Chemical Bonding Cheat Sheet

Key Definitions

• Chemical Bond: The force holding atoms together in a molecule.

• Ionic Bond: Electrostatic attraction between oppositely charged ions.

• Covalent Bond: Sharing of electron pairs between atoms.

• Polar Covalent Bond: Unequal sharing of electrons due to electronegativity differences.

• Metallic Bond: Attraction between metal cations and delocalized electrons.

Important Concepts

Types of Bonds

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

• Covalent Bonds: Formed between non-metals; can be single, double, or triple.

• Metallic Bonds: Conduct electricity and heat; malleable and ductile.

Bond Polarity

• Non-polar Covalent: Equal sharing of electrons (e.g., Cl₂).

• Polar Covalent: Unequal sharing (e.g., H₂O).

• Ionic: Complete transfer of electrons (e.g., NaCl).

Key Formulas

• Electronegativity Difference: ΔEN = EN(A) - EN(B)

• Bond Order: Bond Order = (Number of bonding electrons - Number of antibonding electrons) / 2

• Lattice Energy: U = k(Q1 * Q2) / r

Common Mistakes to Avoid

Common Mistake: Confusing ionic and covalent bonds; remember ionic involves transfer, covalent involves sharing.

Memory Tricks

Tip: "Ionic = Transfer, Covalent = Share" — helps to remember bond types.

Key Diagrams

Ionic Bond: Na⁺ Cl⁻
  Na  →  Cl
Covalent Bond: H - H
  H   H
Polar Covalent: H - O
  H   O
      |
      H