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Course Question & AnswerAdvanced Inorganic Chemistry
Purpose of Course showclose
Advanced Inorganic Chemistry is designed to give you the knowledge to explain everyday phenomena of inorganic complexes. You will study the various aspects of their physical and chemical properties and learn how to determine the practical applications that these complexes can have in industrial, analytical, and medicinal chemistry.
This course will begin with the discussion of symmetry and point group theory and its applications in the field of vibrational spectroscopy. We will then study molecular orbital (MO) theory specifically applied to metal organic complexes. MO theory will be critical in understanding the following: 1) the relative position of ligands in the spectrochemical series, 2) the electronic transitions and related selection rules, and 3) the application of spectroscopy of metals. The course will then move onto the study of the oxidation states of transition metals and their redox properties. A firm grasp of the chemical redox properties of transition metals is critical to understanding their reaction mechanisms and stability in solution. We will then look at catalysis reactions utilizing inorganic complexes, including industrial practices. Lastly, we will take a look at some real-world applications of transition metal complexes in the fields of medicinal chemistry, solar energy, electronic displays, and batteries.
Course Information showclose
Welcome to CHEM 202. Below, please find general information on this course and its requirements.
Course Designer: Joanna Smithback, Ph.D.
Primary Resources: This course utilizes several free, online resources; however, the majority of information is taken from the following sites:
- UC Davis: ChemWiki
- MIT: Principles of Chemical Science
- Jim Clark’s Chemguide
Requirements for Completion: This course comprises a variety of lectures and reading materials. Several of the reading assignments contain practice problems to guide your learning. To successfully complete this course, you must score at least a 70% on the cumulative final.
Time Commitment: This course should take approximately 108 hours to complete, exclusive of the final exam. The 50-question exam should take no more than 2 hours.
Tips/Suggestions: The material in this course is progressive. If you find that you are having difficulty understanding some of the concepts, it is suggested that you revisit the previous unit of this course or review the information contained in the prerequisite courses.
Learning Outcomes showclose
- Explain symmetry and point group theory and demonstrate knowledge of the mathematical method by which aspects of molecular symmetry can be determined.
- Use molecular symmetry to predict or explain the chemical properties of a molecule, such as dipole moment and allowed spectroscopic transitions.
- Construct simple molecular orbital diagrams and obtain bonding information from them.
- Demonstrate an understanding of valence shell electron pair repulsion (VSEPR), which is used for predicting the shapes of individual molecules.
- Explain spectroscopic information obtained from coordination complexes.
- Identify the chemical and physical properties of transition metals.
- Demonstrate an understanding of transition metal organometallics.
- Define the role of catalysts and explain how they affect the activation energy and reaction rate of a chemical reaction.
- Identify the mechanisms of both ligand substitution and redox processes in transition metal complexes.
- Discuss some current, real-world applications of transition metal complexes in the fields of medicinal chemistry, solar energy, electronic displays, and ion batteries.
Course Requirements showclose
In order to take this course, you must:
√ Have access to a computer.
√ Have continuous broadband Internet access.
√ Have the ability/permission to install plug-ins or software (e.g. Adobe Reader or Flash).
√ Have the ability to download and save files and documents to a computer.
√ Have the ability to open Microsoft files and documents (.doc, .ppt, .xls, etc.).
√ Have competency in the English language.
√ Have read the Saylor Student Handbook.
√ Have completed General Chemistry I & II (CHEM101& CHEM102), Organic Chemistry I (CHEM103), Inorganic Chemistry (CHEM107), and Analytical Chemistry (CHEM108) as listed in “The Core Program” of the Chemistry discipline.
Unit Outline show close
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Unit 1: Symmetry
The concept of symmetry is critical to understanding certain physical properties of metal compounds, such as vibrational modes. In this unit, we will discuss specific symmetry elements, including reflection planes, rotation axes, and inversion centers. While a molecule can have many symmetry elements, some will specifically determine the molecule’s physical properties. This unit teaches you how to assign symmetry elements and point groups to a given molecule. You will learn to interpret the character tables, which will help you prioritize symmetry elements and classify molecules according to their respective point groups. Note that certain characteristic properties of molecules, which may include polarity, chirality, and vibrational mode, correspond to each point group. Character tables will allow you to identify spectroscopic properties of the compounds.
Unit 1 Time Advisory show close
Unit 1 Learning Outcomes show close
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1.1 Symmetry Elements, Group Theory, and Irreducible Representations
- Web Media: YouTube: Mechanophore’s “Elements of Symmetry”
Link: YouTube: Mechanophore’s “Elements of Symmetry” (YouTube)
Instructions: Please watch the video (runtime = 5:38 minutes). This video illustrates the three basic elements of symmetry. Please note that there are more than three point groups; however, some arise from a combination of the three basic elements. (For example, an improper rotation, S, arises from a rotation, C, combined with a mirror plane, ?.)
Terms of Use: Please respect the terms of use displayed on the webpage above.See a broken link? Please let us know!
- Reading: UC Davis: ChemWiki’s “Group Theory: Theory”
Link: UC Davis: ChemWiki’s “Group Theory: Theory” (HTML)
Instructions: Please read the entire webpage. Once you have familiarized yourself with the symmetry elements and terminology, the bulk of information can be condensed into the flowchart presented in Table 2.12. Please follow the link under the “Symmetry Point Groups” section for more information on each of the individual point groups.
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- Web Media: YouTube: Mechanophore’s “Elements of Symmetry”
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1.2 Point Groups and Schoenflies Notation
- Reading: The International Union of Crystallography: L. S. Dent Glasser’s “Symmetry”
Link: The International Union of Crystallography: L. S. Dent Glasser’s “Symmetry” (HTML)
Also available in:
PDF
Instructions: Please read all sections. This material may also be downloaded as a PDF in pamphlet form. Point groups are primarily used by crystallographers for symmetry notation in place of the group theory methods described previously. Also note that Schoenflies notation is an older notation system and is listed alongside the Hermann-Mauguin notation as such.
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- Reading: The International Union of Crystallography: L. S. Dent Glasser’s “Symmetry”
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1.3 Character Tables
- Reading: UC Davis: ChemWiki’s “Character Table”
Link: UC Davis: ChemWiki’s “Character Table” (HTML)
Instructions: Please read the entire webpage. Also, please work through the questions pertaining to BF3 at the bottom of the page. These questions will guide you in understanding the type of information obtained from character tables.
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- Reading: UC Davis: ChemWiki’s “Character Table”
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1.4 Using Group Theory and Character Tables
- Reading: UC Davis: ChemWiki’s “Group Theory and its Application to Chemistry”
Link: UC Davis: ChemWiki’s “Group Theory and its Application to Chemistry” (HTML)
Instructions: Please read the material covered in the first five sections (up to and including 5.3). This material explains how group theory is applied. Follow the example of ammonia provided. The first external link provides an interesting video demonstration of solving the Rubik’s cube based on the group theory discussion provided.
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- Assessment: University of Rhode Island’s “Chemistry 401: Symmetry and Point Groups—Practice Problems”
Link: University of Rhode Island’s “Chemistry 401: Symmetry and Point Groups—Practice Problems” (HTML)
Instructions: Please work through problems 1–4. The answers are provided by clicking on the links at the end of each question.
