7: Observing Two Major Classes of Chemical Reactions
- Page ID
- 514169
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)- To observe evidence of double displacement reactions, including precipitate formation, gas evolution, and color change.
- To observe evidence of redox reactions, such as metal displacement and the evolution of gases.
- To apply solubility rules to predict precipitate formation and confirm products based on the activity series of metals from experimental observations.
- To write balanced molecular, total ionic, and net ionic equations for double displacement and redox reactions.
INTRODUCTION
Part A: Double Displacement (Metathesis) Reactions
In double displacement reactions, elements in two compounds switch places to form new compounds.
\[\ce{AB + CD -> AD + CB}\]
\[\ce{Na2SO4(aq) + BaCl2(aq) -> BaSO4(s) + 2 NaCl(aq)} \label{EQ2}\]
These reactions, also known as metathesis reactions, involve the exchange of ions between compounds in solution, forming new compounds. Typically, a product is a solid, a gas, or a liquid such as water. When a solid forms, it's called a precipitate, as seen in equation \(\ref{EQ2}\).
The formation of solids, liquids, gases, or color changes, as well as temperature changes, can indicate the presence of chemical reactions. Exothermic reactions release heat, while endothermic reactions absorb heat, indicating a chemical reaction.
In this experiment, you'll mix various aqueous solutions and observe chemical reactions, using your observations to write balanced chemical equations.
Part B: Redox (Electron Transfer) Reactions
Redox reactions involve the transfer of electrons between chemical species. Oxidation is the loss of electrons, while reduction is the gain of electrons. These reactions are fundamental to many chemical and biological processes.
In this experiment, you will investigate redox reactions involving metals and metal ions in aqueous solutions. The relative reactivity of metals will be determined by observing whether a metal can displace the ions of another metal from the solution. This data can be used to write and balance the molecular and net ionic equation for each observed reaction and construct an activity series, which ranks metals in order of their reactivity.
- 7.1: Observing Two Major Classes of Chemical Reactions - Experiment
- This page provides crucial safety measures for managing corrosive and toxic chemicals, stressing protective eyewear and swift response to contact. It includes a materials list for experiments, covering chemical solutions and metal samples. The experimental procedure consists of double displacement and redox reactions, with outlined solutions and expected results.
- 7.2: Observing Two Major Classes of Chemical Reactions - Pre-lab
- This page discusses essential concepts in chemical reactions, emphasizing double displacement reactions, oxidation, and reduction through electron transfer, alongside the activity series of metals. It distinguishes between single displacement and redox reactions. Practical applications include predicting precipitate formation and writing balanced equations (molecular, complete ionic, net ionic).
- 7.3: Observing Two Major Classes of Chemical Reactions - Data and Report
- This page covers experimental methods and observations for double displacement and redox reactions, emphasizing the recording of molecular, complete ionic, and net ionic equations. It addresses reaction identification, acid-base categorization, and creating an activity series for metals. Additionally, it promotes reflection on oxidation-reduction processes and their everyday relevance through post-lab questions.