Wednesday, 20 July 2011

Computer Science Video Lectures

I was about to post video lectures in Business and Management when I found an amazing collection of undergraduate (and a few graduate) Computer Science video lecture courses.

Don't forget to check my other posts on Computer Science andTheoretical Computer Science video lectures.

Here are this month's video lectures, most of them from New Jersey Institute of Technology and some from Google, and other places


A Taste of Haskell (Functional Programming Language)



  • Haskell Video Lecture Part I
  • Haskell Video Lecture Part II
  • Lecture Notes (.pdf)
  • Description:Haskell is the world's leading purely functional programming language that offers a radical and elegant attack on the whole business of writing programs. In the last two or three years there has been an explosion of interest in Haskell, and it is now being used for a bewildering variety of applications.In this tutorial, the lecturer will try to show you why programming in Haskell is such fun, and how it makes you think about programming in a new way.
    He's going to use xmonad as his running example; it's an X11 window manager written entirely in 500 lines of Haskell. Based on xmonad he will show you how to
    • write functional programs
    • test them using QuickCheck
    • write imperative programs
    • call foreign functions
    • use Haskell for scripting applications
    The lecturer won't assume you know any functional programming at all, but he will assume that you are an experienced professional programmer, so he'll will move along quite briskly.

Monday, 11 July 2011

axonomy of Chemical Species, Origins of Modern Chemistry

axonomy of Chemical Species, Origins of Modern Chemistry
This video course by Prof. Donald Sadoway, MIT, explores the basic principles of chemistry and their application to engineering systems. It deals with the relationship between electronic structure, chemical bonding, and atomic order. It also investigates the characterization of atomic arrangements in crystalline and amorphous solids: metals, ceramics, semiconductors, and polymers (including proteins). Topics covered include organic chemistry, solution chemistry, acid-base equilibria, biochemistry, chemical kinetics, diffusion, and phase diagrams.


www.rudrachem.blogspot.com

Orissa Joint Entrance Exam OJEE 2011 Notification

JOINT ENTRANCE EXAMINATION-2011, ORISSA

Date of Examination :
Sunday, May 1, 2011 (MCA;MBA;PGDM;PGCM;PGDM(Executive);M.Pharm)
Sunday, May 8, 2011 (B.TECH;B.ARCH;MBBS;BDS;B.PHARM; Diploma Test for Lateral Entry (Engineering/Technology/Pharmacy);PGAT(M.Tech/M.Arch))
Sale of Application form begins on : February 25, 2011
Last date of sale of application forms : March 18, 2011
Last date of receipt of completed application form : March 21, 2011
Online registration through OJEE-2011 website begins on : February 25, 2011
Last date for online registration : March 15, 2011
Last date of receipt of confirmation slip and demand draft : March 21, 2011
(for online applicant only)

For further detail information regarding OJEE‐2011, Please log on to www.odishajee.com

Admission Guidance(Chennai TOP Colleges)-2011

Hello all of u. We will provide you free guidance for following courses who wish to join TOP rated colleges in Tamilnadu.B.E.,B.Tech(All branches),Pharma-D,Ag.B.Sc,M.E,M.tech(All specializations),M-Pharm,MBA(B-schools),MCA etc.. for more details please feel free to ask any questions regarding career and further education @ 9642819693

Admissions for B.Tech/B.E || B.Tech/B.E Online Admissions @ Saagam.com

Saagam.com started the service of “Online Admissions Booking for Educational Institutions”.
From Saagam.com you can directly book your admission in your dreamed college without any mediator. 
Colleges which provides the Online Admissions for B.Tech/B.E
AMC Engineering College, 
K.S Institute of Technology, 
Reva institution of Technology and management, 
Sri Venkateswara Engineering College, 
T.John Institute of Technology.
Visit the below given address for more details about admissions such as course details, fees, eligibility and etc.
http://saagam.com/admissions/colleges/?s=2&l=2&cc=3&c=-&f=-&p=1
If you have any queries please feel free to send a mail to info@saagam.com. Saagam Team always welcomes you to clarify your queries. 
***************** All the Best ***************
 Saagam.com

Bachelor of Science in Nursing

Are you an RN who wants to earn a BSN? Can’t imagine juggling work, school and family? This degree is flexible, affordable and doable. Choose the smart way to move ahead in your nursing career.
The RN to BSN program at SUNY Delhi provides educational mobility for registered nurses who are seeking a Bachelor of Science in Nursing. The curriculum is designed with the working registered nurse in mind and offers versatility and flexibility as the program is 100% online. Precepted practicum experiences for select courses are completed in the student's hometown area.
The program emphasizes critical thinking and practice skills necessary for clinical management of patients within a constantly changing health care environment.
A total of 120 credits is required to earn a BSN at SUNY Delhi, however, the length of the program varies depending on the number of appropriate courses transferred in from previous college coursework. Students typically transfer in between 60 and 80 credits.
Accreditation NLNAC Accreditation logo
SUNY Delhi's RN to BSN Program is accredited by the National League for Nursing Accrediting Commission. NLNAC is located at 3343 Peachtree Road NE, Suite 500, Atlanta, Georgia, 30326; phone: 404-975-5000. 
Program Highlights
  • Flexible scheduling that meets the needs of working professionals by allowing students to advance in the program part-time or full-time, with opportunities to begin the program in Fall, Spring, or Summer semesters
  • Easy to use, web-supported classes with technical assistance
  • A state of the art curriculum delivered by a faculty with the highest credentials in the field
  • Affordable SUNY tuition rates
  • An opportunity to pursue your degree with other motivated professionals
  • Additional online upper division liberal arts courses available from SUNY Delhi  

ACS Career Fair – August 28-31, 2011

International Year of Chemistry 2011 (IYC 2011)

http://portal.acs.org/portal/acs/corg/content?_nfpb=true&_pageLabel=PP_SUPERARTICLE&node_id=14&use_sec=false&sec_url_var=region1&__uuid=d9a2b823-a4ee-4493-b795-f5dc2685529c

