Why is lead sulfide found in nature, whereas lead oxide is less common? This question probably applies to other heavier metals as well.  The only rationalization I can figure out is that lead in the +2 oxidation state (which is most common) is a borderline soft acid and prefers to take electrons from a soft sulfur instead of trying to react with a hard oxygen.
Is this the right direction?  Thank you in advance.
Lead(IV) and sulfide ions are large and polarizable, making them soft in the context of hard/soft acid/base theory (HSAB), which states that ions with similar hardness will form stronger bonds.  The oxide ion is hard and therefore has a tendency to form weaker interactions with Pb(IV).

HSAB theory has been discussed on Chem.SE in this question and this answer.