In a ______ reaction, one element is kicked out or replaced by another element in the reaction.
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An interactive review for your upcoming exam! ***Any text written inpink links to additional information and activities.*** ***Any text written in yellowrequires you to make use of your internet handout.***
A chemical reaction is the process in which atoms present in the starting substances rearrange to give new chemical combinations present in the substances formed by the reaction.� These starting substances of a chemical reaction are called the reactants, and the new substances that result are called the products.�
Observable indications of a chemical reaction can include: BUT REMEMBER!!! The only way to be positively sure that a chemical reaction has occurred �is through chemical analysis of the products!� We might not be able to observe one of the above indicators� ***Remember our �invisible� acid/base reaction???*** ~CHEMICAL EQUATIONS~ A chemical reaction can be accurately summarized with �a properly written chemical equation. A properly written chemical equation provides information about reactants, products, molecule-to-molecule relationships between reactants and products, and mole-to-mole relationships between reactants and products. ***What are three pieces of information that a chemical equation DOES NOT provide?*** Since there�s still so much information to be gained from a chemical equation, we need to become experts at writing them out! But just what is a �properly written chemical equation�? A properly written equation is a chemical equation that�
To be sure that a chemical equation obeys the law of conservation of mass, you have to be sure that the� equation is balanced.� Practice your balancing skills using the CHEMBALANCER.� Write out your answers on the accompanying internet handout. ***How did you do???*** Ok, well now that we�ve reviewed chemical equations, let�s see if we can �apply these concepts in the MINI REVIEW!!! Directions:� Write out and balance the correct chemical equations for the following �reactions on the accompanying handout. (Don�t forget to indicate the state �in parentheses.) 1.� When solid sodium nitrate is heated, it decomposes to give solid sodium nitrite and oxygen gas. 2.� When solid calcium phosphate and aqueous sulfuric acid solution react, aqueous phosphoric acid and solid calcium sulfate are produced. 3.� An aqueous solution of ammonium chloride and barium hydroxide is heated, and the compounds react to give off ammonia gas.� Barium chloride solution and water are also products. 4.� Gaseous ammonia reacts with oxygen gas to yield nitrogen gas and water. 5.� Copper(II) oxide is boiled in an aqueous solution of� sulfuric acid to form copper(II) sulfate and water.� ���� ~5 BASIC CHEMICAL REACTIONS~��� We can categorize chemical reactions according to the way in which the atoms or molecules of the reactants form new groupings. Many chemical reactions can be classified as belonging to one of five main groups. 1. �SYNTHESIS REACTIONS Also known as a composition reaction, a synthesis reaction is a reaction in which two or more substances combine to form a new compound. It is represented by the general equation: A + X�AX �whereA and X can be elements or compounds and AX is a compound. Examples of synthesis reactions include: � Synthesis of sodium chloride Na(s) + Cl(g)� � Synthesis of magnesium oxide Mg(s) + O2(g)� � Synthesis of water H2(g) + O2(g) � 2.� DECOMPOSITION REACTION A decomposition reaction is the reverse of a synthesis reaction and is a reaction in which a single compound undergoes a reaction that produces two or more simpler substances. It is represented by the general equation: AX�A+X ������� whereAX is the compound and andA and X can be elements or compounds. �������������� Most decomposition reactions take place only when energy in the form of ���� electricity or heat is added.������������� �������������� Examples of decomposition reactions include: � Decomposition of water H2O(l)� � Decomposition of lead (II) carbonate PbCO3(s)� � Decomposition of sodium iodide NaI(s)� 3.� SINGLE-REPLACEMENT REACTIONS A single-replacement reaction, or displacement reaction, is a reaction in which one element replaces a similar element in a compound.� It is represented by the general equation: A + BX�AX + B Or Y + BX�BY + X whereA, B, X, and Y are elements and AX, BX, and BY are compounds. Many single-replacement reactions take place in water, and in comparison to both synthesis and decomposition reactions, the amount of energy required for a single-replacement reaction is smaller . Examples of single-replacement reactions include: � Thermite reaction Al(s) + Fe2O3(s)� � Reaction of solid calcium and water Ca(s) + H2O(l)� � Reaction of solid lithium and chlorine gas Li(s) + Cl2(g)� 4.