5: Introduction to Chemical Reactions
- Page ID
- 15924
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)Chemical change is a central concept in chemistry. The goal of chemists is to know how and why a substance changes in the presence of another substance or even by itself. Because there are tens of millions of known substances, there are a huge number of possible chemical reactions. In this chapter, we will find that many of these reactions can be classified into a small number of categories according to certain shared characteristics.
- 5.0: Prelude to Introduction to Chemical Reactions
- This page discusses yeasts, particularly Saccharomyces cerevisiae, highlighting their critical role in food production, such as bread and alcoholic beverages. Yeasts convert sugars into carbon dioxide and ethanol, causing bread to rise and improving texture. Their importance is emphasized in various food industries, as many products depend on them for production.
- 5.1: The Law of Conservation of Matter
- This page explains that a scientific law is a confirmed general principle that encapsulates multiple observations, representing the pinnacle of scientific understanding. It highlights the law of conservation of matter in chemistry, which states that within a closed system, matter is constant and aligns with the law of conservation of mass.
- 5.2: Chemical Equations
- This page explains chemical reactions, highlighting the significance of balanced equations to uphold the conservation of matter. It outlines how to represent reactions using formulas and symbols, clarifying reactants and products. The page details the process of balancing equations through examples, such as methane reacting with chlorine and the reaction between lead (II) nitrate and sodium chloride.
- 5.3: Quantitative Relationships Based on Chemical Equations
- This page explains stoichiometry, focusing on calculating substance amounts in chemical reactions using balanced equations and the role of coefficients for reactant-to-product ratios. It uses cooking as an analogy to illustrate this concept. The text also details balancing a specific chemical equation involving KMnO4, confirming oxygen atom equality on both sides, and stresses the importance of coefficients in representing substance ratios.
- 5.4: Some Types of Chemical Reactions
- This page explains the classification of chemical reactions into types: combination (multiple reactants form a single product), decomposition (a single substance breaks down into multiple products), and combustion (a substance reacts with oxygen, producing carbon dioxide and water). It highlights the significance of classification for understanding and predicting reaction outcomes, and includes examples and exercises for each type.
- 5.5: Oxidation-Reduction (Redox) Reactions
- This page covers oxidation-reduction (redox) reactions, illustrating them with the zinc and hydrochloric acid reaction where zinc displaces hydrogen. It emphasizes electron transfer, defining oxidation as electron loss and reduction as electron gain, both of which occur concurrently. The practical applications of redox chemistry are highlighted, particularly in batteries, including those used in pacemakers, which have improved from NiCad to lithium/iodine types.
- 5.6: Redox Reactions in Organic Chemistry and Biochemistry
- This page highlights the significance of redox reactions in organic chemistry and biochemistry, emphasizing their roles in combustion, respiration, and photosynthesis. It discusses the use of oxidizing agents in organic reactions, the importance of antioxidants in reducing oxidative damage, and how photosynthesis converts carbon dioxide and water into glucose, underscoring the essential nature of these processes for life on Earth.
- 5.E: Introduction to Chemical Reactions (Exercises)
- This page covers the law of conservation of matter, which states that matter remains constant in closed systems, requiring balanced chemical equations. It discusses various types of reactions, including redox, combination, and combustion, alongside biochemical processes like photosynthesis and cellular respiration. Exercises focus on writing, balancing equations, and understanding reaction types.
- 5.S: Introduction to Chemical Reactions (Summary)
- This page covers essential chemistry concepts, focusing on the law of conservation of matter in closed systems. It explains the representation of chemical reactions through balanced equations with coefficients for reactants and products. Additionally, it details various reaction types, emphasizing oxidation-reduction (redox) reactions, which are vital for biological processes such as respiration and photosynthesis, highlighting the importance of antioxidants in metabolic reactions.