Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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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.
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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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