Chemistry
Types of Chemical Reactions
Chemical reactions can be classified into several types, including synthesis, decomposition, single displacement, double displacement, and combustion reactions. Synthesis reactions combine two or more substances to form a new compound, while decomposition reactions break down a compound into its constituent elements. Single displacement reactions involve an element replacing another in a compound, and double displacement reactions involve the exchange of ions between two compounds. Combustion reactions involve the rapid combination of a substance with oxygen, often producing heat and light.
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eBook - PDF- Ageetha Vanamudan(Author)
- 2023(Publication Date)
- Delve Publishing(Publisher)
CHEMICAL REACTIONS CHAPTER5 CONTENTS 5.1 History of Chemical Reactions ........................................................... 77 5.2 Chemical Reactions of Various Types ................................................. 79 5.3 Several Theories Exist to Explain Acid-Base Reactions ........................ 87 5.4 Photolysis Reactions .......................................................................... 92 Introduction to Molecular Science 76 A chemical reaction occurs when one or more reactants are converted into one or more distinct products. Compounds and chemical elements are examples of substances. By rearranging the atoms of the reactants, chemical reactions produce a wide range of products. Chemical reactions are crucial in contemporary culture, technology, and even life itself. Fuel combustion, iron smelting, glass, and pottery manufacture, beer production, and the creation of wine and cheese are some examples of chemical processes that have been employed for millennia. In addition to the chemical reactions that occur in the earth’s crust, atmosphere, and seas, several complex processes occur in all living systems. It is necessary to distinguish between chemical reactions and physical changes. Physical transitions include ice melting into water and water evaporating to create vapor (Rastogi & Sani, 2011). A substance’s physical properties may change throughout metamorphosis, but its chemical identity does not. Water (H 2 O ) is the same substance regardless of its physical state since each molecule includes two hydrogen atoms and one oxygen atom. When water reacts with sodium metal (Na), it produces molecular hydrogen (H 2 ) and sodium hydroxide (NaOH). This denotes the occurrence of a chemical reaction or change. Understanding the fundamentals of chemical interactions. Figure 5.1: Chemical analysis of chemical reactants. Source: By No machine-readable author provided. Burn~commonswiki as- sumed (based on copyright claims).
eBook - ePubReaction Green Metrics
Problems, Exercises, and Solutions
- John Andraos(Author)
- 2018(Publication Date)
- CRC Press(Publisher)
4 Chemical Reaction Classifications4.1 IdentifyingTypes ofReactionsThere are five major classes of chemical reaction types encountered in organic chemistry: additions, eliminations, rearrangements, redox reactions, and substitutions. Every organic reaction that has ever been discovered or will be discovered in the future can be slotted in at least one of these categories. Generally, most of the named organic reactions that form the workhorse toolbox for organic chemists are categorized uniquely into one of these classes. Modern reactions have attributes that have features of more than one of these classes. Each of these reaction classes may be depicted using a visual algebraic approach using LEGO®-like cartoons to illustrate what is occurring.4.1.1 Terms, Definitions, and Examples Additions Addition reactions involve coupling of two or more components in an acyclic (linear) or a cyclic sense. The visual algebraic operation is addition. Eliminations (Fragmentations) Eliminations or fragmentations involve the splitting apart of a substrate or an intermediate. The visual algebraic operation is subtraction. Multi-ComponentMulti-component reactions are a special sub-class of addition reactions involving at least three substrate structures combining together to produce a product. The order of addition of those substrates may or may not matter depending on the reaction mechanism. This is the most powerful method of constructing ring-containing compounds with the least number of reaction steps.RearrangementsRearrangement reactions involve a reshuffling of atom connectivity of the substrate or a reaction intermediate. The visual algebraic operation is reshuffling. Rearrangements of substrates always have 100% atom economy. Reactions involving rearrangements of transient intermediates always have atom economies less than 100% since by-products always arise.
