Manganese exhibits oxidation states from

Options

A. `+II" to "+VII`
B. `+I" to "+VI`
C. `+I" to "+V`
D. `+III" to "+V`

Answer

To determine the oxidation states of manganese (Mn), we will follow these steps:

### Step 1: Identify the Atomic Number and Electronic Configuration
- Manganese has an atomic number of 25.
- Its electronic configuration is:
\[ \text{Mn: } [\text{Ar}] 4s^2 3d^5 \]

### Step 2: Understand Oxidation States
- Oxidation states indicate the degree of oxidation (loss of electrons) of an atom in a compound.
- Manganese, being a transition metal, can exhibit multiple oxidation states due to its ability to lose electrons from both the 4s and 3d orbitals.

### Step 3: Determine the Possible Oxidation States
- Manganese can lose electrons from the 4s and 3d orbitals:
- Losing 2 electrons from the 4s orbital gives a +2 oxidation state.
- Further losing electrons from the 3d orbital can lead to additional oxidation states:
- +3 (1 electron from 3d)
- +4 (2 electrons from 3d)
- +5 (3 electrons from 3d)
- +6 (4 electrons from 3d)
- +7 (5 electrons from 3d)

### Step 4: List the Range of Oxidation States
- The oxidation states of manganese range from +2 (when it loses 2 electrons from 4s) to +7 (when it loses all 5 electrons from 3d).
- Therefore, the oxidation states exhibited by manganese are from +2 to +7.

### Conclusion
- The correct answer is that manganese exhibits oxidation states from **+2 to +7**.

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