Friday, 8 July 2011

Chemistry Central Journal conferences in July

The broad, multidisciplinary nature of Chemistry Central Journal means that we are always interested in research that links together work from different subject areas. That is why next week, we will be attending conferences onThe Science of Ageing – Global Progress, and Catalysis and Sensing for the Environment (CASE).
The Science of Ageing takes place in Brighton, UK from 11th–14th July and is being co-organised by Lizzy Ostler, Section Editor for Chemistry Central Journal. Studies into ageing have traditionally been dominated by biological research groups, but in recent years, the potential impact of chemical analysis and small molecule interventions has become widely recognised. Research into ageing spans the full range of chemistry and there are an increasing number of chemists working in this area.
To highlight this, Chemistry Central Journal has organised a lunch reception on the penultimate day of the meeting specifically for the chemists who are attending. Here, we will formally announce a new thematic series on Chemistry of Ageing to recognise the growing contributions that chemists are making to the field.
The CASE meeting is a one-day conference at the University of Birmingham, UK organised by Chemistry Central Journal Editorial Board Member John Fossey. In addition to the more traditional lectures, the conference will feature three lightning sessions, in which the speaker must deliver 20 slides with just 20 seconds allowed per slide. The lightning sessions, powered by Chemistry Central Journal, are an example of the changing way in which chemistry is communicated.

Toward a More Efficient Use of Solar Energy

 The exploitation and utilization of new energy sources are considered to be among today's major challenges. Solar energy plays a central role, and its direct conversion into chemical energy, for example hydrogen generation by water splitting, is one of its interesting variants. Titanium oxide-based photocatalysis is the presently most efficient, yet little understood conversion process. In cooperation with colleagues from Germany and abroad, scientists of the KIT Institute for Functional Interfaces (IFG) have studied the basic mechanisms of photochemistry by the example of titania and have presented new detailed findings.
                                          Even though hydrogen production from water and sunlight by means of oxide powders has been studied extensively for several decades, the basic physical and chemical mechanisms of the processes involved cannot yet be described in a satisfactory way. Together with colleagues from the universities of St. Andrews (Scotland) and Bochum and Helmholtz-Forschungszentrum Berlin, scientists at KIT's Institute for Functional Interfaces, headed by Professor Christof Wöll, have succeeded in gathering new findings on the fundamental mechanisms of photochemistry on titanium dioxide (TiO2


Titanium dioxide, or titania, is a photoactive material occurring in nature in the rutile and anatase modifications, the latter of which being characterized by a ten times higher photochemical activity. When the white TiO2 powder, which is also used as a pigment in paints and sunscreens, is exposed to light, electrons are excited and can, for example, split water into its components oxygen and hydrogen. The hydrogen produced in that way is a "clean" energy source: No climate-killing greenhouse gases are generated but only water is produced during combustion. Titanium dioxide is also used to manufacture self-cleaning surfaces from which unwanted films are removed through photochemical processes triggered by incident sunlight. In hospitals, this effect is used for sterilizing specially coated instruments by means of UV irradiation 

So far, the physical mechanisms of these photochemical reactions on titania surfaces and especially the reason for the much higher activity of anatase could not be explained. The powder particles used in photoreactors are as tiny as a few nanometers only and are thus too small for use in studies by means of the powerful methods of surface analysis. By using instead mm-sized single-crystal substrates, the researchers were for the first time able to precisely study photochemical processes on the surface of titanium dioxide by means of a novel infrared spectrometer.
Using a laser-based technique, the scientists, in addition, determined the lifetime of light-induced electronic excitations inside the TiO2 crystals. According to Professor Christof Wöll, Head of the IFG, exact information about these processes is of great importance: "A short lifetime means that the excited electrons fall back again at once: We witness some kind of an internal short circuit. In the case of a long lifetime, the electrons remain in the excited state long enough to be able to reach the surface of the crystal and to induce chemical processes." Anatase is particularly well suited for the latter purpose because it is provided with a special electronic structure that prevents "internal short circuits."
Knowledge of this feature will allow the researchers to further optimize shape, size, and doping of anatase particles used inside photoreactors. The objective is to develop photoactive materials with higher efficiencies and longer lifetimes: "The results obtained by Professor Wöll and his co-workers are of great importance regarding the generation of electrical and chemical energy from sunlight, and especially regarding the optimization of photoreactors," says Professor Olaf Deutschmann, spokesman of the Helmholtz Research Training Group on "Energy-related Catalysis

QuantumWise

When Every Atom MattersPDFPrintE-mail

First-principles simulation software for nanoscience

Atomistix ToolKit (ATK) from QuantumWise is a software package that offers unique capabilities for simulating electrical transport properties of nanodevices on the atomic scale. Based on an open architecture which integrates a powerful scripting language with a graphical user interface, ATK is a comprehensive platform for studies in nanoelectronics, using methods that range from both accurate quantum-mechanical first-principles and fast semi-empirical methods to classical potentials for very fast geometry optimizations and molecular dynamics calculations.
A special focus is placed on treating large-scale systems, with several thousand atoms. Moreover, ATK includes a very advanced electrostatic model to allow realistic simulations of nanoscale transistor structures.
ATK also offers basic electronic structure calculations, including geometry optimization, of molecules and periodic structures like bulk crystals, nanotubes, slabs, etc.
The software is used by over 100 research groups at leading universities, government labs, and electronics companies around the world, in a wide range of application areas. Since 2006, over 300 scientific articles were published using ATK, and many new unique features are planned for release during 2011.

NMR/MRI Applied to Microfluidic Chromatography


ScienceDaily (July 6, 2011) — By pairing an award-winning remote-detection version of NMR/MRI technology with a unique version of chromatography specifically designed for microfluidic chips, researchers with the U.S. Department of Energy (DOE)'s Lawrence Berkeley National Laboratory (Berkeley Lab) have opened the door to a portable system for highly sensitive multi-dimensional chemical analysis that would be impractical if not impossible with conventional technologies.

