Oxidation reactions just involve a transfer of electrons, the only reason it's called oxidation is because oxygen is commonly used in those reactions. There are lots of reduction and oxidation reactions that occur without oxygen.
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.
A redox reaction involves the transfer of electrons between species, leading to changes in oxidation states. While a single-displacement reaction involves one element being replaced by another in a compound, it may not always involve electron transfer. For example, if the displacement does not result in a change in oxidation states, the reaction would not be classified as a redox reaction. Therefore, while all redox reactions can be single-displacement reactions, not all single-displacement reactions qualify as redox reactions.
No, oxidation does not always turn something into a gas. Oxidation is a chemical reaction in which a substance loses electrons, leading to a change in its chemical composition. This process can result in various outcomes, such as the formation of a gas, solid, or solution.
the oxidation states are always 0 for both atoms
Because standard potential is not an additive property. That is, the standard potential for a reaction will always been a certain value, no matter if you have one mol or a billion mols. Each mol has the same potential and undergoes the reaction independent of all the other mols.
Removing oxygen does prevent oxidation from occurring since oxidation is a chemical reaction that involves the gain of oxygen by a substance. Without oxygen present, oxidation cannot take place.
The combination of two elements (a metal and a nonmetal) is always a redox reaction.
oxygen, redox
Redox or oxidation-reduction reactions.
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.
A redox reaction involves the transfer of electrons between species, leading to changes in oxidation states. While a single-displacement reaction involves one element being replaced by another in a compound, it may not always involve electron transfer. For example, if the displacement does not result in a change in oxidation states, the reaction would not be classified as a redox reaction. Therefore, while all redox reactions can be single-displacement reactions, not all single-displacement reactions qualify as redox reactions.
Oxidation is an element or an ion getting a positive charge by removing valence electrons and Reduction is an element or an ion getting a negative charge by gaining free electrons. In chemical reactions reduction occurs by gaining the free electrons emitted by oxidation. Therefor oxidation and reduction proceed simultaneously.Oxidation is an element or an ion getting a positive charge by removing valence electrons and Reduction is an element or an ion getting a negative charge by gaining free electrons. In chemical reactions reduction occurs by gaining the free electrons emitted by oxidation. Therefor oxidation and reduction proceed simultaneously.
They must always occur in the same reaction; if one element or compound is oxidized, another one must be reduced.
It is always found in the oxidation state of 0
No, oxidation does not always turn something into a gas. Oxidation is a chemical reaction in which a substance loses electrons, leading to a change in its chemical composition. This process can result in various outcomes, such as the formation of a gas, solid, or solution.
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.
The oxidation number of S in S8 is ZERO!