Question

ex: aluminum oxide = al₂o₃, you would type: al2o3 rubidium fluoride

Explanation:

Step1: Determine the ions

Rubidium (Rb) forms \(Rb^+\) ion (since it is in Group 1 of the periodic table and loses one electron). Fluorine (F) forms \(F^-\) ion (since it is in Group 17 and gains one electron).

Step2: Apply the criss - cross rule

For a compound formed by \(Rb^+\) and \(F^-\), using the criss - cross rule (the magnitude of the charge of one ion becomes the subscript of the other ion). Here, the charge of \(Rb^+\) is \(+ 1\) and the charge of \(F^-\) is \(-1\). So, the subscript of \(Rb\) is \(1\) and the subscript of \(F\) is \(1\).

Answer:

RbF