Final answer:
Atomic radius is a measure of an atom's size and varies predictably across the periodic table, decreasing across periods and increasing down groups. Elements are arranged in increasing atomic radius by considering their position in the periodic table and the general trend that atomic size increases with added electron shells and decreases with stronger nuclear charge.
Step-by-step explanation:
The question addresses the concept of atomic radius, which is a measure of the size of an atom. Atomic radius trends can be observed in both periods (rows) and groups (columns) on the periodic table. Generally, atomic radius decreases across a period from left to right due to the increasing positive charge of the nucleus which pulls electrons closer. Conversely, atomic radius increases down a group as additional electron shells are added, making the atom larger.
Listed below are examples of how you would arrange elements in order of increasing atomic radii based on their position on the periodic table:
- For the elements Mg, Cl, S, Na, the order of increasing atomic radii is Cl < S < Mg < Na.
- In the case of In, Ca, Mg, Sb, Xe, the correct order is Mg < Ca < In < Sb < Xe.
- When arranging Sr, Ca, Si, Cl, the order is Cl < Si < Ca < Sr.
- Predicting which element has the largest atomic radius among Li, Rb, N, F, I, the largest is Rb, and the smallest is F.
- The effect on the atomic radius of an atom gaining an electron would typically be an increase due to increased electron-electron repulsion. For example, when an oxygen atom gains an extra electron to become an oxide ion (O-), its radius increases compared to the neutral atom.
- If an atom were to lose an electron, the remaining electrons would experience a reduced repulsion and be held closer to the nucleus, hence the atomic radius would decrease. For instance, when sodium (Na) loses an electron to form a sodium ion (Na+), its atomic radius is smaller than that of the neutral atom.