Principles of Molecular Recognition. 2014/2015 Fall term
|
|
|
- Britton Banks
- 5 years ago
- Views:
Transcription
1 Principles of Molecular Recognition 2014/2015 Fall term
2 General information Péter Kele (MTA-TTK, V/5.02A) Lectures are available at: Oral exam (officially January 28, 2015 upon arrangement)
3 Useful literature Lakowicz, Joseph: Principles of fluorescence spectrosopy Valeur, Bernard: Molecular fluorescence Wang, Anslyn: Chemosensors
4 Chemosensing, chemosensors Field of chemosensing is rapidly growing Medical diagnostics, environmental monitoring, toxicological analysis, forensics, cell biology, biochemistry etc. Chemosensing is interdisciplinary (e.g. chemistry, physics, biology) Supramolecular chemistry - mainly non-covalent interactions
5 Sensors - chemsensors Sensor in analytical chemistry: a chemical indicator in an instrument that produces signal indicative of the presence of an analyte Sensor in supramolecular chemistry: is a host molecule (receptor) that changes color, emission, redox potential etc. upon binding of an analyte (quantification still requires instrumentation)
6 Chemsensor modules Receptor (Host): recognizes the analyte (Guest) synthetic receptors - design, creation (chemistry) Transducer: linker (transfers the changes) Signaling unit: produces signal upon guest induced changes (physics)
7 Molecular recognition Receptor analyte interaction (Host-guest) Reversibility / reusability is of utmost importance Interactions work together to form stable intramolecular / intermolecular configurations Mostly noncovalent forces (but: sugars boronic acids)
8 Governing forces in supramolecular chemistry van der Waals interactions Ionic interactions Hydrogen bond p-cation interaction Metal chelation Covalent interaction
9 van der Waals Interactions Weakest, but can be predominant in aqueous media A collective term for noncovalent forces, inversely proportional to the inverse of the sixth power of separation Formerly, used interchangeably with London forces Van der Waals: London, Debye, Keesom) sum of attractive and repulsive interactions
10 van der Waals Interactions E ~ 1 / r 6 Dipole - dipole interactions of freely rotating dipoles (orientational force, Keesom force) Dipole - induced dipole (induction force, Debye force) - A nonpolar and a polar molecule with permanent dipole
11 van der Waals Interactions Induced dipole - induced dipole (London forces, dispersion forces) - Present in all atoms and molecules - Due to the presence of instantaneous dipoles - One instantaneous dipole induces the other - Can be attractive or repulsive
12 Cation p interactions A cation and an aromatic p electron cloud In the gas phase mainly electrostatic interaction In the solution phase electrostatic + dispersion and inductive forces (London and Debye) also important In nature (e.g. Lys-Trp, Arg-Phe etc.)
13 Hydrogen bond Strongest secondary interaction Strongly polarized H-atom (H-donor) Lone pairs of N, F, O (H-acceptor) Residual positive and negative charges Reasons to form (electrostatic, or covalent bond??)
