Biochemistry 675, Lecture 8 Electrostatic Interactions
|
|
- Amberly Wilkinson
- 6 years ago
- Views:
Transcription
1 Biochemistry 675, Lecture 8 Electrostatic Interactions Previous Classes Hydrophobic Effect Hydrogen Bonds Today: Electrostatic Interactions Reading: Handout:P.R. Bergethon & E.R. Simons, Biophysical Chemistry, Springer-Verlag Portions of Ch. 11 & 12
2 Charged residues are found on the surface of proteins
3 The surfaces of biological molecules can be highly charged The EMBO Journal (2006) 25, , doi: /sj.emboj Molecular basis of RNA recognition by the human alternative splicing factor Fox-1 Sigrid D Auweter, Rudi Fasan, Luc Reymond, Jason G Underwood, Douglas L Black, Stefan Pitsch and Frédéric H-T Allain Overview of the solution structure of the RBD of Fox-1 in complex with UGCAUGU
4 The surfaces of biological molecules can be highly charged camp-dependent protein Kinase (1YDR) bound to peptidic H7 protein kinase inhibitor
5
6 Electrostatic interactions are long range and fall off in strength gradually with distance E 1/r n
7 Electrostatic interactions are strong Coulomb s law Interaction energy between an Na + and Cl - separated by 3Å is-110 kcal/mol (in vacuum) Interaction energies of 2 opposite charges in a protein 10 Å apart:-16 kcal/mol (if dielectric is 2) But!Competing interactions with water: desolvation of a unit charge costs about 60 kcal/mol
8 Interaction of Charges with water; The Born Model
9
10 Born Model: A model for understanding Ion-water interactions-a thermodynamic cycle w discharge + w transfer + w charging + (-ΔG i-s )=0 There are no interactions in the transfer of the uncharged sphere into water so w transfer =0 and ΔG i-s = w discharge + w charging
11 ΔG i-s = w discharge + w charging w discharge : Can be determined from the work of charging a sphere in a vacuum; work of transferring infinitesimal bits of charge to the sphere until it has the correct charge w ch arg ing = (z i e o )2 8πε o r i Therefore: w disch arg e = (z i e o )2 8πε o r i For the work of charging the sphere in solvent we have to consider solvent. The dielectric constant must influence charging in solvent. remember: F q 1 q 2 4πε o εr 2 Work of charging the sphere in the solvent: w ch arg ing = (z i e o )2 8πε o εr i
12 ΔG i s = w disch arg e + w ch arg ing ( ΔG i s = z e i o) 2 ( + z e i o) 2 8πε o r i 8πε o εr i ( ΔG i s = z e i o) 2 (1 1 8πε o r i ε ) MolarBasis ΔG i s = N A Enthalpy ( z i e o ) 2 (1 1 8πε o r i ε ) ΔG i s = ΔH i s TΔS i s ΔH i s = N A z i e o ( ) 2 8πε o r i (1 1 ε T ε 2 ε T )
13 Compare the theoretical prediction to the experimentally measured enthalpies of solvation (Fig )
14 Add the structural features of water: 1. Water is a dipole 2. Three types of water can be considered Bulk water An immobilized layer An intermediate layer
15 Thermodynamic cycle For the modified Born Model
16 Good agreement between the calculated and Measured enthalpies of ion-solvent interactions
17 Consider the significance of ion-solvent interactions for everyday procedures used in the lab Example: Salting out
18 What about the other ions?
19 Ion:ion interactions What is the free energy of ion:ion interactions ΔG i-i? Consider an ion in a solution with many other ions: ΔG i i = n i µ i i n i is the number of ions that the reference ion interacts with and µ i-i is the chemical potential for each ion that interacts with the reference. The chemical potential of a single ionic species will be related to the work of charging up a mole of ions of interest while in the proximity of other ions. w ch arg ing = (z i e o )2 8πε o εr i In terms of chemical potential: Δµ i i = N A w ch arg ing Δµ i i = N A z i e o 2 ψ ψ is the electrostatic potential of the ion
20 In order to determine the chemical potential change for the interaction between the total ionic assembly and the ion of interest we must know the electrostatic field at each individual ion that is a result of the other ions in solution. This requires information about the spatial distribution of the ions in the solution relative to the reference ion.
21
22 Erich Armand Arthur Joseph Hückel (in Engl. often spelled Huckel or Hueckel) b. August 9, 1896, Berlin, Germany d. 1980, Marburg, Germany A German physicist and physical chemist. He is known for two major contributions: (a) The Debye-Hückel theory of electrolytic solutions, (b) The Hückel method of approximate molecular orbital (MO) calculations on p-electron systems.
