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Question

Which of the following statement is false:

A
The dipole moment of CH3F is greater than CH3Cl
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B
In PCl3, the axial bond length is longer than the equatorial bond length
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C
In XeOF4, the central atom Xe doesnot lie on the plane of the square
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D
In PF2Cl3, both the F atoms lie on the axial bond
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Solution

The correct option is A The dipole moment of CH3F is greater than CH3Cl
XeOF4 is square pyramidal in shape.

Due to lone pair - bond pair repulsion the four F atoms move away from lone pair resulting in the movement of Xe towards lone pair.

The most electronegative substituent lies at the axial position to minimize bond pair - lone pair repulsion.

PCl5 shows up sp3d hybridisation with the involvement of axial d2z orbital. Since, the axial Cl is at 90o hence suffers relatively greater repulsion increasing the axial bond length.

In CH3F and CH3Cl, the size of F is smaller than Cl leading smaller CF bond length decreasing the dipole moment.

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