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- Reading: UC Davis: ChemWiki’s “Group Theory and its Application to Chemistry”
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Unit 2: Molecular Orbital Theory and Symmetry
Molecular orbital (MO) theory is a detailed explanation of how electrons are distributed in molecules. In your organic chemistry courses, valence bond theory (VBT) was used to explain chemical bonding and molecular structure. VBT allows that each atom in a molecule retains its own electrons, located in atomic orbitals. In this unit, MO theory will be introduced. MO theory assumes that electrons in a molecule do not belong to single atoms but to the entire molecule as a whole. It also maintains that electrons are not located in atomic orbitals but molecular orbitals, located in specific spatial regions within the molecule. These molecular orbitals are used to explain the molecule’s chemical behavior and reactivity. Knowledge of molecular orbitals is essential to understanding the spectrochemical series and predicting ligand substitution in metal complexes.
Unit 2 Time Advisory show close
Unit 2 Learning Outcomes show close
- Reading: UC Davis: ChemWiki’s “Group Theory and its Application to Chemistry”
Link: UC Davis: ChemWiki’s “Group Theory and its Application to Chemistry” (HTML)
Instructions: Please read the material covered in section 6. This material introduces the relationship covered in this unit between molecular orbital theory and symmetry.
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- Reading: UC Davis: ChemWiki’s “Group Theory and its Application to Chemistry”
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2.1 Linear Combination of Atomic Orbitals
- Reading: Mark Bishop’s Chemistry Site’s “MO Theory”
Link: Mark Bishop’s Chemistry Site’s “MO Theory” (HTML)
Instructions: Please read the entire webpage. This material gives background information on molecular orbitals and bond order. Please work through the examples presented in the text.
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- Web Media: YouTube: Mechanophore’s “Hybrid Atomic Orbitals”
Link: YouTube: Mechanophore’s “Hybrid Atomic Orbitals” (YouTube)
Instructions: Please watch the video (runtime = 5:16 minutes). This material explains the need for hybrid atomic orbitals when discussing chemical bonding.
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- Web Media: YouTube: Mechanophore’s “Molecular Orbitals from Hybrid Atomic Orbitals”
Link: YouTube: Mechanophore’s ”Molecular Orbitals from Hybrid Atomic Orbitals” (YouTube)
Instructions: Please watch the video (runtime = 7:02 minutes). This material describes how molecular orbitals arise from hybridized atomic orbitals involved in bonding.
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- Web Media: YouTube: Mechanophore’s “Linear Combination of Atomic Orbitals”
Link: YouTube: Mechanophore’s “Linear Combination of Atomic Orbitals” (YouTube)
Instructions: Please watch the video (runtime = 4:29 minutes). This material illustrates what happens during bonding by using a wavefunction approach.
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- Reading: Mark Bishop’s Chemistry Site’s “MO Theory”
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2.2 Bonding and Antibonding Orbitals
- Reading: UC Davis: ChemWiki’s “Bonding and Antibonding Orbitals”
Link: UC Davis: ChemWiki’s “Bonding and Antibonding Orbitals” (HTML or PDF)
Instructions: Please read the entire webpage. This material gives a brief description of bonding and antibonding orbitals, as well as an example of a homonuclear diatomic molecule, H2. The outside link at the end of the reading refers to an older version of the molecular orbital theory lecture. You may watch it here; however, a more recent lecture covering molecular orbital theory is found in subunit 2.4.
You can access the PDF version of this webpage by clicking “Make PDF” at the top of the page.
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- Reading: UC Davis: ChemWiki’s “Bonding and Antibonding Orbitals”
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2.3 Symmetry and Overlap
- Reading: UC Davis: ChemWiki’s “Overlap of Atomic Orbitals”
Link: UC Davis: ChemWiki’s “Overlap of Atomic Orbitals” (HTML)
Instructions: Please read the entire webpage. Click on the button located at the top of the webpage to activate Java. The virtual experiment allows you to examine the interactions of overlapping atomic orbitals. You may rotate the display by clicking and dragging your mouse within the black area.
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- Reading: UC Davis: ChemWiki’s “Sigma Bonding”
Link: UC Davis: ChemWiki’s “Sigma Bonding” (HTML)
Instructions: Please read the entire webpage. Click on the button located at the top of the webpage to activate Java. The virtual experiment demonstrates a sigma interaction between the two s orbitals.
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- Reading: UC Davis: ChemWiki’s “Symmetry Requirements”
Link: UC Davis: ChemWiki’s “Symmetry Requirements” (HTML)
Instructions: Please read the entire webpage. Click on the button located at the top of the webpage to activate Java. The virtual experiment demonstrates the interaction between s and p atomic orbitals, resulting in nonbonding molecular orbitals. An explanation of what occurs is found below the display.
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- Reading: UC Davis: ChemWiki’s “Overlap of Atomic Orbitals”
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2.4 Molecular Orbital Theory
- Lecture: MIT: Principles of Chemical Science, Fall 2008: “Lecture 14: Molecular Orbital Theory”
Link: MIT: Principles of Chemical Science, Fall 2008: “Lecture 14: Molecular Orbital Theory” (Adobe Flash, Mp4, or iTunes)
Also available in:
YouTube
Instructions: Please watch the lecture (runtime = 51:24 minutes). Please also watch the first part of Lecture 15 (approx. 3:45) for a conclusion to the lecture on MO theory.
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- Reading: UC Davis: ChemWiki’s “Molecular Orbital Theory”
Link: UC Davis: ChemWiki’s “Molecular Orbital Theory” (HTML)
Instructions: Please read the entire webpage and work through the five questions found at the end of the reading. This material ties together all of the material you have learned in Unit 2.
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- Lecture: MIT: Principles of Chemical Science, Fall 2008: “Lecture 14: Molecular Orbital Theory”
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2.5 Molecular Orbital Diagrams
- Reading: UC Davis: ChemWiki’s “Molecular Orbital Diagrams”
Link: UC Davis: ChemWiki’s “Molecular Orbital Diagrams” (HTML)
Instructions: Please read the entire webpage. Click on the button located at the top of the webpage to activate Java. The virtual experiment allows you to examine what each molecular orbital looks like on the molecule, either individually or together, by examining its isosurfaces.
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- Reading: UC Davis: ChemWiki’s “Molecular Orbital Diagrams”
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Unit 3: Transition Metals
Transition metals differ from s- and p-block metals because electrons in the d orbitals are available for coordination and bonding. Each atom has a total of 5 d orbitals, accommodating up to 10 electrons total. In a metal complex, these d orbitals do not possess the same energy as they do in single isolated atoms; rather, they have different energies that are determined by their specific molecular geometry and their coordinated ligands. Electrons populate the low energy d orbitals first; however, these electrons can be easily excited from a low energy d orbital to a higher energy d orbital (a process known as “electronic excitation”) or can be easily removed from the metal complex (a process known as “ionization”). The physical/chemical behavior and reactivity of a transition metal depend strongly on the number of d-electrons in the molecule. In this unit, you will learn how d orbitals are organized in a metal complex and how electrons populate these orbitals. The resulting electronic structure of the transition metal complexes determines properties such as magnetism and color.