14 Hydrophobic effect a disputed phenomena Interaction of non-polar moieties in water Formation of water-water interactions (strong H-bond) at the expense of weak water-nonpolar interaction (DH-favored) Oriented H-bonds (DS-disfavored) Although: removal of non-polar from water and water released to the bulk is DS favored (less ordered)
15 Ionic interactions Classical electronic (Coulombic) interaction - Classical ionic - Salt bridges (balancing of electrostatic forces between three or more entities) - E.g. Asp-Lys-Glu (COO - - NH3 + - COO - )
16 Covalent interactions Restricted to a few special reversible reactions Strong affinity In aqueous solutions Intrinsic functional group selectivity
17 Boronic acid based chemosensors Boronic acids have strong affinity to Lewis bases - Diols (sugars) - Aminoalcohols - Hydroxy acids - Amino acids - Alcohols - Fluoride, cyanide
18 Boronic acid based chemosensors Special electronic features Boron has an open shell with 3 valence electrons in trigonal form (sp 2 hybridized + empty p orbital) Lewis acidic properties (can bind Lewis bases / nucleophiles) Several factors affect affinity
19 Boronic acid based chemosensors Small O-C-C-O dihedral angle Low pka of the diol and boronic acid favor binding at neutral ph pka effect is not unidirectional (bell shaped relationship between the diol and the boronic acid) ~ between the pka of the two Combined effect of pka and diehdral angle : catechol > cis-diols on five membered rings > linear diols > cis-diols on six membered rings Strong B-O bond is formed (rehybridizes to sp 3 )
20 Boronic acid based chemosensors OH B OH O B O H 2 O H 2 O HO OH H 2 O H 2 O H + H + OH B OH OH -H 2 O +H 2 O H + H + B O O OH
21 Metal chelation chemistry Metal coordination to the host framework Binding affinity of host (ligand) towards analyte Principles of metal chelation - Hard-soft acid-base concept (HSAB) - Hard and soft refer to polarizability of LA-LB pairs associated through dative bonds - Hard acids prefer hard bases, soft bases prefer soft acids - E.g. alkali, alkali earth metals prefer O, amine, amide N; late transition metals prefer imine N, and S donors
22 Ligands (Hosts) Ligands are classified by the number of coordinating (donor) atoms E.g. bidentate ligand (bite angle, chelate ring -5 or 6 membered (less torsion)) Chelates of higher denticity - By linear repetition of bidentate motifs - Branching from common bridgehead atom Chelate effect: refers to the enhanced stability of metal complexes of multidentate ligands as compared to those of monodentate ligands
23 The macrocyclic effect Increasing denticity with proper bite angle enhances stability of the complex Preorganized cyclic ligands have stronger binding affinity than acyclic ligands (Entropy) H N H N H N H N N N N N H H H H H H Cyclam, Ni(II) [Ni(1)] Ni(II) [Ni(2)] 2+ logk = 22.2; DH = kcal/mol; DS = +21cal/K/mol logk = 16.1; DH = kcaklmol; DS = +15cal/K/mol
24 The macrocyclic effect Ion-cavity concept : complementarity between host cavity and metal ion size Rule of three (three-point binding) E.g. 18-crown-6 ether binds K + the best O O O 2,5 2,0 1,5 K + Rb + O O O logk 1,0 0,5 Na + Cs + 0,0 Li + 0,8 1,0 1,2 1,4 1,6 1,8 Ionic radius ( )
25 The macrocyclic effect Deviation from this for cyclenes E.g. cyclen binds larger metal ions better than cyclam H N H N H N H N N H N H N H N H Cyclen Cyclam
26 Preorganization of donor atoms Binding is more favorable when ground-state conformation of the ligand resembles that in the complex Restricted torsional motions facilitates appropriate conformations Enthalpy vs. entropy COO OOC N OOC N COO OOC N OOC N COO COO EDTA CDTA logk for Cu(II) complexes: logk for Fe(II) complexes:
27 Examples for receptors (ligands, hosts)
28 Bidentate ligands (Often 1:2; 1:3 stoichiometry)
29 Bidentate ligands (Often 1:2; 1:3 stoichiometry) Cu(II) and Co(II) binding ligands (Hard)
30 Bidentate ligands (Often 1:2; 1:3 stoichiometry) Changing donor atoms Mg(II) (hard) Pb(II) (mixed) Pb(II) (Soft)
31 Bidentate ligands (Often 1:2; 1:3 stoichiometry) Neutral imine: Borderline hard/soft Zn(II)
32 Acyclic multidentate ligands Wrap around the metal Zn(II)
33 Acyclic multidentate: Linear chelates Less selective for size Pb(II) 1:1 with 38 2:1 with 39
34 Acyclic multidentate: Linear chelates Soft binders Ag(I) and Hg(II) Cu(I) 1:1 with 38 2:1 with 39
35 Acyclic multidentate: Linear chelates Tetrapeptide motif Pb(II) Cu(II)
36 Acyclic multidentate: Linear chelates Ca(II) Fe(III)
37 Acyclic multidentate: Branched chelates Ca(II) Fe(III) Zn(II); Cd(II) mainly
38 Acyclic multidentate: Branched chelates Zn(II); Cd(II) mainly Zn(II) binders
39 Acyclic multidentate: Branched chelates Hg(II) binders
