Redox
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To find the initial and final oxidation states of a species using a titration: 1. Find the moles of the known reactant and electrons transferred 2. Calculate the moles of electrons transferred per mole of the unknown species to get the change in oxidation state 3. A common mistake is thinking the number of moles of electrons transferred is equal to the coefficient in the half-reaction, when it is actually the number of electrons transferred per mole of reactants.
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![Redox
If given an unfamiliar species, e.g. [Co(NH3)6]2+,
how do I know what can it oxidise/ reduce to?
Look for the species in data booklet.](data:image/gif;base64,R0lGODlhAQABAIAAAAAAAP///yH5BAEAAAAALAAAAAABAAEAAAIBRAA7)
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- The conversion of chemical energy to electrical energy in galvanic/voltaic cells where a spontaneous redox reaction generates an electric current.
2. What are some common types of electrochemical cells?
Some common types of electrochemical cells include:
- Galvanic/voltaic cells such as batteries, which harness the spontaneous redox reaction between two half-cells to generate a voltage. Examples include zinc-
Electron Spin Resonance (ESR) Spectroscopy
Electron Spin Resonance Spectroscopy
Also called EPR Spectroscopy
Electron Paramagnetic Resonance Spectroscopy
Non-destructive technique
Applications
Extensively used in transition metal complexes
Deviated geometries in crystals
23524801-Potentiometry.ppt
Potentiometry is an electroanalytical technique that measures the potential of electrochemical cells under conditions of zero or negligible current. It uses reference and indicator electrodes to measure voltages generated from chemical reactions. Potentiometric cells consist of a reference electrode that maintains a constant potential, a salt bridge to prevent mixing, an analyte solution, and an indicator electrode whose potential varies with analyte concentration. Common reference electrodes include the standard hydrogen electrode, calomel electrode, and silver/silver chloride electrode. Indicator electrodes can be metallic, glass membrane, liquid membrane, crystalline membrane, or gas sensing probes. Potentiometry allows for direct, rapid measurements of ion concentrations and is used in titrations and physiological applications.
T21 IB Chemistry- Spectroscopy continued
This document outlines lessons for a spectroscopy course, including:
1. A review of infrared spectroscopy, mass spectroscopy, and proton NMR spectroscopy.
2. Practice using these techniques to answer exam questions and deduce organic compound structures.
3. Details on high resolution proton NMR, including spin-spin coupling and interpreting splitting patterns.
4. Interpreting NMR spectra to determine functional groups and hydrogen environments.
5. A brief overview of X-ray crystallography and some practice questions reviewing all three techniques.
The course aims to build students' skills in applying spectroscopy methods to organic compound analysis through lessons, examples, and practice questions.
YR12 IB CHEM Lesson 1 Spectroscopic identification of organic compounds.pptx
The document discusses several techniques used to identify organic compounds, including index of hydrogen deficiency (IHD), mass spectrometry (MS), proton nuclear magnetic resonance spectroscopy (1H NMR), and infrared spectroscopy (IR). IHD uses a compound's molecular formula to determine the number of double or triple bonds. MS involves bombarding samples with electrons to form molecular ions that can fragment, providing structural information. 1H NMR provides data on proton environments that also reveals structure. IR identifies functional groups by their absorption of infrared radiation at characteristic frequencies. These techniques are powerful tools for determining organic molecular structures and compositions.
Absorption spectrum of a conjugated dye
This experiment examines the absorption spectra of conjugated dyes using spectroscopy. The objectives are to study how the electronic energy levels of molecules vary with molecular size, and to compare theoretical models to experimental results. Absorption spectra are obtained for several dyes and the maximum wavelength is used to determine the energy difference between the excited and ground states. Theoretical models like the particle in a box model are applied to predict absorption wavelengths, which are then compared to measured values.
04 redox reactions__dissoln.__precip
This document provides a summary of key concepts in oxidation-reduction (redox) reactions:
1) Redox reactions involve the transfer of electrons between chemical species, either through the complete transfer of electrons to form ionic bonds, or partial transfer to form covalent bonds. Oxidation is the loss of electrons and reduction is the gain of electrons.
2) Redox pairs are couples of oxidized and reduced forms of elements that differ in their oxidation state. Common redox pairs include Fe3+/Fe2+, O2/H2O, and MnO4-/MnO2.
3) The standard electrode potential (E°) indicates the tendency of half-reactions to occur.
electrochemistry
Electrochemistry is the study of chemical reactions that involve the transfer of electrons between species. Key concepts include redox reactions, electrode potentials, and the Nernst equation. Electrochemical cells harness the energy of spontaneous redox reactions through the movement of electrons in an external circuit and the compensating flow of ions through an electrolyte. The standard cell potential (E°cell) is equal to the sum of the standard reduction potentials of the cathode and anode half-reactions.
Assignment volumetric analysis_jh_sir-3591
This document provides information about mole concept, oxidation-reduction reactions, and titrations. It begins with defining oxidation and reduction processes and listing examples. Rules for determining oxidation numbers and methods for calculating individual oxidation numbers are outlined. The concepts of oxidizing agents, reducing agents, and disproportionation reactions are explained. The document describes how to balance redox reactions using the ion-electron method in both acidic and basic media. Equivalents, normality, and the law of equivalence are defined. Finally, the document discusses types of titrations and provides a table of common redox titrations.
Kumada cross coupling reaction
The Kumada cross-coupling reaction is a nickel or palladium catalyzed reaction between a Grignard reagent and an organic halide. The reaction proceeds through four steps - oxidative addition, transmetallation, isomerization, and reductive elimination. It is similar to other cross-coupling reactions like Negishi, Stille, Hiyama, and Suzuki reactions. The reaction exhibits cis/trans selectivity and can be made enantioselective using a chiral palladium catalyst. It has applications in synthesizing drugs like Aliskiren and materials for organic solar cells.
