How does steric hindrance cause sulfur hexafluoride to have almost no reaction chemistry?

Question

Sulfur hexafluoride ($\ce{SF6}$) is, according to the Wikipedia page, a hypervalent substance. However, according to the page in regards to $\ce{SF6}$ reactions:

There is virtually no reaction chemistry for $\ce{SF6}$. The main contribution to the inertness of $\ce{SF6}$ is the steric hindrance of the sulfur atom, whereas its heavier group 16 counterparts, such as $\ce{SeF6}$ are more reactive than $\ce{SF6}$ as a result of less steric hindrance

The linked steric hindrance provides many examples of how that chemical process works, but specifically, what steric hindrance (or any other) mechanism results in $\ce{SF6}$ possessing virtually no reaction chemistry?

Answer 1

As you can see:

Sulfur (16) is significantly smaller than Se (34). That size difference means that there is more room between the fluorine atoms on Se than on Sulfur. That is what steric hindrance means. Think of steric hindrance as limited access. The smaller the atom the less access there is. Oxygen is so small that less than 6 fluorine atoms can crowd around it because of steric hindrance... probably more like four.

So because there is more room between the fluorine atoms on Se there is more opportunity for other atoms to attack the central atom Se, but sulfur is completely shielded by inert fluorine.