Delta S=0 for elemental molecules?

[He whose name cannot be spoken]

I don't understand why the Delta S is 0 when forming elemental molecules (like O₂ or N₂, for example).

By grouping them together, shouldn't entropy decrease since there are less possible states for them to be in?

[Chem_Mod]

The entropy of formation is 0 because they are elemental molecules, meaning this is how they are found in nature, therefore there is no entropy change associated with them being formed.

[Daniel Chen 2L]

The Delta S for formation is 0 because they are already in their standard states. That's how they are found in nature. Trying to find the change in entropy for the formation of standard states from their standard states, is like trying to change something into the thing they already are, like trying to take O2 gas and change it to O2 gas. You can't do that because it's already O2 gas. That's why it's 0.