Unit 3 Time Advisory show close
Unit 3 Learning Outcomes show close
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3.1 Physical Properties
- Reading: UC Davis: ChemWiki’s “Periodic Trends”
Link: UC Davis: ChemWiki’s “Periodic Trends” (HTML)
Instructions: Please read the entire webpage and work through the six questions found at the end of the reading. This material covers the basic periodic trends of d-block transition metals.
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- Reading: UC Davis: ChemWiki’s “Periodic Trends”
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3.2 VSEPR Structures of Transition Metals
- Reading: UC Davis: ChemWiki’s “Molecular Geometry”
Link: UC Davis: ChemWiki’s “Molecular Geometry” (HTML)
Instructions: Please read the entire webpage. This material describes valence shell electron pair repulsion and how it gives rise to molecular geometries. Please also click on the individual geometries of the molecules for a more thorough explanation of each.
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- Reading: UC Davis: ChemWiki’s “Molecular Geometry”
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3.3 Nomenclature of Transition Metal Complexes
- Lecture: MIT: Principles of Chemical Science, Fall 2008: “Lecture 27: Transition Metals”
Link: MIT: Principles of Chemical Science, Fall 2008: “Lecture 27: Transition Metals” (Adobe Flash, Mp4, or iTunes)
Also available in:
YouTube
Instructions: Please watch the lecture, starting around 9:30 (total runtime = 45:07 minutes). This material covers the introductory material about d-block transition metals, including nomenclature and electron counting.
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- Reading: University of Rhode Island’s “Chemistry 401 Nomenclature of Transition Metal Complexes”
Link: University of Rhode Island’s “Chemistry 401 Nomenclature of Transition Metal Complexes” (HTML)
Instructions: Please read the entire webpage and work through the given examples. The only way to become fluent in nomenclature is practice! This material covers naming transition metal complexes, first addressing the cationic and neutral molecules, then covering the anionic molecules.
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- Reading: Purdue University: George M. Bodner’s “Nomenclature of Complexes”
Link: Purdue University: George M. Bodner’s “Nomenclature of Complexes” (HTML)
Instructions: Please read the entire webpage and work the five review problems at the bottom. The only way to become fluent in nomenclature is practice! This material summarizes the naming process of transition metal complexes.
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- Lecture: MIT: Principles of Chemical Science, Fall 2008: “Lecture 27: Transition Metals”
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3.4 Isomers of Transition Metal Complexes
- Reading: University of the West Indies: Robert J. Lancashire’s “Isomerism in Coordination Compounds”
Link: University of the West Indies: Robert J. Lancashire’s “Isomerism in Coordination Compounds” (HTML)
Instructions: Please read the entire webpage. This material covers several types of isomers of transition metal complexes. It is important to note which are structural isomers and which are stereoisomers.
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- Reading: Purdue University: George M. Bodner’s “Isomers”
Link: Purdue University: George M. Bodner’s “Isomers” (HTML)
Instructions: Please read the entire webpage. The images in this material are helpful in remembering the different types of isomers and their subsequent naming.
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- Reading: University of the West Indies: Robert J. Lancashire’s “Isomerism in Coordination Compounds”
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3.5 Electron Configurations of Transition Metals
- Reading: Purdue University: George M. Bodner’s “Transition Metals”
Link: Purdue University: George M. Bodner’s “Transition Metals” (HTML)
Instructions: Please read the entire webpage and work through the practice problem. This material familiarizes you with the electron configuration of transition metals and introduces oxidation states, which will be further discussed in sub-subunit 3.5.2.
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- Reading: Purdue University: George M. Bodner’s “Transition Metals”
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3.5.1 Eighteen Electron Rule
- Reading: Rob Toreki’s Organometallic HyperTextBook: “The 18 Electron Rule”
Link: Rob Toreki’s Organometallic HyperTextBook: “The 18 Electron Rule” (HTML)
Instructions: Please read the entire webpage. Also work the 10 self-test problems at the bottom of the page. This material introduces the two main methods of counting electrons. Both will give you the correct answer if executed properly. You may choose which one you wish to use, or attempt both.
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- Reading: Rob Toreki’s Organometallic HyperTextBook: “The 18 Electron Rule”
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3.5.2 Oxidation States
- Reading: UC Davis: ChemWiki’s “Oxidation States of Transition Metals”
Link: UC Davis: ChemWiki’s “Oxidation States of Transition Metals” (HTML)
Instructions: Please read the entire webpage. This material describes the multiple oxidation states of transition metals and how electrons are lost from the full valence. Please be aware that Co and Cr have unique electron filling in their highest s orbitals. The external links at the bottom of the page show how to approach these types of problems stepwise and are an invaluable learning tool.
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- Reading: UC Davis: ChemWiki’s “Oxidation States of Transition Metals”
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3.6 Valence Bond Theory
- Reading: Purdue University: George M. Bodner’s “The Valence-Bond Approach to Bonding in Complexes”
Link: Purdue University: George M. Bodner’s “The Valence-Bond Approach to Bonding in Complexes” (HTML)
Instructions: Please read the entire webpage and work through the practice problem. This material describes how electron configurations can be used to describe bonding in metal complexes.
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- Reading: Purdue University: George M. Bodner’s “The Valence-Bond Approach to Bonding in Complexes”
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3.7 Crystal Field Theory
- Lecture: MIT: Principles of Chemical Science, Fall 2008: “Lecture 28: Crystal Field Theory”
Link: MIT: Principles of Chemical Science, Fall 2008: “Lecture 28: Crystal Field Theory” (Adobe Flash, Mp4, or iTunes)
Also available in:
YouTube
Instructions: Please watch the lecture (runtime = 45:24 minutes). This material covers crystal field theory.
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- Reading: UC Davis: ChemWiki’s “Crystal Field Theory”
Link: UC Davis: ChemWiki’s “Crystal Field Theory” (HTML or PDF)
Instructions: Please read the entire webpage. This material introduces the idea of splitting within the orbitals. This phenomenon gives rise to color and magnetic properties of complexes. Please also work the five problems at the end of the reading. The answers can be found at the bottom of the page of files by clicking on the “answers” link. They are referenced by molecular geometry and spin type. You may access the PDF version of this page by clicking the “Make PDF” button on the link above.
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- Reading: Purdue University: George M. Bodner’s “Crystal Field Theory”
Link: Purdue University: George M. Bodner’s “Crystal Field Theory” (HTML)
Instructions: Please read the entire webpage and work through the practice problem. This material describes the splitting of orbital energy levels in crystal field theory. Please notice that the molecular geometry of the molecule and the nature of the ligand play important roles in the electronic configurations.
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- Lecture: MIT: Principles of Chemical Science, Fall 2008: “Lecture 28: Crystal Field Theory”
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3.7.1 Spectrochemical Series
- Reading: UC Davis: ChemWiki’s “Spectrochemical Series”
Link: UC Davis: ChemWiki’s “Spectrochemical Series” (HTML)
Instructions: Please read the entire webpage. This material discusses the spectrochemical series, or the influence of the ligands on orbital splitting. The sigma and pi orbital interactions are also discussed.