23 Petrus (Peter) Josephus Wilhelmus Debye was born March 24, 1884, at Maastricht, the Netherlands. Debye won Nobel Prize in Chemistry, 1936, "for his contributions to our knowledge of molecular structure through his investigations on dipole moments and on the diffraction of X-rays and electrons in gases". Debye died on November 2, 1966, and was buried on Pleasant Grove Cemetery, Cayuga Heights, Tompkins County, New York, U.S.A.
24 Debye-Hückel Model 1923 Treatment: A reference ion residing in a dielectric continuum. Dielectric constant is 80 Reference ion is charged-therefore, in its immediate vicinity there will be neutralization by the continuum of charge that surrounds it. At equilibrium the charge on the central ion will be exactly counterbalanced by the counter charge atmosphere: Principle of Electroneutrality: z i e o X i = 0
25
Bchem 675 Lecture 9 Electrostatics-Lecture 2 Debye-Hückel: Continued Counter ion condensation
Bchem 675 Lecture 9 Electrostatics-Lecture 2 Debye-Hückel: Continued Counter ion condensation Ion:ion interactions What is the free energy of ion:ion interactions ΔG i-i? Consider an ion in a solution
More informationFree energy, electrostatics, and the hydrophobic effect
Protein Physics 2016 Lecture 3, January 26 Free energy, electrostatics, and the hydrophobic effect Magnus Andersson magnus.andersson@scilifelab.se Theoretical & Computational Biophysics Recap Protein structure
More informationThe change in free energy on transferring an ion from a medium of low dielectric constantε1 to one of high dielectric constant ε2:
The Born Energy of an Ion The free energy density of an electric field E arising from a charge is ½(ε 0 ε E 2 ) per unit volume Integrating the energy density of an ion over all of space = Born energy:
More informationPeter Debye and Electrochemistry
Peter Debye and Electrochemistry A K Shukla and T Prem Kumar A K Shukla is Professor and Chairman, Solid State and Structural Chemistry Unit, Indian Institute of Science, Bangalore. His research interests
More informationMolecule Matters van der Waals Molecules
Molecule Matters van der Waals Molecules 3. Rg HF Complexes are Debye Molecules! E Arunan In this article, Debye s contributions to understanding van der Waals attractive forces, specifically, dipole induced
More informationBiochemistry,530:,, Introduc5on,to,Structural,Biology, Autumn,Quarter,2015,
Biochemistry,530:,, Introduc5on,to,Structural,Biology, Autumn,Quarter,2015, Course,Informa5on, BIOC%530% GraduateAlevel,discussion,of,the,structure,,func5on,,and,chemistry,of,proteins,and, nucleic,acids,,control,of,enzyma5c,reac5ons.,please,see,the,course,syllabus,and,
More informationMolecular Modeling -- Lecture 15 Surfaces and electrostatics
Molecular Modeling -- Lecture 15 Surfaces and electrostatics Molecular surfaces The Hydrophobic Effect Electrostatics Poisson-Boltzmann Equation Electrostatic maps Electrostatic surfaces in MOE 15.1 The
More informationBIOC : Homework 1 Due 10/10
Contact information: Name: Student # BIOC530 2012: Homework 1 Due 10/10 Department Email address The following problems are based on David Baker s lectures of forces and protein folding. When numerical
More informationOther Cells. Hormones. Viruses. Toxins. Cell. Bacteria
Other Cells Hormones Viruses Toxins Cell Bacteria ΔH < 0 reaction is exothermic, tells us nothing about the spontaneity of the reaction Δ H > 0 reaction is endothermic, tells us nothing about the spontaneity
More informationElectrolytes. Chapter Basics = = 131 2[ ]. (c) From both of the above = = 120 8[
Chapter 1 Electrolytes 1.1 Basics Here we consider species that dissociate into positively and negatively charged species in solution. 1. Consider: 1 H (g) + 1 Cl (g) + ()+ () = { } = (+ )+ ( ) = 167[
More informationSolutions and Non-Covalent Binding Forces
Chapter 3 Solutions and Non-Covalent Binding Forces 3.1 Solvent and solution properties Molecules stick together using the following forces: dipole-dipole, dipole-induced dipole, hydrogen bond, van der
More informationPhys 102 Lecture 2 Coulomb s Law & Electric Dipoles
Phys 102 Lecture 2 Coulomb s Law & Electric Dipoles 1 Today we will... Get practice using Coulomb s law & vector addition Learn about electric dipoles Apply these concepts! Molecular interactions Polar
More informationschematic diagram; EGF binding, dimerization, phosphorylation, Grb2 binding, etc.
