I need to draw a Lewis dot and cross diagram for the phosphorus hexafluoride ion for my IB Chemistry HL. I tried but ended up with the phosphorus atom having 12 shared electrons with 6 fluorine atoms. But doesn't phosphorus only have 5 electrons to covalently bond with? Ahhhh.
I need to draw a Lewis dot and cross diagram for the phosphorus hexafluoride ion for my IB Chemistry HL. I tried but ended up with the phosphorus atom having 12 shared electrons with 6 fluorine atoms. But doesn't phosphorus only have 5 electrons to covalently bond with? Ahhhh.
Help would be much appreciated
Merry [Belated] Christmas !
Just do it one step at a time...
Phosphorus has 5 outer electrons = 5 Each fluorine provides 1 electron = 6 The negative charge must be added in = 1 -------------------------------------------------------- add together Total electrons around the phosphorus = 12
This makes 6 pairs = electronically octahedral
Each P-F bond requires 2 electrons and there are 6 P-F bonds = 12 electrons
Hence all electrons used up in bonding. Ionic shape is also octahedral.
Phosphorus has 5 outer electrons = 5 Each fluorine provides 1 electron = 6 The negative charge must be added in = 1 -------------------------------------------------------- add together Total electrons around the phosphorus = 12
This makes 6 pairs = electronically octahedral
Each P-F bond requires 2 electrons and there are 6 P-F bonds = 12 electrons
Hence all electrons used up in bonding. Ionic shape is also octahedral.
Thank you!
Haven't learnt about VSEPRT and hybridisation yet... but will do so soon