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Order these elements from highest to lowest ionization energy 1 | Chlorine, CI | Fluorine, F 3 | lodine, I | Bromine, Br 2.

Order these elements from highest to lowest ionization energy 1 | Chlorine, CI | Fluorine, F 3 | lodine, I | Bromine, Br 2.

Chemistry
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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Ionization Energy Trend

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**Order these elements from highest to lowest ionization energy** 1. Fluorine, F 2. Chlorine, Cl 3. Bromine, Br 4. Iodine, I In this exercise, you are asked to arrange the elements based on their ionization energy. Ionization energy is the amount of energy required to remove an electron from an atom. Fluorine has the highest ionization energy among these elements, followed by chlorine, bromine, and iodine, which has the lowest. **Explanation:** - **Fluorine (F):** As the element with the highest ionization energy in this group, fluorine exhibits a strong ability to attract electrons due to its high electronegativity and small atomic size. - **Chlorine (Cl):** Slightly larger than fluorine, chlorine has a slightly lower ionization energy. - **Bromine (Br):** With increased atomic size, bromine's ionization energy is lower than that of chlorine. - **Iodine (I):** The largest atom in this series, iodine's electrons are further from the nucleus, resulting in the lowest ionization energy. This order reflects the general trend in the periodic table, where ionization energy decreases down a group due to the increasing distance of the outermost electrons from the nucleus.
Transcribed Image Text:**Order these elements from highest to lowest ionization energy** 1. Fluorine, F 2. Chlorine, Cl 3. Bromine, Br 4. Iodine, I In this exercise, you are asked to arrange the elements based on their ionization energy. Ionization energy is the amount of energy required to remove an electron from an atom. Fluorine has the highest ionization energy among these elements, followed by chlorine, bromine, and iodine, which has the lowest. **Explanation:** - **Fluorine (F):** As the element with the highest ionization energy in this group, fluorine exhibits a strong ability to attract electrons due to its high electronegativity and small atomic size. - **Chlorine (Cl):** Slightly larger than fluorine, chlorine has a slightly lower ionization energy. - **Bromine (Br):** With increased atomic size, bromine's ionization energy is lower than that of chlorine. - **Iodine (I):** The largest atom in this series, iodine's electrons are further from the nucleus, resulting in the lowest ionization energy. This order reflects the general trend in the periodic table, where ionization energy decreases down a group due to the increasing distance of the outermost electrons from the nucleus.
**Activity: Ordering Elements by Ionization Energy** Instructions: Arrange the following elements from highest to lowest ionization energy. 1. Potassium, K 2. Hydrogen, H 3. Sodium, Na 4. Lithium, Li Drag and drop the elements into the correct order based on their ionization energies. Use your knowledge of periodic trends to complete the task.
Transcribed Image Text:**Activity: Ordering Elements by Ionization Energy** Instructions: Arrange the following elements from highest to lowest ionization energy. 1. Potassium, K 2. Hydrogen, H 3. Sodium, Na 4. Lithium, Li Drag and drop the elements into the correct order based on their ionization energies. Use your knowledge of periodic trends to complete the task.
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