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The polarity of (i) (CH3)(2) P(CF3)(3) a...

The polarity of (i) `(CH_3)_(2) P(CF_3)_(3)` and (ii) `(CH_3)_(3) P(CF_3)_(2)` respectively are?

A

(i) Non Polar(ii) Polar

B

(i) Polar (ii) Non Polar

C

(i) Non Polar (ii) Non Polar

D

(i) Polar (ii) Polar

Text Solution

AI Generated Solution

The correct Answer is:
To determine the polarity of the compounds (i) `(CH_3)_(2) P(CF_3)_(3)` and (ii) `(CH_3)_(3) P(CF_3)_(2)`, we need to analyze their structures and the arrangement of their substituents around the central phosphorus atom. ### Step-by-Step Solution: 1. **Identify the Central Atom and Hybridization:** - The central atom in both compounds is phosphorus (P). - Phosphorus has the electronic configuration of 3s² 3p³. It can undergo hybridization to form sp³ hybrid orbitals, which allows it to form five bonds (triagonal bipyramidal geometry). 2. **Draw the Structures:** - For `(CH_3)_(2) P(CF_3)_(3)`: - Phosphorus is bonded to two methyl groups `(CH_3)` and three trifluoromethyl groups `(CF_3)`. - The more electronegative `CF_3` groups will occupy the axial positions due to their higher electronegativity compared to `CH_3`. - The structure will have two `CH_3` groups in equatorial positions and three `CF_3` groups in axial positions. - For `(CH_3)_(3) P(CF_3)_(2)`: - Phosphorus is bonded to three methyl groups `(CH_3)` and two trifluoromethyl groups `(CF_3)`. - Again, the `CF_3` groups will occupy the axial positions, while the `CH_3` groups will occupy the equatorial positions. 3. **Analyze the Polarity:** - **For `(CH_3)_(2) P(CF_3)_(3)`**: - The `CF_3` groups are more electronegative and will pull electron density towards themselves, creating dipole moments. - The dipole moments from the two `CF_3` groups in axial positions will cancel each other out, but the `CF_3` in the equatorial position will create a net dipole moment. - Therefore, this molecule is **polar**. - **For `(CH_3)_(3) P(CF_3)_(2)`**: - The two `CF_3` groups in axial positions will have dipole moments that are equal in magnitude but opposite in direction, thus they will cancel each other out. - The three `CH_3` groups will not contribute to any significant dipole moment. - Therefore, this molecule is **non-polar**. 4. **Conclusion:** - The polarity of `(CH_3)_(2) P(CF_3)_(3)` is **polar**. - The polarity of `(CH_3)_(3) P(CF_3)_(2)` is **non-polar**. ### Final Answer: - (i) Polar - (ii) Non-polar
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