Alexander Pines, a faculty senior scientist in Berkeley Lab's Materials Sciences Division and the Glenn T. Seaborg Professor of Chemistry at the University of California (UC) Berkeley, is one of the word's foremost authorities on NMR (nuclear magnetic resonance) and its daughter technology, MRI (Magnetic Resonance Imaging). In this latest development, he led a collaboration in which a remote detection NMR/MRI technique that can rapidly identify the chemical constituents of samples in microfluidic "lab-on-a-chip" devices was used to perform analyses in a microscale monolithic chromatograph column.
"We have presented the first demonstration that a monolithic chromatograph column can be used to separate small molecules on a timescale that is compatible with NMR/MRI detection, an important first step to portable chromatographic devices," says Vikram Bajaj, a project scientist in the Pines' group who is the corresponding author of a paper describing this work in the journal Analytical Chemistry.
The Analytical Chemistry paper is titled "Remotely Detected NMR for the Characterization of Flow and Fast Chromatographic Separations Using Organic Polymer Monoliths." Co-authoring the paper with Pines and Bajaj were Thomas Teisseyre, Jiri Urban†, Nicholas Halpern-Manners, Stuart Chambers and Frantisek Svec.
Chromatography is one of the indispensable tools of chemistry. By dissolving sample into a fluid -- called the "mobile phase" -- and flushing it through a solid medium -- called the "stationary phase" -- chemists can separate the sample's constituent chemical species -- called analytes -- for identification and measurement, as well as for purification purposes. Analytes will be separated on the basis of how fast each individual species diffuses through the stationary phase.
"The coupling of our remote NMR/MRI technology with monolithic chromatography columns in a microfluidic chip enables us to obtain high resolution, velocity-encoded images of a mobile phase flowing through the stationary phase," Bajaj says. "Our technique provides both real-time peak detection and chemical shift information for small aromatic molecules, and demonstrates the unique power of magnetic resonance, both direct and remote, in studying chromatographic processes."
The coupling of remote NMR/MRI to chromatography was made possible by the polymer monolithic column, a technology developed by Analytical Chemistry paper co-author Frantisek Svec, a chemist who directs the Organic and Macromolecular Synthesis facility at Berkeley Lab's Molecular Foundry, a DOE nanoscience center. In conventional chromatography, the stationary phase column is typically filled with porous polymer beads or some other discrete medium whose physical or chemical properties modulate the diffusion rates of analytes passing through. In Svec's stationary phase, a chromatography column is filled with a monolithic solid polymer -- meaning it is a single, continuous piece -- that is perforated throughout with nanoscopic pores.
"Polymer monoliths as a separation media can be compared to a single large particle that does not contain inter-particular voids," Svec says. "As a result, all the mobile phase must pass through the stationary phase as convective flow rather than diffusion during chromatographic processes. This convective flow greatly accelerates the rate of analyte separation."
The remote NMR/MRI technology whose development was led by Pines won a 2011 R&D 100 Award. These awards, known as the "Oscars of Innovation," recognize the year's 100 most significant proven technological advances. Through a combination of remote instrumentation, JPEG-style image compression algorithms and other key enhancements, this remote NMR/MRI technology can zoom in on microscopic objects of interest within a sample flowing through the columns of a microfluidic chip with unprecedented spatial and time resolutions.
"Our remote NMR/MRI technology enables time-resolved imaging of multi-channel flow, dispenses with the need for large and expensive magnets for analysis, allows us to analyze complex and unprocessed mixtures in one pass, and adds portability to NMR/MRI," Bajaj says.
The key to the success of remote NMR/MRI technology is the decoupling of the NMR/MRI signal encoding and detection phases. NMR/MRI signals arise from a property found in the atomic nuclei of almost all molecules called "spin," which makes the nuclei act as if they were bar magnets with poles that point either "north" or "south." Obtaining an NMR/MRI signal from a sample depends upon an excess of nuclear spins pointing in one direction or the other. In a conventional NMR/MRI set-up, in which the signal encoding and detection phases take place within one machine, this require the presence of a powerful external magnetic field. The remote NMR/MRI technology developed by Pines and his group, in which NMR?MRI signal encoding and detection are carried out independently, can detect NMR/MRI signals without the need of such a strong magnet, yet it still provides the same outstanding sensitivity of conventional NMR/MRI.
"With our remote NMR/MRI technology and the polymer monoliths of Frank Svec's group, we were able to look inside optically opaque microfluidic columns and measure the velocity of the flowing fluid during a chromatographic separation," Bajaj says. "We were also able to demonstrate in-line monitoring of chromatographic separations of small molecules at high flow rates."
Results using the remote NMR/MRI technique with the polymer monoliths showed a much better ability to discriminate between different analytes at the molecular level, Bajaj says, than comparable analysis using spectrometry based on either mass or optical properties. This paves the way for multidimensional analysis, in which the result of a chromatographic separation would be encoded into an NMR/MRI signal by charge, size or some other factor and stored. The encoded fluid would then be run through a second separation and those results would also be encoded into an NRM/MRI signal and stored.
"This would allow us to create a multidimensional chromatography experiment that does not require the fluid volume to be physically partitioned," Bajaj says. "The fluid would, quite literally, be partitioned in the magnetic degrees of freedom instead."
This research was funded by the DOE Office of Science.
Email or share this story:

nano coating/sealant

the uses and importance of nanotechnology in our day to day life.

http://www.nanocare-ag.com/produkte/

Branch offices: New family of gold-based nanoparticles could serve as biomedical 'testbed'

ScienceDaily (2011-07-07) -- Researchers have demonstrated a sort of gold nanoparticle "testbed" to explore how the tiny particles behave in biological systems.

