Because for oxidation to take place the electrons lost by the substance that is oxidized must be accepted by atoms or ions of another substance.
Also, for reduction to occur the electrons gained by the substance that is being reduced must be transferred from the atoms of ions of another substance.
Therefore, oxidation and reduction are complementary processes: that is to say that oxidation cannot occur without reduction and visa versus.
Oxidation is the chemical process that must always accompany a reduction process, as they occur simultaneously in a redox reaction where electrons are exchanged between reactants.
If one substance is losing electrons (where it is gaining charge, or oxidizing), we must assume those electrons are going to another substance in the reaction, which will cause the charge to go down, or reduce. This type of equation is called a Redox (reduction-oxidation) reaction.
It's not entirely clear what the question is asking... but oxidation involves the loss of electrons from an atom or ion, and reduction involves the gain of electrons. The other parts of a redox (reduction-oxidation) reaction may involve atoms forming and breaking bonds, but the oxidation or reduction part is just about losing or gaining electrons. You might be talking about what is called a "half-reaction." A half-reaction is the part of the reaction that is only either the oxidation step or the reduction step. Neither is a complete reaction, but put together the two half-reactions give the overall reactions. In the oxidation half-reaction, electrons come out as products, and in the reduction half-reaction electrons go in as reactants. Remember: OIL RIG Oxidation Is Loss; Reduction Is Gain.
Zero. The oxidation of one compound must be matched by the reduction of another.
Ioding when combined in a compound is usually combined as the iodide. Iodide ions are negatively charged (ie each ion has an extra electron compared with an iodine atom). When elemental iodine is liberated, iodine atoms are formed from these ions which in turn pair up to form iodine molecules. When an Iodine ion changes into an atom it must lose the extra electron. From the acronym 'OILRIG' (Oxidation Is Loss of electrons, Reduction Is Gain of electrons) it is clear that as the elemental iodine has formed because of the loss of an electron the process must involve oxidation.
Oxidation is the chemical process that must always accompany a reduction process, as they occur simultaneously in a redox reaction where electrons are exchanged between reactants.
Oxidation is characterized by the loss of electrons, and reduction is characterized by the gain of electrons. Since there must be an electron loser and an electron receiver, oxidation and reduction are always complimentary.
Yes, an element can undergo both oxidation and reduction in the same reaction. The reaction between Zinc and Copper Sulphate is a perfect example. This type of reaction is called a redox reaction.
They must always occur in the same reaction; if one element or compound is oxidized, another one must be reduced.
what must be present for oxidation-reduction to occur?
It is not mandatory; acids are also titrated.
If one substance is losing electrons (where it is gaining charge, or oxidizing), we must assume those electrons are going to another substance in the reaction, which will cause the charge to go down, or reduce. This type of equation is called a Redox (reduction-oxidation) reaction.
oxidation-reduction reaction
It's not entirely clear what the question is asking... but oxidation involves the loss of electrons from an atom or ion, and reduction involves the gain of electrons. The other parts of a redox (reduction-oxidation) reaction may involve atoms forming and breaking bonds, but the oxidation or reduction part is just about losing or gaining electrons. You might be talking about what is called a "half-reaction." A half-reaction is the part of the reaction that is only either the oxidation step or the reduction step. Neither is a complete reaction, but put together the two half-reactions give the overall reactions. In the oxidation half-reaction, electrons come out as products, and in the reduction half-reaction electrons go in as reactants. Remember: OIL RIG Oxidation Is Loss; Reduction Is Gain.
Redox. You can't have the re without the dox, or is that ox without the red? You can't throw away electrons, nor will electrons pop out of thin air.Oxidation is the loss of electrons, reduction is the gain of electrons. In order for one atom to lose electrons another atom must gain them. Hence, reduction must be accompanied by oxidation and vice versa.
Zero. The oxidation of one compound must be matched by the reduction of another.
Ioding when combined in a compound is usually combined as the iodide. Iodide ions are negatively charged (ie each ion has an extra electron compared with an iodine atom). When elemental iodine is liberated, iodine atoms are formed from these ions which in turn pair up to form iodine molecules. When an Iodine ion changes into an atom it must lose the extra electron. From the acronym 'OILRIG' (Oxidation Is Loss of electrons, Reduction Is Gain of electrons) it is clear that as the elemental iodine has formed because of the loss of an electron the process must involve oxidation.