Which of the following molecule is polar and non-planar

Options

A. `XeF_(4)`
B. `XeF_(5)^(-)`
C. `CH_(2)F_(2)`
D. `ClF_(3)`

Answer

To determine which of the given molecules is polar and non-planar, we will analyze each option step by step.

### Step 1: Analyze Option A - XeF4
- **Valence Electrons Calculation**:
- Xenon (Xe) has 8 valence electrons.
- Each Fluorine (F) has 7 valence electrons, and there are 4 Fluorine atoms: 4 × 7 = 28.
- Total = 8 + 28 = 36 valence electrons.
- **Lewis Structure**:
- 36 valence electrons divided by 8 (for the octet rule) gives us 4 bond pairs and 2 lone pairs.
- The arrangement is square planar due to the 4 bond pairs and 2 lone pairs.
- **Polarity**:
- The molecule is symmetrical, and the dipole moments cancel out, resulting in a net dipole moment of 0.
- **Conclusion**: XeF4 is non-polar and planar.

### Step 2: Analyze Option B - XeF5^-
- **Valence Electrons Calculation**:
- Xenon (Xe) has 8 valence electrons.
- 5 Fluorine atoms contribute 28 valence electrons (5 × 7 = 35).
- The negative charge adds 1 electron: 8 + 35 + 1 = 44 valence electrons.
- **Lewis Structure**:
- 44 valence electrons divided by 8 gives us 5 bond pairs and 2 lone pairs.
- The shape is distorted octahedral due to the presence of lone pairs.
- **Polarity**:
- The molecule is non-planar, and the dipole moments do not cancel out completely, resulting in a net dipole moment that is not equal to 0.
- **Conclusion**: XeF5^- is polar and non-planar.

### Step 3: Analyze Option C - CH2F2
- **Valence Electrons Calculation**:
- Carbon (C) has 4 valence electrons, and each Hydrogen (H) has 1 (2 × 1 = 2), and each Fluorine (F) has 7 (2 × 7 = 14).
- Total = 4 + 2 + 14 = 20 valence electrons.
- **Lewis Structure**:
- The structure has 2 bond pairs with H and 2 bond pairs with F, leading to a tetrahedral shape.
- **Polarity**:
- The molecule is polar due to the presence of F atoms, but it is not non-planar; it is tetrahedral.
- **Conclusion**: CH2F2 is polar but planar.

### Step 4: Analyze Option D - ClF3
- **Valence Electrons Calculation**:
- Chlorine (Cl) has 7 valence electrons, and each Fluorine (F) has 7 (3 × 7 = 21).
- Total = 7 + 21 = 28 valence electrons.
- **Lewis Structure**:
- The structure has 3 bond pairs and 2 lone pairs, leading to a T-shaped molecular geometry.
- **Polarity**:
- The T-shaped structure is polar, but it is also non-planar due to the presence of lone pairs.
- **Conclusion**: ClF3 is polar and non-planar.

### Final Conclusion
After analyzing all options:
- **Option A**: Non-polar and planar.
- **Option B**: Polar and non-planar.
- **Option C**: Polar but planar.
- **Option D**: Polar and non-planar.

Thus, the correct answer is **Option B (XeF5^-)** and **Option D (ClF3)** are both polar and non-planar. However, since the question asks for one, we conclude with **Option B** as the primary answer.