Predict the order of increasing ionic radius for each of the following sets of elements.Use the element symbols and make sure you use correct capitalization.  If there is a charge place the sign then the number without using spaces.  Example:  Ca+2 or F-1 D)    O-2, Se-2, S-2Smallest to Largest

To predict the order of increasing ionic radius for the given set of elements (O-2, Se-2, S-2), we need to consider the following:

1. Ionic radius generally increases as we move down a group in the periodic table. This is because the number of electron shells increases, resulting in larger atomic size.

2. Within a group, as we move from left to right, the ionic radius generally decreases. This is due to the increasing nuclear charge, which attracts the electrons more strongly and reduces the atomic size.

Based on these trends, we can predict the order of increasing ionic radius for the given set of elements:

Smallest to Largest: O-2, S-2, Se-2

This means that the oxygen ion (O-2) will have the smallest ionic radius, followed by the sulfur ion (S-2), and finally, the selenium ion (Se-2) will have the largest ionic radius.