12 **Periodic Trends and Ionization Energy****Question:**Rank the following in order of *increasing* first ionization energy (IE₁) based on periodic trends.Elements: P, Cl, Sb**Options:**1. ⃝ Cl < P < Sb2. ⃝ Sb < Cl < P3. ⃝ none of these4. ⃝ P < Sb < Cl5. ⃝ Sb < P < Cl **Explanation of Concepts:**- **Ionization Energy (IE₁):** The first ionization energy is the energy required to remove the outermost electron from a neutral atom in its gaseous state.- **Periodic Trends:** - **Across a Period (Left to Right):** Ionization energy typically increases across a period because of increasing nuclear charge, which holds the electrons more tightly. - **Down a Group (Top to Bottom):** Ionization energy typically decreases down a group because the outer electrons are further from the nucleus and experience more shielding from the inner electrons.Using these trends, determine the correct order of increasing ionization energy for the elements given. Double-check the accuracy against periodic trends and the position of the elements:- Phosphorus (P)- Chlorine (Cl)- Antimony (Sb)Select the appropriate answer based on the trends.

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Answered: O Cl< P < Sb O Sb < Cl< P O none of…

Science

Chemistry

O Cl< P < Sb O Sb < Cl< P O none of these O P < Sb < CI O Sb < P < Cl

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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