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Circle the species with largest ionization energy and explain your reasoning. Os, Fe*, Co, Ru

Circle the species with largest ionization energy and explain your reasoning. Os, Fe*, Co, Ru

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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**Question:** Circle the species with the largest ionization energy and explain your reasoning. Os, Fe⁺, Co, Ru **Explanation:** To determine which species has the largest ionization energy, consider the periodic trends: 1. **Ionization Energy Trend:** Ionization energy generally increases across a period (left to right) and decreases down a group (top to bottom) in the periodic table. 2. **Charge:** Ionized species often have different ionization energies compared to their neutral counterparts. Removing more electrons from an already positively charged ion requires more energy. 3. **Electron Configuration:** Look at the electronic configuration of each element, as configurations that are stable (e.g., filled or half-filled subshells) will typically have higher ionization energies. **Analysis:** - **Os (Osmium):** Located in period 6, transition metal. - **Fe⁺ (Iron ion):** Ion with a positive charge; removing another electron will require energy. - **Co (Cobalt):** Located in period 4, transition metal. - **Ru (Ruthenium):** Located in period 5, transition metal. Given these factors, Fe⁺ is likely to have the highest ionization energy due to the removal of an electron from an already positively charged ion, making it more difficult compared to the other neutral atoms.
Transcribed Image Text:**Question:** Circle the species with the largest ionization energy and explain your reasoning. Os, Fe⁺, Co, Ru **Explanation:** To determine which species has the largest ionization energy, consider the periodic trends: 1. **Ionization Energy Trend:** Ionization energy generally increases across a period (left to right) and decreases down a group (top to bottom) in the periodic table. 2. **Charge:** Ionized species often have different ionization energies compared to their neutral counterparts. Removing more electrons from an already positively charged ion requires more energy. 3. **Electron Configuration:** Look at the electronic configuration of each element, as configurations that are stable (e.g., filled or half-filled subshells) will typically have higher ionization energies. **Analysis:** - **Os (Osmium):** Located in period 6, transition metal. - **Fe⁺ (Iron ion):** Ion with a positive charge; removing another electron will require energy. - **Co (Cobalt):** Located in period 4, transition metal. - **Ru (Ruthenium):** Located in period 5, transition metal. Given these factors, Fe⁺ is likely to have the highest ionization energy due to the removal of an electron from an already positively charged ion, making it more difficult compared to the other neutral atoms.
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