40 Acyclic multidentate: Branched chelates Mg(II); Ca(II) binders
41 Acyclic multidentate: Branched chelates Ca(II) binders
42 Acyclic multidentate: Branched chelates Zn(II) chelators
43 Macrocyclic ligands: (aza)crown ethers
44 Macrocyclic ligands: lariat ethers Lariat aza-crowns (Hg(II), Mg(II), Pb(II) chelators
45 Macrocyclic ligands: (aza)crown ethers Stoichiometry vs. Cavity size 1:2 with 12-crown-4 1:2 with15-crown- 5 1:2 with18-crown- 6
46 Macrocyclic ligands: (aza)crown ethers Changing donor atoms
47 Macrocyclic ligands: (aza)crown ethers Lanthanide (III) binders
Solutions 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
Paper No. 1: ORGANIC CHEMISTRY- I (Nature of Bonding and Stereochemistry)
Subject Chemistry Paper No and Title Paper 1: ORGANIC - I (Nature of Bonding Module No and Title Module Tag CHE_P1_M10 TABLE OF CONTENTS 1. Learning Outcomes 2. Introduction 3. Non-Covalent Interactions
Unit 6: Molecular Geometry
Unit 6: Molecular Geometry Molecular Geometry [6-5] the polarity of each bond, along with the geometry of the molecule determines Molecular Polarity. To predict the geometries of more complicated molecules,
Physical Chemistry - Problem Drill 01: Chemistry and Physics Review
Physical Chemistry - Problem Drill 01: Chemistry and Physics Review No. 1 of 10 1. Chemical bonds are considered to be the interaction of their electronic structures of bonding atoms involved, with the
Aqueous 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
Chimica Farmaceutica
Chimica Farmaceutica Drug Targets Why should chemicals, some of which have remarkably simple structures, have such an important effect «in such a complicated and large structure as a human being? The answer
Biochemistry,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,
Rama 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
CH1010 Exam #2 Study Guide For reference see Chemistry: An Atoms-focused Approach by Gilbert, Kirss, and Foster
CH1010 Exam #2 Study Guide For reference see Chemistry: An Atoms-focused Approach by Gilbert, Kirss, and Foster Chapter 3: Atomic Structure, Explaining the Properties of Elements Trends to know (and be
16 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
Intermolecular and Intramolecular Forces. Introduction
Intermolecular and Intramolecular Forces Introduction Atoms can form stable units called molecules by sharing electrons. The formation of molecules is the result of intramolecular bonding (within the molecule)
Atoms can form stable units called molecules by sharing electrons.
Atoms can form stable units called molecules by sharing electrons. The formation of molecules is the result of intramolecular bonding (within the molecule) e.g. ionic, covalent. Forces that cause the aggregation
Chapter 2 Structure and Properties of Organic Molecules. Advanced Bonding: Review
hapter 2 Structure and Properties of Organic Molecules hemistry 231 Organic hemistry I Fall 2007 Advanced Bonding: Review Atomic Quantum Mechanics cannot explain how molecules like 4 form: Valence Bond
IMFA s. intermolecular forces of attraction Chez Chem, LLC All rights reserved.
IMFA s intermolecular forces of attraction 2014 Chez Chem, LLC All rights reserved. **London Dispersion Forces Also know as Van der Waals forces A momentary non symmetrical electron distribution that can
NAME. EXAM I I. / 36 September 25, 2000 Biochemistry I II. / 26 BICH421/621 III. / 38 TOTAL /100
EXAM I I. / 6 September 25, 2000 Biochemistry I II. / 26 BIH421/621 III. / 8 TOTAL /100 I. MULTIPLE HOIE (6 points) hoose the BEST answer to the question by circling the appropriate letter. 1. An amino
Chapters and 7.4 plus 8.1 and 8.3-5: Bonding, Solids, VSEPR, and Polarity
Chapters 7.1-2 and 7.4 plus 8.1 and 8.3-5: Bonding, Solids, VSEPR, and Polarity Chemical Bonds and energy bond formation is always exothermic As bonds form, chemical potential energy is released as other
Inorganic chemistry 3-stage Lec. 2. Dr- leaqaa
Inorganic chemistry 3-stage Lec. 2 Dr- leaqaa Chemical bonds types: Most chemical bonds fall into 2 categories depending on whether the valence e(s) are transferred or shared. Electron in ionic bond are
Multivalent interactions in human biology
Cooperativity Multivalent interactions in human biology Multivalent interactions in supramolecular chemistry Additivity (?) Multivalent interactions in supramolecular chemistry In order to obtain a
Electronegativity: the ability of an atom to attract bonding electrons
hem 309 Name hapter 3, 4 & 5 Supplemental omework Polarity and IMs Bond Polarity When we talk about a covalent bond as a shared pair of valence electrons, we have learned that these bonding electrons are
Lecture C2 Microscopic to Macroscopic, Part 2: Intermolecular Interactions. Let's get together.