No longer available |Learn more- (Author)
- 2014(Publication Date)
- Academic Studio(Publisher)
Chapter 8 Chemical Reaction A thermite reaction using ferric oxide A chemical reaction is a process that leads to the transformation of one set of chemical substances to another. Chemical reactions can be either spontaneous, requiring no input of energy, or non-spontaneous, typically following the input of some type of energy, viz. heat, light or electricity. Classically, chemical reactions encompass changes that strictly involve the motion of electrons in the forming and breaking of chemical bonds, although the general concept of a chemical reaction, in particular the notion of a chemical equation, is applicable to transformations of elementary particles, as well as nuclear reactions. ___________________WORLD TECHNOLOGIES____________________ The substance (or substances) initially involved in a chemical reaction are called reactants or reagents. Chemical reactions are usually characterized by a chemical change, and they yield one or more products, which usually have properties different from the reactants. Reactions often consist of a sequence of individual sub-steps, the so-called elementary reactions, and the information on the precise course of action is part of the reaction mechanism. Chemical reactions are described with chemical equations, which graphically present the starting materials, end products, and sometimes intermediate products and reaction conditions. Different chemical reactions are used in combination in chemical synthesis in order to obtain a desired product. In biochemistry, series of chemical reactions catalyzed by enzymes form metabolic pathways, by which syntheses and decompositions impossible under ordinary conditions are performed within a cell. History Antoine Lavoisier developed the theory of combustion as a chemical reaction with oxygen Chemical reactions such as combustion in the fire, fermentation and the reduction of ores to metals were known since antiquity.
No longer available |Learn more- (Author)
- 2014(Publication Date)
- Research World(Publisher)
Chapter 10 Chemical Reaction A thermite reaction using ferric oxide A chemical reaction is a process that leads to the transformation of one set of chemical substances to another. Chemical reactions can be either spontaneous, requiring no input of energy, or non-spontaneous, typically following the input of some type of energy, viz. heat, light or electricity. Classically, chemical reactions encompass changes that strictly __________________WORLD TECHNOLOGIES___________________ involve the motion of electrons in the forming and breaking of chemical bonds, although the general concept of a chemical reaction, in particular the notion of a chemical equation, is applicable to transformations of elementary particles, as well as nuclear reactions. The substance (or substances) initially involved in a chemical reaction are called reactants or reagents. Chemical reactions are usually characterized by a chemical change, and they yield one or more products, which usually have properties different from the reactants. Reactions often consist of a sequence of individual sub-steps, the so-called elementary reactions, and the information on the precise course of action is part of the reaction mechanism. Chemical reactions are described with chemical equations, which graphically present the starting materials, end products, and sometimes intermediate products and reaction conditions. Different chemical reactions are used in combination in chemical synthesis in order to obtain a desired product. In biochemistry, series of chemical reactions catalyzed by enzymes form metabolic pathways, by which syntheses and decompositions impossible under ordinary conditions are performed within a cell. History Antoine Lavoisier developed the theory of combustion as a chemical reaction with oxygen Chemical reactions such as combustion in the fire, fermentation and the reduction of ores to metals were known since antiquity.
eBook - PDF- Morris Hein, Susan Arena, Cary Willard(Authors)
- 2021(Publication Date)
- Wiley(Publisher)
We will study the relationship among quantities of reactants and products in the next chapter. 8.3 Why Do Chemical Reactions Occur? LEARNING OBJECTIVE: Determine the factors that cause reactions to occur. Chemical equations represent chemical changes or reactions. But how can we predict whether or not a chemical reaction will occur? Chemists have learned over time to see observations in reactants that seem to predict when reactants will become products. These “driving forces” that indicate reactants will change into products are • Formation of a solid • Formation of a gas • Formation of water • Transfer of electrons If any of these things occur when chemicals are placed together, a chemical reaction is prob- able. Therefore, to predict whether a reaction will occur we need to consider these “driving 164 CHAPTER 8 Chemical Equations forces.” We will consider these forces as we learn more about chemical reactions and become better at predicting the outcome of mixing reactants. 8.4 Types of Chemical Equations LEARNING OBJECTIVE: Give examples of a combination reaction, decomposition reaction, single-displacement reaction, and double-displacement reaction. Reactions are classified into types to assist in writing equations and in predicting other reac- tions. Many chemical reactions fit one or another of the four principal reaction types that we discuss in the following paragraphs. Reactions are also classified as oxidation–reduction. Spe- cial methods are used to balance complex oxidation–reduction equations. (See Chapter 17.) Synthesis (Combination) Reaction In a synthesis reaction, two reactants combine to give one product. Synthesis is one of the most important activities of chemistry. Producing new compounds including new medicines and synthetic compounds such as plastics have greatly influenced our lives. The general form of the equation is A + B ⟶ AB CHECK YOUR UNDERSTANDING 8.3 Synthesis Reactions A strip of Mg burning in air produces MgO (left of the flame).
