Out of `CHCl_(3), CH_(4) and SF_(4)` the molecules do not having regular geometry are:

Options

A. `CHCl_(3)` only
B. `CHCl_(3) and SF_(4)`
C. `CH_(4)`
D. `CH_(4) and SF_(4)`

Answer

To determine which of the given molecules (CHCl₃, CH₄, and SF₄) do not have regular geometry, we need to analyze the molecular structures and the presence of lone pairs on the central atoms.

### Step 1: Analyze CHCl₃ (Chloroform)
- **Central Atom**: Carbon (C)
- **Valence Electrons**: Carbon has 4 valence electrons, and each chlorine (Cl) has 7 valence electrons.
- **Bonds**: In CHCl₃, carbon forms three bonds with chlorine atoms and one bond with a hydrogen atom.
- **Lone Pairs**: Carbon has no lone pairs.
- **Geometry**: The presence of different atoms (Cl and H) bonded to the central atom means that CHCl₃ does not have a regular geometry.

### Step 2: Analyze CH₄ (Methane)
- **Central Atom**: Carbon (C)
- **Valence Electrons**: Carbon has 4 valence electrons, and each hydrogen (H) has 1 valence electron.
- **Bonds**: In CH₄, carbon forms four bonds with four hydrogen atoms.
- **Lone Pairs**: Carbon has no lone pairs.
- **Geometry**: Since all bonds are with the same type of atom (H), CH₄ has a regular tetrahedral geometry.

### Step 3: Analyze SF₄ (Sulfur Tetrafluoride)
- **Central Atom**: Sulfur (S)
- **Valence Electrons**: Sulfur has 6 valence electrons, and each fluorine (F) has 7 valence electrons.
- **Bonds**: In SF₄, sulfur forms four bonds with four fluorine atoms.
- **Lone Pairs**: Sulfur has one lone pair remaining after forming the four bonds.
- **Geometry**: The presence of a lone pair means that SF₄ does not have a regular geometry; it adopts a seesaw shape due to the lone pair.

### Conclusion
- **Molecules without Regular Geometry**: CHCl₃ and SF₄ do not have regular geometry.
- **Molecule with Regular Geometry**: CH₄ has regular geometry.

### Final Answer
The molecules that do not have regular geometry are **CHCl₃ and SF₄**.

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