8: Chemical Reactions
- Page ID
- 568637
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)- 8.1: Evidence of a Chemical Reaction
- This page covers chemical reactions, explaining how substances transform into new ones with altered properties through the breaking of bonds and rearrangement of atoms. It includes examples like rusting and combustion reactions and discusses observable signs of reactions such as color changes and gas release. The page also differentiates between chemical and physical changes, offering exercises for better understanding.
- 8.2: The Chemical Equation
- This page outlines the fundamental aspects of chemical reactions, detailing the identification of reactants and products, and the conversion of word equations to chemical equations. It defines chemical reactions as transformations involving bond changes and illustrates the structure of chemical equations, where reactants appear on the left and products on the right.
- 8.3: How to Write Balanced Chemical Equations
- This page covers the essentials of balancing chemical equations, stressing the roles of coefficients and subscripts. It explains that subscripts represent atom counts in molecules and should remain unchanged, while coefficients can be modified to achieve balance.
- 8.4: Classifying Chemical Reactions
- This page covers various types of chemical reactions, including acid-base, combination, decomposition, single, and double replacement reactions. It highlights the significance of categorizing these reactions for predicting products and emphasizes the importance of balancing chemical equations.
- 8.5: Aqueous Solutions and Solubility
- This page provides an overview of electrolytes, categorizing them as strong or weak based on their dissociation in water. It explains ion-dipole interactions and the dissociation of ionic compounds, highlighting factors influencing solubility. The page outlines solubility rules, indicating that while most bromides are soluble except for PbBr2, and phosphates like Sr3(PO4)2 are insoluble, certain compounds are classified as soluble or insoluble.
- 8.6: Precipitation Reactions
- This page covers precipitation reactions that form insoluble products when two solutions mix, exemplified by silver nitrate and potassium dichromate producing silver dichromate. It emphasizes the importance of recognizing strong electrolytes and applying solubility rules to predict reaction outcomes, noting that some mixtures, like sodium chloride and potassium bromide, do not react.
- 8.7: Writing Chemical Equations for Reactions in Solution- Molecular, Complete Ionic, and Net Ionic Equations
- This page covers precipitation reactions, using barium chloride and sodium sulfate as examples. It details the three step process of writing the complete chemical equation, complete ionic equation, and net ionic equations for double- and single-replacement reactions. The idea of spectator ions are also addressed.
- 8.8: Acid–Base Reactions
- This page covers neutralization reactions between acids and bases that produce salts and water, providing general reactions and examples like sodium and calcium hydroxide. It also introduces gas-evolution reactions, detailing how acids react with carbonates to yield carbon dioxide, water, and salts.