Thursday, 7 July 2011

Science News

http://rudrachem.blogspot.com/p/physical-chemistry/2011/06/110627123036.htm

chemistry of cooking

http://www.sciencedaily.com/videos/2009/0112-chemistry_of_cooking.htm

EVAPORATION


It is the process whereby atoms or molecules in a liquid state (or solid state if the substance sublimes) gain sufficient energy to enter the gaseous state.
It is the opposite process of condensation. The thermal motion of a molecule of liquid must be sufficient to overcome the surface tension and evaporate, that is, its kinetic energy must exceed the work function of cohesion at the surface.
Evaporation therefore, proceeds more quickly at higher temperature, at higher flow rates between the gaseous and liquid phase and in liquids with lower surface tension (i.e.
higher vapor pressure).
Since only a small proportion of the molecules are located near the surface and are moving in the proper direction to escape at any given instant, the rate of evaporation is limited.
Also, as the faster-moving molecules escape, the remaining molecules have lower average kinetic energy, and the temperature of the liquid thus decreases.
This phenomenon is also called evaporative cooling.
This is the reason that evaporating sweat cools the human body.
For more information about the topic Evaporation, read the full article at Wikipedia.org

greatest discoveries in the field of chemistry

http://science.discovery.com/convergence/100discoveries/big100/chemistry.html

Saturday, 16 April 2011

Latimer diagram and frost diagram

Schaums Outline Of Chemistry Foundations

A solved-problem Outline for students with no high school chemistry background or a poor course in high school chemistry. All topics are presented at an elementary level to commensurate with the introductory course; simpler math is assumed and developed, a less intense approach to the basic concepts of chemistry, and a simpler manner of presentation. There are hundreds of solved and supplementary problems.

A solved-problem Outline for students with no high school chemistry background or a poor course in high school chemistry. All topics are presented at an elementary level to commensurate with the introductory course; simpler math is assumed and developed, a less intense approach to the basic concepts of chemistry, and a simpler manner of presentation. There are hundreds of solved and supplementary problems.click here to download




CSIR Bio-inorganic Chemistry paper

 Download the question papers for CSIR exam which is given below if you have any problem in downloading . write your problem in the comment section.All the best wishes for your preparation.

click here to download

Cellular Neurobiology(MIT)

Physics I: Classical Mechanics

Genomics and Computational Biology (Audio only)


This course will assess the relationships among sequence, structure, and function in complex biological networks as well as progress in realistic modeling of quantitative, comprehensive, functional genomics analyses. Exercises will include algorithmic, statistical, database, and simulation approaches and practical applications to medicine, biotechnology, drug discovery, and genetic engineering. Future opportunities and current limitations will be critically addressed. In addition to the regular lecture sessions, supplementary sections are scheduled to address issues related to Perl, Mathematica and biology.

Structural Aspects of Biomaterials

Video Lectures: Course Bioeng/ME C117
http://webcast.berkeley.edu/courses/archive.php?seriesid=1906978263
Course covers:
Course Overview, Biocompatibility/FDA Regulatory Agency, Orthopedics, Case Study: Sulzer Recall, Case Study: Hip Implant Corrosion, Final Project Outline, Sterilization Case Study, Wear in Total Joint Replacements, Total Shoulder Replacements; Contact Stress, Contact Stress in Devices; Stress Shielding, Guest Lecture: Dr. Michael Ries, Chief of Arthoroplasty, UCSF, UHMWPE Fatigue, Fatigue Design, Guest Lecture: Dr. Andy Kohm, Spinal Implants, Kyphon, Defect Tolerant Philosophy, Guest Lecture: Professor Rob Ritchie, Fracture in Minerized Tissues, MSME, Dental Materials, Guest Lecture: Vascular Mechanics, In Class Demonstrations: Knee, HIp, Dental, Cardio, Guest Lecture: Dr. Scott Robertson, Stents: Fatigue and Fracture, LBL, Guest Lecture: Dr. Alan Pelton, Stent Design, Nitinol Device Company (NDC), Midterm, No Lecture, Soft Tissue Reconstruction, Breast Implants, Exam Solutions, Wrap-up, No Lecture, Student Presentations

Friday, 15 April 2011

APOLOGY TO ALL

As I am very new to the world of bloggers I do not have much idea about this. If you face some kind of trouble while browsing at my site I apologize for that.

d- and f- Block Chemistry

d- and f- Block Chemistry book provides the fundamentals of d- and f-block metals, including aspects of structure, bonding, chemical thermodynamics and spectroscopy, which underpin studies of the chemistry of these elements. Aims to provide an introduction to the principles underlying the chemistry of the d- and f-block metals. It briefly describes the origins, uses, and importance of these elements before considering the factors underlying their chemical properties. It describes aspects of structure, bonding, chemical thermodynamics and spectroscopy, which underpin studies of the chemistry of these elements. Examples are drawn from different parts of the d- and f-blocks to illustrate particular points and study questions allow you to practice the application of the principles learned.
Click here to download

Thursday, 14 April 2011

Applied Thermodynamics :

Applied thermodynamics is the science of the relationship between heat, work, and systems that analyze energy processes. The energy processes that convert heat energy from available sources such as chemicalfuels into mechanical work are the major concern of this science. Thermodynamics consists of a number of analytical and theoretical methods which may be applied to machines for energy conversion. Related topics:




The Pleasure of Finding Things Out (1981)

Richard Feynman Physics Video Lectures

Richard P. Feynman (1918-1988) was a scientist, teacher, great orator, and musician. He worked on atomic bomb, invented quantum electrodynamics, translated Mayan hieroglyphics, and cut to the heart of the Challenger disaster. But beyond all of that, Dick Feynman was a unique and multi-faceted individual.
www.FeynmanPhysicsLectures.com

keynotes In Organic Chemistry

at
The development of university organic chemistry curricula and the trend towards modularisation of chemistry courses has driven the need for smaller, highly focussed and accessible organic chemistry textbooks, which complement the very detailed “standard texts”, to guide students through the key principles of the subject.
This concise and accessible book provides organic chemistry notes for students studying chemistry and related courses at undergraduate level, covering core organic chemistry in a format ideal for learning and rapid revision. The material is organised so that fundamental concepts are introduced early, then built on to provide an overview of the essentials of functional group chemistry and reactivity, leading the student to a solid understanding of the basics of organic chemistry. Graphical presentation of information is central to the book, to facilitate the rapid assimilation, understanding and recall of critical concepts, facts and definitions.
Students wanting a comprehensive and accessible overview of organic chemistry to build the necessary foundations for a more detailed study will find this book an ideal source of the information they require. In addition, the structured presentation, highly graphical nature of the text and practice problems with outline answers will provide an invaluable framework and aid to revision for students preparing for examinations. 

