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Lewis Structures for Iodine and Phosphorus?
Ok why is the shape of IF5 a square pyramidal (5 bonds and 1 non bonding pair). Can't Iodine only hold t bonds? Can someone explain this to me
And why is this any different than the PF5? Can phosphorus only hold 5 bonds?
1 Answer
- 1 decade agoFavorite Answer
okay, the first thing you need to consider is the number of valence electron in Iodine and Phosphorus. Iodine have 7 valence electron and it is able to share a maximum of seven electron with its bonding pair. when fluorine reacts with iodine, 5 single bond form between iodine and fluorine. % iodine ion are used to make bonds, leaving 7-5=2 electrons to make an unbounded electron pair. that's why it has a square pyramidal shape.
phosporous only have 5 valence electron and all of these electrons are used to make bond with 5 fluorine atoms. As all 5 electron are occupied there is no unbounded pair of electron. thats why PF5 have a trigonal bi pyramidal shape.