Define a transition metal and write the electronic configurations for Mn2+ and Fe2+ ions, explaining why Fe2+ is readily oxidized to Fe3+ but Mn2+ is not readily oxidized to Mn3+.

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Asked on May 24, 2026Chemistry

This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.

Accepted Answer · 2026-05-24T02:29:30.475Z

Welcome back wisdom — been a while! Let's pick up where you left off. SECTION B: INORGANIC CHEMISTRY 3 (a) (i) Define a transition metal. A transition metal is an element that has a partially filled d subshell in at least one of its common oxidation states. These elements are typically found in the d-block of the periodic table. 3 (a) (ii) Using the box below, write out the electronic configuration for Mn^2+ and Fe^2+ ions (Mn=25, Fe=26). For Fe (Z=26): Ground state is [Ar] 3d^6 4s^2. Fe^2+ is formed by losing the two 4s electrons, resulting in [Ar] 3d^6. For Mn (Z=25): Ground state is [Ar] 3d^5 4s^2. Mn^2+ is formed by losing the two 4s electrons, resulting in [Ar] 3d^5. Here are the electronic configurations in the 3d orbitals: |c|c|c|c|c| 5|c|3d \\ & & & & \\ _26Fe^2+ : (Ar) |c|c|c|c|c| 5|c|3d \\ & & & & \\ _25Mn^2+ : (Ar) 3 (b) Account for the fact that Fe^2+ ions are readily oxidized to Fe^3+ ions but Mn^2+ ions are not readily oxidized to Mn^3+ ions. Step 1: Determine the electronic configurations of the ions involved. Fe^2+ has an electronic configuration of [Ar] 3d^6. Fe^3+ has an electronic configuration of [Ar] 3d^5. Mn^2+ has an electronic configuration of [Ar] 3d^5. Mn^3+ has an electronic configuration of [Ar] 3d^4. Step 2: Analyze the stability of the configurations. The 3d^5 configuration represents a half-filled d subshell, which is particularly stable due to exchange energy and symmetry. Step 3: Explain the oxidation of Fe^2+ to Fe^3+. Fe^2+ (3d^6) readily loses an electron to form Fe^3+ (3d^5). This conversion is favorable because it results in the highly stable half-filled 3d^5 configuration. Step 4: Explain why Mn^2+ is not readily oxidized to Mn^3+. Mn^2+ already possesses the highly stable half-filled 3d^5 configuration. Oxidizing Mn^2+ to Mn^3+ would mean losing an electron from this stable 3d^5 configuration to form a less stable 3d^4 configuration. This process requires a significant amount of energy and is therefore not readily favorable. 3 (c) Give the transition metal or transition metal compound used as catalyst in the following conversions. The conversions are not visible in the provided image. Please provide the conversions for this part. Drop the next question 📸

Accepted Answer · 2026-05-24T02:29:30.475Z

Welcome back wisdom — been a while! Let's pick up where you left off. SECTION B: INORGANIC CHEMISTRY 3 (a) (i) Define a transition metal. A transition metal is an element that has a partially filled d subshell in at least one of its common oxidation states. These elements are typically found in the d-block of the periodic table. 3 (a) (ii) Using the box below, write out the electronic configuration for Mn^2+ and Fe^2+ ions (Mn=25, Fe=26). For Fe (Z=26): Ground state is [Ar] 3d^6 4s^2. Fe^2+ is formed by losing the two 4s electrons, resulting in [Ar] 3d^6. For Mn (Z=25): Ground state is [Ar] 3d^5 4s^2. Mn^2+ is formed by losing the two 4s electrons, resulting in [Ar] 3d^5. Here are the electronic configurations in the 3d orbitals: |c|c|c|c|c| 5|c|3d \\ & & & & \\ _26Fe^2+ : (Ar) |c|c|c|c|c| 5|c|3d \\ & & & & \\ _25Mn^2+ : (Ar) 3 (b) Account for the fact that Fe^2+ ions are readily oxidized to Fe^3+ ions but Mn^2+ ions are not readily oxidized to Mn^3+ ions. Step 1: Determine the electronic configurations of the ions involved. Fe^2+ has an electronic configuration of [Ar] 3d^6. Fe^3+ has an electronic configuration of [Ar] 3d^5. Mn^2+ has an electronic configuration of [Ar] 3d^5. Mn^3+ has an electronic configuration of [Ar] 3d^4. Step 2: Analyze the stability of the configurations. The 3d^5 configuration represents a half-filled d subshell, which is particularly stable due to exchange energy and symmetry. Step 3: Explain the oxidation of Fe^2+ to Fe^3+. Fe^2+ (3d^6) readily loses an electron to form Fe^3+ (3d^5). This conversion is favorable because it results in the highly stable half-filled 3d^5 configuration. Step 4: Explain why Mn^2+ is not readily oxidized to Mn^3+. Mn^2+ already possesses the highly stable half-filled 3d^5 configuration. Oxidizing Mn^2+ to Mn^3+ would mean losing an electron from this stable 3d^5 configuration to form a less stable 3d^4 configuration. This process requires a significant amount of energy and is therefore not readily favorable. 3 (c) Give the transition metal or transition metal compound used as catalyst in the following conversions. The conversions are not visible in the provided image. Please provide the conversions for this part. Drop the next question 📸

Define a transition metal and write the electronic configurations for Mn2+ and Fe2+ ions, explaining why Fe2+ is readily oxidized to Fe3+ but Mn2+ is not readily oxidized to Mn3+.

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Define a transition metal and write the electronic configurations for Mn2+ and Fe2+ ions, explaining why Fe2+ is readily oxidized to Fe3+ but Mn2+ is not readily oxidized to Mn3+.

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