11.14: Answer Key
- Page ID
- 574241
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)- 11.14.1: Chapter 1 - Atoms, Molecules and Ions
- This page covers fundamental concepts of atomic theory and chemistry, including atom properties, isotopes, and molecular formulas. It discusses Dalton's postulates and their limitations, particularly regarding isotopes. Key concepts include subatomic particles like protons and neutrons, alpha particles' behavior, average atomic mass, and the difference between empirical and molecular formulas. The page also presents calculations with moles and molecular mass, supported by examples and exercises.
- 11.14.2: Chapter 2 - Electronic Structure and Periodic Properties
- This page explains electron behavior in atomic models, detailing the Bohr model's quantized orbits and the quantum mechanical model's probabilistic wavefunctions. It introduces key quantum numbers. Additionally, it classifies elements and compounds into categories like metals, nonmetals, and ionic or covalent substances, providing examples and identifying elements with their symbols and ions.
- 11.14.3: Chapter 3 - Chemical Bonding and Molecular Geometry
- This page covers chemical bonding concepts, including proton and electron behavior, anion and cation formation, and electron configurations. It contrasts ionic and covalent bonds while exploring molecular structures, geometries, and the influence of electron pairs on molecular shapes and polar characteristics. Specific configurations like tetrahedral and bent forms, along with examples such as CS32−, illustrate real-world bond angles and molecular dipoles.
- 11.14.4: Chapter 4 - Advanced Theories of Bonding
- This page explains the types of chemical bonds, specifically σ and π bonds, detailing electron overlap, strength, and hybridization states (sp, sp2, sp3). It discusses bonding versus antibonding orbitals, electron pairing's impact on stability, and bond order calculations. Additionally, it illustrates hybridization concepts in nitrogen and phosphorus, showing how their structures are influenced by d orbital availability.
- 11.14.5: Chapter 5 - Thermochemistry
- This page covers intensive and extensive properties related to heat production from burning wood, highlighting temperature consistency and total heat output based on material quantity. It distinguishes between heat capacity (extensive) and specific heat (intensive), and includes calculations for enthalpy changes and energy requirements in heating and chemical reactions.
- 11.14.6: Chapter 6 - Thermodynamics
- This page explores the concept of spontaneity in chemical reactions, emphasizing that they occur without external energy and are linked to changes in entropy (ΔS). It includes examples like plastic oxidation and particle arrangements affecting entropy. The relationship between entropy, energy states, and phase changes is examined, as well as the influence of temperature and conditions on spontaneity.
- 11.14.7: Chapter 7 - Fundamental Equilibrium Concepts
- This page covers chemical equilibrium, detailing how reactions reach a stable state with concentrations of reactants and products changing at equal rates, without necessarily being equal. It underscores the significance of closed systems and introduces equilibrium constants (Kc, Kp) and reaction quotients (Qc) for analyzing changes based on concentration, temperature, and volume.
- 11.14.8: Chapter 8 - Acid-Base Equilibria
- This page covers Brønsted-Lowry acids and bases, including examples of amphiprotic species and reactions, highlighting proton transfer and equilibrium states. It explains acidity trends related to electronegativity and oxidation states across the periodic table, emphasizing stronger acids and hydronium ion production. Additionally, calculations for equilibrium concentrations of weak acids and bases are provided, showcasing how to apply assumptions in dilute solutions.
- 11.14.9: Chapter 9 - Electrochemistry
- This page covers oxidation-reduction (redox) reactions, including reduction and oxidation examples, electrochemical cells, and electrode materials. It highlights the roles of reducing and oxidizing agents, maintaining electrical neutrality in half-cells, and factors influencing cell potential. Additionally, it differentiates between batteries and fuel cells in terms of reactants and byproducts and explains cathodic protection with various metals.
- 11.14.10: Chapter 10 - Kinetics
- This page covers reaction rates, detailing instantaneous, initial, and average rates. It examines how molarity, temperature, and reactant size affect reaction speed and reactivity. Key concepts include activation energy, catalysts, and collision rates. The page also discusses plotting data to determine reaction orders and employing the rate law for a clearer understanding of reaction kinetics, highlighting the interplay of various factors on reaction rates.