oxygen, halogens, or sulfur.
- Examples: Hydrogen chloride HCl, Sulfuric acid H2SO4, Ethanoic (Acetic) acid CH3COOH.
- Acid Dissociation
- In water, acids dissociate to form Hydrogen ions and anions (acid residue).
- Example: HCl (aq) → H+(aq) + Cl−(aq).
- Classification
- Monoprotic: One exchangeable hydrogen. Example: HCl.
- Diprotic: Two exchangeable hydrogens. Example: H2SO4.
- Triprotic: Three exchangeable hydrogens. Example: H3PO4.
- Strength of Acids
- Strong acids dissociate completely in water (irreversible). Example: Hydrogen chloride.
- Weak acids partially dissociate (reversible). Example: Ethanoic acid in vinegar.
- Attention: Strength is not related to concentration! Do not confuse “strong”/“weak” with “concentrated”/“dilute”.
Properties of Bases 🛁
- Definition:
- Arrhenius base: Produces OH− ions.
- Brønsted–Lowry base: Accepts H+ ions.
- Example: Think of bases like soap (usually basic)! They interact with acids (like lemon) to neutralize them!
- Common Bases
- Mostly metal hydroxides, like NaOH and Mg(OH)2, or ammonia, NH3.
- Strength and Solubility
- Strong Bases: Fully dissociate in water. Example: Sodium hydroxide, NaOH.
- Weak Bases: Partially dissociate in water. Example: Ammonia, NH3.
- Note: Some strong bases like Ca(OH)2 have low solubility but still fully dissociate in solution.
- Covalent Hydroxides
- Formed by less active metals and are weak bases. Example: Iron(III) hydroxide, Fe(OH)3.
- Ammonia and Amines
- Ammonia is a unique inorganic base, without metal, acting as a weak Brønsted–Lowry base.
- Amines, organic derivatives of ammonia, exhibit similar acid–base properties. Example: Methylamine,CH3NH2.
- Reaction with Acids
- Bases react with acids to form salts and water, a process called neutralization.
- Example: Sodium hydroxide reacting with hydrochloric acid forms sodium chloride (table salt) and water!
Unlock the Full Content! 
Dive deeper and gain exclusive access to premium files of Chemistry SL. Subscribe now and get closer to that 45 🌟
Chemistry SL
Chapter 6 - What Are The Mechanisms Of Chemical Change?
Explore Acids & Bases: Reactivity Properties
498 words
3 mins read
Last edited on 5th Nov 2024
Table of content
Properties of Acids 🍋
- Definition
- Brønsted–Lowry Acids have at least one exchangeable (weakly bound) hydrogen atom.
- They dissociate in water to form H+ (Hydronium) ions.
- Example: Hydrogen chloride HCl.
- Examples and Real-World Analogy
- Think of acids like a lemon (citric acid)! They contain hydrogen ions that can detach or "squeeze out," much like lemon juice!
- Exchangeable Hydrogen
- Usually bonds with electronegative atoms like oxygen, halogens, or sulfur.
- Examples: Hydrogen chloride HCl, Sulfuric acid H2SO4, Ethanoic (Acetic) acid CH3COOH.
- Acid Dissociation
- In water, acids dissociate to form Hydrogen ions and anions (acid residue).
- Example: HCl (aq) → H+(aq) + Cl−(aq).
- Classification
- Monoprotic: One exchangeable hydrogen. Example: HCl.
- Diprotic: Two exchangeable hydrogens. Example: H2SO4.
- Triprotic: Three exchangeable hydrogens. Example: H3PO4.
- Strength of Acids
- Strong acids dissociate completely in water (irreversible). Example: Hydrogen chloride.
- Weak acids partially dissociate (reversible). Example: Ethanoic acid in vinegar.
- Attention: Strength is not related to concentration! Do not confuse “strong”/“weak” with “concentrated”/“dilute”.
Properties of Bases 🛁
- Definition:
- Arrhenius base: Produces OH− ions.
- Brønsted–Lowry base: Accepts H+ ions.
- Example: Think of bases like soap (usually basic)! They interact with acids (like lemon) to neutralize them!
- Common Bases
- Mostly metal hydroxides, like NaOH and Mg(OH)2, or ammonia, NH3.
- Strength and Solubility
- Strong Bases: Fully dissociate in water. Example: Sodium hydroxide, NaOH.
- Weak Bases: Partially dissociate in water. Example: Ammonia, NH3.
- Note: Some strong bases like Ca(OH)2 have low solubility but still fully dissociate in solution.
- Covalent Hydroxides
- Formed by less active metals and are weak bases. Example: Iron(III) hydroxide, Fe(OH)3.
- Ammonia and Amines
- Ammonia is a unique inorganic base, without metal, acting as a weak Brønsted–Lowry base.
- Amines, organic derivatives of ammonia, exhibit similar acid–base properties. Example: Methylamine,CH3NH2.
- Reaction with Acids
- Bases react with acids to form salts and water, a process called neutralization.
- Example: Sodium hydroxide reacting with hydrochloric acid forms sodium chloride (table salt) and water!
Unlock the Full Content!
Dive deeper and gain exclusive access to premium files of Chemistry SL. Subscribe now and get closer to that 45 🌟
AI Assist
Expand
Hello there,
how can I help you today?
how can I help you today?