Lecture 1: Noncovalent Biomolecular Interactions Bioengineering and Modeling of biological processes -e.g. tissue engineering, cancer, autoimmune disease Example: RTK signaling, e.g. EGFR Growth responses
More information16 years ago TODAY (9/11) at 8:46, the first tower was hit at 9:03, the second tower was hit. Lecture 2 (9/11/17)
16 years ago TODAY (9/11) at 8:46, the first tower was hit at 9:03, the second tower was hit By Anthony Quintano - https://www.flickr.com/photos/quintanomedia/15071865580, CC BY 2.0, https://commons.wikimedia.org/w/index.php?curid=38538291
More informationProtein Folding experiments and theory
Protein Folding experiments and theory 1, 2,and 3 Protein Structure Fig. 3-16 from Lehninger Biochemistry, 4 th ed. The 3D structure is not encoded at the single aa level Hydrogen Bonding Shared H atom
More informationChem 321 Lecture 11 - Chemical Activities 10/3/13
Student Learning Objectives Chem 321 Lecture 11 - Chemical Activities 10/3/13 One of the assumptions that has been made in equilibrium calculations thus far has been to equate K to a ratio of concentrations.
More informationBiophysics II. Hydrophobic Bio-molecules. Key points to be covered. Molecular Interactions in Bio-molecular Structures - van der Waals Interaction
Biophysics II Key points to be covered By A/Prof. Xiang Yang Liu Biophysics & Micro/nanostructures Lab Department of Physics, NUS 1. van der Waals Interaction 2. Hydrogen bond 3. Hydrophilic vs hydrophobic
More informationAqueous solutions. Solubility of different compounds in water
Aqueous solutions Solubility of different compounds in water The dissolution of molecules into water (in any solvent actually) causes a volume change of the solution; the size of this volume change is
More informationA Gentle Introduction to (or Review of ) Fundamentals of Chemistry and Organic Chemistry
Wright State University CORE Scholar Computer Science and Engineering Faculty Publications Computer Science and Engineering 2003 A Gentle Introduction to (or Review of ) Fundamentals of Chemistry and Organic
More informationLecture 2 and 3: Review of forces (ctd.) and elementary statistical mechanics. Contributions to protein stability
Lecture 2 and 3: Review of forces (ctd.) and elementary statistical mechanics. Contributions to protein stability Part I. Review of forces Covalent bonds Non-covalent Interactions: Van der Waals Interactions
More informationChap 10 Part 4Ta.notebook December 08, 2017
Chapter 10 Section 1 Intermolecular Forces the forces between molecules or between ions and molecules in the liquid or solid state Stronger Intermolecular forces cause higher melting points and boiling
More informationChapter 1. Topic: Overview of basic principles
Chapter 1 Topic: Overview of basic principles Four major themes of biochemistry I. What are living organism made from? II. How do organism acquire and use energy? III. How does an organism maintain its
More informationPrinciples of Enzyme Catalysis Arthur L. Haas, Ph.D. Department of Biochemistry and Molecular Biology
Principles of Enzyme Catalysis Arthur L. Haas, Ph.D. Department of Biochemistry and Molecular Biology Review: Garrett and Grisham, Enzyme Specificity and Regulation (Chapt. 13) and Mechanisms of Enzyme
More informationAn introduction to Molecular Dynamics. EMBO, June 2016
An introduction to Molecular Dynamics EMBO, June 2016 What is MD? everything that living things do can be understood in terms of the jiggling and wiggling of atoms. The Feynman Lectures in Physics vol.
