Introduction:
In order to determine which molecule is more polar between NO2 and N2O, we need to consider their molecular geometries and the polarity of the individual bonds within the molecules. Polar molecules arise when there is an uneven distribution of electron density, resulting in a partial positive and partial negative charge.

Molecular Geometry:
The molecular geometry of a molecule is determined by the arrangement of its atoms in space. This arrangement affects the overall polarity of the molecule.

- NO2: Nitrogen dioxide has a bent molecular geometry due to the presence of a lone pair of electrons on the central nitrogen atom. The oxygen atoms are bonded to the nitrogen atom, creating a bent shape.
- N2O: Nitrous oxide has a linear molecular geometry since it consists of two nitrogen atoms bonded to a central oxygen atom. The nitrogen-oxygen bonds are arranged in a straight line.

Bond Polarity:
The polarity of a bond is determined by the difference in electronegativity between the atoms involved. Electronegativity is the ability of an atom to attract electrons towards itself in a covalent bond.

- NO2: Nitrogen has an electronegativity of 3.04, while oxygen has an electronegativity of 3.44. The nitrogen-oxygen bonds in NO2 are polar due to the difference in electronegativity between these atoms.
- N2O: Both nitrogen and oxygen have similar electronegativities, with nitrogen having an electronegativity of 3.04 and oxygen having an electronegativity of 3.44. Therefore, the nitrogen-oxygen bonds in N2O are also polar.

Overall Polarity:
To determine the overall polarity of a molecule, we need to consider both the bond polarities and the molecular geometry.

- NO2: The bent molecular geometry and polar nitrogen-oxygen bonds in NO2 result in an overall polar molecule. The oxygen atoms, which are more electronegative than nitrogen, pull the electron density towards themselves, creating a partial negative charge on the oxygen atoms and a partial positive charge on the nitrogen atom.
- N2O: Despite having polar nitrogen-oxygen bonds, the linear molecular geometry of N2O results in an overall nonpolar molecule. The polar bonds in N2O are arranged symmetrically, canceling out any dipole moments and resulting in a molecule with no net dipole.

Conclusion:
In conclusion, NO2 is more polar than N2O. The bent molecular geometry and the presence of polar nitrogen-oxygen bonds in NO2 contribute to its overall polarity, while the linear molecular geometry of N2O leads to a cancellation of dipole moments, making it a nonpolar molecule.