Chemical Bonding and Molecular Structure Cheat Sheet

Key Definitions

• Chemical Bond: A force that holds atoms together in a molecule. ✅

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

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

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

• Hybridization: Mixing of atomic orbitals to form new hybrid orbitals. ✅

Important Concepts

Types of Bonds

• Ionic Bonds: Formed between metals and non-metals (e.g., NaCl).

• Covalent Bonds: Formed between non-metals (e.g., H₂O).

• Metallic Bonds: Delocalized electrons in metals (e.g., Cu).

Molecular Geometry

• VSEPR Theory: Predicts molecular shapes based on electron pair repulsion. ✅

• Hybridization Types:

• sp: Linear (180°)

• sp²: Trigonal planar (120°)

• sp³: Tetrahedral (109.5°)

Key Formulas

• ΔEN: Difference in electronegativity

• EN(A): Electronegativity of atom A

• EN(B): Electronegativity of atom B

Common Mistakes to Avoid

Common Mistake: Confusing ionic and covalent bonds based on the type of elements involved. Remember: metals + non-metals = ionic; non-metals + non-metals = covalent.

Memory Tricks

Tip: "H2O" — Hydrogen bonds with Oxygen (remember water's structure).

Key Diagrams

     O
    / \
   H   H

   Na+ Cl-
    |  |
  NaCl (Ionic Bond)

   H   H
    \ /
     C
    / \
   H   H