Question

16 ccc patterns rank the electronegativity values of lithium, oxygen, potassium, and selenium from lowest to highest. explain their general electronegativity trends in the periodic table.

Explanation:

Step1: Recall Electronegativity Trends

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

Step2: Locate Elements in Periodic Table

• Lithium (Li): Group 1, Period 2.
• Oxygen (O): Group 16, Period 2.
• Potassium (K): Group 1, Period 4.
• Selenium (Se): Group 16, Period 4.

Step3: Compare Based on Trends

• For Group 1: K (Period 4) has lower electronegativity than Li (Period 2) (decreases down group).
• For Group 16: Se (Period 4) has lower electronegativity than O (Period 2) (decreases down group).
• Across Period 2: Li (Group 1) < O (Group 16) (increases across period).
• Across Period 4: K (Group 1) < Se (Group 16) (increases across period).
• Overall order: K (lowest) < Li < Se < O (highest).

Step4: Explain Trends

Electronegativity increases across a period because atomic radius decreases (nuclear charge attracts electrons more strongly) and decreases down a group because atomic radius increases (electrons are farther from nucleus, less attraction).

Answer:

The order of electronegativity from lowest to highest is potassium (K) < lithium (Li) < selenium (Se) < oxygen (O). Electronegativity increases across a period (due to decreasing atomic radius, stronger nuclear attraction for electrons) and decreases down a group (due to increasing atomic radius, weaker nuclear attraction for electrons). So K (Group 1, Period 4) < Li (Group 1, Period 2) (down - group decrease), Li (Group 1, Period 2) < O (Group 16, Period 2) (across - period increase), K (Group 1, Period 4) < Se (Group 16, Period 4) (across - period increase), Se (Group 16, Period 4) < O (Group 16, Period 2) (down - group decrease), leading to K < Li < Se < O.