Question

1. predict the order of increasing electronegativity in each of the following groups of elements: s, se, cl.

Explanation:

Step1: Recall Electronegativity Trends

Electronegativity increases across a period (from left to right) and decreases down a group (from top to bottom) in the periodic table.

Step2: Locate Elements in Periodic Table

• S (sulfur) and Se (selenium) are in Group 16. Se is below S, so electronegativity: Se < S.
• S is in Group 16, Period 3; Cl (chlorine) is in Group 17, Period 3. Across Period 3, electronegativity increases: S < Cl.

Step3: Combine Trends

From the above, Se < S < Cl.

Answer:

Se < S < Cl