To determine which one has stronger Debye forces, let’s consider the nature of Debye forces and the properties of the given substances.

Debye forces, also known as London dispersion forces or van der Waals forces, are weak intermolecular forces that arise due to temporary fluctuations in electron distribution. These forces occur between all molecules, including noble gases and polar molecules.

Now, let’s analyze the given options:

(a) Ne, HCl:
Ne represents neon, which is a noble gas. Noble gases have complete valence electron shells and are therefore non-polar. HCl, on the other hand, is a polar molecule because it consists of a highly electronegative atom (chlorine) and a less electronegative atom (hydrogen). Polar molecules tend to have stronger intermolecular forces than non-polar molecules due to the presence of permanent dipoles.

In this case, HCl would have stronger Debye forces compared to Ne because of its polar nature. The dipole-dipole interactions in HCl contribute to stronger intermolecular forces.

(b) He, HCl:
He represents helium, another noble gas. As mentioned before, noble gases have complete valence electron shells, making them non-polar. HCl is still a polar molecule due to the electronegativity difference between hydrogen and chlorine.

Similarly to the previous case, HCl would have stronger Debye forces compared to He because of its polar nature. The presence of permanent dipoles in HCl allows for stronger intermolecular attractions.

In both cases, the polar molecule HCl would exhibit stronger Debye forces compared to the noble gases (Ne and He) due to the dipole-dipole interactions resulting from the polarity of HCl.