eBook - PDF- Young, William Vining, Roberta Day, Beatrice Botch(Authors)
- 2017(Publication Date)
- Cengage Learning EMEA(Publisher)
Chemical Reactions and Solution Stoichiometry Unit Outline 9.1 Types of Chemical Reactions 9.2 Aqueous Solutions 9.3 Reactions in Aqueous Solution 9.4 Oxidation–Reduction Reactions 9.5 Stoichiometry of Reactions in Aqueous Solution In This Unit… The science of chemistry brings three central benefits to society. First, chemistry helps explain how the world works, principally by examining nature on the molecular scale. Second, chemical analysis is used to iden-tify substances, both natural and artificial. This is evident every time a person’s blood is tested to determine cholesterol level or when athletes undergo testing for banned drug use. Finally, the science of chemistry is unique in that it involves the ability to create new forms of matter by combining the elements and existing compounds in new but controlled ways. The creation of new chemical compounds is the subject of this unit. Here, we explore different Types of Chemical Reactions, emphasizing the reactions that take place in aqueous solution. 9 AlbertSmirnov/iStockphoto.com Copyright 2018 Cengage Learning. All Rights Reserved. May not be copied, scanned, or duplicated, in whole or in part. WCN 02-300 Unit 9 Chemical Reactions and Solution Stoichiometry 230 9.1 Types of Chemical Reactions 9.1a Combination and Decomposition Reactions Chemical reactions involve the transformation of matter, the reactants, into different materials, the products. A combination reaction is one in which typically two or more reactants, usually elements or compounds, combine to form one product, usually a compound. In one type of combination reaction, two elements combine to form a compound. For example, the elements hydrogen and oxygen combine to form water, giving off large amounts of energy in the process (Figure 9.1.1): 2 H 2 (g) 1 O 2 (g) S 2 H 2 O(g) This combination reaction was used to generate power from the main engines in the space shuttle, which flew its final mission in 2011.
eBook - PDF- C N R Rao(Author)
- 2009(Publication Date)
- World Scientific(Publisher)
6 CHEMICAL REACTIONS 226 Understanding Chemistry Chemistry is a study of reactions between substances. It is therefore important to understand the nature of chemical reactions. One can make new substances by making use of various chemical reactions. We shall try to understand how reactions can be associated with rates, and the factors that influence the rates. We then survey a few simple types of reactions and show how chemists innovate new strategies for making molecules using catalysts and new routes for synthesis. 6.1 Which reactions occur? Some reactions occur spontaneously. We can understand this by analogy with potential energy. If we store water in a dam at the top of a hill, it has high potential energy. If there were no dam, water would have flowed down. Objectives • In this lesson, we shall try to understand why and how chemical reactions occur and the factors that affect them. • We then go through different types of reactions, which include catalysis and light-induced reactions. • A combination of chemical reactions is necessary to prepare complex compounds. Chemists continue to discover new ways of assembling molecules. The supramolecular route provides a rich resource for new molecular systems. Chemical reactions 227 increasing chemical potential energy increasing stability reactants products direction of spontaneous reaction In other words, the products have to be more stable than the reactants. One may, therefore, say that when energy is released in a chemical reaction, it will be spontaneous. This is the case of exothermic reactions. Thus, combustion (burning) is a spontaneous reaction. Remember combustion is associated with the release of heat (energy). Chemical reactions occur spontaneously when the potential energy of the products is lower than the potential energy of the reactants. 228 Understanding Chemistry 6.2 Chemical equilibrium We used the word equilibrium when describing states of substances in Lesson 1.
