Why is Oxygen a negative 1 charge (anion) in Hydrogen Peroxide?

Question

In H2O2, the Oxygen has an ion of 1-, why???

Please help.

Answer 1

This is because the oxidisation number for hydrogen is always +1.
Hydrogen ions are monatomic ions and according the the rules of assigning oxidation numbers, the oxidation number of monatomic ions equals the charge of the ions.

Now why oxygen is negative 1
Any complete molecule (not ions) must have a charge of 0.
Hydrogen ions have a charge and oxidation number of +1 and because there is two of them, the charge is +2. For the molecule to be 0, we need 2 ions of oxygen and they need to have an oxidisation number of -1.
H+H+O+O=0
+1+1-1-1 = 0

Therefore, oxygen has an oxidation number of -1.

Answer 2

Peroxide Anion

Answer 3

This Site Might Help You.

RE:
Why is Oxygen a negative 1 charge (anion) in Hydrogen Peroxide?
In H2O2, the Oxygen has an ion of 1-, why???

Please help.

Answer 4

H2o2 Charge

Answer 5

I love Tigresses answer. Just remember that the structure of H2O2 is H-0-0-H

Answer 6

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Oxidation state of an element in a combined state can be calculated as follows: 1. The O.S. of an atom in elemental form (whether uncombined, or combined, say H2), is always zero. The O.S. of ANY atom in uncombined state is always zero. 2. The algebraic sum of the oxidation states of the atoms in a neutral compound is zero. 3. the algebraic sum of the oxidation states of all the atoms in an ion will be equal to the charge of that ion. 4. Except in metal hydrides( say LiH or NaH), Hydrogen will always show +1 O.S. 5. In case of oxygen, O.S. will be -2 in case of oxides (say water), -1 in case of peroxide ( saya hydrogen peroxide, H2O2), or -0.5 in case of superoxide (say potassium superoxide, KO2). In compounds with fluorine, it assumes +2 O.S (Say OF2) or +1 (say O2F2, dioxygen difluoride), this is due to higher electronegativity of Fluorine. 6. In interhalogen compounds, the more electronegative halogen will have the negative O.S. Eg in IF7, Iodine has O.S. +7 and F has -1. 7. One covalent bond will always contribute for one O.S. and similarly two covalent bond will always contribute for two O.S and so on for three. 8. The more electronegative element in the covalent bond gets negative O.S. for that bond and vice-versa. 9. If the covalent bond is present in between the same electronegative elements or the same element, the contribution of the O.S. is zero. 10. If a co-ordinate bond is present between the two atoms, then the contribution of O.S. for that bond is 2 if and only if the the co-ordinate bond is from less electronegative to more electronegative element. Otherwise, it is zero. The most important concept is that O.S. is not a property of the element, but of a particular atom bonded in a particular way in a particular atom. Now, let us discuss your queries. 3. BrCl Look at Rule 6. Your answer is correct. 5. OF2 Check Rule 5. Your answer is correct. 6.S8 Check Rule 9. Your answer is correct. 7. Mg In uncombined state, the O.S. of any element is zero. Rule 1. 8. K2W4O13 Correct. 11. C60 Check Rule 9. Your answer is correct. 13. NbOF6 ^3- Correct. Polyatomic is any species which contains multiple atoms. Monoatomic species has only one atom in their molecule, for example, inert gases. Diatomic ones include H2, O2, N2 etc. Triatomic ones are O3, H2O etc. Tetratomic ones are NH3, PH3 etc. Technically, all species having more than 2 atoms are taken as polyatomic. All metallic ions are cations, but the converse is not true. A cation is any species which has lost one or more electrons from its valence shell. As metals have greater tendency to lose these electrons, they form cations readily. Anion are those which accept electrons in their valence shell, halides form anions easily. It is not necessary that other elements cannot form cations or anions. Hypothetically, all elements can form cations or anions. Due to energy loss or gain, some have relatively higher tendency to lose electron and form cation and some want to form anions, to attain stable electronic configuration of the nearest inert gas in the periodic table. That's all. O.S. of transition metals can be calculated in the same way as before. There is no set value of O.S. for transition metals, it varies from compound to compound. For example, manganese will take O.S. +7 in KMnO4, +4 in MnO2 and even +2. These form very interesting portions of inorganic chemistry. In the Mendeleev periodic table (with 8 groups), the group number indicates the number of valence electrons supposed to be in the valence shell of an element. If you are really interested, i would suggest that you go for good books, and read them thoroughly. Inorganic Chemistry by J.D. Lee is the best for inorganic, I.L. Finar is the bible of Organic Chemistry and Maron-Prutton is quite good for physical chemistry. Of course, these are books meant for higher levels, so you should get the concepts right from other good books before you can enjoy the detailed analysis in these wonderful books. CHemistry Cube (chemistry3) by OUP is also a fantastic book.