� DOUBLE-REPLACEMENT REACTIONS A double replacement reaction is a reaction in which the ions of two compounds exchange places in an aqueous solution to form two new compounds.� One of the new compounds that form are usually a precipitate, an insoluble gas that bubbles out of solution, or a molecular compound (usually water).� The other compound which forms is usually soluble and remains in solution. Double-replacement reactions are represented by the general equation: AX + BY�AY + BX whereA, X, B, and Y in the reactants represent ions and products AY and BX represent ionic or molecular compounds. Examples of double-replacement reactions include: � Reactions of silver nitrate with sodium chloride and silver nitrate with sodium iodide AgNO3(aq) + NaCl(aq)� AgNO3(aq) + NaI(aq)� � Reaction of sulfuric acid and sodium hydroxide H2SO4(aq) + NaOH(aq)� ***There are two special cases which have specific names given to them.*** 1. When the reaction is between two ionic compounds and they form a precipitate, this reaction is also called a precipitation. The first examples given above show precipitation reactions. 2. When the reaction is between an acid (any compound that forms hydrogen ions) and a base (any compound that forms hydroxide ions), water is formed as one of the products. This is called neutralization.� An example of a neutralization reaction is seen in the reaction above between sulfuric acid and sodium hydroxide. 5.� COMBUSTION REACTIONS A combustion reaction is a reaction in which a substance combines with oxygen and releases a large amount of energy in the form of heat and light. Examples of combustion reactions include: � Three balloons of H2 and one of H2/O2 mixture H2(g) + O2(g)� � Burning of methane (a hydrocarbon) CH4(g) + O2(g)� � Burning of hexane (a hydrocarbon) C6H14(l) + O2(g) �� ***Typically, combustion reactions occur when hydrocarbons react with oxygen to produce carbon dioxide and water, and will have the general equation� CxHy + O2� CO2+ H2O where x represents the number of carbon atoms and y the number of hydrogen atoms in the hydrocarbon Hydrocarbons are a class of compounds that primarily consist of hydrogen and carbon.*** ***DID YOU WATCH ALL OF THE MINI-FILMS THAT PROVIDED AN EXAMPLE FOR EACH REACTION TYPE???*** Another section reviewed� Time for another MINI REVIEW!!! Directions:� Write out or complete and balance each of the following equations and identify each as synthesis, decomposition, single-replacement, double-replacement, or combustion 1.� C3H8(g) + O2(g)� � 2.� Solid sodium reacted with water produces aqueous sodium hydroxide and hydrogen ���� gas. 3.� CaCO3(s)� � 4.� AgNO3(aq) + KI(aq)� 5.� Hydrogen gas reacts with iodine gas to form hydrogen iodide gas. ~ACTIVITY SERIES~ It is possible to arrange metals in the order of their chemical reactivity�s and thereby establish an activity series of metals.� The activity series helps to predict whether or not single replacement reactions of metals with metal ions and of metals with water and acids will occur.
Final section reviewed� one last MINI REVIEW!!! Directions:� Using the activity series, predict whether each of the following reactions will occur, and write the balanced equations that you predict will occur.� For those that you predict won�t occur, simply write NR (for no reaction). 1.� Pb(s) + ZnCl(s)� 2.� Cl2(g) + KBr(aq)� 3.� Al(s) + Pb(NO3)2(aq)� 4.� Cu(s) + FeSO4(aq)� 5.� Ni(s) + O2(g)� Well, that concludes the internet review! The accompanying internet review handout must be handed in on the day of the exam! And don�t forget to study hard for the exam � Go over your quiz, your homework assignments, and the review handout!� And come to class with any questions you might still have!� HAPPY STUDYING!!! Which reaction type is an element booted out and replaced by an other element?Replacement – when one element replaces another element in a compound, or if two elements in different compounds trade places, the reaction is called a replacement.
When one element replaces another in a compound a N has occurred?A single replacement reaction occurs when one element replaces another in a single compound. This type of reaction has the general equation: A + BC → B + AC. In this equation, A represents a more reactive element and BC represents the original compound.
What is the reaction called in which an element is displaced by another element?When an element displaces another element from its compound, a displacement reaction occurs.
What is the name of the type of reaction where a more reactive element replaces another element in a compound?A displacement reaction, also named single-replacement reaction, is a type of oxidation-reduction chemical reaction where an element or ion is replaced by another element or ion in a compound.
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