-3
Hydrogen takes +I and fluorine takes -I oxidation states in hydrogen fluoride.
No. Fluorine has only two oxidation states. 0 in F2 and -1 in fluoride ion
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
1. NH4Cl is an electrically neutral compound, so the sum of the oxidation states must be zero. 2. Nitrogen is a Group 5 element and is assigned an oxidation state of -3. 3. In its covalent compounds with nonmetals, hydrogen is assigned an oxidation state of +1. There are 4 hydrogen atoms, so contributes a charge of +4. 4. The oxidation state of a monatomic ion is the same as its charge. As a Group 7 element, chlorine is assigned an oxidation state of -1. 5. Adding up the oxidation states, -3, +4, -1, gives an overall charge of 0.
Ox(N)= -3
Hydrogen takes +I and fluorine takes -I oxidation states in hydrogen fluoride.
No. HNO3 already has hydrogen and nitrogen in their highest possible oxidation states.
No. Fluorine has only two oxidation states. 0 in F2 and -1 in fluoride ion
Hydrogen, Nitrogen, Oxygen, Fluorine, Chlorine, Bromine, and Iodine are all diatomic in their natural states.
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
It has a range of oxidation states from -3 to +5
1. NH4Cl is an electrically neutral compound, so the sum of the oxidation states must be zero. 2. Nitrogen is a Group 5 element and is assigned an oxidation state of -3. 3. In its covalent compounds with nonmetals, hydrogen is assigned an oxidation state of +1. There are 4 hydrogen atoms, so contributes a charge of +4. 4. The oxidation state of a monatomic ion is the same as its charge. As a Group 7 element, chlorine is assigned an oxidation state of -1. 5. Adding up the oxidation states, -3, +4, -1, gives an overall charge of 0.
Ox(N)= -3
Ca & Mg
-3, -2, -1, 0, 1, 2, 3, 4 and 5 oxidation states
O = -2 oxidation state H = +1 oxidation state
The size of oxygen is bigger than fluorine therefore has the ability to stabilized higher oxidation state.