The CF2Cl2 molecule, commonly known as dichlorodifluoromethane, has a central carbon atom bonded to two fluorine atoms and two chlorine atoms. To determine the electronic and molecular geometries, we first need to analyze the arrangement of electron pairs around the central carbon atom.
The carbon atom has four valence electrons and forms four single bonds: two with fluorine and two with chlorine. This results in a total of four bonding pairs of electrons. Since there are no lone pairs on the carbon atom, the electronic geometry is based solely on these bonding pairs.
According to the VSEPR (Valence Shell Electron Pair Repulsion) theory, four bonding pairs of electrons will arrange themselves to minimize repulsion and adopt a tetrahedral geometry. Therefore, the electronic geometry of CF2Cl2 is tetrahedral.
Next, we can look at the molecular geometry. With all four bonds being identical in terms of their bond type (single bonds) and considering that the surrounding atoms (fluorine and chlorine) are different, the molecule retains a tetrahedral arrangement of the atoms themselves. This means that the molecular geometry also remains tetrahedral, as there are no lone pairs affecting the shape. However, the difference in electronegativity between fluorine and chlorine does create a polar molecule, but it does not change the basic shape.
In summary, for the CF2Cl2 molecule:
Electronic Geometry: Tetrahedral
Molecular Geometry: Tetrahedral