CSIR UGC JRF NET Chemistry question Paper


list of colleges for MBBS in India

The Origin of Life


In modern organisms, there is a division of labour between two kinds of molecule: DNA, which stores and transmits genetic information, and proteins, which do all the work. They are connected by the 'genetic code', whereby DNA specifies what kinds of proteins can be made. This process of translation is well understood, but it is far too complicated to have arisen by chance in the primitive oceans. How can this apparent paradox be resolved?

Wednesday, 13 April 2011

Introduction to Organic Chemistry II (CHEM 222, McGill University)

Introduction to Organic Chemistry I (CHEM 212, McGill University)

Intro to Organic Chemistry Video Lectures  

Course description:
A survey of reactions of aliphatic and aromatic compounds including modern concepts of bonding, mechanisms, conformational analysis, and stereochemistry.

Course topics:
Chemical Structure Families. Chemistry Nomenclature. Alkanes. Chirality. Stereo Nomenclature. Alkyl Halides. Alkenes. Alkynes. Aromatics.

General Chemistry (CHEM 6A, 6B and 6C, UCSD - University of California San Diego)

introduction to chemistry

General Chemistry (Chem 1A, University of California Berkeley)
http://www.rudrachem.blogspot.com
Course description:
Stoichiometry of chemical reactions, quantum mechanical description of atoms, the elements and periodic table, chemical bonding, real and ideal gases, thermochemistry, introduction to thermodynamics and equilibrium, acid-base and solubility equilibria, introduction to oxidation-reduction reactions.

Course topics:
Atoms, Molecules, Stoichiometry. Atomic Structures, Molecular Formulae. Solutions, Reactions and Bulk Matter. Light Waves, Absorption, Emission. Light, Particles, Photons. Matter: Particles/Waves. Quantum Mechanics: H Atom. Quantum Mechanics Orbitals. Spin, Pauli Principle, Electronic Configurations. Periodic Properties, Trends. Chemical Bonds, Lewis Structures. Covalent Bonding, Resonance. Molecular Structure, VSEPR, Isomers. Covalent, Ionic Bonding, MOs. Hybridization MOs, Resonance. Ideal Gases, Compressibility, Absolute Temperature. Kinetic Gas Theory. Real Gases, Phase Transitions. Thermodynamics: First Law. Thermochemistry, Enthalpy. Specific Heat, Calorimetry, Metabolism. Bond Energies. Entropy, Second Law. Entropy, Second Law. Equilibrium, Mass Action. Equilibrium, Temperature, Le Chatelier. Free Energy, Equilibrium Constant. Heterogeneous Equilibrium. Strong Acids and Bases, pH. Weak Acids and Bases, pK. Titration of Weak Acids. Buffers, Indicators, Acid Strength. Polyprotic Acids, Amino Acids. Reducton Potentials. Galvanic Cells. Nuclear and Radiochemistry. Nuclear Applications. UC Berkeley and the Actinides.


GATE QUESTION PAPERS


CSIR NET JRF Free Online Coaching study material



Monday, 11 April 2011

Women in Nanotechnology Short Science Video Documentary


The Women in Nanotechnology project (WomenInNano) was a 3 year EU Research Project with the aim of finding out ways to support and encourage women working in Nanotechnology.  In 2008 the Vega Science Trust was asked to make a short video film documenting the final meeting to illuminate the work of the project and record the conclusions of the project.

WomenInNano logoWomen in Nanotechnology (WomenInNano): Short Documentary
The Women in Nanotechnology project (WomenInNano) was a 3 year EU Research Project with the aim of finding out ways to support and encourage women working in Nanotechnology.  In 2008 the Vega Science Trust was asked to make a short video film documenting the final meeting to illuminate the work of the project and record the conclusions of the project.

request to all visitors

PLEASE GIVE SOME COMMENTS AND SUGGESTIONS SO THAT I CAN MAKE THIS BLOG MORE INTERESTING AND MORE USEFUL.

BUKYBALL WORKSHOP

Scientist Sir Harry Kroto has given workshops around the world in his quest to engage a range of age groups in learning about science.  In these video recordings you can hear about everything from galaxy formation and fullerenes, to juggling, politics and tortoises.

CHARLES H. TOWNS-SCIENCE VIDEO INTERVIEW

Charles Hard Townes received the Nobel Prize for Phyiscs in 1964 "for fundamental work in the field of quantum electronics, which has led to the construction of oscillators and amplifiers based on the maser-laser principle"  He was award half of the Prize.  The other half of the prize was shared betweeen Nicolay Gennadiyevich Basov and Aleksandr Mikhailovich Prokhorov.
 

INTRODUCTION TO QUANTUM MECHANICS


Lecture notes : MIT


Course Description

This course covers topics in time-dependent quantum mechanics, spectroscopy, and relaxation, with an emphasis on descriptions applicable to condensed phase problems and a statistical description of ensembles.

Thermodynamics & Kinetics


video lecture: MIT


Course Description

This subject deals primarily with equilibrium properties of macroscopic systems, basic thermodynamics, chemical equilibrium of reactions in gas and solution phase, and rates of chemical reactions.

Chemistry of Biomolecules I


lecture notes: MIT

Course Description

5.451 is a half-semester introduction to natural product biosynthetic pathways. The course covers the assembly of complex polyketide, peptide, terpene and alkaloid structures. Discussion topics include chemical and biochemical strategies used to elucidate natural product pathways.

Principles of Chemical Science

video lecture: (MIT)


This course provides an introduction to the chemistry of biological, inorganic, and organic molecules. The emphasis is on basic principles of atomic and molecular electronic structure, thermodynamics, acid-base and redox equilibria, chemical kinetics, and catalysis.

kinetics


1 Chemical kinetics
Prepared by V. Aditya vardhan
adichemadi @ gmail.com
Prepared by
V. ADITYA VARDHAN
VAAGDEVI JUNIOR COLLEGE
WARANGAL
CHEMICAL KINETICS
Chemical kinetics deals with
1) Study of rates of reactions
2) Factors affecting rate of reaction
3) Study of mechanisms of reactions
Rate of reaction  : The rate of reaction is defined as the change in molar concentration of either
reactants or products in unit time.
 
