2007-07-25 05:41:44 · 3 answers · asked by boo 1 in Science & Mathematics ➔ Chemistry
formal charge is NOT oxidation state
(oxidation state for F is -1, B is +3)
formal charge for fluorine is 0
formal charge for boron is -1
All bonds are single bonds, you just split each B-F bond. one electron goes to boron, one electron goes to fluorine. Then you count. You will find All fluorine has 7 electrons, it is the same as the element, so no gain or loss. Boron has 4 electrons, it is 1 more than element, so it is -1 (since electron is negative).
2007-07-25 06:07:45 · answer #1 · answered by Carborane 6 · 1⤊ 0⤋
BF4- is a polyatomic ion, not an atom.
The charge on each F is -1, on B it is +3.
2007-07-25 12:48:03 · answer #2 · answered by ag_iitkgp 7 · 0⤊ 1⤋
It is a polyatomic ion.
To calculate the formal charge
B = +3
F = -1
You can consider the oxiadation numbers .
( +3 -4 )
the polyatomic ion has charge :
( -1 )
2007-07-25 13:05:34 · answer #3 · answered by Dr.A 7 · 0⤊ 1⤋