The angle between two covalent bonds is maximum for `(CH_(4), H_(2)O, CO_(2))` `"______"` .

Explanation

To determine which molecule has the maximum angle between two covalent bonds among \( CH_4 \) (methane), \( H_2O \) (water), and \( CO_2 \) (carbon dioxide), we need to analyze the molecular geometry and bond angles of each compound.

### Step 1: Analyze the structure of Methane (\( CH_4 \))
- **Geometry**: Methane has a tetrahedral geometry.
- **Hybridization**: The carbon atom is \( sp^3 \) hybridized.
- **Bond Angle**: The bond angle in a tetrahedral structure is approximately \( 109.5^\circ \).

### Step 2: Analyze the structure of Water (\( H_2O \))
- **Geometry**: Water has a bent (or V-shaped) geometry due to the presence of lone pairs.
- **Hybridization**: The oxygen atom is also \( sp^3 \) hybridized.
- **Bond Angle**: The bond angle in water is less than that of a tetrahedral structure due to lone pair repulsion, specifically about \( 104.5^\circ \).

### Step 3: Analyze the structure of Carbon Dioxide (\( CO_2 \))
- **Geometry**: Carbon dioxide has a linear geometry.
- **Hybridization**: The carbon atom is \( sp \) hybridized.
- **Bond Angle**: The bond angle in a linear structure is \( 180^\circ \).

### Step 4: Compare the bond angles
- Methane (\( CH_4 \)): \( 109.5^\circ \)
- Water (\( H_2O \)): \( 104.5^\circ \)
- Carbon Dioxide (\( CO_2 \)): \( 180^\circ \)

### Conclusion
The maximum angle between two covalent bonds is found in carbon dioxide (\( CO_2 \)), which has a bond angle of \( 180^\circ \).

### Final Answer
The angle between two covalent bonds is maximum for \( CO_2 \).

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