The number of molecules with a bond angle greater than H2O can be determined by analyzing the molecular geometry of each molecule. The bond angle in H2O is approximately 104.5 degrees. Molecules with a bond angle greater than this value will have a different molecular geometry, leading to a larger bond angle.

Let's analyze each molecule individually:

1. CH4 (methane):
- Methane has a tetrahedral molecular geometry, with a bond angle of 109.5 degrees. This is larger than the bond angle in H2O, so CH4 satisfies the condition.

2. NH3 (ammonia):
- Ammonia has a trigonal pyramidal molecular geometry, with a bond angle of approximately 107 degrees. This is also larger than the bond angle in H2O, so NH3 satisfies the condition.

3. H2S (hydrogen sulfide):
- Hydrogen sulfide has a bent molecular geometry, with a bond angle of approximately 92 degrees. This is smaller than the bond angle in H2O, so H2S does not satisfy the condition.

4. PH3 (phosphine):
- Phosphine has a trigonal pyramidal molecular geometry, similar to ammonia, with a bond angle of approximately 93.5 degrees. This is smaller than the bond angle in H2O, so PH3 does not satisfy the condition.

5. Cl2O (dichlorine monoxide):
- Dichlorine monoxide has a bent molecular geometry, with a bond angle of approximately 110 degrees. This is larger than the bond angle in H2O, so Cl2O satisfies the condition.

6. F2O (oxygen difluoride):
- Oxygen difluoride has a bent molecular geometry, similar to H2O, with a bond angle of approximately 103 degrees. This is slightly smaller than the bond angle in H2O, so F2O does not satisfy the condition.

Based on this analysis, we can conclude that out of the given molecules, CH4, NH3, and Cl2O have bond angles greater than H2O. Therefore, the correct answer is '3'.