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- Reading: UC Davis: ChemWiki’s “Spectrochemical Series”
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3.7.2 Crystal-Field Splitting Parameter
- Reading: UC Davis: ChemWiki’s “Energy Level Splitting”
Link: UC Davis: ChemWiki’s “Energy Level Splitting” (HTML)
Instructions: Please read the entire webpage. This material focuses on the splitting of energy levels and the spectroscopic implications that arise from it. This information helps explain why a ruby is red while an emerald is green.
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- Reading: UC Davis: ChemWiki’s “Energy Level Splitting”
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3.7.3 High Spin/Low Spin Complexes
- Reading: UC Davis: ChemWiki’s “High Spin and Low Spin”
Link: UC Davis: ChemWiki’s “High Spin and Low Spin” (HTML)
Instructions: Please read the entire webpage. This information allows you to determine whether a complex will be high spin or low spin, which is critical in predicting its spectroscopic and magnetic behavior. Work through the four examples in the text and then the six questions at the end of the reading.
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- Reading: UC Davis: ChemWiki’s “High Spin and Low Spin”
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3.7.4 Magnetism
- Reading: UC Davis: ChemWiki’s “Magnetic Properties of Coordination Complexes”
Link: UC Davis: ChemWiki’s “Magnetic Properties of Coordination Complexes” (HTML)
Instructions: Please read the entire webpage. This information discusses magnetism, focusing on paramagnetism and how the electron configuration causes a complex to react to a magnetic field.
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- Reading: UC Davis: ChemWiki’s “Magnetic Properties of Coordination Complexes”
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3.7.5 Jahn-Teller Distortions
- Reading: University of Rhode Island’s “Chemistry 401: Thermodynamics, Geometries Other Than Octahedral, Jahn-Teller”
Link: University of Rhode Island’s “Chemistry 401: Thermodynamics, Geometries Other Than Octahedral, Jahn-Teller” (HTML)
Instructions: Please read the entire webpage. This material describes how changes in molecular geometry affect the stability of a complex. When this occurs through slight distortions from “true” geometries, it is referred to as a Jahn-Teller distortion. Note that LFSE stands for ligand field stabilization energy and is also a measure of stability.
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- Reading: University of Rhode Island’s “Chemistry 401: Thermodynamics, Geometries Other Than Octahedral, Jahn-Teller”
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3.8 Ligand Field Theory
- Reading: Purdue University: George M. Bodner’s “Ligand Field Theory”
Link: Purdue University: George M. Bodner’s “Ligand Field Theory” (HTML)
Instructions: Please read the entire webpage. This material describes a third theory to explain the bonding and properties of coordination complexes.
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- Reading: Purdue University: George M. Bodner’s “Ligand Field Theory”
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3.8.1 Sigma Bonding
- Reading: UC Davis: ChemWiki’s “Sigma Bonding”
Link: UC Davis: ChemWiki’s “Sigma Bonding” (HTML)
Also available in:
PDF
Instructions: Please read the entire webpage. This material summarizes ligand-field theory and provides an interactive visual representation of a sigma bond between Cr and CO.
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- Reading: UC Davis: ChemWiki’s “Sigma Bonding”
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3.8.2 Pi Bonding
- Reading: UC Davis: ChemWiki’s “Pi Bonding in Coordination Compounds”
Link: UC Davis: ChemWiki’s “Pi Bonding in Coordination Compounds” (HTML)
Also available in:
PDF
Instructions: Please read the entire webpage. This material provides an interactive visual representation of the pi interaction between Cr and CO.
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- Assessment: University of Rhode Island’s “Chemistry 401: d-Metal Complexes Practice Problems”
Link: University of Rhode Island’s “Chemistry 401: d-Metal Complexes Practice Problems” (HTML)
Instructions: Please work through problems 1–11. The answers are provided by clicking on the links at the end of each question.
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- Reading: UC Davis: ChemWiki’s “Pi Bonding in Coordination Compounds”
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Unit 4: Electronic Spectra of Transition Metal Complexes
As mentioned in the previous unit, electrons in d orbitals can be easily excited to higher energy d orbitals. The intense colors of transition metal complexes are indicative of these transitions. The unique absorption spectra that arise from metal complexes are often used in trace metal analysis by spectrophotometric techniques. Electronic excitations are measured using UV-Vis spectroscopy, which will be discussed in this unit. Other spectroscopic techniques used for metal complexes will be discussed in the next unit.
Unit 4 Time Advisory show close
Unit 4 Learning Outcomes show close
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4.1 Introduction to the Electronic Transitions and Colors in Transition Metal Complexes
- Lecture: MIT: Principles of Chemical Science, Fall 2008: “Lecture 30: Magnetism and Spectrochemical Theory”
Link: MIT: Principles of Chemical Science, Fall 2008: “Lecture 30: Magnetism and Spectrochemical Theory” (Adobe Flash, Mp4, or iTunes)
Also available in:
YouTube
Instructions: Please watch the lecture (runtime = 39:22 minutes). This material demonstrates, theoretically and visually, the ability of metal complexes to appear as radically different colors based on the type of ligand and its interaction with the metal.
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- Reading: Jim Clark’s Chemguide: “The Colours of Complex Metal Ions”
Link: Jim Clark’s Chemguide: “The Colours of Complex Metal Ions” (HTML)
Instructions: Please read the entire webpage. This material discusses the physical process of color perception as well as the electronic properties that created colored complexes.
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- Reading: UC Davis: ChemWiki’s “Colors of Coordination Complexes”
Link: UC Davis: ChemWiki’s “Colors of Coordination Complexes” (HTML)
Instructions: Please read the entire webpage and work through the three examples within the text. This material demonstrates how the crystal field and ligand field theories are applied to predict photophysical properties of transition metal complexes.
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- Lecture: MIT: Principles of Chemical Science, Fall 2008: “Lecture 30: Magnetism and Spectrochemical Theory”
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4.2 UV-Vis Spectra
- Reading: University of Alberta’s Inorganic Chemistry Spectroscopy Tutorial: “UV-Visible Spectroscopy”
Link: University of Alberta’s Inorganic Chemistry Spectroscopy Tutorial” “UV-Visible Spectroscopy” (HTML and Adobe Flash)
Instructions: Please navigate the pages of the tutorial on UV-Vis spectroscopy. Be sure to click on the links within the presentation for answers to questions and supplemental information. This material explains how UV-Vis light interacts with inorganic complexes to produce UV-Vis spectra.
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- Reading: University of Alberta’s Inorganic Chemistry Spectroscopy Tutorial: “UV-Visible Spectroscopy”
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4.3 Tanabe-Sugano Diagrams
- Reading: UC Davis: ChemWiki’s “Tanabe-Sugano Diagrams”
Link: UC Davis: ChemWiki’s “Tanabe-Sugano Diagrams” (HTML)
Instructions: Please read the entire webpage. The material shows how Tanabe-Sugano diagrams are used to analyze spectroscopic data and manipulate photophysical properties of complexes. Please also work through the five questions at the bottom of the webpage.
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- Reading: UC Davis: ChemWiki’s “Tanabe-Sugano Diagrams”
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4.4 Charge Transfer in Electronic Spectroscopy
- Reading: UC Davis: ChemWiki’s “Electronic Spectroscopy: Interpretation”
Link: UC Davis: ChemWiki’s “Electronic Spectroscopy: Interpretation” (HTML)
Instructions: Please read the entire webpage. The material is a review of electronic spectra; however, it also discusses metal-ligand and ligand-metal charge transfer in metal complexes.
