Question

drag each tile to the correct box. arrange the elements in order of increasing atomic radius. use the periodic table to help you. mg ba f s boxes with <

Explanation:

Step1: Recall atomic radius trends

Atomic radius increases down a group (as more electron shells are added) and decreases across a period (due to increasing effective nuclear charge).

Step2: Analyze each element's position

• F (Fluorine): Period 2, Group 17.
• S (Sulfur): Period 3, Group 16.
• Mg (Magnesium): Period 3, Group 2.
• Ba (Barium): Period 6, Group 2.

Step3: Compare across periods and groups

• Across Period 2 to 3: F (Period 2) < S (Period 3), Mg (Period 3).
• In Group 2: Mg (Period 3) < Ba (Period 6) (down the group, radius increases).
• Across Period 3 (Groups 2 and 16): Mg (Group 2) > S (Group 16) (radius decreases across period).

So order: F < S < Mg < Ba.

Answer:

F < S < Mg < Ba