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

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

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter6: The Periodic Table And Atomic Structure
Section: Chapter Questions
Problem 6.83PAE: 6.83 The graph below shows the first three ionization energies for sodium, magnesium, and aluminum....
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**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 < Sb 2. ⃝ Sb < Cl < P 3. ⃝ none of these 4. ⃝ P < Sb < Cl 5. ⃝ 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.
Transcribed Image Text:**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 < Sb 2. ⃝ Sb < Cl < P 3. ⃝ none of these 4. ⃝ P < Sb < Cl 5. ⃝ 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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