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- Reading: UC Davis: ChemWiki’s “Electronic Spectroscopy: Interpretation”
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4.5 Selection Rules of Electronic Transitions
- Reading: UC Davis: ChemWiki’s “Selection Rules and Transition Moment Integral”
Link: UC Davis: ChemWiki’s “Selection Rules and Transition Moment Integral”
Instructions: Please read the entire webpage. The material explains allowed and forbidden electronic transitions with reference back to character tables discussed in Unit 1. It also provides vibrational and rotational selection rules.
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- Reading: University of the West Indies: Robert J. Lancashire’s “Selection Rules for Electronic Spectroscopy”
Link: University of the West Indies: Robert J. Lancashire’s “Selection Rules for Electronic Spectroscopy” (HTML)
Instructions: Please read the entire webpage. The material presented is a concise summary of the spin and LaPorte (orbital) selection rules of electronic spectra.
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- Reading: UC Davis: ChemWiki’s “Selection Rules and Transition Moment Integral”
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Unit 5: Spectroscopy of Transition Metal Complexes
Spectroscopic techniques are usually associated with organic molecules and analytical methods. However, inorganic chemists also use these physical methods to identify compounds and explore their practical applications. The interaction of radiation in infrared (IR) spectroscopy, or magnetic fields in nuclear magnetic resonance (NMR) spectroscopy and electron paramagnetic resonance (EPR) spectroscopy, with metal complexes, allows examination of their physical properties. This unit discusses how these spectra are produced as well as what information can be obtained from the spectra. In particular, EPR of these complexes has proven useful in the fields of semiconductors and biochemistry for predicting chemical properties.
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5.1 Infrared Spectroscopy
- Reading: University of Alberta’s Inorganic Chemistry Spectroscopy Tutorial: “Infrared Spectroscopy”
Link: University of Alberta’s Inorganic Chemistry Spectroscopy Tutorial “Infrared Spectroscopy” (HTML and Adobe Flash)
Instructions: Please navigate the pages of the tutorial on IR spectroscopy. Be sure to click on the links within the presentation for answers to questions and supplemental information. This material explains how IR radiation interacts with inorganic complexes to produce IR spectra.
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- Reading: University of Alberta’s Inorganic Chemistry Spectroscopy Tutorial: “Infrared Spectroscopy”
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5.2 Nuclear Magnetic Resonance Spectroscopy
- Reading: University of Alberta's Inorganic Chemistry Spectroscopy Tutorial “Nuclear Magnetic Resonance (NMR) Spectroscopy”
Link: University of Alberta's Inorganic Chemistry Spectroscopy Tutorial “Nuclear Magnetic Resonance (NMR) Spectroscopy” (HTML and Adobe Flash)
Instructions: Please navigate the pages of the tutorial on NMR spectroscopy. Be sure to click on the links within the presentation for answers to questions and supplemental information. This material explains how the magnetic field interacts with inorganic complexes to produce NMR spectra.
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- Reading: Rob Toreki’s Organometallic HyperTextBook: “Fluxionality”
Link: Rob Toreki’s Organometallic HyperTextBook: “Fluxionality” (HTML)
Instructions: Please read the entire webpage. Also work the three self-test problems at the bottom of the page. This material discusses dynamic NMR and how to resolve and interpret spectra of fluxional molecules.
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- Reading: University of Alberta's Inorganic Chemistry Spectroscopy Tutorial “Nuclear Magnetic Resonance (NMR) Spectroscopy”
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5.3 Electron Paramagnetic Resonance Spectroscopy
- Reading: UC Davis: ChemWiki’s “EPR: Theory”
Link: UC Davis: ChemWiki’s “EPR: Theory” (HTML)
Instructions: Please read the entire webpage. The material introduces the theory of electron paramagnetic resonance (EPR), which is similar to NMR spectroscopy. Because it gives information about its surroundings, EPR is often utilized for biochemical and semiconductor applications.
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- Reading: UC Davis: ChemWiki’s “EPR: Theory”
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Unit 6: Organometallics of Transition Metals
Organometallic chemistry is the study of chemical compounds containing bonds between carbon atom(s) and a metal. Organometallic chemistry combines aspects of inorganic chemistry and organic chemistry. The properties of these complexes are largely dependent on the molecular orbital splittings involved. These were discussed in Unit 3, which you may wish to revisit at this time. Organometallic complexes have characteristics of both organic molecules and transition metals, and therefore they have a wide variety of applications, both current and potential. Many biological molecules, like hemoglobin and chlorophyll, are actually organometallic complexes.
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- Lecture: MIT: Principles of Chemical Science, Fall 2005: “Lecture 32: Coordination Complexes and Ligands”
Link: MIT: Principles of Chemical Science, Fall 2005: “Lecture 32: Coordination Complexes and Ligands” (Adobe Flash, Mp4, or iTunes)
Also available in:
YouTube
Instructions: Please watch the lecture (runtime = 50:57 minutes). This material covers ligand interaction in coordination complexes and relies on your knowledge of molecular orbital splitting to understand why. Be sure you have a firm grasp of the material covered in Unit 3 prior to watching this video.
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- Reading: Purdue University: George M. Bodner’s “Coordination Complexes and Ligands”
Link: Purdue University: George M. Bodner’s “Coordination Complexes and Ligands” (HTML)
Instructions: Please read the entire webpage and work the practice problem contained within the text. This material gives an overview of the chemistry involved in coordination complexes and their ligands.
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- Lecture: MIT: Principles of Chemical Science, Fall 2005: “Lecture 32: Coordination Complexes and Ligands”
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6.1 Different Types of Ligands
- Reading: Jim Clark’s Chemguide: “An Introduction to Complex Metal Ions”
Link: Jim Clark’s Chemguide: “An Introduction to Complex Metal Ions” (HTML)
Instructions: Please read the entire webpage. This material examines the relationship between a central metal ion and its ligands, or what is bound to it. Discussion also includes different types of ligands, starting with simple anion and monodentate ligands and progressing to polydentate ligands.
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- Reading: Jim Clark’s Chemguide: “An Introduction to Complex Metal Ions”
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6.2 Chelating Ligands and the Dentate Terminology
- Reading: University of Rhode Island’s “Chemistry 401 Ligands”
Link: University of Rhode Island’s “Chemistry 401 Ligands” (HTML)
Instructions: Please read the entire webpage. The material includes terminology relating to ligands and their binding nature as well as several structures of the ligands themselves. Oftentimes, ligands are represented by abbreviation only, so it is useful to familiarize yourself with their structure here.
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- Reading: Rob Toreki’s Organometallic HyperTextBook: “Coordination Number and Coordination Chemistry Definitions”
Link: Rob Toreki’s Organometallic HyperTextBook: “Coordination Number and Coordination Chemistry Definitions” (HTML)
Instructions: Please read the entire webpage. This site presents more complex problems dealing with determining the coordination numbers of molecules. It also defines a few more terms. Focus on the terminology here; aromatic ring systems and coordination numbers will be addressed in subunit 6.3.
