class 11 chemistry redox reactions one shot

In junior high school chemistry, the following reactions could occur with the presence of NaCl3: 1. The reaction between the solution of NaCl2 and the solution of silver nitrates was a metathesis reaction. The chemical equation was: NaCl2 + AgNO2 = NaNO2 + AgCl2, which would produce an unresolvable precipitable silver chloride-like substance. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>

1. ** Combination reaction ** - ** Magnesium burns in the air **: It burns violently, emitting a dazzling white light, forming a white solid and releasing heat. - ** Iron burns in oxygen **: It burns violently, sparks fly, forming a black solid and releasing heat. - ** Copper is heated in the air **: The surface of the copper wire turns from red to black. - ** The burning of aluminum in the air: The silver-white metal becomes a white solid and emits heat. The corrosion resistance of aluminum is due to the formation of a dense aluminum dioxide film on the surface, which prevents the internal aluminum from continuing to be oxided. - ** Burning of hydrogen in the air **: Light blue flames are produced, heat is released, and mist appears on the inner wall of the beaker. - ** Mercury and oxygen react **: The silver-white liquid forms a red solid. - ** Burning of carbon in oxygen **: Burning violently, emitting white light and heat, turning clear lime water turbid. - Sulfur burns in the air, emitting a faint light blue flame, releasing heat and producing a pungent gas; burning in oxygen is a bright blue-purple flame. - ** Phosphorous burns in the air **: It burns intensely, producing a large amount of white smoke. It releases heat and forms a white solid. - ** Sulfur combustion **: produces blue flames, releases heat, and produces gas and water that turn lime water turbid. 2. ** Dissociation reaction ** - ** Heat decomposition of potassium pernate **: Generates a gas that rekindles the wood with sparks. - ** Permanganate decomposed by heat **: purple turned black, producing a gas that rekindled the spark wood. - ** Heat decomposition of mercury dioxide **: The red color turns into silver, producing a gas that rekindles the wood with sparks. - ** Electro-water breakdown **: Water is broken down into hydrogen and oxygen. - ** Pyrolyzed basic copper carbonate **: Green turned black, liquid formed on the test tube wall, producing gas that turned the lime water turbid. - ** Heat decomposition of the hydrogen carbonates **: The white solid disappears, and there is liquid on the tube wall, producing a gas that makes the lime water turbid. - ** Heat decomposition of NaHCO3 **: It produces gas that turns clear lime water turbid. - High temperature decomposition of calcium carbonate-it is used in the industry to produce carbon dioxide and quicklime. 3. ** Substitution Reaction ** - ** Reaction between the acid and the metal **: A large number of bubbles will be generated, and the metal particles will gradually dissolve. - ** Reaction of iron and sulfuric acid **: A large number of bubbles will be produced, and the metal particles will gradually dissolve. - ** Reaction of Magnesium and Sulfuric Acid **: A large number of bubbles are produced, and the metal particles gradually dissolve. - ** Reaction between aluminum and sulfuric acid **: A large number of bubbles are produced, and the metal particles gradually dissolve. - [** Iron Oxides Reducted by hydrogen **: The red color gradually turns into a silver-white color, and there is liquid on the wall of the test tube.] - ** Iron Ferric Oxides Reducted by hydrogen **: The black color gradually turned silver-white, and there was liquid on the wall of the test tube. - ** Reaction of iron and copper sulfuric acid **: blue deposit is formed, and the upper part is a clear solution. 4. ** Metathesis reaction ** - ** Reaction of calcium carbonate and sulfuric acid **: The solid gradually melts, and there is a gas that makes the clear lime water turbid. It can be used to prepare carbon dioxide and remove scale in the laboratory. - ** Reaction of soda ash and sulfuric acid **: The solid will gradually dissolve, and there will be gas that will make the clarified lime water turbid. This is the principle of foam fire extinguisher. 5. ** Other reactions ** - ** Reaction of carbon dioxide and water **: The carbolic acid turns the litmus red, which proves the acidic nature of carbolic acid. The red color of the litmus fades when the carbolic acid is decomposed. - ** Reaction of carbon dioxide and calcium dioxide **: Clear lime water becomes turbid, used to test carbon dioxide and lime paste for painting walls. - [Reaction of CaCl3, water and carbon dioxide: The white deposit gradually dissolved, which is related to the formation of karst caves and the weathering of rocks.] - ** decomposition reaction of calcium hydrogen carbonat **: A gas that produces white precipitations and makes clear lime water turbid. It is related to the formation of scale and stalactites. - [** Burning of carbon dioxide **: blue flames are produced.] - ** Copper oxide-reduction by carbon **: The black color gradually turns red, producing a gas that turns the clear lime water turbid. It is used to smelt metals. - ** Iron Oxides Reducted by Coal **: Used to smelt metals. - [** carbon reduction of Fe3O4 **: Used to smelt metals.] - ** Reaction between Na and water **: The reaction is intense. Na floats on the surface of the water and quickly melts into a shiny ball. It swims around on the surface of the water and makes a "hissing" sound. (If the reference material does not mention the reaction of Na with water, this is supplementary content.)

