Which of the statement are true?
I.`H_2O` molecule has V shape with two lone pairs of electrons II.`SF_4` molecules has see saw shape with one lone pair of electrons III.`CIF_3` is T shaped molecules with two lone pairs of electrons

Options

A. I andII
B. ii and III
C. I and III
D. All of the above

Answer

To determine which of the statements are true, we need to analyze each statement regarding the molecular geometry and the number of lone pairs of electrons present in each molecule.

### Step 1: Analyze Statement I - H₂O
- **Molecular Formula**: H₂O
- **Valence Electrons**: Oxygen has 6 valence electrons, and each hydrogen has 1, giving a total of 8 valence electrons.
- **Lone Pairs**: Oxygen has 2 lone pairs of electrons.
- **Shape**: The molecular geometry of H₂O is bent or V-shaped due to the two lone pairs pushing down on the hydrogen atoms.

**Conclusion**: Statement I is **True**.

### Step 2: Analyze Statement II - SF₄
- **Molecular Formula**: SF₄
- **Valence Electrons**: Sulfur has 6 valence electrons, and each fluorine has 7, giving a total of 34 valence electrons.
- **Lone Pairs**: There is 1 lone pair on the sulfur atom.
- **Shape**: The molecular geometry of SF₄ is see-saw due to the presence of one lone pair, which distorts the tetrahedral arrangement.

**Conclusion**: Statement II is **True**.

### Step 3: Analyze Statement III - ClF₃
- **Molecular Formula**: ClF₃
- **Valence Electrons**: Chlorine has 7 valence electrons, and each fluorine has 7, giving a total of 28 valence electrons.
- **Lone Pairs**: Chlorine has 2 lone pairs of electrons.
- **Shape**: The molecular geometry of ClF₃ is T-shaped due to the presence of two lone pairs, which affects the arrangement of the fluorine atoms.

**Conclusion**: Statement III is **True**.

### Final Summary:
- Statement I: True
- Statement II: True
- Statement III: True

### Overall Conclusion:
All three statements are **True**.

---