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- Reading: University of Rhode Island’s “Chemistry 401 Ligands”
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6.3 Metal Coordination to Aromatic Systems
- Reading: Rob Toreki’s Organometallic HyperTextBook: “Cyclopentadienyl Ligands”
Link: Rob Toreki’s Organometallic HyperTextBook: “Cyclopentadienyl Ligands” (HTML)
Instructions: Please read the entire webpage. This material addresses bonding between metal ions and aromatic ring systems such as cyclopentadiene. Cyclopentadiene is commonly abbreviated Cp and is an instance where you are required to remember the structure. Fluxionality of the ligands, which was discussed in subunit 5.2, is also mentioned here.
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- Reading: Rob Toreki’s Organometallic HyperTextBook: “Cyclopentadienyl Ligands”
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Unit 7: Oxidation and Reduction Chemistry
One of the most unique properties of transition metals is their ability to take multiple oxidation states. This ability is extremely important in reaction mechanisms, such as the “oxidative addition” or “reductive elimination” of ligands, which will be discussed in the next unit. Oxidation states are also critical in determining the total electron count, geometrical shape, and magnetic properties of the metal complexes. In fact, the reactivity of transition metals and their metal complexes is highly dependent on their oxidation states and redox properties. Biologically important molecules utilize these abilities, especially in enzymes. For example, iron usually has a +2 or +3 charge; however, it has been observed as a +4 or even +5 charge in the transition state of methane monooxygenase. You will learn about these exceptions in your bioinorganic chemistry course.Unit 7 Time Advisory show close
Unit 7 Learning Outcomes show close
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7.1 Reduction-Oxidation Reactions (Redox)
- Reading: Jim Clark’s Chemguide: “Definitions of Oxidation and Reduction (Redox)”
Link: Jim Clark’s Chemguide: "Definitions of Oxidation and Reduction (Redox)" (HTML)
Instructions: Please read the entire webpage. This material is a review of general electrochemistry and terminology.
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- Reading: Western Oregon University: Dr. Arlene Courtney’s “Diagrams That Provide Useful Oxidation-Reduction Information”
Link: Western Oregon University: Dr. Arlene Courtney’s “Diagrams That Provide Useful Oxidation-Reduction Information” (HTML)
Instructions: Please read the entire webpage. This material defines what relevant information can be obtained from Latimer, Frost, and Pourbaix diagrams.
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- Reading: Purdue University: George M. Bodner’s “Oxidation-Reduction Reactions”
Link: Purdue University: George M. Bodner’s “Oxidation-Reduction Reactions” (HTML)
Instructions: Please read the entire webpage and work the six practice problems contained within the text. This material demonstrates how to balance redox reactions under various conditions, such as in acid or base.
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- Reading: Jim Clark’s Chemguide: “Definitions of Oxidation and Reduction (Redox)”
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7.1.1 Half Reactions
- Reading: Jim Clark’s Chemguide: “Writing Ionic Equations for Redox Reactions”
Link: Jim Clark’s Chemguide: “Writing Ionic Equations for Redox Reactions” (HTML)
Instructions: Please read the entire webpage. This material reviews how to balance redox reactions using the half-reaction method. Examples 2 and 3 are quite involved but well-explained. Please note: these reactions are done in acidic or neutral media.
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- Reading: Jim Clark’s Chemguide: “Writing Ionic Equations for Redox Reactions Done Under Alkaline Conditions”
Link: Jim Clark’s Chemguide: "Wringing Ionic Equations for Redox Reactions Done Under Alkaline Conditions" (HTML)
Instructions: Read the entire webpage. This material reviews how to balance redox reactions using the half-reaction method in basic media.
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- Reading: Jim Clark’s Chemguide: “Writing Ionic Equations for Redox Reactions”
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7.1.2 Kinetic factors (Outer Sphere and Inner Sphere Electron Transfer)
- Reading: University of Rhode Island’s “Chemistry 401: Kinetic Considerations”
Link: University of Rhode Island’s “Chemistry 401: Kinetic Considerations” (HTML)
Instructions: Please read the entire webpage. This material discusses overpotentials and mechanisms of electron transfers. Simply stated, this helps explain why a reaction may not proceed even though it is energetically favored.
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- Reading: University of Rhode Island’s “Chemistry 401: Kinetic Considerations”
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7.2 Pourbaix Diagrams
- Reading: Western Oregon University: Dr. Arlene Courtney’s “Pourbaix Diagrams”
Link: Western Oregon University: Dr. Arlene Courtney’s "Pourbaix Diagrams" (HTML)
Instructions: Please read the entire webpage. This material dissects Pourbaix diagrams, which are used to predict the dominant ionic species given certain conditions. Please work the four example problems found in the body of the text to ensure that you understand how to read these types of diagrams.
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- Reading: Western Oregon University: Dr. Arlene Courtney’s “Pourbaix Diagrams”
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7.3 Marcus Theory of Electron Transfer
- Reading: University of Oxford: Dr. Dermot O’Hare’s “Lecture 3: Electron Transfer Reactions”
Link: University of Oxford: Dr. Dermot O’Hare’s “Lecture 3: Electron Transfer Reactions” (HTML)
Instructions: Please use the “next page” link in the upper right corner to navigate through the slides. The presentation covers the first part of a lecture on electron transfer reactions.
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- Reading: University of Oxford: Dr. Dermot O'Hare's “Lecture 4”
Link: University of Oxford: Dr. Dermot O'Hare's "Lecture 4" (HTML)
Instructions: Use the “next page” link in the upper right corner to navigate through the slides. The presentation continues the lecture on electron transfer reactions.
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- Reading: University of Oxford: Dr. Dermot O’Hare’s “Lecture 3: Electron Transfer Reactions”
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Unit 8: Reaction Mechanisms of d-Metal Complexes
Ligands in a metal ion complex can be substituted by other ligands to give the new metal complex certain novel chemical or physical properties. Ligand substitutions can occur via a number of different mechanisms. In metal complexes with different ligands, some ligands can be substituted faster and easier than other ligands. The geometries of molecules also play an important role in substitution reactions. In order to make a prediction of the reaction product, the mechanism of ligand substitution must be identified.
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8.1 Equilibrium Constants and Stability of Coordination Compounds
- Reading: University of the West Indies: Robert J. Lancashire’s “Stability”
Link: University of the West Indies: Robert J. Lancashire’s “Stability” (HTML)
Instructions: Please read the entire webpage. The material makes an important distinction between kinetic and thermodynamic stability.
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- Reading: University of the West Indies: Robert J. Lancashire’s “Stability, Chelation and the Chelating Effect”
Link: University of the West Indies: Robert J. Lancashire’s “Stability, Chelation and the Chelating Effect” (HTML)
Instructions: Please read the entire webpage and watch the seven-second video clip at the end of the text. Please also attempt “CALCULATION # ONE” and “CALCULATION # TWO” contained within the text. The chelate effect is presented with regard to stability and chelation. It is important to note that monodentate ligands are easier to displace, and therefore they are considered less favorable, than polydentate ligands.