Lecture C2 Microscopic to Macroscopic, Part 2: Intermolecular Interactions Let's get together. Most gases are NOT ideal except at very low pressures: Z=1 for ideal gases Intermolecular interactions come
There are two types of bonding that exist between particles interparticle and intraparticle bonding.
There are two types of bonding that exist between particles interparticle and intraparticle bonding. Intraparticle bonding describes the forces that exist within a particle such as a molecule or ionic
Other 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
Biological Anion Receptors
Binding of Anions 1 Binding of Anions 2 Biological Anion Receptors 3 Concepts in Anion Host Design FACTORS WITCH AFFECT ANION COMPLEXATION Prevailing interactions which take place in anion binding: hydrogen
Intermolecular Forces I
I How does the arrangement of atoms differ in the 3 phases of matter (solid, liquid, gas)? Why doesn t ice just evaporate into a gas? Why does liquid water exist at all? There must be some force between
Atomic and molecular interaction forces in biology
Atomic and molecular interaction forces in biology 1 Outline Types of interactions relevant to biology Van der Waals interactions H-bond interactions Some properties of water Hydrophobic effect 2 Types
States of matter Part 1
Physical pharmacy I 1. States of matter (2 Lectures) 2. Thermodynamics (2 Lectures) 3. Solution of non-electrolyte 4. Solution of electrolyte 5. Ionic equilibria 6. Buffered and isotonic solution Physical
States of matter Part 1. Lecture 1. University of Kerbala. Hamid Alghurabi Assistant Lecturer in Pharmaceutics. Physical Pharmacy
Physical pharmacy I 1. States of matter (2 Lectures) 2. Thermodynamics (2 Lectures) 3. Solution of non-electrolyte 4. Solution of electrolyte 5. Ionic equilibria 6. Buffered and isotonic solution Physical
Molecular Geometry: VSEPR model stand for valence-shell electron-pair repulsion and predicts the 3D shape of molecules that are formed in bonding.
Molecular Geometry: VSEPR model stand for valence-shell electron-pair repulsion and predicts the 3D shape of molecules that are formed in bonding. Sigma and Pi Bonds: All single bonds are sigma(σ), that
Electrons and Molecular Forces
Electrons and Molecular Forces Chemistry 30 Ms. Hayduk Electron Configuration Atomic Structure Atomic Number Number of protons in the nucleus Defines the element Used to organize the periodic table 1 Bohr
Lec.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
BIBC 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
Chapter 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
When intermolecular forces are strong, the atoms, molecules, or ions are strongly attracted to each other, and draw closer together.
INTERMOLECULAR FORCES: THE FORCE BEHIND VARIOUS PROPERTIES WHY? Intermolecular forces are largely responsible for the properties of affinity, solubility, volatility, melting/ boiling point, and viscosity.
Ch 6 Chemical Bonding
Ch 6 Chemical Bonding What you should learn in this section (objectives): Define chemical bond Explain why most atoms form chemical bonds Describe ionic and covalent bonding Explain why most chemical bonding
Chap 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
CHEMICAL BONDS A CHEMICAL BOND IS A FORCE OF ATTRACTION HOLDING THE ATOMS OR IONS TOGETHER.
