Chemistry Principles Lecture Notes

Introduction

• Speaker: Mahmoud Abdel Latif
• Topic: Chemistry principles, chapter 2, GC1
• Focus on naming anions.

Types of Anions

1. Monoatomic Anions

   • Definition: Anions derived from a single atom, resulting from gaining electrons.
   • Naming Rule: Add the suffix -ide to the root of the element's name.
     • Examples:
       • Hydrogen ➜ Hydride
       • Nitrogen ➜ Nitride
       • Oxygen ➜ Oxide
       • Sulfur ➜ Sulfide
       • Fluorine ➜ Fluoride
       • Chlorine ➜ Chloride

2. Polyatomic Anions

   • Definition: Anions that contain more than one atom.
   • Subcategories:
     • Central atom with oxygen (Oxanes)
     • Central atom with oxygen and hydrogen (Acids)
   • Examples of Polyatomic Anions:
     • Cyanide, Hydroxide, Peroxide, Azide, Carbide

Naming Polyatomic Anions

Central Atom with Oxygen (Oxanes)

• Formula: XOM⁻N (X = central atom, M = number of oxygen, N = charge)
• Naming Rules:
  • Change the ending of the name of the central atom:
    • -ate for a higher number of oxygen atoms
    • -ite for a lower number of oxygen atoms
  • Prefixes: per- for four oxygen atoms, hypo- for one oxygen atom
  • Examples:
    • Carbonate (CO₃²⁻), Nitrate (NO₃⁻), Sulfate (SO₄²⁻), Phosphate (PO₄³⁻)

Central Atom with Oxygen and Hydrogen (Acids)

• Naming Rule: Add Hydrogen in front of the polyatomic anion name.
  • Examples:
    • Carbonate ➜ Hydrogen Carbonate (Bicarbonate)
    • Phosphate ➜ Hydrogen Phosphate
    • Sulfate ➜ Hydrogen Sulfate (Bisulfate)

Naming Ionic Compounds

• Cations are named first followed by anions.
• Naming Monoatomic Cations: Take name from the element.
• Naming Monoatomic Anions: Add -ide.
• Examples:
  • Sodium Chloride (NaCl)
  • Iron(III) Chloride (FeCl₃)

Naming Acids

1. If an anion does not contain oxygen:
   • Add hydro-, root of the anion, and -ic + acid (e.g., Hydrochloric Acid).
2. If an anion contains oxygen:
   • If ending in -ate, replace with -ic + acid.
   • If ending in -ite, replace with -ous + acid.

Examples of Acids

• Hydrochloric Acid (HCl)
• Nitric Acid (HNO₃)
• Sulfuric Acid (H₂SO₄)

Binary Compounds

• Formed between two elements (ionic or covalent).
• Naming Rules:
  • First element full name; second element base + -ide.
  • Use Greek prefixes to indicate the number of atoms (e.g., mono, di, tri).

Organic Chemistry

• Focuses on carbon compounds.
• Functional Groups:
  • Alcohols (OH): Methanol
  • Amines (NH₂): Methylamine
  • Carboxylic Acids (COOH): Acetic Acid

Common Anions to Memorize

• Cyanide, Azide, Hydroxide, Peroxide, Acetate, Bicarbonate.

Practice Naming Compounds

• Copper(I) Bromide ➜ Copperous Bromide
• Iron(III) Sulfide ➜ Ferric Sulfide

Conclusion

• Final thoughts on naming conventions and practice.
• Encouragement to contact for help with future topics.
• Farewell and well wishes for the next chapter.