More informationCHAPTER 21: Reaction Dynamics
CHAPTER 21: Reaction Dynamics I. Microscopic Theories of the Rate Constant. A. The Reaction Profile (Potential Energy diagram): Highly schematic and generalized. A---B-C B. Collision Theory of Bimolecular
More informationINTERMOLECULAR AND SURFACE FORCES
INTERMOLECULAR AND SURFACE FORCES SECOND EDITION JACOB N. ISRAELACHVILI Department of Chemical & Nuclear Engineering and Materials Department University of California, Santa Barbara California, USA ACADEMIC
More informationWhy Proteins Fold. How Proteins Fold? e - ΔG/kT. Protein Folding, Nonbonding Forces, and Free Energy
Why Proteins Fold Proteins are the action superheroes of the body. As enzymes, they make reactions go a million times faster. As versatile transport vehicles, they carry oxygen and antibodies to fight
More informationBIBC 100. Structural Biochemistry
BIBC 100 Structural Biochemistry http://classes.biology.ucsd.edu/bibc100.wi14 Papers- Dialogue with Scientists Questions: Why? How? What? So What? Dialogue Structure to explain function Knowledge Food
More informationContents. 2. Fluids. 1. Introduction
Contents 1. Introduction 2. Fluids 3. Physics of Microfluidic Systems 4. Microfabrication Technologies 5. Flow Control 6. Micropumps 7. Sensors 8. Ink-Jet Technology 9. Liquid Handling 10.Microarrays 11.Microreactors
More informationLec.1 Chemistry Of Water
Lec.1 Chemistry Of Water Biochemistry & Medicine Biochemistry can be defined as the science concerned with the chemical basis of life. Biochemistry can be described as the science concerned with the chemical
More informationModule 8: "Stability of Colloids" Lecture 38: "" The Lecture Contains: Calculation for CCC (n c )
The Lecture Contains: Calculation for CCC (n c ) Relation between surface charge and electrostatic potential Extensions to DLVO theory file:///e /courses/colloid_interface_science/lecture38/38_1.htm[6/16/2012
More informationChapter 11 section 6 and Chapter 8 Sections 1-4 from Atkins
Lecture Announce: Chapter 11 section 6 and Chapter 8 Sections 1-4 from Atkins Outline: osmotic pressure electrolyte solutions phase diagrams of mixtures Gibbs phase rule liquid-vapor distillation azeotropes
More informationBIOC 530 Fall, 2011 BIOC 530
Fall, 2011 Course Information Course Description Graduate-level discussion of the structure, function, and chemistry of proteins and nucleic acids, control of enzymatic reactions. Please see the course
More informationAll-atom Molecular Mechanics. Trent E. Balius AMS 535 / CHE /27/2010
All-atom Molecular Mechanics Trent E. Balius AMS 535 / CHE 535 09/27/2010 Outline Molecular models Molecular mechanics Force Fields Potential energy function functional form parameters and parameterization
More informationTopic0990 Electrical Units In attempting to understand the properties of chemical substances, chemists divide chemistry into two parts.
Topic99 Electrical Units In attempting to understand the properties of chemical substances, chemists divide chemistry into two parts. In one part, chemists are interested in understanding intramolecular
More informationCHEM 110: CHAPTER 8 Basic Concepts of Chem Bonding. Lewis Structures of Atoms: The Lewis Dot Diagram
1 CHEM 110: CHAPTER 8 Basic Concepts of Chem Bonding Lewis Structures of Atoms: The Lewis Dot Diagram Lewis Dot Diagrams (developed by chemist Gilbert Lewis) are used to indicate the number of valence
More informationMolecular Forces in Biological Systems - Electrostatic Interactions; - Shielding of charged objects in solution
Molecular Forces in Biological Systems - Electrostatic Interactions; - Shielding of charged objects in solution Electrostatic self-energy, effects of size and dielectric constant q q r r ε ε 1 ε 2? δq
More information3. Solutions W = N!/(N A!N B!) (3.1) Using Stirling s approximation ln(n!) = NlnN N: ΔS mix = k (N A lnn + N B lnn N A lnn A N B lnn B ) (3.
3. Solutions Many biological processes occur between molecules in aqueous solution. In addition, many protein and nucleic acid molecules adopt three-dimensional structure ( fold ) in aqueous solution.
More informationMultimedia : Boundary Lubrication Podcast, Briscoe, et al. Nature , ( )
3.05 Nanomechanics of Materials and Biomaterials Thursday 04/05/07 Prof. C. Ortiz, MITDMSE I LECTURE 14: TE ELECTRICAL DOUBLE LAYER (EDL) Outline : REVIEW LECTURE #11 : INTRODUCTION TO TE ELECTRICAL DOUBLE
More informationMolecular Simulation III
Molecular Simulation III Quantum Chemistry Classical Mechanics E = Ψ H Ψ ΨΨ U = E bond +E angle +E torsion +E non-bond Molecular Dynamics Jeffry D. Madura Department of Chemistry & Biochemistry Center
More informationAtoms & Their Interactions
Lecture 2 Atoms & Their Interactions Si: the heart of electronic materials Intel, 300mm Si wafer, 200 μm thick and 48-core CPU ( cloud computing on a chip ) Twin Creeks Technologies, San Jose, Si wafer,
More information2 Structure. 2.1 Coulomb interactions
2 Structure 2.1 Coulomb interactions While the information needed for reproduction of living systems is chiefly maintained in the sequence of macromolecules, any practical use of this information must
More informationChapter Notes Subject: Chemistry Class: XI Chapter: Thermodynamics Top concepts
Chapter Notes Subject: Chemistry Class: XI Chapter: Thermodynamics Top concepts 1. The branch of science which deals with study of different forms of energy and their interconversion is called thermodynamics.
