I understand that H2S has no hybridization so the bond angle is closer to 90 than 109.5 degrees and that's the reason why H2S bond angle is less than H2O.

However, assuming hybridization occurs why would H2S have a smaller bond angle? In H2S the sp3 hybrid orbitals are bigger than H2O and so the bond pair-bond pair repulsion decreases so with just this statement, the bond pairs should be able to come closer to each other. However, the lone pair-bond pair repulsions are also smaller now so with just this statement shouldn't the bond pairs also be able to move further away from each other?

So eventually how do we know which factor outweighs the other factor? We know that H2S has a smaller bond angle so that would mean the decrease in repulsion between the two bond pairs are more significant than the decrease of repulsion between the lone pair and bond pair - but why is this so and not the other way around?

Thanks in advance for the help