Here's why:
* Hybridization: The carbon atom in CF2H2 undergoes sp3 hybridization. This means it forms four hybrid orbitals that are arranged in a tetrahedral shape.
* Repulsion: The four electron pairs around the carbon atom (two C-F bonds, two C-H bonds) repel each other to maximize distance and minimize energy.
* Ideal Angle: In an ideal tetrahedral geometry, the bond angle is 109.5 degrees.
However, the actual bond angle in CF2H2 might be slightly less than 109.5 degrees. This is because the fluorine atoms are more electronegative than hydrogen atoms. This leads to a slight increase in electron density around the fluorine atoms, causing a greater repulsion between the C-F bonds and a slightly smaller bond angle.
In summary: The bond angles in CF2H2 are close to 109.5 degrees, but slightly less due to the electronegativity of fluorine.