CHEMICAL BONDS A CHEMICAL BOND IS A FORCE OF ATTRACTION HOLDING THE ATOMS OR IONS TOGETHER. q Elements tend to enter into chemical reaction to gain stability q This is satisfied by completing the octet
14: Organic Synthesis: Disconnection Approach. 17: Principles of molecular associations and organizations: Non-covalent synthesis
Subject Chemistry Paper No and Title Module No and Title Module Tag 14: Organic Synthesis: Disconnection Approach 17: Principles of molecular associations and organizations: Non-covalent synthesis CHE_P14_M17
Dipole-Dipole Interactions https://www.youtube.com/watch?v=cerb1d6j4-m London Dispersion Forces https://www.youtube.com/watch?
CATALYST Lesson Plan GLE Physical Science 22. Predict the kind of bond that will form between two elements based on electronic structure and electronegativity of the elements (e.g., ionic, polar, nonpolar)
Water: The Solvent for Biochemical Reactions
Chapter 2 Water: The Solvent for Biochemical Reactions 11 SUMMARY Section 2.1 Section 2.2 Section 2.3 Section 2.4 Water is a polar molecule, with a partial negative charge on the oxygen and partial positive
Chapter 2 Water: The Solvent for Biochemical Reactions
Chapter 2 Water: The Solvent for Biochemical Reactions SUMMARY Section 2.1 Water is a polar molecule, with a partial negative charge on the oxygen and partial positive charges on the hydrogens. There are
Polar molecules vs. Nonpolar molecules A molecule with separate centers of positive and negative charge is a polar molecule.
CHM 123 Chapter 8 8.5 8.6 Polar covalent Bonds and Dipole moments Depending on the relative electronegativities of the two atoms sharing electrons, there may be partial transfer of electron density from
CHEM 261 HOME WORK Lecture Topics: MODULE 1: The Basics: Bonding and Molecular Structure Text Sections (N0 1.9, 9-11) Homework: Chapter 1:
CHEM 261 HOME WORK Lecture Topics: MODULE 1: The Basics: Bonding and Molecular Structure Atomic Structure - Valence Electrons Chemical Bonds: The Octet Rule - Ionic bond - Covalent bond How to write Lewis
STRUCTURE. Dr. Sheppard CHEM 2411 Spring 2015
STRUCTURE Dr. Sheppard CHEM 2411 Spring 2015 Klein (2nd ed.) sections 1.8-1.10, 1.12-1.13, 2.7-2.12, 3.2, 3.4-3.5, 3.8-3.9, 4.6-4.13, 4.14, 8.5, 15.16, 21.3 Topics Structure Physical Properties Hybridization
Ch 2 Polar Covalent Bonds
h 2 Polar ovalent Bonds Two primary bond types: ovalent (shared e -1 s) and Ionic (transferred e -1 s) Ionic bonds can have covalent character, such as with Na:l. An e -1 pair on l -1 can fill the 3s orbital
Water. Dr. Diala Abu-Hassan, DDS, PhD Lecture 2 MD summer Dr. Diala Abu-Hassan
Water, DDS, PhD Dr.abuhassand@gmail.com Lecture 2 MD summer 2014 1 Lecture Content Importance of water in biological systems Noncovalent interactions Water structure Water properties Water as a solvent
Molecular Geometry and intermolecular forces. Unit 4 Chapter 9 and 11.2
1 Molecular Geometry and intermolecular forces Unit 4 Chapter 9 and 11.2 2 Unit 4.1 Chapter 9.1-9.3 3 Review of bonding Ionic compound (metal/nonmetal) creates a lattice Formula doesn t tell the exact
Protein- Ligand Interactions
Protein- Ligand Interactions Outline Introduction Interm olecular bonding forces Electrostatic or ionic bonds Hydrogen bonds Van der Waals interactions Dipole- dipole and ion- dipole interactions Repulsive
Patrick: An Introduction to Medicinal Chemistry 5e Chapter 01
Questions Patrick: An Introduction to Medicinal Chemistry 5e 01) Which of the following molecules is a phospholipid? a. i b. ii c. iii d. iv 02) Which of the following statements is false regarding the
Shapes of Molecules VSEPR
Shapes of Molecules In this section we will use Lewis structures as an introduction to the shapes of molecules. The key concepts are: Electron pairs repel each other. Electron pairs assume orientations
Primary bonding: e- are transferred or shared Strong ( KJ/mol or 1-10 ev/atom) Secondary Bonding: no e -
Types of Bondings Primary bonding: e- are transferred or shared Strong (100-1000 KJ/mol or 1-10 ev/atom) Ionic: Strong Coulomb interaction among negative atoms (have an extra electron each) and positive
Unit 1 Module 1 Forces of Attraction page 1 of 10 Various forces of attraction between molecules
Unit 1 Module 1 Forces of Attraction page 1 of 10 Various forces of attraction between molecules 1. Ionic bonds 2. Covalent bonds (also co-ordinate covalent bonds) 3. Metallic bonds 4. Van der Waals forces
