Introduction
For this Module, I chose to explain and elucidate the topic, “Oxidation-Reduction Reaction” also known as Red-Ox Reaction not just because it is required for us to elaborate the most complicated matter for us, but also for the reason that I wanted to improve my understanding and comprehension regarding this topic. I really had a difficult time especially during assessments because I wasn’t a hundred percent sure that my answers were correct—I even had questions left out unanswered. I reflected on what I must do. Gladly, our teacher thought of this so that we can help ourselves by looking back at the topic and, slowly and surely understand it again step by step.
I believe that creating a module like this one wouldn’t be as easy
…show more content…
The Red-Ox Reaction is essential to some occurrences in life such as respiration, corrosion and photosynthesis. But first, let’s describe first what is Reduction. Reduction is the process of gaining an electron and decrease of oxidation state occurs. It’s somehow confusing right? Remember that the LOWER the Oxidation State, the HIGHER number or electrons there are, meaning, more negative means more electrons [1]. On the other hand, Oxidation is the process of losing an electron and increase in oxidation state take place [1]. Always keep in mind the statement I stated regarding Electrons and Oxidation state. There are some Reduction Oxidation Reactions Articles that say that other factors can cause Red- Ox reaction such as Oxygen transfer, Hydrogen transfer. Let’s talk a little bit about Oxygen Transfer. When a compound gains Oxygen, it is called Oxidation, it is easy o remember since the “OXI” in Oxidation is similar to the “OXY” in Oxygen. On the other hand, when a compound loses Oxygen, it is called Reduction.[2] Example: [3] Extraction of iron from its ore: Fe2O3 + 3CO 2Fe + …show more content…
The 3CO gained Oxygen, therefore undergoes Oxidation. The CH3CH2OH lost Hydrogen, therefore undergoes Oxidation. The CH3CHO gained Hydrogen, therefore undergoes Reduction.
Lastly, is the electron transfer, This is where I will focus because this was the one taught to us. The two topics a while ago were just examples of other Oxidation Reduction Reaction. In Electron Transfer, Remember the same mnemonics “OIL RIG” because in Electron Transfer, Oxidation is loss of electrons, while of course, Reduction is gain of electrons.[2] Example: [6]
Cu2+ + Mg Cu + Mg2+
B. Solving for the Oxidation
A part of the Red-Ox Reaction is the Half- Reaction. It can either be Reduction or Oxidation. We can now that Half Reaction occurred when there is a change in the Oxidation State. Oxidation State/ Number is the number allotted to an element in chemical combination that corresponds to the number of electrons lost-- gained, if the number is negative, by an atom of that element in the compound. [7]
So, now, let us find out how to get the oxidation number of an element.
Example: [8]
Na2SO4
How do we find for S?
When the flame was blown out and the glowing wooden splint was placed halfway into the test tube containing H2O2 and MnO2 crystals, the splint reignited and caught flame once again. This demonstrates the decomposition of H2O2 into water and hydrogen. MnO2 is a catalyst that increases the rate at which H2O2 decomposes. Adding oxygen to a fire will cause it to burn faster and hotter and the oxygen rich test tube allowed the splint to reignite.
3. Pyruvate is converted in two steps; firstly pyruvate releases CO₂ which is converted to acetaldehyde. Then secondly acetaldehyde is reduced by NADH to ethanol.
“Chemistry is the study of substances; their properties, structure, and the changes they undergo” (Lower). Chemistry is the study of all the stuff in the world and especially how they change. My experiment deals mostly with the change of substances. Some of the concepts involved in my experiment are Oxidation/Reduction (redox) reactions, electrolysis, pH, and electrical currents. A redox reaction is a reaction in which there is a transfer of electrons from one substance to another. There are two paired parts to a redox reaction: the oxidation and the reduction. The oxidation is the loss of electrons while the reduction is the gain of electrons. They always occur together because one substance has to receive the electrons that another substance is giving up. Electrolysis is a process where electricity goes through a liquid, which causes chemical reactions to occur. pH is the measure of how acidic or basic something is. More exactly, it is, at least indirectly, the number of hydrogen ions there are in a liter of solution. A hydrogen ion is a hydroge...
