General Information:Chemical reactions are an everyday occurrence, but not everyone may realize it. There are six chemical reactions happening all around us, but this experiment will only focus on five. The different types of reactions are: single displacement/replacement, double displacement/replacement, synthesis, combustion and decomposition. Some reactions form new compounds, while others can destroy a previous compound. Say no to plagiarism. Get a tailor-made essay on “Why Violent Video Games Should Not Be Banned”? Get an Original Essay In order to discover which elements will displace others, it is crucial to examine the metals' activity series. This table will help you determine which metals and halogens are most or least reactive. The most active elements will replace the least active elements in single or double movement. However, some metals are not reactive. In this case, no chemical reaction will occur and this is often indicated by the writing “NR” (No Reaction). Single and double displacement are reactions that form new compounds. Simple replacement occurs when one element replaces the atoms of another element in a compound. An example of this is: Cu(s) + 2AgNO3(aq) ? 2Ag(s) + Cu(NO3)2 (aq)In this equation, copper in solid form and silver nitrate in solution produce a silver precipitate and copper(II) nitrate in solution. Double displacement is very similar to single displacement in that there is an exchange of ions between two compounds. An example of this is: Ca(OH)2(aq) + 2HCl(aq) ? CaCl2(aq) + 2H2O (l)In this equation, a solution of calcium hydroxide and hydrogen chloride produces calcium chloride in solution and water. An important feature of the double displacement is the product formed from the chemical equation. The products will produce either a precipitate, gas, or water. Synthesis is a completely different type of reaction in which two or more substances react and form a single product. When there are only two elements, the reaction will always be synthetic. An example of this is: 2Na(s) + Cl2(g)? 2NaCl(s)In this equation, sodium in its solid form and chlorine gas react to produce the compound sodium chloride in solid form. Decomposition reactions are opposite to synthesis reactions in that the decomposition involves a compound that breaks down into two or more elements. decompositions normally require an energy source such as heat or electricity. An example of this is: NH4NO3(s)? N2O(g) + 2H2O(g)In this reaction, solid ammonium nitrate decomposes to produce water and nitrous oxide in their gaseous forms. Combustion is the last reaction in this experiment and one of the easiest to classify. Indeed, the combustion products are always water and carbon dioxide. In combustion reactions, oxygen combines with another substance, usually hydrocarbons, to release energy in the form of heat. An example of this is: CH4(g) + 2O2(g)? CO2(g) + 2H2O(g)In this equation, the gases methane and oxygen are added to produce carbon dioxide and water. Objective: Demonstrate and identify different types of reactions. Hypothesis: If the products of a reaction are CO2 and H2O, then combustion has occurred. If two or more substances combine into a single compound, then synthesis has occurred. If a compound separates into two or more elements and/or compounds, then decomposition has occurred. If the anions or cations of a compound change locations, then a simple.