* Molecular Geometry: The central carbon atom in 1,2-dibromopropane is bonded to two bromine atoms, one hydrogen atom, and a CH2 group. This results in a tetrahedral geometry around the central carbon.

* Electronegativity Difference: Bromine (Br) is more electronegative than carbon (C) and hydrogen (H). This means that the bromine atoms pull electron density towards themselves, creating partial negative charges (δ-) on the bromine atoms and partial positive charges (δ+) on the carbon and hydrogen atoms.

* Dipole Moment: The unequal sharing of electrons creates a dipole moment within each C-Br bond. Since the molecule is not symmetrical, these dipole moments do not cancel each other out. Instead, they combine to create a net dipole moment for the entire molecule.

Therefore, the presence of a net dipole moment makes 1,2-dibromopropane a polar molecule.