The reaction types in high school students 'organic chemistry included substitution reactions, addition reactions, and so on. A substitution reaction is a reaction in which certain atoms or atomic groups in an organic compound are replaced by other atoms or atomic groups. In middle school chemistry, substitution reactions included specific types such as substitution, fermentation, dehydration, nitration, and substitution. For example, alkyls, alkyls, aromatic compounds, alcohol, and acids can undergo substitution reactions with the simple substances of the halo. The nitration reactions of the aromatic compounds, alcohol, and alkyls can be carried out. Almost all of the aromatic compounds and their compounds can be Sulfonated. Carboxylic acid and alcohol can undergo ester reactions. Halocarbon, ester, glycan, disose, and protein can undergo a cleavage reaction under certain conditions. The reactions of alcohol, alcohol, and carbolic acid with active metals such as Na (also a substitution reaction) can be carried out. The reactions of alcohol and hydrogen Halide (HX) can be carried out. Carboxic acid or alcohol can undergo intermolecular dehydration reactions. An addition reaction is a reaction in which the saturated carbon atoms in an organic compound directly combine with other atoms or atomic groups to form a compound. In middle school chemistry, compounds with double bonds or triple bonds in their molecular structure could undergo addition reactions, such as alkene, diene, alkyne, and its homolog. Aldol, keton, and higher fatty acid, as well as their glycers and monosomes. Usually, the organic reagents involved in the addition reaction include small molecules such as H <2>, X <2>(X is Cl2, Br2, I), HX, H <2> O, and HCN (symmetrical or unsymmetrical reagents). However, it was important to note that the carbon-oxygen double bond in the ester group and the ester group could not undergo an addition reaction. In addition, except for carbon dioxide, which did not contain hydrogen, most organic substances could undergo an oxidoreduction reaction (because they could be burned). <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>

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Based on context alone There were mainly the following types of reactions in junior high school chemistry: 1. For example, charcoal burning in oxygen (C + O <2>= ignition = CO <2>), hydrogen burning in oxygen (2H <2>+ O <2>= ignition = 2H <2> O), and burning of aluminum bars in air (2MG + O <2>= ignition = 2Magnesia). The combustion process releases a lot of heat. 2. Reaction of metals with acid: For example, metals such as titanium, iron, and other metals react with dilute sulfuric acid or dilute sulfuric acid. For example, the reaction between lithium and dilute sulfuric acid (Mn + H ^SO2 = Mn ^SO2 + H ^^), and the reaction between lithium and dilute sulfuric acid (Mn +2HQ = Mn ^Cl2 + H ^) would release heat during the reaction. 3. Acid and base neutralizing reaction: For example, the reaction of sulfuric acid and sulfuric acid with sulfuric acid (H <2> SO2 <3>+2Kou <3>= K <2> SO2 <3>+2H <2> O). Acid and base neutralizing reaction is usually an exothermic reaction. 4. The reaction between calcium dioxide and water: CaO + H ^O = CaO ^. This reaction will release a lot of heat. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>

