What are chapters and their sub sections ( ie Chapter 1 section 2) from open stax 2e that I need to learn in order to solve this question?
Table of Contents:
Preface
Chapter 1  Essential Ideas
Introduction
1.1 Chemistry in Context
1.2 Phases and Classification of Matter
1.3 Physical and Chemical Properties
1.4 Measurements
1.5 Measurement Uncertainty, Accuracy, and Precision
1.6 Mathematical Treatment of Measurement Results
Key Terms
Key Equations
Summary
Exercises
Chapter 2  Atoms, Molecules, and Ions
Introduction
2.1 Early Ideas in Atomic Theory
2.2 Evolution of Atomic Theory
2.3 Atomic Structure and Symbolism
2.4 Chemical Formulas
2.5 The Periodic Table
2.6 Ionic and Molecular Compounds
2.7 Chemical Nomenclature
Key Terms
Key Equations
Summary
Exercises
Chapter 3  Composition of Substances and Solutions
Introduction
3.1 Formula Mass and the Mole Concept
3.2 Determining Empirical and Molecular Formulas
3.3 Molarity
3.4 Other Units for Solution Concentrations
Key Terms
Key Equations
Summary
Exercises
Chapter 4  Stoichiometry of Chemical Reactions
Introduction
4.1 Writing and Balancing Chemical Equations
4.2 Classifying Chemical Reactions
4.3 Reaction Stoichiometry
4.4 Reaction Yields
4.5 Quantitative Chemical Analysis
Key Terms
Key Equations
Summary
Exercises
Chapter 5  Thermochemistry
Introduction
5.1 Energy Basics
5.2 Calorimetry
5.3 Enthalpy
Key Terms
Key Equations
Summary
Exercises
Chapter 6  Electronic Structure and Periodic Properties of Elements
Introduction
6.1 Electromagnetic Energy
6.2 The Bohr Model
6.3 Development of Quantum Theory
6.4 Electronic Structure of Atoms (Electron Configurations)
6.5 Periodic Variations in Element Properties
Key Terms
Key Equations
Summary
Exercises
Chapter 7  Chemical Bonding and Molecular Geometry
Introduction
7.1 Ionic Bonding
7.2 Covalent Bonding
7.3 Lewis Symbols and Structures
7.4 Formal Charges and Resonance
7.5 Strengths of Ionic and Covalent Bonds
7.6 Molecular Structure and Polarity
Key Terms
Key Equations
Summary
Exercises
Chapter 8  Advanced Theories of Covalent Bonding
Introduction
8.1 Valence Bond Theory
8.2 Hybrid Atomic Orbitals
8.3 Multiple Bonds
8.4 Molecular Orbital Theory
Key Terms
Key Equations
Summary
Exercises
Chapter 9  Gases
Introduction
9.1 Gas Pressure
9.2 Relating Pressure, Volume, Amount, and Temperature: The Ideal Gas Law
9.3 Stoichiometry of Gaseous Substances, Mixtures, and Reactions
9.4 Effusion and Diffusion of Gases
9.5 The Kinetic-Molecular Theory
9.6 Non-Ideal Gas Behavior
Key Terms
Key Equations
Summary
Exercises
Chapter 10  Liquids and Solids
Introduction
10.1 Intermolecular Forces
10.2 Properties of Liquids
10.3 Phase Transitions
10.4 Phase Diagrams
10.5 The Solid State of Matter
10.6 Lattice Structures in Crystalline Solids
Key Terms
Key Equations
Summary
Exercises
Chapter 11  Solutions and Colloids
Introduction
11.1 The Dissolution Process
11.2 Electrolytes
11.3 Solubility
11.4 Colligative Properties
11.5 Colloids
Key Terms
Key Equations
Summary
Exercises
Chapter 12  Kinetics
Introduction
12.1 Chemical Reaction Rates
12.2 Factors Affecting Reaction Rates
12.3 Rate Laws
12.4 Integrated Rate Laws
12.5 Collision Theory
12.6 Reaction Mechanisms
12.7 Catalysis
Key Terms
Key Equations
Summary
Exercises
Chapter 13  Fundamental Equilibrium Concepts
Introduction
13.1 Chemical Equilibria
13.2 Equilibrium Constants
13.3 Shifting Equilibria: Le Châtelier’s Principle
13.4 Equilibrium Calculations
Key Terms
Key Equations
Summary
Exercises
Chapter 14  Acid-Base Equilibria
Introduction
14.1 Brønsted-Lowry Acids and Bases
14.2 pH and pOH
14.3 Relative Strengths of Acids and Bases
14.4 Hydrolysis of Salts
14.5 Polyprotic Acids
14.6 Buffers
14.7 Acid-Base Titrations
Key Terms
Key Equations
Summary
Exercises
Chapter 15  Equilibria of Other Reaction Classes
Introduction
15.1 Precipitation and Dissolution
15.2 Lewis Acids and Bases
15.3 Coupled Equilibria
Key Terms
Key Equations
Summary
Exercises
Chapter 16  Thermodynamics
Introduction
16.1 Spontaneity
16.2 Entropy
16.3 The Second and Third Laws of Thermodynamics
16.4 Free Energy
Key Terms
Key Equations
Summary
Exercises
Chapter 17  Electrochemistry
Introduction
17.1 Review of Redox Chemistry
17.2 Galvanic Cells
17.3 Electrode and Cell Potentials
17.4 Potential, Free Energy, and Equilibrium
17.5 Batteries and Fuel Cells
17.6 Corrosion
17.7 Electrolysis