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- Reading: University of the West Indies: Robert J. Lancashire’s “Stability”
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8.2 Mechanisms of Ligand Substitution
- Reading: Jim Clark’s Chemguide: “Complex Metal Ions—Ligand Exchange Reactions”
Link: Jim Clark’s Chemguide: “Complex Metal Ions—Ligand Exchange Reactions” (HTML)
Instructions: Please read the entire webpage. The reactions presented here primarily deal with water displacement from hexaaqua complexes.
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- Reading: Jim Clark’s Chemguide: “Complex Metal Ions—Ligand Exchange Reactions”
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8.2.1 Kinetic and Thermodynamic Considerations
- Reading: University of Oxford: Dr. Dermot O’Hare’s “Introduction to Inorganic Reaction Mechanisms”
Link: University of Oxford: Dr. Dermot O’Hare’s “Introduction to Inorganic Reaction Mechnisms” (HTML)
Instructions: Please read the information covered on the webpage. This material discusses general considerations and terminology of reaction mechanisms. It is important to note that proposed mechanisms can never be proven, but some may be disproven.
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- Reading: University of Oxford: Dr. Dermot O’Hare’s “Introduction to Inorganic Reaction Mechanisms”
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8.2.2 Substitution of Square Planar Complexes
- Reading: University of Oxford: Dr. Dermot O'Hare’s “Lecture 1”
Link: University of Oxford: Dr. Dermot O'Hare’s “Lecture 1” (HTML)
Instructions: Use the “next page” link in the upper right corner to navigate through the slides. The presentation focuses on reaction mechanisms of square planar metal complexes.
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- Reading: University of Oxford: Dr. Dermot O'Hare’s “Lecture 1”
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8.2.3 Substitution in Octahedral Complexes
- Reading: University of Oxford: Dr. Dermot O’Hare’s “Lecture 2”
Link: University of Oxford: Dr. Dermot O’Hare’s “Lecture 2” (HTML)
Instructions: Use the “next page” link in the upper right corner to navigate through the slides. The presentation focuses on reaction mechanisms of octahedral metal complexes.
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- Reading: University of Oxford: Dr. Dermot O’Hare’s “Lecture 2”
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8.3 Reaction Kinetics
- Lecture: MIT: Principles of Chemical Science, Fall 2005: “Lecture 33: Ligand Substitution Reactions: Kinetics”
Link: MIT: Principles of Chemical Science, Fall 2005: “Lecture 33: Ligand Substitution Reactions: Kinetics” (Adobe Flash, Mp4, or iTunes)
Also available in:
YouTube
Instructions: Watch the lecture (runtime = 46:18 minutes) on the kinetics of ligand substitution reactions. Please also watch the beginning of Lecture 34 for the conclusion of the lecture on kinetics (approx 8:22 minutes). It is important to note that reactions may be photochemically or thermally driven, and the same reactants could have completely different products depending on the mechanism.
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- Lecture: MIT: Principles of Chemical Science, Fall 2005: “Lecture 33: Ligand Substitution Reactions: Kinetics”
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Unit 9: Catalysis
In general, catalysts can be divided into two categories—heterogeneous and homogeneous. In a heterogeneous reaction system, the catalyst is in a different phase than are the reactants. Consider, for example, the synthesis of isopropylbenzene, where isopropylbenzene is produced by alkylation of benzene with propylene using a crystalline zeolite (an aluminum silicate molecular sieve)as a catalyst. The reagents are in gas phase, and the reaction takes place only when these reagents are activated on the zeolite (solid) surface. In homogeneous catalysis, on the other hand, the reagents and the catalyst are in the same phase, usually dissolved in solution. Consider, for example, olefin metathesis using Grubbs’s catalyst, where both reagents and the catalyst (a ruthenium-based carbine) are dissolved in the same solution.
Unit 9 Time Advisory show close
In this unit, you will draw upon much of the knowledge of inorganic chemistry you have accumulated thus far in your studies in order to understand catalytic cycles in industrial applications. Industrial applications studied in this unit specifically include the conversion of ammonia to nitric acid, the Haber process, and the Contact Process.
Unit 9 Learning Outcomes show close
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9.1 General Principle
- Reading: Jim Clark’s Chemguide: “Types of Catalysis”
Link: Jim Clark’s Chemguide: “Types of Catalysis” (HTML)
Instructions: Please read the entire webpage. This material explains the basic concepts of catalysis. The two major types of catalysis are homogeneous, where the reactants and catalyst are in the same phase, and heterogeneous, where the reactants and the catalyst are in different phases. Examples of each are given.
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- Reading: Jim Clark’s Chemguide: “Types of Catalysis”
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9.2 Industrial Applications of Inorganic Catalysis
- Reading: Jim Clark’s Chemguide: “Catalysts in Inorganic Industrial Processes”
Link: Jim Clark’s Chemguide: “Catalysts in Inorganic Industrial Processes” (HTML)
Instructions: Please read the entire webpage. The conversion of ammonia to nitric acid is covered in detail on this page. Please follow the links to read more about the Contact Process, for the production of sulfuric acid, and the Haber Process, for the production of ammonia. Also note whether the processes involve homogeneous or heterogeneous catalysis.
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- Reading: Jim Clark’s Chemguide: “Catalysts in Inorganic Industrial Processes”
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Unit 10: Practical Applications of Inorganic Compounds
Inorganic compounds and organometallic compounds have many interesting real-world applications. Some simple compounds, such as cis-[Pt(NH3)2Cl2], are the basis for successful chemotherapy drugs. Medicinal inorganic chemistry as a discipline has only existed for about the last 30 years, since the discovery of the antitumor activity of cisplatin, cis-[Pt(NH3)2Cl2]. Pt-based combination chemotherapy remains the mainstay for the treatment of solid malignancies (especially testicular, ovarian, and small cell lung cancers). In this unit, we will also learn about the application of other transition metal complexes to medicine.
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Other organometallic complexes exhibit unique photophysical properties, such as light absorption and light emissions, that find useful applications in solar cells and electronic displays. Exploitation of the redox properties of metal complexes allows new generations of batteries to constantly emerge into the market. This unit looks at the practical applications and new technologies in each of these areas.
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10.1 Medicinal and Pharmaceutical Chemistry
- Reading: PBWorks’ “Organometallic Pharmaceuticals”
Link: PBWorks’ “Organometallic Pharmaceuticals” (HTML)
Also available in:
PDF
Instructions: Please read the entire webpage. This material gives a short background of organometallic chemistry and how organometallic complexes are useful in the pharmaceutical field. The two main classifications discussed here are anticancer drugs and antimicrobials.
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- Reading: PBWorks’ “Organometallic Pharmaceuticals”
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10.1.1 Platinum
- Reading: Mitch Miller for University of Bristol’s Molecule of the Month (August 2000): “Cisplatin”
Link: Mitch Miller for University of Bristol’s Molecule of the Month (August 2000): “Cisplatin” (HTML)
Instructions: Please use the available information links on the left side of the screen to navigate through the information. You may also access interactive views of the molecules by clicking on the “Chime” or ChemSymphony” links under the structure on the left side of the page.
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- Reading: University of Illinois: Jane L. Stanley’s “Overcoming Resistance to the Antitumor Action of Cisplatin: New Compounds and Modes of Delivery”
Link: University of Illinois: Jane L. Stanley’s “Overcoming Resistance to the Antitumor Action of Cisplatin: New Compounds and Modes of Delivery” (PDF)
Instructions: Please click on the third from last link in the “Literature Seminar” section of Fall 2004 to open the PDF file. This article discusses some of the problems and new advances with platinum-based anticancer drugs.
