Shapes Revision Cards

Page 1: Electron Pair Repulsion Theory

Card 1 – Electron Pair Repulsion Theory

• Front: Electron Pair Repulsion Theory

• Back:

  • Electron pairs repel to maximize distance between themselves.

  • Key Concepts:

    • Bond pairs repel equally.

    • Lone pairs exert greater repulsion than bonded pairs, affecting molecular shape.

Card 2 – Determining the Number of Electron Pairs

• Front: Determining the Number of e- pairs

• Back:

  • Write the equations covered in the lesson:

    • To calculate the total number of electron pairs

    • To determine the number of lone pairs

Page 2: Molecular Shapes and Bond Angles

Shapes Based on Electron Pairs

• For each number of electron pairs, identify bond pairs (bp) and lone pairs (lp):

4 Electron Pairs

• Front: 4 Electron Pairs

• Back:

  • 4 bond pairs, 0 lone pairs

  • Shape: Tetrahedral

  • Bond Angle: 109.5°

3 Electron Pairs

• 3 bond pairs, 1 lone pair

  • Shape: Pyramidal

  • Bond Angle: 107° (109.5° - (1 × 2.5°))

2 Electron Pairs

• 2 bond pairs, 2 lone pairs

• Shape: V-shaped

• Bond Angle: 104.5° (109.5° - (2 × 2.5°))

Additional Combinations for Electron Pairs

• 2 Electron Pairs:

  • 2 bond pairs, 0 lone pairs

• 3 Electron Pairs:

  • 3 bond pairs, 0 lone pairs

  • 2 bond pairs, 1 lone pair

• 5 Electron Pairs:

  • 5 bond pairs, 0 lone pairs

  • 4 bond pairs, 1 lone pair

    • Leave space for applications questions

  • 3 bond pairs, 2 lone pairs

  • 2 bond pairs, 3 lone pairs

    • Leave space for applications questions

• 6 Electron Pairs:

  • 6 bond pairs, 0 lone pairs

  • 5 bond pairs, 1 lone pair

    • Leave space for applications questions

  • 4 bond pairs, 2 lone pairs