A 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
The 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:
Intermolecular Forces and Phase Equilibria
Intermolecular Forces and Phase Equilibria Chemistry 36 Spring 2002 Intermolecular Forces What happens to gas phase molecules when subjected to increased pressure? Volume occupied by gas decreases (IGL)
Chemistry Chapter 6 Test Review
Chemistry Chapter 6 Test Review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A mutual electrical attraction between the nuclei and valence electrons
One Q partial negative, the other partial negative Ø H- bonding particularly strong. Abby Carroll 2
Chemistry Notes v Polarity Experiment Ø Things involved Polarity Solubility Dispersion Ø Polarity Shaving cream has soap steric acid Water is polar Food coloring is polar/ionic because dissolved Like dissolves
Ionic and Covalent Bonding
1. Define the following terms: a) valence electrons Ionic and Covalent Bonding the electrons in the highest occupied energy level always electrons in the s and p orbitals maximum of 8 valence electrons
Chapter 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?
The Logic of Biological Phenomena
The Logic of Biological Phenomena molecules are lifeless yet, in appropriate complexity and number, molecules compose living things What makes living things distinct? they can grow they can move they can
schematic 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
DEFINITION. The electrostatic force of attraction between oppositely charged ions
DEFINITION The electrostatic force of attraction between oppositely charged ions Usually occurs when a metal bonds with a non-metal Ions are formed by complete electron transfer from the metal atoms to
Week 11/Th: Lecture Units 28 & 29
Week 11/Th: Lecture Units 28 & 29 Unit 27: Real Gases Unit 28: Intermolecular forces -- types of forces between molecules -- examples Unit 29: Crystal Structure -- lattice types -- unit cells -- simple
Organic Chemistry. Introduction to Organic Molecules and Functional Groups
For updated version, please click on http://ocw.ump.edu.my Organic Chemistry Introduction to Organic Molecules and Functional Groups by Dr. Seema Zareen & Dr. Izan Izwan Misnon Faculty Industrial Science
Name: Date: Blk: Examine your periodic table to answer these questions and fill-in-the-blanks. Use drawings to support your answers where needed:
Name: Date: Blk: NOTES: BONDING Examine your periodic table to answer these questions and fill-in-the-blanks. Use drawings to support your answers where needed: I. IONIC BONDING Ionic bond: formed by the
BCMP 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
Fundamental Interactions: 6 Forces
Fundamental Interactions: 6 Forces In nuclear and high-energy physics 6 fundamental forces are recognized, which describe the structure of matter. - the strong interaction - the weak interaction act inside
Bonding and Dynamics. Outline Bonding and Dynamics Water Interactions Self Ionization of Water Homework
Liquid Water Structure In liquid water, most of the water molecules have the same local environment as in ice but the long range structure of ice disappears due to motion of the molecules. Bonds between
BASICS OUTLINE 8/23/17. Start reading White (CH 1) QoD Schedule
BASICS Start reading White (CH 1) QoD Schedule OUTLINE Periodic table & electronic configurations. Periodic properties: ionic radius, electron negativity, 1st ionization potential Covalent & ionic bonding
Chemical Bonding. Section 1 Introduction to Chemical Bonding. Section 2 Covalent Bonding and Molecular Compounds
Chemical Bonding Table of Contents Section 1 Introduction to Chemical Bonding Section 2 Covalent Bonding and Molecular Compounds Section 3 Ionic Bonding and Ionic Compounds Section 4 Metallic Bonding Section
General Physical Chemistry II
General Physical Chemistry II Lecture 13 Aleksey Kocherzhenko October 16, 2014" Last time " The Hückel method" Ø Used to study π systems of conjugated molecules" Ø π orbitals are treated separately from
Solutions and Intermolecular Forces
Solutions and Intermolecular Forces REVIEW Chemical Bonds Three basic types of bonds: Ionic Electrostatic attraction between ions Covalent Sharing of electrons Metallic Metal atoms bonded to several other
Chapter 6. Preview. Objectives. Molecular Compounds
