The type of magnetism exhibited by `[Mn(H_(2)O)_(6)]^(2+)` ion is `"________"` .

Explanation

To determine the type of magnetism exhibited by the `[Mn(H₂O)₆]²⁺` ion, we can follow these steps:

### Step 1: Determine the oxidation state of manganese (Mn) in the complex.
- The complex is `[Mn(H₂O)₆]²⁺`. Since water (H₂O) is a neutral ligand, the oxidation state of Mn is +2.

### Step 2: Find the electronic configuration of Mn²⁺.
- The atomic number of manganese (Mn) is 25. The electronic configuration of neutral Mn is:
\[ \text{Mn: } [Ar] 3d^5 4s^2 \]
- When Mn loses two electrons to form Mn²⁺, the electrons are removed from the 4s orbital first:
\[ \text{Mn}^{2+}: [Ar] 3d^5 \]

### Step 3: Analyze the electron configuration of Mn²⁺.
- The electron configuration of Mn²⁺ is 3d⁵. In this configuration, all five d-orbitals are half-filled:
\[ \uparrow \quad \uparrow \quad \uparrow \quad \uparrow \quad \uparrow \]
- This indicates that there are 5 unpaired electrons present in the 3d subshell.

### Step 4: Determine the type of magnetism.
- The presence of unpaired electrons in an ion indicates that it will exhibit paramagnetism. Paramagnetic substances are attracted to magnetic fields due to the presence of unpaired electrons.

### Final Answer:
The type of magnetism exhibited by the `[Mn(H₂O)₆]²⁺` ion is **paramagnetism**.

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