Flame reaction between metal and its compound
Many metals or their compounds would produce a special color when burned. This phenomenon was called the flame color reaction. The flame reaction was a special property of the alkali-earth metals. It was a kind of physical change. In principle, the high-temperature flame caused these substances to be vaporized. The electrons of the metal atoms or compounds were excited by the high-temperature flame to jump to the high-energy level orbit. When the electrons returned from the high-energy level orbit to the low-energy level orbit, they emitted a certain wave length of light according to the energy level difference between the different orbits, so that the metal burning flame presented a characteristic color. During the flame reaction experiment, a clean platinum wire (or iron wire) could be used to burn the color of the metal in the alcohol lamp until the color was the same as before (to avoid the impurities on the platinum wire interfering with the test). Then, the metal wire was dipped in the solution to be tested and burned to observe the characteristic color of the metal in the solution to be tested. To observe the flame color of the potassium element, it had to be observed through a blue-colored tungsten glass to eliminate the interference of the flame color of the potassium element. The flame reaction colors of common metals were: Na yellow, Li purple, K purple, rubidium light purple, calcium brick, Stronghold red, copper green, Ba yellow green. The flame reaction was a property of metal elements, whether it was atoms or ions, but not all elements had a special color. In chemistry, the flame reaction was often used to identify metal elements or metal ions. Based on the principle of the flame reaction, it was applied to fireworks, light lamps, and other aspects of life. Spectral analysis developed from the flame reaction was also used to determine various elements and substances. Read more exciting novels for free
Experimental Report on the Reaction of Metal and Compound Solution
The following is an example of an experimental report on the reaction of a metal and a compound solution: ** 1. Purpose of the experiment ** 1. To explore the law of the reaction between metals and compound solutions. 2. Comparing the order of activity of different metals. ** 2. Experiment Principle ** The more active metal could replace the less active metal from its compound solution. By observing the reaction phenomenon (such as whether there is a new metal separation, the color change of the solution, etc.) to determine whether the reaction occurred, and then determine the order of metal activity. ** 3. Laboratory supplies ** 1. ** Instrument **: Test tube, test tube rack, tweezers, etc. 2. ** Pharmaceuticals **: aluminum sheet, iron sheet, copper sheet, copper sulfuric acid solution, aluminum sulfuric acid solution, silver nitrates solution, etc. ** 4. Experimental Steps ** 1. Reaction of aluminum and copper sulfuric acid solution - He took a test tube and added a suitable amount of copper sulfuric acid solution. - He used a pair of tweezers to pick up a piece of aluminum and put it into the copper sulfuric acid solution. - Observation: There is a red substance on the surface of the aluminum sheet, and the color of the solution gradually lightens. The reaction equation is: 2AI + 3CuSO = Al2 (SO)+ 3Cu. 2. Reaction of iron and copper sulfuric acid solution - He took out another test tube and added the copper sulfuric acid solution. - He used a pair of tweezers to pick up a piece of iron and put it into the solution. - Red substances were observed on the surface of the iron sheet, and the color of the solution became lighter. The reaction equation was: FeSO2 + CuSO2 = FeSO2 + Cu2. 3. Reaction of Copper with Aluminium-Sulphate Solution - He took out a test tube and added the solution. - He placed a piece of copper. - Observed phenomenon: No obvious phenomenon, indicating that copper cannot replace the aluminum in the aluminum sulfuric acid solution, and the mobility of copper is weaker than that of aluminum. 