The Effect of Changing the Concentration of the Enzyme Catalyst on the Rate of Reaction on Hydrogen Peroxide Planning -------- Hydrogen Peroxide Water + Oxygen 2H2O2 2H2O + O2 Introduction - Background Information ------------------------------------- To help me understand what a chemical reaction is or involves I did some research. A chemical reaction is a process by which atoms or groups of atoms are redistributed, resulting in a change in the molecular composition of substances.
The purpose of this lab was to to cycle solid copper through a series of chemical forms and return it to its original form. A specific quantity of copper undergo many types of reactions and went through its whole cycle, then returned to its solid copper to be weighted. We observed 5 chemical reactions involving copper which are: Redox reaction (which includes all chemical reactions in which atoms have their oxidation state changed), double displacement reaction, precipitation reaction, decomposition reaction, and single displacement reaction.
For example, what are the names of Fe2O3 and FeO. Iron oxide is not an adequate answer; it fails to distinguish between the two possible oxidation states of iron. Is it iron (II) or iron (III). To decide, you must know use the combination of the oxide's fixed oxidation state of 2- with iron's oxidation state required to total for a compound charge of zero. The compound iron(II) oxide, FeO, iron had the oxidation state of 2+ which balances the charge of the oxide ion which is 2-. For the compound iron(III) oxide, Fe2O3, the roman numeral placed after the name of the metal clearly states the charge of each iron atom as 3+. The older system of naming applies either the suffixes —ic for the ion of higher charge and —ous for the ion of lower charge; thus Fe3+ ion can be referred to as ferric and Fe2+ ion as ferrous.
... the reaction to shift to the right would be to remove products. A third way is to change the temperature. Since this is an endothermic reaction, +∆H, we can imagine that “heat” is a reactant. Thus, if we add heat, it will shift to the right. To be classified as a redox reaction, we need at least two elements to change oxidation states. The easiest way to look at a reaction and determine this is if you have an element by itself on one side of the reaction and it is in a compound on the other side. Most of the time, the oxidation number of each element in a compound is their common charge. The sum of oxidation numbers must equal the compounds overall charge. Elements in the natural state (by themselves) have an oxidation number of 0. The reducing agent is the species responsible for reducing the other chemical. Therefore, the reducing agent is oxidized itself.
by the amount of C02 produced by the reaction or by the amount of 02 consumed.
Oxidation-reduction reactions can be used to stereochemically control and produce many different organic molecules. The oxidation step in this process increases the number of carbon oxygen bonds by losing a hydrogen and breaking that bond. Through the reduction step, carbon-oxygen bond is broken and the hydrogen is returned.
== CaCO3(s) + 2HCC(l) CaCl2 (aq) + H2O(l) + CO2. = =
Smith, Roland. Conquering Chemsitry: HSC course. 4th ed. Vol. 1. N/A: Cengage Learning Australia, 2010. 74-90. 1 vols. Print.
The purpose of the experiment is to identify and understand reactions under kinetic and thermodynamic control. A reaction under kinetic and thermodynamic control can form two different types of products. A reaction under kinetic control is known to be irreversible and the product is formed quickly. A reaction under thermodynamic control is known to require rigorous conditions. It is also reversible. The final product is more stable than the product made by kinetic control. The chart below shows the two types of reaction coordinates:
This equation also shows fermentation process, which proves an anaerobic respiration, which means that oxygen is absent from the process. Anaerobic respiration takes place in organisms and releases a small amount of energy very quickly. In most organisms, it consists of a chain of chemical reactions called glycolysis, which break down glucose into pyrutic acid.
To control the rates of chemical reactions is imperative to the continued existence of our species. Controlled chemical reactions allow us to move forward in society, constantly. We find new ways to provide light and heat our homes, cook our food, and pursue in crafts that benefit our society. There are, however, just as there are advantages, disadvantages to the efficiency of controlling the rate of reactions, which in some cases can be fatal to our scientific development and progression. The growth of humankind necessitates that we must be able to control the rate of chemical reactions.