More informationThinking Like a Chemist UNIT 5 DAY 1
Thinking Like a Chemist UNIT 5 DAY 1 What are we going to learn today? Note some important details on the syllabus Become familiar with the course website Meet the teaching team Review the Mechanics of
More informationLigand-receptor interactions
University of Silesia, Katowice, Poland 11 22 March 2013 Ligand-receptor interactions Dr. Pavel Polishchuk A.V. Bogatsky Physico-Chemical Institute of National Academy of Sciences of Ukraine Odessa, Ukraine
More informationChapter 13. Properties of Solutions. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 13 Properties of John D. Bookstaver St. Charles Community College Cottleville, MO are homogeneous mixtures of two or more pure substances. In a solution, the solute is dispersed
More information1044 Lecture #14 of 18
Lecture #14 of 18 1044 1045 Q: What s in this set of lectures? A: B&F Chapter 13 main concepts: Section 1.2.3: Diffuse double layer structure Sections 13.1 & 13.2: Gibbs adsorption isotherm; Electrocapillary
More informationq 2 Da This looks very similar to Coulomb doesn t it? The only difference to Coulomb is the factor of 1/2.
Born Lets now think about a somewhat different, but related problem that is associated with the name Born. Using a name (usually the name of the guy who first discovered or solved the problem) to describe
More informationEnduring Understandings & Essential Knowledge for AP Chemistry
Enduring Understandings & Essential Knowledge for AP Chemistry Big Idea 1: The chemical elements are fundamental building materials of matter, and all matter can be understood in terms of arrangements
More informationWater. 2.1 Weak Interactions in Aqueous Sy stems Ionization of Water, Weak Acids, and Weak Bases 58
Home http://www.macmillanhighered.com/launchpad/lehninger6e... 1 of 1 1/6/2016 3:07 PM 2 Printed Page 47 Water 2.1 Weak Interactions in Aqueous Sy stems 47 2.2 Ionization of Water, Weak Acids, and Weak
More informationLecture: P1_Wk1_L1 IntraMolecular Interactions. Ron Reifenberger Birck Nanotechnology Center Purdue University 2012
Lecture: IntraMolecular Interactions Distinguish between IntraMolecular (within a molecule) and InterMolecular (between molecules) Ron Reifenberger Birck Nanotechnology Center Purdue University 2012 1
More informationRama Abbady. Zina Smadi. Diala Abu-Hassan
1 Rama Abbady Zina Smadi Diala Abu-Hassan (00:00) (10:00) Types of Molecules in the Cell 1. Water Molecules: a large portion of the cell mass is water (70% of total cell mass). 2. Organic molecules (carbon
More informationBiochemistry 530: Introduction to Structural Biology. Autumn Quarter 2014 BIOC 530
Biochemistry 530: Introduction to Structural Biology Autumn Quarter 2014 Course Information Course Description Graduate-level discussion of the structure, function, and chemistry of proteins and nucleic
More informationStudyHub: AP Chemistry
StudyHub+ 1 StudyHub: AP Chemistry Solution Composition and Energies, Boiling Point, Freezing Point, and Vapor Pressure StudyHub+ 2 Solution Composition: Mole Fraction: Formula: Mole Fraction of Component
More informationProtein Folding & Stability. Lecture 11: Margaret A. Daugherty. Fall How do we go from an unfolded polypeptide chain to a
Lecture 11: Protein Folding & Stability Margaret A. Daugherty Fall 2004 How do we go from an unfolded polypeptide chain to a compact folded protein? (Folding of thioredoxin, F. Richards) Structure - Function
More informationChpt 8 Chemical Bonding Forces holding atoms together = Chemical Bonds
Chpt 8 Chemical Bonding Forces holding atoms together = Chemical Bonds Kinds of chemical bonds: 1. Ionic 2. Covalent 3. Metallic Useful guideline: Octet rule Atoms tend to gain, lose, or share e - to achieve
More informationBCMP 201 Protein biochemistry
BCMP 201 Protein biochemistry BCMP 201 Protein biochemistry with emphasis on the interrelated roles of protein structure, catalytic activity, and macromolecular interactions in biological processes. The
More information40 46, 51, ,
cha02680_fm.indd Page xxvi 12/27/12 4:05 PM GG-009 /Volumes/107/GO01228/CHANG_11E/ANCILLARY/CHANG/007_665610_1_P1 BIG IDEA 1: The chemical elements are fundamental building materials of matter, and all
More informationCopyright 2018 Dan Dill 1
TP Do we get the same amount of energy back from making bonds between an ion and water molecules, as it took to break the ionic bonds holding an ion in the solid? + 1. The energy is the same 2. More energy
More informationCHEM 545 Theory and Practice of Molecular Electronic Structure. Anna I. Krylov. DON T PANIC.
