The noble gas that would most likely form a compound with fluorine is xenon (Xe).

Here's why:

* Electronegativity: Fluorine is the most electronegative element, meaning it has a strong pull on electrons. Xenon, while still a noble gas, has a relatively low ionization energy compared to other noble gases, making it easier to remove an electron. This combination of factors creates a potential for a bond to form.

* Size: Xenon is the largest of the noble gases, meaning its outermost electrons are further from the nucleus and experience less attraction. This makes them more susceptible to interaction with other elements.

While other noble gases like krypton can form compounds with fluorine under extreme conditions, xenon is the most likely and the most readily observed to form compounds with fluorine.

Example: Xenon hexafluoride (XeF₆) is a well-known and relatively stable compound formed between xenon and fluorine.