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The resultant dipole moment (mu) of two ...

The resultant dipole moment `(mu)` of two compounds `NOF` and `NO_(2)F` is `1.81 D` and `0.47D` respectively Which dipole momnet do you predict ? .

A

`1.81 D` for `NO_(2)F` and `0.47 D` for `NOF` .

B

`0.47 D` for `NO_(2)F` and `1.81 D` for `NOF`

C

For both `NO_(2)F` and `NOF` dipole moment `(mu)` is `1.81 D`

D

For both `NO_(2)F` and `NOF` dipole moment `(mu)` is `0.47 D`

Text Solution

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The correct Answer is:
To determine the dipole moments of the compounds NOF and NO2F, we can analyze their structures and the resulting symmetry. Here’s a step-by-step breakdown of the solution: ### Step-by-Step Solution: 1. **Identify the Compounds**: We have two compounds: Nitrogen Oxyfluoride (NOF) and Nitrogen Dioxide Fluoride (NO2F). 2. **Draw the Structure of NOF**: - NOF consists of a nitrogen atom (N) bonded to one oxygen atom (O) via a double bond and to one fluorine atom (F) via a single bond. - The nitrogen atom has a lone pair of electrons, resulting in a bent molecular geometry. 3. **Determine the Dipole Moment of NOF**: - The dipole moment vectors will point from the nitrogen to the more electronegative atoms (O and F). - The resultant dipole moment of NOF is given as **1.81 D**. 4. **Draw the Structure of NO2F**: - NO2F has a nitrogen atom bonded to two oxygen atoms (double bonds) and one fluorine atom (single bond). - This compound has a trigonal planar geometry due to the arrangement of the bonds around the nitrogen atom. 5. **Determine the Dipole Moment of NO2F**: - In NO2F, the dipole moments from the N=O bonds and the N-F bond will partially cancel each other due to the symmetry of the trigonal planar structure. - The resultant dipole moment of NO2F is given as **0.47 D**. 6. **Compare the Dipole Moments**: - Since NOF has a bent structure, it has a higher dipole moment (1.81 D) compared to the more symmetrical NO2F (0.47 D). - The symmetry in NO2F reduces the overall dipole moment. 7. **Conclusion**: - Based on the analysis, we can conclude that NOF has a higher dipole moment than NO2F due to its asymmetrical structure. ### Final Answer: The dipole moments are: - NOF: **1.81 D** - NO2F: **0.47 D**
To determine the dipole moments of the compounds NOF and NO2F, we can analyze their structures and the resulting symmetry. Here’s a step-by-step breakdown of the solution: ### Step-by-Step Solution: 1. **Identify the Compounds**: We have two compounds: Nitrogen Oxyfluoride (NOF) and Nitrogen Dioxide Fluoride (NO2F). 2. **Draw the Structure of NOF**: - NOF consists of a nitrogen atom (N) bonded to one oxygen atom (O) via a double bond and to one fluorine atom (F) via a single bond. ...
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