Answer:
PF4+ < PF3 < OF2
Explanation:
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In this case, the two non-shared pairs of electrons present on the OF2 occupy more space and causes the FOF bond angle to be the largest one (180°) due to its planar arrangement. Furthermore, PF3 has just 1 non-shared pair of electrons, therefore there is less space for the bonds to be trigonally arranged, it means, a smaller angle (120°). Finally, PF4+ shows a perfectly tetrahedral arrangement therefore it has the smallest bond angle (109.5°).
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The order of increasing F-A-F bond angle is PF3 < OF2 < PF4+
The bond angle refers to the angle between two atoms that are bonded to the same atom. The size of the bond angle depends on the number of electron domains that surround the central atom.
PF3 will have the a trigonal planar geometry and the least bond angle of about 97°. OF2 is a bent molecule and has a bond angle of about 103°. PF4+ is tetrahedral and has bond angle of 109°.
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