The angle between two covalent bonds is maximum in ……..`(CH_(4),H_(2)O,CO_(2)`)

Answer

To determine which molecule has the maximum angle between two covalent bonds among CH₄, H₂O, and CO₂, we can analyze the molecular geometry and hybridization of each compound.

### Step 1: Analyze CH₄ (Methane)
- **Structure**: CH₄ has a tetrahedral geometry.
- **Hybridization**: The carbon atom undergoes sp³ hybridization, forming four sigma bonds with hydrogen atoms.
- **Bond Angle**: The ideal bond angle in a tetrahedral arrangement is approximately 109.5°.

### Step 2: Analyze H₂O (Water)
- **Structure**: H₂O has a bent shape due to the presence of lone pairs on the oxygen atom.
- **Hybridization**: The oxygen atom is also sp³ hybridized, but it has two lone pairs and two bonding pairs.
- **Bond Angle**: The bond angle is reduced due to lone pair-lone pair and lone pair-bond pair repulsions, resulting in a bond angle of about 104.5°.

### Step 3: Analyze CO₂ (Carbon Dioxide)
- **Structure**: CO₂ has a linear geometry.
- **Hybridization**: The carbon atom is sp hybridized, forming two double bonds with oxygen atoms.
- **Bond Angle**: The bond angle in a linear molecule is 180°.

### Conclusion
Comparing the bond angles:
- CH₄: 109.5°
- H₂O: 104.5°
- CO₂: 180°

The maximum angle between two covalent bonds is found in **CO₂**, with a bond angle of 180°.

### Final Answer
The angle between two covalent bonds is maximum in **CO₂**.

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