Answer:
Step-by-step explanation:
The atomic radius generally decreases across a period (from left to right) on the periodic table due to increasing effective nuclear charge, while it increases down a group (from top to bottom) due to the addition of more electron shells.
In this case, we are comparing two isotopes of tellurium (Te) with different mass numbers: 124Te and 130Te. Since these isotopes are in the same group (Group 16, also known as the oxygen group), they have the same number of valence electrons and similar electron configurations.
Given that the atomic number (number of protons) of 124Te is lower than that of 130Te, we can infer that 124Te is located higher in the same group on the periodic table. As we move down the group, atomic radius tends to increase due to the addition of electron shells.
Therefore, the **atomic radius of 124Te is larger** than the atomic radius of 130Te.