4. Reaction of Copper with Silver Nitrate Solution - He took out a test tube and added the silver nitrates solution. - Put in the copper plate. - A silver-white substance was seen on the surface of the copper plate, and the color of the solution changed. The reaction equation was: Cu + 2AgNO = Cu(NO) 2 + 2AG. ** 5. Experimental results and analysis ** 1. Through the reaction between aluminum and copper sulfuric acid solution, and the reaction between iron and copper sulfuric acid solution, it could be seen that aluminum and iron were more mobile than copper. 2. Copper did not react with the aluminum sulfuric acid solution, further indicating that the mobility of aluminum was stronger than copper. 3. Copper reacted with silver nitrates, which meant that copper was more mobile than silver. Based on the above experimental results, the order of metal activity was as follows: Al > Cu > Ag, Fe > Cu> ** 6. Experiment conclusion ** 1. The order of metal activity affects the reaction between the metal and the compound solution. The more active metal can replace the less active metal. 2. When describing the reaction phenomenon between metal and metal compound solution, it was necessary to pay attention to the attachment of new metal to the surface of the original metal and the change in color of the solution. 3. This kind of reaction must be carried out in a solution. The metal compound must be water-dissolved, and the metal compound that is not water-dissolved generally does not react with the metal. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Experimental Phenomenon of the Reaction between Metal and Compound Solution
When a metal reacted with a compound solution, the following experimental phenomena occurred: 1. For the reaction between metal and metal compound solution: - A more active metal can replace a less active metal from its compound solution. For example, both aluminum and iron could react with a copper sulfuric acid solution. There were two points to note when describing this reaction phenomenon. One was that the replaced metal adhered to the surface of the original metal. For example, if the iron wire was immersed in the copper sulfuric acid solution, the surface of the iron nail immersed in the solution would be covered with a red substance (copper); if the aluminum wire was immersed in the copper sulfuric acid solution, the surface of the aluminum wire immersed in the solution would be covered with a layer of purple-red substance (copper). The second was that the color of the solution would change. For example, when iron reacted with copper sulfuric acid, the solution would gradually turn from blue to light green. This was because the reaction of [FeCuSO4 = CuFeSO4] had occurred, and the resulting solution of iron sulfuric acid was light green. 2. For the reaction between metals and acid solutions, metals such as titanium, aluminum, and iron could react with sulfuric acid and dilute sulfuric acid. The intensity of the reaction was different, and the order of activity of these metals could be judged by this. However, this was not a typical phenomenon of the reaction between metals and compound solutions. 3. In the reaction of a metal with multiple salt solutions (For example, when a certain amount of Mn powder is added to the mixed solution of [Al1 (NO3) 3],[Cu2 (NO3) 2], and [AgNO3], there will be a filter residue (metal) and a filtered liquid after the reaction.) However, this was mainly the result of the reaction. The phenomenon in the reaction process still followed the law of the reaction between the metal and the metal compound solution, such as the replacement metal attaching to the original metal surface, the color change of the solution, and so on. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
The Principle of the Reaction of the Formation of a Compound from an Acid to a Compound
The formation of protein from the protein was through dehydration condensation. In this process, the carbon group (-COCH) of one molecular group was linked to the carbon group (-CH <2>) of another molecular group. At the same time, a molecular water was removed to form a bond (-CO-CH <2>-). In this way, multiple molecular groups were linked to form a chain. The chain was further twisted and folded to form a protein with a certain spatial structure. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
There must be a reaction order for a compound reaction. Why is it different?