CHEM 545 Theory and Practice of Molecular Electronic Structure Anna I. Krylov http://iopenshell.usc.edu/chem545/ DON T PANIC USC Fall 2014 Things to do: 1. Install IQmol (by this Thursday). http://iqmol.org/.
More informationChemical thermodynamics the area of chemistry that deals with energy relationships
Chemistry: The Central Science Chapter 19: Chemical Thermodynamics Chemical thermodynamics the area of chemistry that deals with energy relationships 19.1: Spontaneous Processes First law of thermodynamics
More information21 Electric Fields Karl Haab,
21 Electric Fields Karl Haab, 2008 1 Objectives Calculate el. force between charges electric field and field strength electric potential, p.d. application: the electron gun 2 Some fundamental facts Objects
More informationChapter 9. Chemical Bonding I: The Lewis Model. HIV-Protease. Lecture Presentation
Lecture Presentation Chapter 9 Chemical Bonding I: The Lewis Model HIV-Protease HIV-protease is a protein synthesized by the human immunodeficiency virus (HIV). This particular protein is crucial to the
More informationThermodynamic Studies of Some Symmetrical Electrolyte s Solution in Aqueous-Organic Solvent Mixtures
ISSN 122-8594 JUJS 218 Jahangirnagar University Journal of Science Vol. 41, No.1, pp.87-98 Thermodynamic Studies of Some Symmetrical Electrolyte s Solution in Aqueous-Organic Solvent Mixtures Md. Minarul
More informationLecture 5: Electrostatic Interactions & Screening
Lecture 5: Electrostatic Interactions & Screening Lecturer: Prof. Brigita Urbanc (brigita@drexel.edu) PHYS 461 & 561, Fall 2009-2010 1 A charged particle (q=+1) in water, at the interface between water
More informationChapter 6 Part 1 Structure of the atom
Chapter 6 Part 1 Structure of the atom What IS the structure of an atom? What are the properties of atoms? REMEMBER: structure affects function! Important questions: Where are the electrons? What is the
More informationWeek 14/Th: Lecture Units 34 & 35
Week 14/Th: Lecture Units 34 & 35 Unit 33: Colligative Properties Unit 34: Introduction to Equilibria -- Rate of reaction -- Reaction pathway -- Forward / Reverse Rxns. Unit 35: Equilibrium Constants --
More informationCh 9 Liquids & Solids (IMF) Masterson & Hurley
Ch 9 Liquids & Solids (IMF) Masterson & Hurley Intra- and Intermolecular AP Questions: 2005 Q. 7, 2005 (Form B) Q. 8, 2006 Q. 6, 2007 Q. 2 (d) and (c), Periodic Trends AP Questions: 2001 Q. 8, 2002 Q.
More information2.Ionization Energies
2.Ionization Energies Ionization energy, IE, is the energy required to remove one electron from an atom or ion; an endothermic process that is, A A + + 1 e - H = +ve The energy, in kj mol -1, required
More informationPhysics (
Question 2.12: A charge of 8 mc is located at the origin. Calculate the work done in taking a small charge of 2 10 9 C from a point P (0, 0, 3 cm) to a point Q (0, 4 cm, 0), via a point R (0, 6 cm, 9 cm).