eBook - PDF- James M. Beard(Author)
- 2016(Publication Date)
- CRC Press(Publisher)
47 CHAPTER 4 Types of Chemical Compounds and Their Reactions The world of chemistry contains millions of compounds and a huge number of dif-ferent Types of Chemical Reactions. In order to keep track of all of this information it is necessary to categorize the material in some way. In this chapter, we are going to break down the field of chemistry into roughly five areas. The first three areas are based on Types of Chemical Reactions that account for a vast majority of all chemi-cal reactions. We will then look at organic chemistry, which is based on a particular type of chemical compound, and, finally, we will look at certain nuclear processes. ACIDS AND BASES Acids Although there are a large number of chemical reactions that could be discussed, only three general classes of reactions—acid–base, precipitation, and oxidation– reduction—are discussed in this chapter. These three classes of reactions explain the chemical behavior of a large variety of substances. There are three major theories of acids and bases. This chapter focuses only on one of them, the simplest and the oldest. This theory was developed by a Swedish chemist, Svante Arrhenius , in the latter part of the 19th century. Let us first con-sider Arrhenius’ definition of acids. Arrhenius said that acids are substances that, when dissolved in water, produce hydrogen ions (H + ). This definition works fairly well with one minor modification. The 20th-century chemists fairly quickly came to the conclusion that H + ions do not exist as such, but rather H + attaches itself to a water molecule to form the hydronium ion (H 3 O + ). An acid can be defined as a substance that, when dissolved in water, produces hydronium ions (H 3 O + ). The properties asso-ciated with acids should be the properties of the H 3 O + ion. What is the behavior that the H 3 O + ion exhibits?
eBook - PDF- Leo J. Malone, Theodore O. Dolter(Authors)
- 2012(Publication Date)
- Wiley(Publisher)
The first three types are the simplest and will be considered in this section. n Fire is certainly dramatic evidence of the occurrence of a chemical reaction. What we see as fire is the hot, glowing gases of a combustion reaction. The easiest way to put out a fire is to deprive the burning substance of a reactant (oxygen) by dousing it with water or carbon dioxide from a fire extinguisher. The reaction of elements or compounds with oxygen is the first of three types of reactions that we will discuss in this section. 6-2.1 Combustion Reactions One of the most important types of reactions that we may refer to in the future is known as a combustion reaction. This type of reaction refers specifically to the reac- tion of an element or compound with elemental oxygen (O 2 ). Combustion usually liberates considerable heat energy and is accompanied by a flame. It is typically referred to as “burning.” When elements undergo combustion, generally only one product (the oxide) is formed. Examples are the combustion of carbon and alumi- num shown here. C(s) + O 2 (g) ¡ CO 2 (g) 4Al(s) + 3O 2 (g) ¡ 2Al 2 O 3 (s) When compounds undergo combustion, however, two or more combustion prod- ucts are formed. When carbon–hydrogen or carbon–hydrogen–oxygen compounds undergo combustion in an excess of oxygen, the combustion products are carbon dioxide and water. (Combustion reactions involving carbon–hydrogen or carbon– hydrogen–oxygen compounds are balanced in the order C, H, O). CH 4 (g) + 2O 2 (g) ¡ CO 2 (g) + 2H 2 O(l) The metabolism of glucose (C 6 H 12 O 6 , blood sugar) occurs in our bodies to produce the energy to sustain our life. We will discuss the energy liberated by this reaction in Chapter 7. But we are now concerned with the product compounds. This combustion reaction occurs at a steady, controlled rate.
eBook - PDFChemistry for Today
General, Organic, and Biochemistry
- Spencer Seager, Michael Slabaugh, Maren Hansen, , Spencer Seager, Spencer Seager, Michael Slabaugh, Maren Hansen(Authors)
- 2021(Publication Date)
- Cengage Learning EMEA(Publisher)
Once reactions are classi- fied as redox or nonredox, many can be further classified into one of several other categories, as shown in Figure 5.4. Notice that according to Figure 5.4, single-replacement, or substitu- tion, reactions are redox reactions, whereas double-replacement, or metathesis, reactions are nonredox. Combination and decomposition reactions can be either redox or nonredox. FIGURE 5.4 A classification of chemical reactions. Combination Double replacement (metathesis) Decomposition Single replacement (substitution) Combination Decomposition Chemical reactions Nonredox Redox FIGURE 5.3 A chemical reaction takes place when antacid tablets are dropped into water. 5.3 Redox Reactions Learning Objective 2 Assign oxidation numbers to elements in chemical formulas, and identify the oxidizing and reducing agents in redox reactions. Almost all elements react with oxygen to form oxides. The process is so common that the word oxidation was coined to describe it. Some examples are the rusting of iron, 4Fe(s) 1 3O 2 (g) S 2Fe 2 O 3 (s) (5.8) and the burning of hydrogen, 2H 2 (g) 1 O 2 (g) S 2H 2 O(/) (5.9) The reverse process, reduction, originally referred to the technique of removing oxygen from metal oxide ores to produce the free metal. Some examples are CuO(s) 1 H 2 (g) S Cu(s) 1 H 2 O(/) (5.10) Colin Anderson Productions pty ltd/Stockbyte/Getty Images Copyright 2022 Cengage Learning. All Rights Reserved. May not be copied, scanned, or duplicated, in whole or in part. Due to electronic rights, some third party content may be suppressed from the eBook and/or eChapter(s). Editorial review has deemed that any suppressed content does not materially affect the overall learning experience. Cengage Learning reserves the right to remove additional content at any time if subsequent rights restrictions require it. 142 Chapter 5 and 2Fe 2 O 3 (s) 1 3C(s) S 4Fe(s) 1 3CO 2 (g) (5.11) Today, the words oxidation and reduction are used in a rather broad sense.
