Question

fill in the element in each list with the largest ionization energy: te, pa, se --> sr, te, rb --> ga, br, f --> cl, ra, ba -->

Explanation:

Step1: Recall ionization - energy trend

Ionization energy increases across a period and decreases down a group in the periodic table.

Step2: Analyze Te, Pa, Se

Se is above Te in Group 16 and Pa is in Group 15. Se has the highest ionization - energy among Te, Pa, Se as it is higher up in the periodic table and closer to the right side compared to Pa.

Step3: Analyze Sr, Te, Rb

Sr is in Group 2, Te in Group 16, and Rb in Group 1. Te has the highest ionization - energy as non - metals have higher ionization energies than metals in the same period.

Step4: Analyze Ga, Br, F

F is in the second period, Br in the fourth period, and Ga in Group 13. F has the highest ionization - energy as it is the most electronegative element and is in the upper right of the periodic table.

Step5: Analyze Cl, Ra, Ba

Cl is a non - metal, Ra and Ba are metals. Cl has the highest ionization - energy as non - metals have higher ionization energies than metals.

Answer:

Se
Te
F
Cl