* Electronegativity Difference: Chlorine is significantly more electronegative than carbon. This means chlorine attracts the shared electrons in the C-Cl bond more strongly, creating a partial negative charge (δ-) on the chlorine atom and a partial positive charge (δ+) on the carbon atom.

* Molecular Geometry: The carbon atom in tert-butyl chloride is attached to four groups: three methyl groups and the chlorine atom. This results in a tetrahedral geometry around the carbon, leading to an uneven distribution of electron density.

Overall, the polar C-Cl bond and the asymmetrical molecular geometry contribute to the polar nature of tert-butyl chloride.