Section 2 Covalent Bonding and Molecular Compounds Preview Objectives Molecular Compounds Formation of a Covalent Bond Characteristics of the Covalent Bond The Octet Rule Electron-Dot Notation Lewis Structures
Intermolecular forces
Intermolecular forces World of Chemistry, 2000 Updated: August 29, 2013 The attractions of molecules to each other are known as intermolecular forces to distinguish them from intramolecular forces, such
Chapter 21 Transition Metals and Coordination Chemistry
Chapter 21 Transition Metals and Coordination Chemistry Some History In the 19 th century, chemists started to prepare colored compounds containing transition metals and other substances like ammonia,
2.2.2 Bonding and Structure
2.2.2 Bonding and Structure Ionic Bonding Definition: Ionic bonding is the electrostatic force of attraction between oppositely charged ions formed by electron transfer. Metal atoms lose electrons to form
Chapter 21 Transition Metals and Coordination Chemistry
Chapter 21 Transition Metals and Coordination Chemistry Some History In the 19 th century, chemists started to prepare colored compounds containing transition metals and other substances like ammonia,
Chapter 6. Preview. Lesson Starter Objectives Chemical Bond
Preview Lesson Starter Objectives Chemical Bond Section 1 Introduction to Chemical Bonding Lesson Starter Imagine getting onto a crowded elevator. As people squeeze into the confined space, they come in
Cartoon courtesy of NearingZero.net. Chemical Bonding and Molecular Structure
Cartoon courtesy of NearingZero.net Chemical Bonding and Molecular Structure Chemical Bonds Forces that hold groups of atoms together and make them function as a unit. 3 Major Types: Ionic bonds transfer
IB Topics 4 & 14 Multiple Choice Practice
IB Topics 4 & 14 Multiple Choice Practice 1. Which compound has the shortest C N bond? CH 3NH 2 (CH 3) 3CNH 2 CH 3CN CH 3CHNH 2. Which of the following series shows increasing hydrogen bonding with water?
Bonding. Chemical Bond: mutual electrical attraction between nuclei and valence electrons of different atoms
Chemical Bonding Bonding Chemical Bond: mutual electrical attraction between nuclei and valence electrons of different atoms Type of bond depends on electron configuration and electronegativity Why do
Lecture 2. The framework to build materials and understand properties
Lecture 2 The framework to build materials and understand properties 1 Trees are made into a solid materials/structures in an environment that consists of small molecules: CO 2, N 2, H 2 0, CH 4 O C 2.58Ǻ
Big Idea: Ionic Bonds: Ionic Bonds: Metals: Nonmetals: Covalent Bonds: Ionic Solids: What ions do atoms form? Electron Electron
Chapter 13: Phenomena Phenomena: Scientists measured the bond angles of some common molecules. In the pictures below each line represents a bond that contains 2 electrons. If multiple lines are drawn together
Hybridisation of Atomic Orbitals
Lecture 7 CHEM101 Hybridisation of Atomic Orbitals Dr. Noha Osman Learning Outcomes Understand the valence bond theory Understand the concept of hybridization. Understand the different types of orbital
ORGANIC - EGE 5E CH. 2 - COVALENT BONDING AND CHEMICAL REACTIVITY
!! www.clutchprep.com CONCEPT: HYBRID ORBITAL THEORY The Aufbau Principle states that electrons fill orbitals in order of increasing energy. If carbon has only two unfilled orbitals, why does it like to
Chemical bonding & structure
Chemical bonding & structure Ionic bonding and structure Covalent bonding Covalent structures Intermolecular forces Metallic bonding Ms. Thompson - SL Chemistry Wooster High School Topic 4.4 Intermolecular
Biomolecules: lecture 9
Biomolecules: lecture 9 - understanding further why amino acids are the building block for proteins - understanding the chemical properties amino acids bring to proteins - realizing that many proteins
Describe the ionic bond as the electrostatic attraction between oppositely charged ions
4.1 Ionic Bonding 4.1.1 - Describe the ionic bond as the electrostatic attraction between oppositely charged ions Ions are formed when electrons are transferred from a metal atom to a non-metal atom in
Coordination Compounds
Coordination Compounds 1. What is a coordination compound composed of? a. Metal Ion b. Ligand c. Counter Ion 2. What is a complex ion? The metal ion and ligand combination. 3. What is a counter ion? An
Atoms have the ability to do two things in order to become isoelectronic with a Noble Gas.
