What may be the stable oxidation state of the transition elements with the following d electron configurations in the ground state of their atoms:`3d^(3),3d^(5),3d^(4)?`

Answer

To determine the stable oxidation states of transition elements with the given d electron configurations (3d^3, 3d^5, and 3d^4), we can analyze each configuration step by step.

### Step 1: Identify the Transition Element for Each Configuration
- **3d^3**: This configuration corresponds to the element Vanadium (V).
- **3d^5**: This configuration corresponds to the element Manganese (Mn).
- **3d^4**: There is no stable transition metal with this exact configuration in its ground state. The closest stable configuration is for Chromium (Cr), which has a configuration of 3d^5 4s^1.

### Step 2: Determine the Stable Oxidation States
- **For 3d^3 (Vanadium)**:
- Vanadium can lose its 3d electrons and 4s electrons to form oxidation states.
- Possible oxidation states: +2, +3, +4, +5.
- The most stable oxidation states are typically +3 and +5.

- **For 3d^5 (Manganese)**:
- Manganese can also lose its 3d and 4s electrons.
- Possible oxidation states: +2, +4, +6, +7.
- The most stable oxidation states are +2, +4, +6, and +7, with +7 being the maximum.

- **For 3d^4**:
- As mentioned, there is no transition metal with a stable ground state configuration of 3d^4. The closest is Chromium (3d^5 4s^1).
- For Chromium, the oxidation states are +2, +3, +6, with +3 being the most stable.

### Summary of Stable Oxidation States
- **3d^3 (Vanadium)**: +2, +3, +4, +5 (most stable: +3, +5)
- **3d^5 (Manganese)**: +2, +4, +6, +7 (most stable: +2, +4, +6, +7)
- **3d^4**: No stable transition metal corresponds to this configuration.