Explanation
Lone pair of the electrons means those electrons which do not participate in chemical bonding.
The shape of XeO2F2 molecule is see-law shape. Bacause, after drawing the Lewis structure and determining the best one based on formal charges, the xenon atom is left with one lone pair, two double bonds to the oxygen atoms and two single bonds to the fluorine atoms. This is a total of 5 electron domains and 4 different atoms, consist with AX4E formula of the see-saw molecular geometry.
Here,
NCl3 → trigonal pyramidal →1070
ASCl3→ trigonal pyramidal →109
SbCl3 → pyramidal →97.20
PCl3 → trigonal pyramidal → about 109.
Hence SbCl3 has smaller bond angle is 97.2%.
From the VSEPR theory the number of electron around Br atom is 6 - five are bond and one is lone pair so geometry is octahedral. but it have one lone pair which repulse the other and so fluorine of corner are forced to upper fluorine and reduce the angle F-Br-F and make 84.8°. So no any F-Br-F bond form 90°
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