CHEMICAL BONDING Atoms have the ability to do two things in order to become isoelectronic with a Noble Gas. 1.Electrons can be from one atom to another forming. Positive ions (cations) are formed when
The broad topic of physical metallurgy provides a basis that links the structure of materials with their properties, focusing primarily on metals.
Physical Metallurgy The broad topic of physical metallurgy provides a basis that links the structure of materials with their properties, focusing primarily on metals. Crystal Binding In our discussions
A REVIEW OF GENERAL CHEMISTRY: ELECTRONS, BONDS AND MOLECULAR PROPERTIES
A REVIEW OF GENERAL CEMISTRY: ELECTRONS, BONDS AND MOLECULAR PROPERTIES A STUDENT SOULD BE ABLE TO: 1. Draw Lewis (electron dot and line) structural formulas for simple compounds and ions from molecular
Chemical Bonding. 5. _c Atoms with a strong attraction for electrons they share with another atom exhibit
CHAPTER 6 REVIEW Chemical Bonding SHORT ANSWER Answer the following questions in the space provided. 1. a A chemical bond between atoms results from the attraction between the valence electrons and of
of its physical and chemical properties.
8.4 Molecular Shapes VSEPR Model The shape of a molecule determines many of its physical and chemical properties. Molecular l geometry (shape) can be determined with the Valence Shell Electron Pair Repulsion
Chapter 6. Chemical Bonding
Chapter 6 Chemical Bonding Section 6.1 Intro to Chemical Bonding 6.1 Objectives Define chemical bond. Explain why most atoms form chemical bonds. Describe ionic and covalent bonding. Explain why most chemical
Edexcel Chemistry A-level
Edexcel Chemistry A-level Topic 2 - Bonding and Structure Flashcards What are ions? What are ions? Charged particles that is formed when an atom loses or gains electrons What is the charge of the ion when
Chapter 7. Ionic & Covalent Bonds
Chapter 7 Ionic & Covalent Bonds Ionic Compounds Covalent Compounds 7.1 EN difference and bond character >1.7 = ionic 0.4 1.7 = polar covalent 1.7 Electrons not shared at
SL Score. HL Score ! /30 ! /48. Practice Exam: Paper 1 Topic 4: Bonding. Name
Name Practice Exam: Paper 1 Topic 4: Bonding SL SL Score! /30 HL Score! /48 1. What is the correct Lewis structure for hypochlorous acid, a compound containing chlorine, hydrogen and oxygen? A. B. C. D.
Electronic structure Crystal-field theory Ligand-field theory. Electronic-spectra electronic spectra of atoms
Chapter 19 d-metal complexes: electronic structure and spectra Electronic structure 19.1 Crystal-field theory 19.2 Ligand-field theory Electronic-spectra 19.3 electronic spectra of atoms 19.4 electronic
CHAPTER 2: Structure and Properties of Organic Molecules
1 HAPTER 2: Structure and Properties of Organic Molecules Atomic Orbitals A. What are atomic orbitals? Atomic orbitals are defined by special mathematical functions called wavefunctions-- (x, y, z). Wavefunction,
Learning Organic Chemistry
Objective 1 Represent organic molecules with chemical formulas, expanded formulas, Lewis structures, skeletal structures. Determine shape (VSEPR), bond polarity, and molecule polarity. Identify functional