Predict the order of increasing atomic radius for each of the following sets of elements.Use the element symbols and make sure you use correct capitalization. C)    Al, Tl, SiSmallest to Largest

To predict the order of increasing atomic radius for the elements Al, Tl, and Si, we need to consider their positions in the periodic table.

First, let's locate these elements in the periodic table:

• Al stands for aluminum and is located in Group 13.
• Tl stands for thallium and is located in Group 13 as well.
• Si stands for silicon and is located in Group 14.

In general, as we move down a group in the periodic table, the atomic radius tends to increase. This is because each subsequent element has an additional energy level, which leads to an increase in the size of the electron cloud surrounding the nucleus.

Comparing Al and Tl, both elements are in the same group, so we can expect their atomic radii to be similar. However, since Tl is located below Al, it will have a slightly larger atomic radius.

Now, let's compare Si with Al and Tl. Si is in a different group, but it is located to the left of Al and Tl. In general, as we move from left to right across a period in the periodic table, the atomic radius tends to decrease. Therefore, Si will have a smaller atomic radius compared to Al and Tl.

Based on this information, the order of increasing atomic radius for the elements Al, Tl, and Si is as follows:

Si < Al < Tl