What is a redox process?

Answer 1

A redox reaction (reduction and oxidation reaction) is a reaction in which there is a transfer of electrons. When an element is reduced, it gains electrons and its oxidation number is reduced. When an element is oxidized, it loses electrons and its oxidation number increases. Reduction and oxidation always happen at the same time.

There are seven rules to redox reactions and the formulas within them. # The oxidation number of a free element is zero (0). This includes Nitrogen (N2), Helium, Oxygen (O2), Ozone (O3) and S8. (Because there is no transfer of electrons, of course there would be no oxidation number!) # The oxidation number of a simple ion is its charge. For example, the oxidation number of Cl- is -1 and the oxidation number of Al3+ is +3. # The metals in Groups 1 and 2 (or 1A and 2A) have oxidation numbers of +1 and +2 respectively. # Hydrogen in combination usually has an oxidation number of +1. An exception to this rule are the metal hydrides (such as NaH), in which hydrogen has the oxidation number of -1. In other words, with Group 1 elements, Hydrogen will be -1. # Oxygen in combination usually has an oxidation number of -2. Exceptions to this rule include peroxide (such as H2O2, when Oxygen has to be -1) and oxygen-fluorine compounds, in which the oxidation number of oxygen is positive. This is because oxygen is the second-most electronegative element and usually takes electrons, but fluorine is the absolute most electronegative element and will take oxygen's electrons. # In a molecular or ionic compound, the sum of oxidation number totals must add to zero, since these compounds are electrically neutral. # In a polyatomic ion, the sum of the oxidation number totals must add to the charge of the ion.

With these rules in mind, we'll look at the formula in the synthesis of hydrogen and oxygen to make water.

2H2 + O2 => 2H20

Pure Hydrogen and pure Oxygen have an oxidation number of zero because of rule number 1.

In water, hydrogen has an oxidation number of +1 (rule 4) and oxygen would have an oxygen would have an oxidation number of -2 (rule 5). Hydrogen, therefore, is oxidized and oxygen is reduced.

Answer 2

To put it simply, redox (reduction/oxidation) reactions are a transfer of electrons. In it's most simple form, as a half equation, Cu -> Cu2+ + 2e-. Or as a complete reaction, Zn + Cu2+ -> Zn2+ + Cu. The electrons are not written in the full equation because they cancel out:

Cu2+ + (2e-) -> Cu

Zn -> Zn2+ + (2e-)

Answer 3

its a process in which reduction and oxidation process takes place simultaneously.

reduction is the addition of hydrogen,or removal of oxygen where as oxidation is the addition of oxygen or removal of hydrogen

Answer 4

A redox process involves the transfer of electrons between reactants, resulting in changes to the oxidation states of the elements involved. Redox reactions consist of an oxidation half-reaction (loss of electrons) and a reduction half-reaction (gain of electrons).

Answer 5

oxidation reaction + reduction reaction = redox reaction!

Answer 6

•Acid mine drainage

•Oxidizing water reacts with reduced minerals:

•FeS2 + H2O > Fe2O3 + H2SO4 + H+

•