eBook - PDF- David A. Ucko(Author)
- 2013(Publication Date)
- Academic Press(Publisher)
NINE Chemical reactions In Chapter One we defined chemistry as the study of the composition, structure, and properties of substances, and the changes that they undergo. So far, by studying the nature of elements and compounds, we have concentrated on the first part of the definition of chemistry. Chapter Nine deals with the second part of our definition: the study of chemical change. This chapter describes how we represent these changes, gives examples of different types of changes, and relates energy to chemical change. To demonstrate an understanding of Chap-ter Nine, you should be able to: 1 Describe the relationship between compound formation and chem-ical change. 2 Identify the symbols in chemical equations. 3 State the law of conservation of mass and describe its relationship to chemical equations. 4 Balance simple chemical equations by trial and error. 5 Interpret balanced chemical equations. 6 Classify chemical reactions according to the type of reaction taking place. 7 Write chemical equations given the reactions in words or given the reactants and type of reaction. 8 Describe the relationship between energy changes and chemical reactions. 9 Describe the major sources and uses of energy. 10 Summarize the chemical process by which a major industrial prod-uct is manufactured. 249 FIGURE 9-1 Iron and sulfur. In (a), these two elements exist as a mixture, and the magnet can separate the iron. In (b), the elements have been combined into a compound, iron sulfide. The iron can no longer be separated with a magnet. (Photo by Al Green.) (a) (b) 9.1 When iron filings are added to powdered sulfur at room temperature, CHEMICAL AND the result is a mixture of iron and sulfur. Once mixed, the iron and PHYSICAL CHANGE sulfur can be physically separated. For example, as shown in Figure 9-1(a), iron can be removed from the mixture with a magnet, leaving only the sulfur behind.
eBook - PDFStantec's Water Treatment
Principles and Design
- John C. Crittenden, R. Rhodes Trussell, David W. Hand, Kerry J. Howe, George Tchobanoglous(Authors)
- 2022(Publication Date)
- Wiley(Publisher)
5-1 Chemical Reactions and Stoichiometry Chemical operations used for water treatment are often described using chemical equations. These chemical equations may be used to develop the stoichiometry that expresses quantitative relationships between reactants and products participating in a given reaction. An introduction to the Types of Chemical Reactions and reaction stoichiometry used in water treatment processes is presented below. Types of Reactions Chemical reactions commonly used in water treatment processes can be described in various ways. For example, the reactions of acids and bases, precipitation of solids, complexation of metals, and oxidation-reduction of water constituents are all important reactions used in water treatment. In general, reactions can be thought of as reversible and irreversible. Irreversible reactions tend to proceed to a given endpoint as reactants are consumed and products are formed until one of the reactants is totally con- sumed. Irreversible reactions are signified with an arrow in the chemical equation, pointing from the reactants to the products. Symbols commonly used in chemical equations are described in Table 5-1. In the following reac- tion, reactants A and B react to form products C and D: A B C D + → + (5-1) Reversible reactions tend to proceed, depending on the specific conditions, until equilibrium is attained at which point the formation of products from 229 5-1 Chemical Reactions and Stoichiometry the forward reaction is equal to the loss of products for the reverse reaction. For example, in Eq. 5-1 the reactants A and B react to form products C and D, whereas in Eq. 5-2 the reactants C and D react to form products A and B: C D A B + → + (5-2) The reactions presented in Eqs.
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