change in concentration
rate r =
time interval
Let ‘dc’ is the decrease in concentration of reactants in a small interval of time ‘dt’ then
dc
r = -
dt
  ( negative sign indicates decrease in concentration )
If ‘dx’ is the increase in concentration of products in a small interval of time ‘dt’ then
dx
r =
dt
  ( positive sign indicates increase in concentration )
E.g., For a reaction, A B 
 
    d A d B
rate r
dt dt

 
In general for a reaction, pP + qQ  rR + sS
the relations between rates of reaction with respect to P,Q,R and S can be written as
        d P d Q d R d S 1 1 1 1
- = - = + = +
p dt q dt r dt s dt
Eg., for the reaction,
      2 g 2 g 3 g
N +3H 2NH  , the relations can be expressed as
      2 2 3 d N d H d NH 1 1
- -
dt 3 dt 2 dt
  
Factors affecting the rate of reaction
1) Nature of reactants:   Rate of a reaction depends on the nature of bonding in the reactants. Ionic
compounds react faster than covalent compounds.
The reactions between ionic compounds in water occur very fast as they involve only exchange of
ions.
Eg., AgCl is precipitated out immediately when AgNO3
 solution is added to NaCl solution.
3 3 AgNO +NaCl AgCl NaNO  
This reaction involves only exchange of ions as shown below and hence occurs very fast.
+ - + - + -
3 3 Ag +NO +Na +Cl AgCl Na NO  
Reactions between covalent compounds take place slowly because they require energy for the
cleavage of existing bonds.
Eg., Following esterification of acetic acid occurs slowly as the breaking of bonds require energy.
C H3 C
OH
O
O C2H5 H C H3 C
OC2H5
O
+ O H2 +
H2SO42 Chemical kinetics
Prepared by V. Aditya vardhan
adichemadi @ gmail.com
Prepared by
V. ADITYA VARDHAN
VAAGDEVI JUNIOR COLLEGE
WARANGAL
2) Concentration:  Rate of a reaction is directly proportional to the concentration of reactants.
rate (r)   cn
where c = concentration
n = order of the reaction
or r = kcn
where k = specific rate
The number of collisions increases with increase in concentration and hence the rate of the reaction
also increases.
The rate of a reaction decreases with time as the concentration of reactants is decreasing. This can
be shown graphically as follows.
concentration of reactants
Time
3) Temperature : The average kinetic energy and hence the number of collisions increase with abso-
lute temperature. Hence rate of reaction increases with increase in temperature.
Usually the rate of a reaction is doubled when the temperature is increased by 10o
C.
Temperature Coefficient : The ratio of rate constants of a reaction at two different temperatures
which differ by 10o
C is called temperature coefficient.
 
o
o
t +10 C
t C
k
Temperature coefficient = 2 to3
k

The relation between rate constant and temperature can be shown by Arrhenius equation.
k = A.e-Ea/RT
Where k = specific rate constant
      A = Frequency factor
      Ea
 = Activation energy
      R = Universal Gas constant
      T = Absolute Temperature
Multiplying by 'ln' (natural logarithm) on both sides,
ln k = ln a
E
A-
RT
or 2.303 log k = 2.303 log
a
E
A-
RT
or log k =
a
E
log A-
2.303 RT
When a graph is plotted by taking log k on y - axis and 1/T on x-axis, a straight line with negative slope
is obtained.
slope =
a
E
-
2.303 R =
a
E
-
4.576
where R = 1.987 cal / K / mole3 Chemical kinetics
Prepared by V. Aditya vardhan
adichemadi @ gmail.com
Prepared by
V. ADITYA VARDHAN
VAAGDEVI JUNIOR COLLEGE
WARANGAL
log A
1
T
Ea
slope =  -
2.303 R
log k
Relation between two rate constants at two different temperatures can be given as
a 2
1 1 2
E k 1 1
log = -
k 2.303R T T
 
 
 
or
  2 1 a 2
1 1 2
T -T E k
log =
k 2.303R TT
4) Catalyst: Catalyst is a substance which alters the rate of reaction without being consumed or without
undergoing any chemical change during the reaction.
A catalyst increases the rate of reaction by providing a new path with lower activation energy for the
reaction. In case of reversible reactions, catalyst lowers the activation energies of both forward and
backward  reaction to the same extent and helps in attaining the equilibrium quickly.

Reaction coordinate
Potential energy
without catalyst
in presence of catalyst
Problems :
1) Write the relations between the rates with respect to reactants & products in the following reaction.
2N2
O  2N2
 + O2
Rate Equation or Rate Expression or Rate Law: Equation that describes mathematical dependance
of rate of reaction on the concentration terms of the reactants is called Rate Equation.
For a general reaction, xA+yB+zC  products.
      r = k A B C x y z
where k= rate constant or specific rate
x,y and z are orders with respects to A,B and C respectively.
Order of reaction :Sum of the powers of the concentration terms in the rate equation is called order
of  reaction.
For a general reaction, xA + yB + zC  products.4 Chemical kinetics
Prepared by V. Aditya vardhan
adichemadi @ gmail.com
Prepared by
V. ADITYA VARDHAN
VAAGDEVI JUNIOR COLLEGE
WARANGAL
if the rate expression is r =         k A B C x y z
Then the order of this reaction is equal to x + y + z
Note: Order of a reaction is to be determined experimentally. It may have positive or negative or zero
or a fractional values.
In case of simple reactions, the order of reaction and hence the rate equation can be written
according to stoichiometric equation. But the actual rate law should be written by conducting experi -
ments.
Depending on the order of reaction, chemical reactions can be divided into zero, first, second &
third order reactions as follows.
Zero order reaction: Total order of the reaction is zero.
Example:
1)  Decomposition of NH3
 on metal surfaces such as gold and molybdenum.
      2 g 2 g 3 g
N +3H 2NH Au

