The chemical reaction is a natural process that always results antarubahan chemical compounds. [1] The compounds or compounds involved early in the reaction is referred to as reactants. Chemical reactions are usually characterized by a chemical change, and will result in one or more products which typically have characteristics different from the reactants. Classically, chemical reactions involve changes involving the movement of electrons in the formation and breaking of chemical bonds, although the general concept is basically a chemical reaction can also be applied to the transformation of elementary particles such as in nuclear reactions.Reactions with different chemical used in chemical synthesis to produce the desired compounds. In biochemistry, series of chemical reactions that are catalyzed by enzymes form metabolic trajectory, in which the synthesis and decomposition is usually not possible in the cell do.grouping of chemical reactions
The diversity of chemical reactions and approaches undertaken in the study resulted in the number of ways to classify these reactions, which often overlap. Below are examples of classification of chemical reactions that are usually used.Isomerization, in which chemical compounds undergo structural rearrangement without any change in its atomic kompoasisiDirect combination or synthesis, in which two or more elements or compounds unite to form a complex product:N2 + 3 H2 → 2 NH3Chemical decomposition or analysis, in which a compound is broken down into smaller compounds that:2 H2O → 2 H2 + O2Single replacement or substitution, characterized by an element is replaced by a more reactive element:2 Na (s) + 2 HCl (aq) → 2 NaCl (aq) + H2 (g)Metathesis or double replacement reaction, two compounds which change each other ions or bonds to form different compounds:NaCl (aq) + AgNO3 (aq) → NaNO3 (aq) + AgCl (s)Acid-base reaction, a reaction widely between the acid with a base. It has various definitions depending on the acid-base concept is used. Some of the most common definitions are:Arrhenius definition: acids dissociate in water releasing H3O + ions; bases dissociate in water releasing OH-ions.Brønsted-Lowry definition: Acids are proton donors (H +) donors; base is the recipient (acceptor) protons. Surrounding the Arrhenius definition.Lewis definition: Acids are electron pair acceptors; bases are electron pair donors. This definition encompasses Brønsted-Lowry definition.Redox reactions, in which there is a change in oxidation number of atoms of compounds that react. This reaction can be interpreted as electron transfer. Examples of redox reactions are:2 S2O32-(aq) + I2 (aq) → S4O62-(aq) + 2 I-(aq)Which one is reduced to I-I2 and S2O32-(thiosulfate anion) is oxidized to S4O62-.Combustion, is a kind of redox reaction in which the materials can be burned to join the elements of an oxidant, usually oxygen, to generate heat and form oxidized products. The term combustion is usually used to refer only to the oxidation of a large scale in the whole molecule. Controlled oxidation at only one single functional group is not included in the combustion process.C10H8 + 12 O2 → 10 CO2 + 4 H2OCH2S + 6 F2 → CF4 + 2 HF + SF6Disproportionation, with one reactant to form two types of products that differ only in oxidation state.2 + → Sn Sn2 + + Sn4Organic reactions, encompassing various types of reactions involving compounds which have carbon as its main element.
The diversity of chemical reactions and approaches undertaken in the study resulted in the number of ways to classify these reactions, which often overlap. Below are examples of classification of chemical reactions that are usually used.Isomerization, in which chemical compounds undergo structural rearrangement without any change in its atomic kompoasisiDirect combination or synthesis, in which two or more elements or compounds unite to form a complex product:N2 + 3 H2 → 2 NH3Chemical decomposition or analysis, in which a compound is broken down into smaller compounds that:2 H2O → 2 H2 + O2Single replacement or substitution, characterized by an element is replaced by a more reactive element:2 Na (s) + 2 HCl (aq) → 2 NaCl (aq) + H2 (g)Metathesis or double replacement reaction, two compounds which change each other ions or bonds to form different compounds:NaCl (aq) + AgNO3 (aq) → NaNO3 (aq) + AgCl (s)Acid-base reaction, a reaction widely between the acid with a base. It has various definitions depending on the acid-base concept is used. Some of the most common definitions are:Arrhenius definition: acids dissociate in water releasing H3O + ions; bases dissociate in water releasing OH-ions.Brønsted-Lowry definition: Acids are proton donors (H +) donors; base is the recipient (acceptor) protons. Surrounding the Arrhenius definition.Lewis definition: Acids are electron pair acceptors; bases are electron pair donors. This definition encompasses Brønsted-Lowry definition.Redox reactions, in which there is a change in oxidation number of atoms of compounds that react. This reaction can be interpreted as electron transfer. Examples of redox reactions are:2 S2O32-(aq) + I2 (aq) → S4O62-(aq) + 2 I-(aq)Which one is reduced to I-I2 and S2O32-(thiosulfate anion) is oxidized to S4O62-.Combustion, is a kind of redox reaction in which the materials can be burned to join the elements of an oxidant, usually oxygen, to generate heat and form oxidized products. The term combustion is usually used to refer only to the oxidation of a large scale in the whole molecule. Controlled oxidation at only one single functional group is not included in the combustion process.C10H8 + 12 O2 → 10 CO2 + 4 H2OCH2S + 6 F2 → CF4 + 2 HF + SF6Disproportionation, with one reactant to form two types of products that differ only in oxidation state.2 + → Sn Sn2 + + Sn4Organic reactions, encompassing various types of reactions involving compounds which have carbon as its main element.
in reaction to the formation of rust is why the color to yellow or brown instead of red?
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