An atom of fluorine has the greatest attraction among all atoms for electrons; therefore, no other atom can extract an electron from a fluorine atom, as would be required for the fluorine to have a positive oxidation state.
Fluorine is a highly electronegative compound, and combines with numerous elements to form compounds with the fluorine in -I oxidation state.
To calculate the oxidation state of fluorine in O2F2, first draw a diagram of the molecule: F-O-O-F Determine the most electronegative atom(s), which are fluorines -- the most electronegative atom there is. Being in the group 7A, a fluoride ion would gain an electron to a -1 charge, so each has an oxidation number of -1. The oxygens, therefore, have an oxidation number of +1 each.
Fluorine is located in period 2 and group 17 in the periodic table. It is the known strongest non metal. It never gains a positive oxidation state. The corresponding acid, HF, is a weak acid. Fluorine reacts with almost all other elements and destroy many of the organic compounds forming carbon tetrafluoride and hydrogen fluoride.
The atomic number of fluorine is 9. Therefore its outermost shell contain 7 electrons and hence its valency (oxidation state) is -1.Hence fluorine will take part in chemical reactions by accepting 1 electron to complete its octet. So it forms negative ion F- .Added:Actually this is the only possible ion form of fluorine, being the most electronegative element of all. Positive ions are impossible.
-2 oxidation state
An element exhibits a positive oxidation state when it is bonded to a more electronegative element. Fluorine is the most electronegative of all the elements. But what if fluorine bonds with extremely elecronegative oxygen and nitrogen ligands like -OCF3, -OTeF5, -OIO2F2, -N(SO2CF3)2, -N3, -N5(pentazole ligand) etc.? eg: F-OTeF5
fluorine
oxidation state of Fluorine is always -1.
FClO4 is the name of Fluorine perchlorate.Here Chlorine is in +7 oxidation state, Fluorine is in -1 oxidation state, 3 atoms of Oxygen (that are double bonded to Chlorine) are in -2 oxidation state, and the forth Oxygen atom (which is connected to Fluorine and Chlorine) is in 0 oxidation state.So, total charge = 7(of Chlorine) -1(of Fluorine) -(2 * 3)(of 3 Oxygen) +0(of Fourth Oxygen) = 0
HF
Fluorine is a highly electronegative compound, and combines with numerous elements to form compounds with the fluorine in -I oxidation state.
To calculate the oxidation state of fluorine in O2F2, first draw a diagram of the molecule: F-O-O-F Determine the most electronegative atom(s), which are fluorines -- the most electronegative atom there is. Being in the group 7A, a fluoride ion would gain an electron to a -1 charge, so each has an oxidation number of -1. The oxygens, therefore, have an oxidation number of +1 each.
Fluorine is located in period 2 and group 17 in the periodic table. It is the known strongest non metal. It never gains a positive oxidation state. The corresponding acid, HF, is a weak acid. Fluorine reacts with almost all other elements and destroy many of the organic compounds forming carbon tetrafluoride and hydrogen fluoride.
Metals form cations and have positive oxidation states.
Under normal conditions, +2 is cadmium's only positive oxidation state.
HFO2 is fluorous acid, though it is purely a hypothetic compound with fluorine in the impossible oxidation state for fluorine of +3!The simplest acid with fluorine in it is the common HF (liquid/gas, Bp. 19.5oC) called: hydrofluoric acid or hydrogen fluoride (oxidation state +1).
In all its compounds, fluorine has an oxidation number of -1. In its diatomic molecular form that is stable at standard temperature and pressure, fluorine is considered to have an oxidation state of 0. Mathematically, -1 is less than 0.