r = k[N2
]
0
[H2
]
0
First order reaction: Total order of the reaction is one.
Examples:
1) Thermal decomposition of N2
O5
N2
O5
  N2
O4
 + 1/2 O2
r = k[N2
O5
]
2) Thermal decomposition of SO2
Cl
2
SO2
Cl
2SO2
+Cl
2
r  = k [ SO2
Cl
2
]
3) Thermal decomposition of H2
O2
H2
O2
  H2
O + 1/2 O2
r  = k[H2
O2
]
4) All radioactive disintegrations
Second order reaction : Total order of the reaction is two.
Examples:
1) Thermal decomposition of N2
O
2N2
O  2N2
 + O2
r= k [N2
O]
2
2) Decomposition of Cl
2
O
2Cl
2
O  2Cl
2
 + O2
r= k [Cl
2
O]
2
Third order reaction : Total order of the reaction is three.
Examples:
1) Reaction between NO and O2
to give NO2
2NO + O2
--------> 2NO2
r = k[NO]
2
[O2
]
2) Reaction between NO and Cl
2
 to give NOCl
2NO + Cl
2
  2NOCl
r = k[NO]
2
 [Cl
2
]5 Chemical kinetics
Prepared by V. Aditya vardhan
adichemadi @ gmail.com
Prepared by
V. ADITYA VARDHAN
VAAGDEVI JUNIOR COLLEGE
WARANGAL
Problems :
1) What is the order of the reaction if the rate law for the reaction A + 2B products is
r = k [A]
1/2
[B]
2
Rate constant (k): The rate of a reaction at the unit concentrations of all the reactants of the reaction is
called specific rate (or) rate constant.
rate = k when [reactants] = 1
Units of rate constant
For a general reaction, A  products
Rate expression can be written as
 
n dc
rate = k A
dt

where n = order of the reaction
 
n
dc 1
k = x
dt A
 Units of
 
n
mole / litre 1
k = x
sec mole / litre
 
1-n
mole / litre
=
sec
  - n-1 n-1 -1
= L .mole .sec
For 1st
 order reaction  sec-1
For 2nd
 order reaction  L.mole-1
sec-1
For 3rd
 order reaction  L2
.mole-2
sec-1
For zero order reaction  mole .L-1
sec-1
Molecularity
Elementary reactions: The chemical reactions which occur in one single step are called elementary
reactions.
But most of the reactions occur in more than one step. The sequence of elementary steps that occur
during a reaction is referred to as mechanism of that reaction.
Rate determining step: The elementary step or reaction with slowest rate is called rate determining step
or rate limiting step. The rate of overall reaction depends on this step.
Molecularity: Total number of atoms or molecules or ions taking part in an elementary reaction is called
molecularity of that elementary reaction (or step).
It is only possible to define the molecularity of an elementary step. But the molecularity of the overall
reaction which involves more than one step cannot be defined.
Molecularity is an integer. It cannot be zero or fractional. The maximum value observed is 3. It can be
deduced theoretically from the proposed mechanism6 Chemical kinetics
Prepared by V. Aditya vardhan
adichemadi @ gmail.com
Prepared by
V. ADITYA VARDHAN
VAAGDEVI JUNIOR COLLEGE
WARANGAL
Differences between Order and Molecularity
Order Molecularity
1) Sum of the powers of concentration terms
in rate expression is called order.
1) Total number of atoms or molecules or
ions taking part in an elementary reaction is
called molecularity
2) It may have zero or positive or negative or
integer or fractional values.
2) It can only have integral values (1,2 or 3).
Its value cannot be zero or fractional.
3) It is determined experimentally 3) It is deduced theoretically from the
mechanism of the reaction.
Integrated rate equations for zero and  first order reactions
Zero order rate equation:
Reactions in which the rate  is independent of the concentrations of reactants are called Zero order
reactions. The integrated rate equation for zero order reactions is derived as follows.
o dc dx
- = =kc
dt dt
or  
o dx
=k a-x k
dt

or dx = k dt
 
or x = kt
or k =
x
t
Where k = specific rate
x = amount of reactant consumed or reacted in time 't'.
First order reaction
For a first order reaction R  P
Let
The initial concentration of reactant = a mol. dm-3
.
Amount of reactant decomposed in 't' sec = x mol. dm-3
.
The concentration of reactant after 't' sec = (a - x ) mol. dm-3
.
 The rate
dx
dt
 
 
 
 at time 't' is proportional to the concentration of reactant (a - x) at that time. Since the
reaction is a first order reaction,
 
dx
a-x
dt

 
dx
k a-x
dt

 
dx
=k.dt
a-x [where k = specific rate]
On integration7 Chemical kinetics
Prepared by V. Aditya vardhan
adichemadi @ gmail.com
Prepared by
V. ADITYA VARDHAN
VAAGDEVI JUNIOR COLLEGE
WARANGAL
 
dx
k.dt
a-x
  
     -ln (a-x) = k.t + c
when t = 0 then x = 0
 -ln a = c
Hence -ln(a-x) = kt-ln a
or
 
a
kt =ln
a-x
or
 
1 a
k = ln
t a-x
or
 
2.303 a
k= log
t a-x
Where a = initial concentration of reactant
x = concentration reacted in an interval of time 't'
(a-x) = concentration of reactant after time 't'
Half life (t
1/2
) of a reaction :The time required for initial concentration of reactants to become half is
called half life.
Half life of first order reaction can be derived as given below.
x = a/2 when t = t
1/2
Then a-x =
a
a-
2
 = a/2
Therefore
1/2 1/2
2.303 a 2.303
k= log log2
t a/2 t
 
  
 
 =
1
2
2.303x 0.3010
t
 (  log2 = 03010)
or 1/2
0.693
t
k

Methods of determination of order of a reaction :
1) Integrated equation method or Trial and error method
* The initial concentration (a) and the concentrations at various intervals of time (a - x) are measured
during the progress of reaction by suitable analytical methods. These values are substituted in the  rate
equations of different rate orders. The order corresponding to the rate equations, which gives constant 'k'
values is taken as the order of reaction.
Rate equations
For  a  Zero order reaction R  P
x = kt
or
  o t
a- a-x R -R x
k = = =
t t t8 Chemical kinetics
Prepared by V. Aditya vardhan
adichemadi @ gmail.com
Prepared by
V. ADITYA VARDHAN
VAAGDEVI JUNIOR COLLEGE
WARANGAL
For  first order reaction     R  P
o
t
R 2.303 a 2.303
k= log = log
t a-x t R
For second order reaction     2R  P
o t
o t
R -R 1 x 1
k= = .
at a-x R t R
For second order reaction R1
 + R2
 P
2.303 ( )
k= log
t(a-b) ( )
b a x
a b x


