Chemical Reactions: Synthesis, Decomposition, Single Replacement, And

A chemical reaction is a process in which the rearrangement of the molecular or ionic structure of a substance is transformed physically or chemically. If the reaction occurs, the starting products will always be different from the products. They also involve the motion of electrons which leads to buildup and breakdown of chemical bonds. There are six types of chemical reactions including Synthesis, Decomposition, Single Replacement, Double Replacement, Combustion, and Acid Base. Each reaction has their own unique characteristics that make them special.
First is Synthesis. Synthesis is a reaction in which two different substances are combined to create one substance. In a lab, slime was made as an example of a synthesis reaction. Combining

Single Replacement is the process of an element reacting with a compound and taking the place of another element. Substance C can take the place of Substance A in the compound of AB. A metal can only replace a metal and a nonmetal can only replace a nonmetal. To predict whether or not the reaction will occur, using an activity series table will help to compare the reactivities of the elements. The reactivity of a metals is based more on the electronegativity making it more difficult to predict the reactivity of the halogens. A real life example is in the Statue of Liberty, the inside structure was made out of steel. The iron in steel reacts with the oxidized copper which protects the color and integrity. The formula for this reaction is Fe + Cu2+ → Fe2+ + Cu. In a lab 17 single replacements reactions were tested however not all had a reaction. Some were quicker and some slower to react compared to others due to different reaction rates in each

Combustion is an exothermic reaction that reacts when in contact with oxygen producing heat and a new product. These reactions are as exothermic as it gets. The general form of a combustion reaction is the reaction between a hydrocarbon and oxygen to create carbon dioxide and water. Hydrocarbon + O₂→CO₂+H₂O. Occasionally, these reactions can release light and produce a flame. To start a reaction, most require a flame to provide heat and initiate the reaction. Combustion is a very common reaction. It's what makes our cars go, and it's what burning is. It is containing carbon which reacts with oxygen to form CO2 and H2O. A simple example of the combustion of Methane, a natural gas, CH4 + 2O2 →CO2 + 2H2O. Another example includes the burning of naphthalene with the equation C10H8 + 12 O2 → 10 CO2 + 4 H2O. The combustion of ethane is 2C2H6 + 7O2 → 4CO2 + 6H2O which is another example. A real life example is the combustion of gunpowder. Gunpowder is a mix of potassium nitrate, charcoal, and sulfur. The potassium nitrate decomposes at a high temperature to provide the oxygen needed. The charcoal and sulfur are the fuels in this reaction. The equation for this reaction is as follows 2 KNO₃ + S +3 C →K₂S + N₂ + 3 CO₂. An incomplete reaction occurs when the oxygen is