Question

question 4. using the periodic table as a guide, arrange the following elements in order of increasing atomic radius by dragging them into the correct sequence. < < < < sulfur (s) cesium (cs) phosphorus (p) fluorine (f) strontium (sr)

Explanation:

Step1: Recall atomic radius trends

Atomic radius increases down a group (due to more electron shells) and decreases across a period (due to increased nuclear charge pulling electrons closer).

Step2: Analyze each element's position

• Fluorine (F): Period 2, Group 17.
• Sulfur (S): Period 3, Group 16.
• Phosphorus (P): Period 3, Group 15 (same period as S, left of S, so larger than S but smaller than elements below).
• Strontium (Sr): Period 5, Group 2.
• Cesium (Cs): Period 6, Group 1 (lowest and leftmost, largest radius).

Step3: Order by increasing radius

Across period 2 - 3: F (period 2) < P, S (period 3). In period 3, P is left of S, so P > S. Down groups: S (period 3) < Sr (period 5) < Cs (period 6). So order: F < S < P < Sr < Cs.

Answer:

Fluorine (F) < Sulfur (S) < Phosphorus (P) < Strontium (Sr) < Cesium (Cs)