The order can also be ascertained graphically as follows
For a zero order reaction, the graph of 'x' versus 't' must be a straight line parallel to time (t)  axis.
x
t
For a first order reaction, the graph of
a
log
a-x
 versus  't'   should be a straight line with positive slope
and should pass through the origin
t
a
a-x
log
For a second order reaction, the graph of
 
x
a-x a  vs 't'   must be a straight line passing through the
origin with a positive slope.
t
x
a(a-x)
t
b(a-x)
a(b-x)
log OR
Half life method
Half life   1
2
t  is inversely proportional to an-19 Chemical kinetics
Prepared by V. Aditya vardhan
adichemadi @ gmail.com
Prepared by
V. ADITYA VARDHAN
VAAGDEVI JUNIOR COLLEGE
WARANGAL
1 n -1
2
1
a
t 
where a = initial concentration
n = order
The order 'n' of a reaction can be calculated by comparing two half lives -  1
2
t
 &   1
2
t
 with initial
concentrations a& a  respectively. .
n-1 1
2
1
2
t
a
=
t a

  
 
   
3) Van't Hoff differential method
The rate
dc
-
dt
 for a reaction of nth
 order is given by the equation,
n dc
- =kc
dt
For two initial concentrations c1
,c2
, we have
n 1
1
dc
- =kc
dt
;
n 2
2
dc
- =kc
dt
1
1
dc
log - log k +nlogc
dt
 
   
 
2
2
dc
log - log k +nlogc
dt
 
  
 
or  
1 2
1 2 1 2
dc dc
log - - log - n log c nlogc n log c logc
dt dt
   
       
   
 
1 2
1 2
dc dc
log - - log -
dt dt
n
log c logc
   
   
   
 

For two different initial concentrations c1
 and c2
, the rates are determined at any given time from c-t graph.
These are substituted in the above equation and 'n' is calculated.
concentration of reactants
Time (t)
c1
concentration of reactants
c2
Time (t)
4) Ostwald's Isolation Method
In this method, order with respect to each reactant is determined separately by taking other reactants
in larger quantity.
For example, for the given reactions A + B  products, the order is determined as follows:
1) First the concentration of 'B' is taken in larger excess and the order (nA) with respect to 'A' is deter-
mined by any of the other three methods.10 Chemical kinetics
Prepared by V. Aditya vardhan
adichemadi @ gmail.com
Prepared by
V. ADITYA VARDHAN
VAAGDEVI JUNIOR COLLEGE
WARANGAL
2) In the second experiment the order (nB) with respect to 'B' is determined by taking 'A' in large excess.
The order of the overall reaction is taken as nA +  nB.
Kinetic Molecular Theory of Reaction Rates or Collision theory of reaction rates :
This theory was proposed by Arrhenius. The main postulates of this theory are
1) Chemical reactions occur due to collisions between reactant molecules.
2) But all the collisions do not lead to the formation of products.
3) Only those collisions taking place between molecules possessing certain minimum amount of energy
can form the products. This minimum amount of energy is called Threshold Energy (ET).
4) The energy possessed by the normal molecules under STP conditions is called 'Average Energy'. The
difference between threshold energy and average energy of the reacting molecules is called Activation
energy (Ea
).
Ea
 = Threshold energy (ET) - Average energy (ER)
5) Some molecules will get threshold energy during collisions and are called activated molecules and
denoted by asterick(*).
6) The collisions taking place between activated molecules are called activated collisions. The reaction
occurs only during the activated collisions.
Activated molecules constitute a small fraction of total molecules. Similarly activated collisions consti-
tute small fraction of total collisions. Hence all the chemical reactions do not occur in fraction of second.
A  +  A                 A* + A A
A* + A*              products
Where A = normal molecule
A* = Activated molecule
7) The number of binary collisions per unit time (Z) is given by
2
AB A B
8kT
Z .n .n  
 

where AB   = Collision diameter
     = reduced mass
A B n &n  are number of molecules of A & B
8) The relation between specific rate (k), temperature (T) and activation energy Ea
 can be given as follows
a -E /RT
k =A.e
     or
a -E /RT
k = p.Z.e
where p = probability factor
The concept of activation energies of both forward and backward reactions (Ea
 and Ea
') can be
shown graphically as follows.11 Chemical kinetics
Prepared by V. Aditya vardhan
adichemadi @ gmail.com
Prepared by
V. ADITYA VARDHAN
VAAGDEVI JUNIOR COLLEGE
WARANGAL
R E
a E
T E
T E
1
a
E
p E
H 
Energy barrier
Where ER = Energy of reactants
EP
 = Energy of products
ET = Threshold energy
Ea
 = Activation energy of  forward reaction
Ea
1
 = Activation energy of  backward reaction
H  = Enthalpy of reaction
Problems :
1) The rate constant of a first order reaction is 1.386 sec-1
. What is it's half life.
2) The initial concentration of  A  is 0.5 moles/litre. If the concentration becomes 0.25 mole/litre in 5 sec.
What is the value of rate constant.
TEST YOUR UNDERSTANDING
State whether the following statements are true or false.
1) The rate of a reaction increases with time as the concentration of reactants decreases.
2) The order of a reaction is always determined experimentally.
3) The units of rate constants for the following reaction are (L / mol /sec).
2NO(g)  + Cl
2
 (g)  2NOCl (g)
4) The half life of zero order reaction is proportional to the initial concentration.
5) The rate of consumption of hydrogen gas is thrice of formation of Ammonia in the following reaction.
N2
 (g) + 3H2
 (g)  2 NH3
 (g)
6) In Ostwald isolation method, the reactant for which the order is going to be determined is taken in
excess when compared to the concentrations of other reactants.
7) A positive catalyst increases the activation energy of both forward and backward reactions.
8) In exothermic reaction the activation energy of forward reaction is always greater than that of back
ward reaction.
9) For a second order reaction, a straight line is obtained when log
a
a x 
 is plotted against time (t)
10) Rate of reaction increases with increasing temperature as the threshold energy increases.