More informationProton Acidity. (b) For the following reaction, draw the arrowhead properly to indicate the position of the equilibrium: HA + K + B -
Proton Acidity A01 Given that acid A has a pk a of 15 and acid B has a pk a of 10, then: (a) Which of the two acids is stronger? (b) For the following reaction, draw the arrowhead properly to indicate
More informationUnit 7: Basic Concepts of Chemical Bonding. Chemical Bonds. Lewis Symbols. The Octet Rule. Transition Metal Ions. Ionic Bonding 11/17/15
Unit 7: Basic Concepts of Chemical Bonding Topics Covered Chemical bonds Ionic bonds Covalent bonds Bond polarity and electronegativity Lewis structures Exceptions to the octet rule Strength of covalent
More informationLecture 2-3: Review of forces (ctd.) and elementary statistical mechanics. Contributions to protein stability
Lecture 2-3: Review of forces (ctd.) and elementary statistical mechanics. Contributions to protein stability Part I. Review of forces Covalent bonds Non-covalent Interactions Van der Waals Interactions
More informationFundamentals of Distribution Separations (III)
Fundamentals of Distribution Separations (III) (01/16/15) K = exp -Δμ 0 ext i - Δμ i RT distribution coefficient C i = exp -Δμ 0 RT - - Δμ i = ΔH i TΔS i 0 0 0 solubility q A---B A + B 0 0 0 ΔH i = ΔH
More informationV. Electrostatics. MIT Student
V. Electrostatics Lecture 26: Compact Part of the Double Layer MIT Student 1 Double-layer Capacitance 1.1 Stern Layer As was discussed in the previous lecture, the Gouy-Chapman model predicts unphysically
More informationMore Chemical Bonding
More Chemical Bonding Reading: Ch 10: section 1-8 Ch 9: section 4, 6, 10 Homework: Chapter 10:.31, 33, 35*, 39*, 43, 47, 49* Chapter 9: 43, 45, 55*, 57, 75*, 77, 79 * = important homework question Molecular
More informationCHEMISTRY XL-14A CHEMICAL BONDS
CHEMISTRY XL-14A CHEMICAL BONDS July 16, 2011 Robert Iafe Office Hours 2 July 18-July 22 Monday: 2:00pm in Room MS-B 3114 Tuesday-Thursday: 3:00pm in Room MS-B 3114 Chapter 2 Overview 3 Ionic Bonds Covalent
More informationChem 112 Dr. Kevin Moore
Chem 112 Dr. Kevin Moore Gas Liquid Solid Polar Covalent Bond Partial Separation of Charge Electronegativity: H 2.1 Cl 3.0 H Cl δ + δ - Dipole Moment measure of the net polarity in a molecule Q Q magnitude
More informationPeptide folding in non-aqueous environments investigated with molecular dynamics simulations Soto Becerra, Patricia
University of Groningen Peptide folding in non-aqueous environments investigated with molecular dynamics simulations Soto Becerra, Patricia IMPORTANT NOTE: You are advised to consult the publisher's version
More informationProperties of Aqueous Solutions
Properties of Aqueous Solutions Definitions A solution is a homogeneous mixture of two or more substances. The substance present in smaller amount is called the solute. The substance present in larger
More information1. Poisson-Boltzmann 1.1. Poisson equation. We consider the Laplacian. which is given in spherical coordinates by (2)
1. Poisson-Boltzmann 1.1. Poisson equation. We consider the Laplacian operator (1) 2 = 2 x + 2 2 y + 2 2 z 2 which is given in spherical coordinates by (2) 2 = 1 ( r 2 ) + 1 r 2 r r r 2 sin θ θ and in
More informationChapter 8. Basic Concepts of Chemical Bonding. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 8 of Chemical John D. Bookstaver St. Charles Community College Cottleville, MO Chemical Bonds Three basic types of bonds Ionic Electrostatic attraction between ions. Covalent
More informationLecture 6. NONELECTROLYTE SOLUTONS
Lecture 6. NONELECTROLYTE SOLUTONS NONELECTROLYTE SOLUTIONS SOLUTIONS single phase homogeneous mixture of two or more components NONELECTROLYTES do not contain ionic species. CONCENTRATION UNITS percent
More informationChapter 13 Properties of Solutions
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 13 Properties of John D. Bookstaver St. Charles Community College St. Peters, MO 2006,
More informationFirst Law of Thermodynamics
First Law of Thermodynamics Remember: ΔE univ = 0 Total energy of the universe is constant. Energy can be transferred: ΔE = q + w q = heat w = work (F*D) = ΔPV 1 st Law, review For constant volume process:
More informationThermodynamics: Free Energy and Entropy. Suggested Reading: Chapter 19
