Oxidation state of Oxygen in:
Peroxides is -1
Superoxides is - 1/2
In compounds, magnesium has a +2 oxidation state; in most but not quite all compounds, oxygen has a -2 oxidation state. In peroxides, oxygen has a -1 oxidation state. In oxygen fluorides, oxygen has positive oxidation states.
As with any element, the oxidation state of oxygen is 0 in its elemental form.
In this ion the oxidation state of sulfur is 6+ and the oxidation state of each oxygen is 2-
The oxidation state of oxygen in O2PtF6 is zero. In a molecule of O2, the oxidation state of each oxygen atom is -2. Additionally, the compound PtF6 has a +6 charge, so the two oxygen atoms in O2PtF6 must have an oxidation state of zero to balance the overall charge of the compound.
O = -2 oxidation state H = +1 oxidation state
In most compounds oxygen will have an oxidation state of -2. The only exceptions are peroxides (-1), superoxides (-1/2), and compounds in which oxygen bonds with fluorine (+1 or +2).
the answer is -2.Related Information:The oxidation number of oxygen when it appears as an element is 0. The oxidation number in all compounds but peroxides is -2. The oxidation number of oxygen in peroxides is -1.
In terms of ionic compounds an oxide contain the oxide ion (O2-) Which is a single oxygen atom with a 2- charge. A peroxide contains the peroxide ion (O22-) which is a particle of two oxygen atoms bonded together and has a 2- charge. Unlike most normal oxides, peroxides tend to be oxidizers or at the very least, unstable. A superoxide contains the superoxide ion (O2-) which consists of two oxygen atoms bonded together and has a 1- charge. This ion is even more strongly oxidizing than the peroxide ion. In covalent compounds oxides are substances that contain oxygen in the 2- oxidation state and not bonded ot other oxygen atoms. Peroxide contain a peroxide group (O2) in which each oxygen atom is bonded to the other oxygen an to another atom, typically carbon or hydrogen. IN this case oxygen is in the 1- oxidation state.
The oxidation number of an element depend on another element it react with to form a compound e.g manganese(iv)oxide mno4 the oxidation number of oxygen there is four while the oxidation number of manganse is 7 in most radox reaction the oxidation number of oxygen is usually 4 when writing the full equation
O standing for oxygen can have multiple oxidation numbers depending on what it is bonded to, in most cases it has a negative 2 oxidation number but in certain cases like peroxides it can have a negative 1 oxidation state.
In compounds, magnesium has a +2 oxidation state; in most but not quite all compounds, oxygen has a -2 oxidation state. In peroxides, oxygen has a -1 oxidation state. In oxygen fluorides, oxygen has positive oxidation states.
The oxidation number of chlorine is -1 in most states but it can be altered in certain compounds.
-1. In simple inorganic compounds other than peroxides and superoxides, oxygen almost always has an oxidation number of -2, but since calcium cations always have an oxidation number of +2, in this compound, the two oxygen atoms must have only -1 charge each. This compound is calcium peroxide, one of the exceptions noted above.
Oxidation is one part of a redox reaction, where redox stands for reduction-oxidation. Oxidation is the loss of electrons or an increase in oxidation state by a molecule, atom, or ion. It need not involve any oxygen and the question is too underspecified to have a sensible answer.
Oxygen usually has an oxidation state of -2.
The oxidation state of oxygen in the compound is -2.
The oxidation state for oxygen in the oxide ion (O2-) is -2. Oxygen typically has an oxidation state of -2 in most of its compounds.