Among the elements Ca, Mg, P and Cl
, the order of increasing atomic radii is:

A. Mg < Ca < Cl < P

B. Cl < P < Mg < Ca

C. P < Cl < Ca < Mg

D. Ca < Mg < P < Cl

To determine the correct order of increasing atomic radii among the elements Ca, Mg, P, and Cl, we need to consider their positions in the periodic table. Atomic radius generally increases as you move down a group and decreases as you move across a period from left to right. Here are the positions of the elements in the periodic table:

Mg (Magnesium): Group 2, Period 3
Ca (Calcium): Group 2, Period 4
P (Phosphorus): Group 15, Period 3
Cl (Chlorine): Group 17, Period 3
Now, let's analyze the trends:

Within a Period (same row): Atomic radius decreases from left to right.

In Period 3, the order is:
𝑀
𝑔
>
𝑃
>
𝐶
𝑙
Mg>P>Cl because Mg is on the far left and Cl is on the far right.
Within a Group (same column): Atomic radius increases from top to bottom.

In Group 2, the order is:
𝑀
𝑔
<
𝐶
𝑎
MgCombining these trends, we can list the elements in order of increasing atomic radii:

Cl (Chlorine): Smallest radius, as it is farthest to the right in Period 3.
P (Phosphorus): Larger than Cl, but still in Period 3.
Mg (Magnesium): Larger than both Cl and P, but smaller than Ca, as it is in Period 3 but on the left side.