Chapter 20
1. Electrochemistry involves electron transfer between chemical species in oxidation-reduction reactions.
2. Oxidation and reduction half-reactions can be balanced using the half-reaction method and combined to give the overall redox reaction.
3. Voltaic cells harness the energy of spontaneous redox reactions by allowing electrons to flow through an external circuit, and cell potential depends on the relative reduction potentials of the half-reactions.
PRINCIPLES OF ESR
Electron spin resonance (ESR) spectroscopy is a technique used to study compounds with unpaired electrons. In ESR, a sample is placed in a static magnetic field and irradiated with microwaves. This causes transitions between the electron spin energy levels. The absorption of microwave energy is detected to obtain an ESR spectrum. ESR spectra provide information about electron environments through parameters like g-values and hyperfine splitting patterns. ESR finds applications in studying transition metal complexes and unstable free radicals.
Electrochemistry
Includes a discussion of Voltaic and electrolytic cells, the Nernst equation and the relationship between electrochemical processes, chemical equilibrium and free energy.
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
Lecture 5.pdf
The document discusses several key concepts in electrochemistry:
1. Junction potentials develop at any point where there is charge separation between solutions of different concentrations. The difference in ion mobility gives rise to liquid junction potentials.
2. At the metal-solution interface, there is an electrical double layer consisting of a tightly bound inner layer and a loosely bound outer layer where the potential decreases exponentially with distance.
3. Currents in electrochemical cells are limited by charge transfer resistance, mass transport resistance, and ohmic solution resistance. Mass transport occurs via diffusion, convection, and migration. Faradic currents are due to redox reactions while non-Faradic currents are due to other processes.
Atoms and Charge
Chemistry is the study of matter and its changes. An atom is the smallest particle of an element that retains the properties of that element. Atoms combine to form compounds with fixed ratios. A chemical change alters the composition of a substance, while a physical change does not. The atomic theory states that elements are composed of atoms and compounds are composed of two or more different elements chemically bonded. The structure of the atom consists of a small, dense nucleus surrounded by electrons. Chemical formulas represent the elements and their ratios in compounds and molecules. Ions are formed when atoms gain or lose electrons. Naming and formulas help identify substances. Acids donate hydrogen ions in water and bases donate hydroxide ions.
NMR applications
1. NMR spectroscopy can be used to investigate molecular properties like conformational isomerism and hydrogen bonding, determine optical purity, and study drug-receptor interactions.
2. 1H NMR spectra provide information on the number of different types of hydrogens, chemical shifts indicating hydrogen types, integration showing the number of each type of hydrogen, and splitting patterns revealing neighboring hydrogens.
3. NMR spectroscopy allows for quantitative analysis including assaying single or multiple components by peak area, determining percent hydrogen in compounds, and analyzing moisture content from water peak ratios.
Electrochemical Cells and Electrode Potentials
Here we discuss about oxidation, reduction reactions, standard Potential, half reaction potential.voltaic Cell , Nernst Equation,
Oxidation-Reduction-Reactions-and-Titrations.ppt
This document discusses oxidation-reduction (redox) reactions and electrochemistry.
1. It explains how to identify redox reactions by checking if the oxidation number (O.N.) of any species changes in the reaction. An example reaction between permanganate and oxalic acid is given.
2. Balancing redox reactions is important, and the document outlines the step-by-step process for balancing both acidic and basic redox reactions.
3. Electrochemical cells are described as either galvanic cells that generate potential or electrolytic cells that consume potential. The standard hydrogen electrode is used as a reference electrode with a standard potential of 0 V.
Intro chem ch 12 chemical bonding sp08
Chemical bonds are attractive forces that hold groups of atoms together. There are two main types of bonds: ionic and covalent. Ionic bonds form between metals and nonmetals and involve the transfer of electrons. Covalent bonds form when atoms share electrons. The octet rule states that atoms seek to obtain a noble gas configuration by gaining, losing, or sharing electrons. Lewis structures can represent ionic and covalent bonding using dots and lines to show valence electrons. Molecular shape is determined by valence shell electron pair repulsion theory.
Intro chem ch 12 chemical bonding sp08
Chemical bonds are attractive forces that hold groups of atoms together. There are two main types of bonds: ionic and covalent. Ionic bonds form between metals and nonmetals via electrostatic attraction as electrons are transferred. Covalent bonds form when atoms share electrons. Lewis structures use dots and lines to represent valence electrons and show how atoms bond to achieve stable electron configurations like the octet rule.
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Redox
- 1. Redox FAQs
- 2. Redox If given an unfamiliar species, e.g. [Co(NH3)6]2+, how do I know what can it oxidise/ reduce to? Look for the species in data booklet.
- 3. Redox How to find initial/ final O.S. of a species using titration? 1. Find the amount (moles) of the known reactant. 2. Find moles of electrons transferred. 3. Find moles of electrons transferred per mole of unknown species = change in O.S.
- 4. Redox How to find initial/ final O.S. of a species using titration? Common Mistake: For the half equation: 2H+ + 2e– H2 If the no. of moles of H+ = 1 no. of moles of e– transferred = 1 NOT 2 since 2H+ takes in 2e–
- 5. Redox How to find initial/ final O.S. of a species using titration? Faster Method (For MCQs) • Find the reacting ratio between the two redox reagents. • Ratio x no. of electrons transferred should be the same for both. Fe2+ MnO4– nratio 4 1 e– 1 ? product 4 4