Chemical Bonding Cheat Sheet

Key Definitions

• Ionic Bond: Electrostatic attraction between oppositely charged ions. ✅

• Covalent Bond: Sharing of electron pairs between atoms. ✅

• Metallic Bond: Attraction between metal ions and delocalized electrons. ✅

• Electronegativity: Ability of an atom to attract electrons in a bond. ✅

Important Concepts

Types of Bonds

• Ionic Bonds: Formed between metals and non-metals; high melting points; conductive in solution.

• Covalent Bonds: Formed between non-metals; can be polar or non-polar; low melting points.

• Metallic Bonds: Characterized by a sea of delocalized electrons; malleable and ductile.

Bond Polarity

• Polar Covalent: Unequal sharing of electrons; difference in electronegativity > 0.4. ✅

• Non-Polar Covalent: Equal sharing of electrons; difference in electronegativity < 0.4. ✅

Key Formulas

• Bond Order:

Key Electronegativity Values

• Fluorine (F): 4.0 ✅

• Oxygen (O): 3.5 ✅

• Chlorine (Cl): 3.0 ✅

Common Mistakes to Avoid

Common Mistake: Confusing ionic and covalent bonds based solely on the types of elements involved.

Common Mistake: Ignoring resonance structures in molecules with delocalized electrons.

Memory Tricks

Tip: "Ionic = Metal + Non-metal" — Remember that ionic bonds involve the transfer of electrons from metals to non-metals.

Mnemonic: "Covalent = Co-Operate" — Atoms share electrons to achieve stability.

Key Diagrams

  Ionic Bonding:
   Na+  Cl- 
     |   |
   [Na] [Cl]
  
  Covalent Bonding:
   H   H
    \ /
     H-H