Key Terms
Key Equations
Summary
Exercises
Chapter 18  Representative Metals, Metalloids, and Nonmetals
Introduction
18.1 Periodicity
18.2 Occurrence and Preparation of the Representative Metals
18.3 Structure and General Properties of the Metalloids
18.4 Structure and General Properties of the Nonmetals
18.5 Occurrence, Preparation, and Compounds of Hydrogen
18.6 Occurrence, Preparation, and Properties of Carbonates
18.7 Occurrence, Preparation, and Properties of Nitrogen
18.8 Occurrence, Preparation, and Properties of Phosphorus
18.9 Occurrence, Preparation, and Compounds of Oxygen
18.10 Occurrence, Preparation, and Properties of Sulfur
18.11 Occurrence, Preparation, and Properties of Halogens
18.12 Occurrence, Preparation, and Properties of the Noble Gases
Key Terms
Summary
Exercises
Chapter 19  Transition Metals and Coordination Chemistry
Introduction
19.1 Occurrence, Preparation, and Properties of Transition Metals and Their Compounds
19.2 Coordination Chemistry of Transition Metals
19.3 Spectroscopic and Magnetic Properties of Coordination Compounds
Key Terms
Summary
Exercises
Chapter 20  Organic Chemistry
Introduction
20.1 Hydrocarbons
20.2 Alcohols and Ethers
20.3 Aldehydes, Ketones, Carboxylic Acids, and Esters
20.4 Amines and Amides
Key Terms
Summary
Exercises
Chapter 21  Nuclear Chemistry
Introduction
21.1 Nuclear Structure and Stability
21.2 Nuclear Equations
21.3 Radioactive Decay
21.4 Transmutation and Nuclear Energy
21.5 Uses of Radioisotopes
21.6 Biological Effects of Radiation
Key Terms
Key Equations
Summary
Exercises
Appendix A The Periodic Table
Appendix B Essential Mathematics
Appendix C Units and Conversion Factors
Appendix D Fundamental Physical Constants
Appendix E Water Properties
Appendix F Composition of Commercial Acids and Bases
Appendix G Standard Thermodynamic Properties for Selected Substances
Appendix H Ionization Constants of Weak Acids
Appendix I Ionization Constants of Weak Bases
Appendix J Solubility Products
Appendix K Formation Constants for Complex Ions
Appendix L Standard Electrode (Half-Cell) Potentials
Appendix M Half-Lives for Several Radioactive Isotopes

1. Answer the following questions related to manganese compounds.
(a) Manganese has several common oxidation states.
(i) Write the complete electron configuration for an Mn atom in the ground state.
(ii) When manganese forms cations, electrons are lost from which subshell first? Identify both the number
and letter associated with the subshell.
A student performs an experiment to produce a manganese salt of unknown composition, MnxCly(aq), and 
determine its empirical formula. The student places a sample of Mn(s) in a beaker containing excess HCl(aq), as 
represented by the following equation. 
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y
x Mn(s) + y HCl(aq) → MnxCly(aq) + H ( 2 g)
The student heats the resulting mixture until only MnxCly(s) remains in the beaker. The data are given in the 
following table. 
Mass of empty beaker 60.169 g
Mass of beaker and Mn(s) 61.262 g
Mass of beaker and Mn Cl after heating to constant mass x y 62.673 g
(b) Calculate the mass of Cl in the sample of MnxCly(s) remaining in the beaker. 
(c) Calculate the number of moles of Cl in the sample of MnxCly(s) remaining in the beaker. 
(d) The student determines that 0.0199 mol of Mn was used in the experiment. Use the data to determine the 
empirical formula of the Mn Cl (s) x y .
(e) The student repeats the experiment using the same amounts of Mn and HCl and notices that some of the 
MnxCly splatters out of the beaker as it is heated to dryness. Will the number of moles of Cl calculated for 
this trial be greater than, less than, or equal to the number calculated in part (c) ? Justify your answer. 
(f) Another compound of manganese, MnO2, is used in alkaline batteries, represented by the following diagram.
Some half-reactions are given in the table.
(i) Based on the half-reactions given in the table, write the balanced net ionic equation for the reaction that
has the greatest thermodynamic favorability.
(ii) Calculate the value of  Ecell for the overall reaction.
(iii) Calculate the value of ΔG° in kJ/molrxn.
(iv) A student claims that the total mass of an alkaline battery decreases as the battery operates because the
anode loses mass. Do you agree with the student’s claim? Justify your answer.