The reaction order was for a specific chemical reaction. It was defined as the sum of the powers of the various concentration terms in the rate equation. It was determined by the chemical reaction mechanism. The reaction mechanism described the instantaneous stages of the reaction. These instantaneous reactions would produce intermediate substances, which could control the reaction order. Compound reactions referred to several chemical reactions in the same reaction system at the same time. The actual reaction system mostly belonged to this category. For compound reactions, the situation was more complicated due to the existence of multiple chemical reactions that were carried out at the same time. Some compound reactions might be able to determine the overall reaction order, but some compound reactions were intertwined with many factors such as the interaction between the reactions, the participation of different reaction components, and the different instant stages of the reaction. It was difficult to describe the entire compound reaction with a simple reaction order. Therefore, compound reactions did not necessarily have a clear and unified reaction order, and were very different from a single reaction. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Experiment on the Reaction of Metal and Metal Salt Solution
The following is an example of an experiment involving the reaction of a metal with a metal salt solution: ** 1. Purpose of the experiment ** To explore the chemical properties of metals, specifically the reaction law between metals and metal salt solutions. ** 2. Laboratory supplies ** 1. ** Metal material **: Copper sheet, iron sheet, copper sheet, etc.(You can choose different metals according to your actual needs). 2. ** Salt Solution **: Copper Sulphate Solution, Silver Nitrate Solution, Salt Solution, etc.(Choose representative salt solutions, including those with different metal ions and different properties such as dissolving). 3. ** Experimental apparatus **: Test tube, tweezers. ** 3. Experimental Steps ** 1. He picked up the piece of metal with a pair of tweezers and placed it in a test tube filled with copper sulfuric acid solution. He observed the experimental phenomenon, such as whether there was any new substance on the surface of the piece of metal and whether the color of the solution had changed. 2. Using the same method, he placed the iron piece into a test tube filled with silver nitrates and observed it. 3. He placed the copper sheet into a test tube filled with a solution of NaCl3 and observed the reaction. ** IV. Reaction Principle and Anticipated Phenomena ** 1. ** Reaction of Copper Sulphate Solution with Copper Sulphate ** - "Reaction principle: According to the order of metal activity, the activity of the metal is stronger than that of copper, and a substitution reaction can occur. The chemical equation is: Mn + CuSO2 = Mn + CuSO2. - "Anticipated phenomenon: The surface of the sheet will gradually be covered with a layer of red copper, and the color of the solution may gradually turn from blue (the color of copper sulfuric acid solution) to light. Because copper ions are replaced by copper, the concentration of copper ions in the solution will decrease." 2. ** Reaction between iron and silver nitrates ** - Reaction principle: Iron is more active than silver, and the reaction equation is: Iron + 2AgNO = Iron (NO) 2 +2Ag. - "Anticipated phenomenon: Silver-white silver will be deposited on the surface of the iron sheet, and the color of the solution may change. As silver ions are replaced by iron, the concentration of silver ions in the solution will decrease. 3. ** Reaction of Copper and Salt Solution ** - Reaction principle: In the order of metal activity, the activity of copper is weaker than that of Na. According to the conditions of the reaction between metal and salt solution, copper cannot replace the Na in the salt solution in this case, so there is no reaction. - [Anticipated phenomenon: No obvious reaction. No new substance will be formed on the surface of the copper plate, and the color of the solution will not change.] ** 5. Points to note in the experiment ** 1. During the experiment, use tweezers carefully to prevent metal pieces from falling or damaging the test tube. 2. When observing the experimental phenomenon, you must pay attention to the color of the solution and the changes in the metal surface. 3. When dealing with the solution and metal after the reaction, it should be handled properly according to the laboratory regulations to avoid contamination. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Redox Reaction of Metal Ions