Thermodynamics: Free Energy and Entropy Suggested Reading: Chapter 19 System and Surroundings System: An object or collection of objects being studied. Surroundings: Everything outside of the system. the
More information6, Physical Chemistry -II (Statistical Thermodynamics, Chemical Dynamics, Electrochemistry and Macromolecules)
Subject Paper No and Title Module No and Title Module Tag 6, Physical -II (Statistical Thermodynamics, Chemical Dynamics, Electrochemistry and Macromolecules) 25, Activity and Mean Activity coefficient
More informationChemistry 1B Fall 2012
Chemistry 1B Fall 2012 Lecture 9 (chapter 13; pp 593-612) [596-614] 7th 2 bonding in molecules Chapter 13 (pp 593-612) Overview of bonding and ionic bonding (lect 9) Chapter 13 (pp 612-650)- Classical
More information12A Entropy. Entropy change ( S) N Goalby chemrevise.org 1. System and Surroundings
12A Entropy Entropy change ( S) A SPONTANEOUS PROCESS (e.g. diffusion) will proceed on its own without any external influence. A problem with H A reaction that is exothermic will result in products that
More informationChapters 11 and 12: Intermolecular Forces of Liquids and Solids
1 Chapters 11 and 12: Intermolecular Forces of Liquids and Solids 11.1 A Molecular Comparison of Liquids and Solids The state of matter (Gas, liquid or solid) at a particular temperature and pressure depends
More informationGHW#3. Chapter 3. Louisiana Tech University, Chemistry 481. POGIL(Process Oriented Guided Inquiry Learning) Exercise on Chapter 3.
GHW#3. Chapter 3. Louisiana Tech University, Chemistry 481. POGIL(Process Oriented Guided Inquiry Learning) Exercise on Chapter 3. Energetics of Ionic Bonding. Why? What are the properties of ionic compounds?
More informationDownloaded from
I.I.T.Foundation - XI Chemistry MCQ #4 Time: 45 min Student's Name: Roll No.: Full Marks: 90 Chemical Bonding I. MCQ - Choose Appropriate Alternative 1. The energy required to break a chemical bond to
More informationElectrochemical Properties of Materials for Electrical Energy Storage Applications
Electrochemical Properties of Materials for Electrical Energy Storage Applications Lecture Note 3 October 11, 2013 Kwang Kim Yonsei Univ., KOREA kbkim@yonsei.ac.kr 39 Y 88.91 8 O 16.00 7 N 14.01 34 Se
More informationInorganic Pharmaceutical Chemistry
Inorganic Pharmaceutical Chemistry Lecture No. 4 Date :25/10 /2012 Dr. Mohammed Hamed --------------------------------------------------------------------------------------------------------------------------------------
More informationPhase Equilibria and Molecular Solutions Jan G. Korvink and Evgenii Rudnyi IMTEK Albert Ludwig University Freiburg, Germany
Phase Equilibria and Molecular Solutions Jan G. Korvink and Evgenii Rudnyi IMTEK Albert Ludwig University Freiburg, Germany Preliminaries Learning Goals Phase Equilibria Phase diagrams and classical thermodynamics
More informationLecture 9. Chemistry 1B Fall 2013 Lecture 9. Chemistry 1B. Fall (chapter 13; pp )
bonding in molecules Chemistry 1B Fall 2013 Lecture 9 (chapter 13; pp 596-614) Chapter 13 (pp 596-614) Overview of bonding and ionic bonding (lect 9) Chapter 13 (pp 621-650)- Classical picture of (pp 602-606)
More informationChapter 12 Section 1
hapter 12 Section 1 Kinetic Molecular Description of Liquids and Solids Noncovalent Forces Intermolecular interactions Electrostatic Forces Dispersion Forces -bonding DNA, RNA Mary J. Bojan hem 110 1 What
More informationLecture Notes 1: Physical Equilibria Vapor Pressure
Lecture Notes 1: Physical Equilibria Vapor Pressure Our first exploration of equilibria will examine physical equilibria (no chemical changes) in which the only changes occurring are matter changes phases.
More informationChapter 3. Crystal Binding
Chapter 3. Crystal Binding Energy of a crystal and crystal binding Cohesive energy of Molecular crystals Ionic crystals Metallic crystals Elasticity What causes matter to exist in three different forms?
More informationBiomolecules are dynamic no single structure is a perfect model
Molecular Dynamics Simulations of Biomolecules References: A. R. Leach Molecular Modeling Principles and Applications Prentice Hall, 2001. M. P. Allen and D. J. Tildesley "Computer Simulation of Liquids",
More information