You have given two species :- NOF and `NO_(2)F` and two dipole moments 1.81D and 0.46D. Then correct statement is:-

Options

A. 1.81 D for `NO_(2)F` and o.47D for NOF
B. 0.47D for `NO_(2)F` and 1.81D for NOF because `NO_(2)F` is linear but NOF is nonlinear molecule
C. 0.47D for `NO_(2)F` because bond moments of NO bond and `NF` bonds are oriented in the opposite direction
D. 0.46D for `NO_(2)F` and 1.81D for NOF

Answer

To solve the question regarding the dipole moments of the two species NOF and NO2F, we need to analyze the information provided and understand the molecular structures and their implications on dipole moments.

### Step-by-Step Solution:

1. **Identify the Given Information**:
- Two species: NOF (Nitrogen Oxyfluoride) and NO2F (Nitrogen Dioxide Fluoride).
- Dipole moments: 1.81 D and 0.46 D (the specific assignment to each molecule is not provided).

2. **Understand Dipole Moment**:
- The dipole moment is a vector quantity that depends on the magnitude of the charge and the distance between the charges. It indicates the polarity of a molecule.
- A higher dipole moment indicates a more polar molecule.

3. **Analyze the Structures**:
- **NOF**: The structure can be visualized as having a nitrogen atom bonded to one oxygen atom (with a double bond) and one fluorine atom. The presence of a lone pair on nitrogen makes the structure non-linear.
- **NO2F**: This molecule has nitrogen bonded to two oxygen atoms and one fluorine atom. The arrangement of these bonds also leads to a non-linear structure.

4. **Electronegativity Considerations**:
- The electronegativity of fluorine (F) is greater than that of nitrogen (N) and oxygen (O). Therefore, the dipole moment will point towards the more electronegative atoms.
- In NOF, the dipole moment will be directed towards both oxygen and fluorine.
- In NO2F, there are two dipole moments (from N=O and N=F), but they are oriented in such a way that they partially cancel each other out due to their opposite directions.

5. **Determine Dipole Moments**:
- Since NO2F has two dipole moments that oppose each other, it will have a smaller resultant dipole moment compared to NOF, which has a single dipole moment directed towards the more electronegative atoms.
- Therefore, it is reasonable to assign the larger dipole moment (1.81 D) to NOF and the smaller dipole moment (0.46 D) to NO2F.

6. **Conclusion**:
- The correct statements based on the analysis are:
- NOF has a dipole moment of 1.81 D.
- NO2F has a dipole moment of 0.46 D.
- The reason for the lower dipole moment in NO2F is due to the cancellation of dipole moments from its structure.

### Final Answer:
- The correct statements are:
- NOF has a dipole moment of 1.81 D.
- NO2F has a dipole moment of 0.46 D.