The oxidoreduction reaction of metal ions included two aspects: reduction reaction and oxidization reaction. In the reduction reaction, the metal ions gain electrons, the number of electrons is reduced, and the metal ions change from a high to a low state, releasing electrons. For example, in some reaction systems, high-priced metal ions would become low-priced metal ions after obtaining electrons. In the oxidization reaction, the metal atom loses its electrons, and the oxidization number increases. It changes from a low-level state to a high-level state while absorbing electrons. The essence of this reaction was the transfer of electrons. In other words, metal atoms lost electrons and became metal ions (the oxidization process), and metal ions gained electrons and became metal atoms (the reduction process). The reaction was usually carried out in an acidic solution, and a reduction indicator was often used to observe the reaction process. In practical applications, the oxidoreduction reaction of metal ions was widely used in the fields of plating, metal corrosion and protection, metal extraction, and so on. Moreover, the metal ions 'oxido-reduction reaction followed the basic laws of electron conservation, charge conservation, and energy conservation. The mobility of a metal was also restricted by the ability of its ions to undergo reduction and oxidization reactions, which affected the properties and uses of the metal in chemical reactions. For example, the more mobile the metal was, the stronger the ability of its atoms to lose electrons, and the weaker the ability of its ions to gain electrons in the reduction reaction. The stronger the ability of its ions to lose electrons in the oxidization reaction, the weaker the ability of metal atoms to generate metal ions. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
The reaction of two metal solutions
The reaction between metal and metal solution belonged to the type of reaction between metal and salt solution. The general reaction formula was: metal + salt solution → new salt + new metal. The reaction conditions were as follows: (1) The mobility of the metals involved in the reaction (except for potassium, calcium, and calcium) was stronger than that of the metal corresponding to the metal ions in the salt;(2) The salt must be water-dissolved. In the reaction between metal ions and solution, there were other types of reactions, such as the precipitations reaction (metal ions and many negative ions can form a difficult-to-dissolve precipitations), the alkali-base reaction (metal ions react with bases in solution, and different metal ions produce different properties of the precipitations. Some precipitations can further react with excessive bases), and so on. For example, in the chemistry review for the middle school entrance examination, it was involved in the reaction of a metal with a variety of salt solutions, such as adding a certain amount of Mn powder to a mixed solution of AI (NO3)3, Cu(NO3)2, and AgNO3. This involved the effect of the metal activity order on the reaction, and thus the composition of the filtered liquid and residue after the reaction. When analyzing the reaction between various metals and acid solutions, the reaction speed could be judged according to the activity of the metal. When the metal of the same mass reacted with a sufficient amount of diluted acid, the amount of hydrogen produced could also be judged according to the relative atomic mass of the metal. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Metal zinc-aquamarine reaction
The surface of the metal could be dissolved in water to form a zinc-ammine complex ion. Then, the internal metal would be exposed to the surface and react with water to form metal and hydrogen. Since the hydrogen dioxide was dissolved in the water, the reaction continued and hydrogen was released. Finally, the reaction equation was: Mn +4NH2 + 2H2O = (Mn (NH2))(Ox) 2 + H2O. At the same time, when mixed with an alkali-based fertilizer such as hydrogen, it was easy to cause a chemical reaction to reduce the fertilizer efficiency; and the zinc-hydrogen complex ion was (Mn (NH2)) 2. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Acid and Metal Reaction Color
Different metals may react with acid to produce different colors: - The reaction between the dilute sulfuric acid and the dilute sulfuric acid produced a large number of bubbles. The chemical equation was: Mn +2HQ = Mn Cl2 + Mn Cl2, Mn + Mn Cl2 = Mn Cl2 + Mn Cl2 + Mn - The reaction between the two metals was intense and produced a large number of bubbles. The chemical equation was as follows: Mn +2HQ = Mn Cl2 + Mn Cl2, Mn + Mn Cl2 = Mn Cl2 + Mn Cl2 + Mn Cl2 = Mn Cl2 + Mn Cl2 = Mn Cl2 + Mn Cl2 + Mn Cl2 = Mn Cl2 + Mn Cl2 = Mn Cl2 + Mn Cl2 + Mn Cl2 = Mn Cl - When iron reacted with diluted sulfuric acid or sulfuric acid, a small amount of bubbles appeared on the surface of the nail. At the same time, the solution turned light green because of the formation of iron sulfuric acid or iron chloride.The reaction equation was: FeCl2 <2>+ H <2>, FeCl2 <2>= FeCl2 <2>+ H <2>, FeCl2 <2>= FeCl2 <2>= FeCl2 <2>+ H <2>. - Copper does not react with dilute sulfuric acid or dilute sulfuric acid. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Reaction of Propionic Acid with Metal
Due to its weak acid nature, it was corrosive to many metals. It could react with metals to form hydrogen and metal proprionate. For example, the reaction of proprionic acid with iron: Fe2 + 2CH3CH2COON = (CH3CH2COO) 2Fe2 + H2. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>