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docs/lectures/organic-chemistry/lesson-2_19-09-2024.md

@@ -629,19 +629,16 @@ The **geometry of a molecule** is determined by the number of "groups" around a
 The arrangement of these groups around the central atom aims to **minimize repulsion** between them, which leads to a stable geometry. This concept is the foundation of **Valence Shell Electron Pair Repulsion (VSEPR) theory**.
 
 1. **Valence Shell Electron Pair Repulsion (VSEPR) Theory**:
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    - The theory states that the electron pairs (bonding pairs and lone pairs) surrounding an atom will position themselves as far apart as possible to minimize repulsion.
    - This helps determine the shape (geometry) of the molecule.
 
 2. **Types of Geometries**:
 
    - **Linear** (180° bond angle):
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      - Occurs when there are **two groups** around the central atom.
      - Example: Carbon dioxide (\( \ce{CO2} \)) has two oxygen atoms bonded to the carbon atom, resulting in a linear shape.
 
    - **Trigonal Planar** (120° bond angle):
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      - Happens when there are **three groups** around the central atom.
      - Example: Boron trifluoride ( \( \ce{BF3} \) ), where three fluorine atoms are bonded to boron in a flat triangle.
 
@@ -653,7 +650,6 @@ The arrangement of these groups around the central atom aims to **minimize repul
    - Lone pairs take up more space than bonding pairs because they are closer to the nucleus. As a result, the presence of lone pairs slightly reduces bond angles.
    - For example, water (\( \ce{H2O} \)) has a tetrahedral electron geometry, but because of two lone pairs on the oxygen atom, the bond angle is reduced from 109.5° to around 104.5°, giving the molecule a bent shape.
 
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 > 🔗 Resources
 > [Hannah Nandor: VESPR Theory](https://www.youtube.com/watch?v=5uwcTOSyMDI)