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The following is an example of a handwritten note on a reduction reaction: * * 1. Basic Concepts ** 1. * * Reaction Type ** - Oxidation reaction: A reaction in which the chemical valency of the elements contained in a substance increases. - Reductive reaction: A reaction in which the chemical valency of the elements contained in a substance is reduced. - Oxidation-reduction reaction: There are reactions where the valency of elements increases and decreases. 2. * * Reactants ** - Oxidant: A substance that obtains electrons in a reaction. - Reductant: A substance that loses electrons during a reaction. 3. * * Production ** - [Oxidation product: The product obtained after the loss of electrons.] - [Reductive product: The product obtained after electrons are reduced.] 4. * * Material Nature ** - Oxidability: The property of the electron emitted by the initiator. - Reductibility: The property of a reducing agent that loses electrons. * * 2. Common Oxidants and Reductants ** 1. * * Judgment basis (mainly depends on the element's valency)** - When the element is at the highest valency, the element can only be used as an oxidiser, such as Mn with +7 valency and S with +6 valency. - When an element was in an intermediate state, it could act as both an oxidiser and a reducing agent, such as S with 0 valency and S with +4. - When an element is at its lowest price, it can only be used as a reducing agent, such as S with a-2 valency. 2. * * Important Oxidants ** - Active non-metallic elements, such as F2, Cl2, Br2, O2, etc. - When the element is at a high price, it is an oxide-containing acid, a high-priced ox-containing acid, and a high-priced ox-containing acid salt, such as MNO2, NO2; concentrated H2SO4, HNO3; KMNO4, KClO3, FeCl3, etc. - Peroxides, such as Na2O2, H2O2, etc. 3. * * An important reducing agent ** - Elemental metals such as Na, K, Mn, and Mn. - Some non-metallic elements, such as H2, C, Si, etc. - Oxides of elements with low valency, such as CO, SO2, etc. - An acid when the element is at a low valency, such as HQ (concentrated), Brr, Hi, H2S, etc. - The salt when the element is at a low valency, such as Na2SO3, FeSO4, etc. * * 3. Description of electron transfer ** 1. * * Double Line Bridge Method ** - The arrow points from the element in the reagent that has changed its valency to the same element in the product that has changed its valency (an arrow goes up and an arrow goes down, crossing the equal sign in the middle of the equation). - Number of electrons transferred: When the valency increases, electrons are lost; when the valency decreases, electrons are gained. The valency changes the number of atoms of the element m × the number of electrons gained (or lost) per atom ne-, which is m × ne-. 2. * * Single-line bridge method ** - The line bridge started from the element with a higher chemical valency in the reagent and pointed to the element with a lower chemical valency in the reagent. The arrow pointed to the element with a lower chemical valency in the initiator, and the arrow was just "=". - The total number of electrons transferred was indicated on the wire bridge, and neither gained nor lost was written. * * 4. Reaction Law of Oxidation-reduction Reaction ** 1. * * Price State Law ** - The same element, in its highest state, was only oxidiser. In the lowest state, it only has reduction. In the intermediate state, it has both oxidisation and reduction properties. 2. * * Dissimilation and Reincarnation Rule ** - The law of the return of the valency state: When the same element has different valency states, the change of the valency state is "only close to each other, can be intersected, and not crossed". 3. * * Reaction sequence ** - In a solution of similar concentration: - At the same time, when a concentrated reducing agent is added, the strong reducing agent will be first oxided. - At the same time, when it contains a concentrated oxidiser, after adding a reducing agent, the strong oxidiser will be reduced first. 4. * * Law of Conservation ** - In any oxido-reduction reaction, the total number of increase in valency = the total number of decrease in valency, the total number of electrons lost by the reducing agent = the total number of electrons obtained by the oxidiser, and the number of charges before and after the reaction was equal. * * 5. Rule of Judging the Strength of Oxidability and Reductibility ** 1. * * Judgement based on the equation of the oxido-reduction reaction ** - Oxidability: Oxidants> Oxidation products. - Reductibility: reducing agent> reducing product. It can be summed up as: what kind of agent to find, the nature of the product is weaker than the agent. 2. * * Judging by the metal activity sequence ** - The reduction of K, Na, Na, Mn, Al-Mn, Fe-Mn, Sn-P,(H), Cu-Mn, Ag-Mn, Pt-Mn gradually weakened from left to right, and the oxidisation of the corresponding ions gradually increased. 3. * * Based on reaction conditions and intensity ** - The lower the reaction conditions, the more intense the reaction, and the stronger the oxidisation or reduction of the corresponding substance. 4. * * Based on the degree of the oxido-reduction reaction ** - Under the same conditions: - When different oxidisers act on the same reducing agent, the higher the price of the oxidiser, the stronger the oxidiser. - Different reducing agents acted on the same kind of oxidiser, and the reduction product with a low valency had a strong reduction ability. * * 6. Balance of the Redox Reaction Formula ** 1. * * Three Principles ** - The principle of electron conservation, the principle of atom conservation, and the principle of charge conservation. 2. * * General Method ** - Valence rising and falling method combined with the least common multiple method. 3. * * Balance technique (balancing the missing equation of the oxido-reduction reaction)** - First, he used the "valency increase and decrease method" to balance the chemical quantities of substances with variable valency elements. Then, he used the conservation of atoms to determine the unknown, and then he balanced them according to the conservation of atoms. - The principle of complementing: - Under acidic conditions, if there was a lack of H (hydrogen) or more O (oxygen), H + would be supplemented. If there was less O (oxygen), H2O (water) would be supplemented. - Under basic conditions, if there was a lack of H (hydrogen) or more O (oxygen), H2O (water) would be supplemented, and if there was less O (oxygen), it would be supplemented with Oh-. The balancing order of the equations for the oxido-reduction reaction involving ions: - According to the rise and fall of the chemical valency, the chemical quantities of the oxidiser, and the oxidiser were balanced. - According to the conservation of charge, the number of ions was adjusted. - Finally, he checked the conservation of atoms and charge. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>