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- Reading: Mitch Miller for University of Bristol’s Molecule of the Month (August 2000): “Cisplatin”
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10.1.2 Ruthenium
- Reading: University of Illinois: Mark Ringenberg’s “Organoruthenium Anticancer Agents: Scope and Reactivity”
Link: University of Illinois: Mark Ringenberg’s “Organiruthenium Anticancer Agents: Scope and Reactivity” (PDF)
Instructions: Please click on the second-to-last link in the “Literature Seminar” section of Fall 2007 to open the PDF file. This article explores a ruthenium-based organometallic complex as a possible replacement to current platinum-based anticancer drugs.
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- Reading: University of Illinois: Mark Ringenberg’s “Organoruthenium Anticancer Agents: Scope and Reactivity”
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10.1.3 Vanadium
- Reading: University of Illinois: Natasha H. Yeung’s “Insulin Mimetic Vanadium Compounds”
Link: University of Illinois: Natasha H. Yeung’s “Insulin Mimetic Vanadium Compounds” (PDF)
Instructions: Please click on the last link in the “Literature Seminar” section of Fall 2004 to open the PDF file. This article introduces a vanadium compound which may prove useful in the treatment and control of diabetes.
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- Reading: University of Illinois: Natasha H. Yeung’s “Insulin Mimetic Vanadium Compounds”
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10.2 Solar Cells
- Reading: Bulletin of Japan Society of Coordination Chemistry, Volume 51 (2008), 3–12: Michael Graetzel’s: “Transition Metal Complexes as Sensitizers for Efficient Mesoscopic Solar Cells”
Link: Bulletin of Japan Society of Coordination Chemistry, Volume 51 (2008), 3–12:Michael Graetzel’s: “Transition Metal Complexes as Sensitizers for Efficient Mesoscopic Solar Cells” (PDF)
Instructions: Please click on the link to download the PDF of this review article. This material is comprehensive about recent advances in inorganic chemistry with the application to solar cells. It also covers some material on electronic displays, which will be discussed in subunit 10.3.
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- Reading: University of Illinois: Tom Mahle’s “Photoelectrochemical Synthesis: Beyond Gratzel Cells”
Link: University of Illinois: Tom Mahle’s “Photoelectrochemical Synthesis: Beyond Gratzel Cells” (PDF)
Instructions: Please click on the third link in the “Literature Seminar” section of Fall 2010 to open the PDF file. This material probes the use of iridium for conversion of solar energy to fuel.
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- Web Media: Science Daily, April 13, 2011: “Device Proves Solar Cell Potential of High Bandgap Inorganic Nanowire Arrays”
Link: Science Daily, April 13, 2011: “Device Proves Solar Cell Potential of High Bandgap Inorganic Nanowire Arrays” (HTML)
Instructions: Please read the article. This material demonstrates advances in inorganic chemistry for the application of zinc chemistry in both nanowires and solar cells.
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- Reading: Bulletin of Japan Society of Coordination Chemistry, Volume 51 (2008), 3–12: Michael Graetzel’s: “Transition Metal Complexes as Sensitizers for Efficient Mesoscopic Solar Cells”
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10.3 Electronic Displays
- Reading: University of Wisconsin’s Exploring the Nanoworld: “LEDs”
Link: University of Wisconsin’s Exploring the Nanoworld “LEDs” (HTML and QuickTime Video)
Instructions: Please read the entire webpage. This material explains how LEDs work, the preparation of LEDs, and practical applications. Remember that chemical compostion affects the molecular orbitals of molecules, and knowledge of how to manipulate these orbitals, in turn, is useful when tuning LEDs.
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- Reading: University of Illinois: Nathan Eddingsaas’ “Cyclometalated Iridium and Platinum Phosphors in OLEDs”
Link: University of Illinois: Nathan Eddingsaas’ “Cyclometalated Iridium and Platinum Phosphors in OLEDs” (PDF)
Instructions: Please click on the second link in the “Literature Seminar” section of Fall 2004 to open the PDF file. This material proposes the inclusion of inorganic complexes into traditional organic light emitting diodes (OLEDs) to increase efficiency.
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- Reading: University of Illinois: Noel Chang’s “Copper Coordination Compounds as Highly Emissive Dopants in Organic LEDs”
Link: University of Illinois: Noel Chang’s “Copper Coordination Compounds as Highly Emissive Dopants in Organic LEDs” (PDF)
Instructions: Please click on the first link in the “Literature Seminar” section of Fall 2010 to open the PDF file. This material discusses the current status of inorganic materials used in OLEDS and proposes the use of copper as a low cost alternative.
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- Web Media: Ars Technica: John Timmer’s "Scientists Make Bendable, Transparent LEDs—Without Organics"
Link: Ars Technica: John Timmer’s “Scientists Make Bendable, Transparent LEDs—Without Organics” (HTML)
Instructions: Please read the article. This material discusses the development of a flexible, transparent LED that is less expensive to produce than traditional organic LEDs. The findings from this research are being applied to development of a new type of television screen. The advancements discussed here are just an example of the inorganic research that occurs on a daily basis.
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- Reading: University of Wisconsin’s Exploring the Nanoworld: “LEDs”
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10.4 Batteries
- Reading: UC Davis: ChemWiki’s “Case Study: Battery Types”
Link: UC Davis: ChemWiki’s “Case Study: Battery Types” (HTML)
Instructions: Please read the entire webpage and work the eight practice problems at the bottom of the page. This material provides a more detailed explanation of the different types of batteries and the chemical reactions that occur in each.
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- Reading: UC Davis: ChemWiki’s “Batteries: Electricity Through Chemical Reactions”
Link: UC Davis: ChemWiki’s “Batteries: Electricity Through Chemical Reactions” (HTML)
Instructions: Please read the entire webpage and work the five practice problems at the bottom of the page. The basic principles of electrochemistry of batteries are covered. Different types of batteries are also introduced.
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- Reading: UC Davis: ChemWiki’s “Rechargeable Batteries”
Link: UC Davis: ChemWiki’s “Rechargeable Batteries” (HTML)
Instructions: Please read the entire webpage. The chemistry of three types of secondary cell (rechargeable) batteries is discussed.
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- Web Media: How Stuff Works: “How Lithium-Ion Batteries Work”
Link: How Stuff Works: “How Lithium-Ion Batteries Work” (HTML and Adobe Flash)
Instructions: Please read the first three sections of this article. Several advantages and disadvantages of lithium-ion batteries are discussed. The reactions inside the batteries are explained and the validity of “exploding batteries” is revealed.
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- Reading: UC Davis: ChemWiki’s “Case Study: Battery Types”
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Final Exam
- Final Exam: The Saylor Foundation’s CHEM202 Final ExamLink: The Saylor Foundation’s CHEM202 Final ExamInstructions: You must be logged into your Saylor Foundation School account in order to access this exam. If you do not yet have an account, you will be able to create one, free of charge, after clicking the link.
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- Final Exam: The Saylor Foundation’s CHEM202 Final Exam
