Document Details

SofterObsidian8012

Uploaded by SofterObsidian8012

Tags

chemical reactions chemistry science notes

Summary

This document discusses different types of chemical reactions, including synthesis, decomposition, single replacement, double replacement, neutralization, and combustion. It provides examples and explanations for each type of reaction, highlighting the reactants and products involved. The document also mentions diatomic molecules and ionic compounds in the context of chemical reactions.

Full Transcript

Types of Chemical Reactions double ,...

Types of Chemical Reactions double , replacement Chemical reactions can be classified as one of six main types: Synthesis decomposition single replacement, , , neutralization lacid-base) , and combustion. You can identify each type of reaction by examining the reactants This. makes it possible to classify a reaction predict the idenity words to know I of the and then products. combustion Classifying Chemical Reactions decomposition identified of reactions : Chemists have six common types Synthesis decomposition single replacement double replacement , , , double replacement, neutralization lacid-base) , and combustion. These six general types reprsent thousands neutralization lacid-base) of reactions. precipitate single replacement Synthesis Synthesis In a synthesis /combustion) reaction , two or more reactants /Hand B) combine to produce a single product (ABI · element + element - > compound · A + B - > AB ↳ (the Letters A and B reprsent elements ( · Example I : To make table salt in a synthesis reaction , two atoms of sodium metal (Na) and one molecule of chlorine gas (2) react to form Sodium Chloride , NAC diatomic molecule , Uz Chlorine occurs as diatomic molecule when it is a. pure element ↳ Notice that Chlorine is written as a · a There are seven common diatomic elements : Hz , N2 , 02 , Fz/Cle , Brz , and 12. When diatomic elements are not combined into a two atoms. compound they exist , as molecules containing · Example 2: Magnesium metal/Mg) reacts with oxygen gas (02) to form magnesium oxide , MgO. The balanced chimical equation is : · 2MgtO- > ZMgO to form ionic compound. When Synthesis reactions between metal previous examples two elements combined an occur a ↳ In both , non-metal , electrons are transferred from the metal to the non-metal producing ions. For ionic compounds you can use the ior and a , , equation. For multivalent metal , such iron charges to predict the product and write the covalent compounds or when a as copper or , is involved , it is more difficult to predict the product. In these cases , you will need extra information to complete the chemical equation to form dinitrogen monoxide (N2O) called nitrous oxide The balanced Example 3: Nitrogen gas (N2) react with oxygen gas (02) also. · can , for this reaction is : equation · 2Ne + 02- > INz0 Decomposition Reactions is breaking compound into smaller compounds separate. A decomposition reaction the reverse of a A decomposition reaction down of a or elements is reaction Synthesis element + element · Compound - > · AB- > A+B o Example 1: Table salt can be decomposed into sodium metal and chlorine gas by melting it at 800°C and passing an electric current through the liquid salt. This is one way to produce sodium metal. > [Nacl- > IWa + Cl2 passed through. it About 4 percent of hydrogen gas used in the world is produced · Example 2 : Water decomposes when an electric current is the called electrolysis. by decomposition. Decomposing water by passing an electric current through water is ↳ THO --2H2 to2 In both decomposition examples above , compound consisting of two elements is decomposed original into decomposition a · the elements. During of an ionic compound , electrons transfer back to the atoms of the metal and each element becomes electrically neutral. As a result , neither of the products is an ion. Single Replacement Reactions single replacement reaction , reactive element /a metal non-metal) and compound react to produce element and another In a a or a a another words , of the elements is replaced by another element The element that is replaced could be metal non-metal. compound. In other one. a or a · element + compound - > element + compound BC > BHAC where A is metal At - · · A+ BC - > C+ BA where A is a non-metal · Example 1 : An example of a single replacement reaction involving copper occurs when copper is placed into a solution of silver nitrate. ↳ Cu + ZAgNOs - > zAg + Cu(NO3Iz non-metal element is combined with a compound the non-metal · Example 2: When a , will replace the other non-metal For. example , fluorine replaces iodive in sodium iodide ↳ F + INal - > Iz + 7 NaF

Use Quizgecko on...
Browser
Browser