Complexes that undergo complete ligand exchange within 1 minute at 25 C are labile. Henry Taube ( ), Nobel laureate of 1983
|
|
- Lionel Horn
- 5 years ago
- Views:
Transcription
1 Complexes that undergo complete ligand exchange within 1 minute at 25 C are labile. Henry Taube ( ), Nobel laureate of 1983
2 Which d n configuration should provide inert octahedral complexes? Inert Complexes d 3 & d 8, low spin d 4 -d 6
3 Limiting Reaction Mechanisms for Ligand Substitution Reactions Reaction Profile D = Dissociative ~ S N 1 From C.N. = 6 to C.N. =5 k -1, k 2 E k 1 ML 5 +X + Y k 1 << k -1 < k 2 ΔE (E a ) ML 5 X + Y ML 5 Y +X ΔG Reaction coordinate What are the kinetics of reactions proceeding via the D mechanism?
4 Kinetics of reactions proceeding via the D mechanism k 1 << k -1 < k 2 Reaction Profile k -1, k 2 k 1 ML 5 +X + Y But: k -1 [X] << k 2 [Y], because k -1 < k 2 and (usually) [X] << [Y]. This leads to: d[ml 5 Y]/dt = k 1 [ML 5 X] ML 5 X + Y ML 5 Y +X The reaction is 1 st order in substrate and hence, the rate of substitution should be independent of Y.
5 A simple case of a reaction proceeding via the D mechanism The rate is independent on the identity of L, the entering ligand
6 Another case of a reaction proceeding via the D mechanism The rate is dependent on the identity of L, the leaving ligand
7 Kinetics of the two limiting reaction mechanisms for Ligand Substitution Reactions in octahedral complexes (r = dp/dt) Dissociative (D) ML 5 X k 1 slow ML 5 + X +Y k 2 fast ML 5 Y r = k 1 [ML 5 X] Associative (A) ML 5 X + Y k 1 slow ML 5 XY -X k 2 fast ML 5 Y r = k 1 [ML 5 X][Y]
8 A reaction proceeding via the A mechanism The identity of entering ligand influences the rate very much ΔS # is negative, consistent with expectation for 2 molecules forming 1 new complex
9 Summary of of ligand substitution (exchange) reaction mechanisms in octahedral complexes ML n X + Y ML n Y + X ML n X Dissociative (D) ML n Y ML n X Associative (A) ML n Y X ML n Y Y ML n XY X I d if dissociation is more important I a if association is more important Y assists the leaving ligand (X) Dissociative Interchange (I D ) Y strongly begins bond formation before X leaves Associative Interchange (I A )
10 Substitution reactions in square-planar complexes and the trans effect Trans effect: The ability of a ligand (T) to labilize a ligand trans to it (X) T = a trans-directing ligand The trans effect series
11 Synthetically useful consequences of the trans effect H 3 N NH 3 H 3 N NH NH 3 H 3 N NH 3 Trans only!! 2-2 NH NH 3 NH 3 Cis only!!
12 Synthetically useful consequences of the trans effect H 3 N NH 3 H 3 N NH NH 3 H 3 N NH 3 H 3 N NH 3 H 3 N NH NH NH 3 NH NH 3 NH 3 The trans effect series
13 The trans effect series and the spectrochemical series Task 1 Note similarities and differences between the two series
14 Task 2 Let s try understanding the trans effect by taking a closer look at a conceivable reaction mechanism Note 1: the energies of square pyramidal and trigonal bipyramidal complexes are very similar and they interconvert very fast. Note 2: π - accepting ligands prefer equatorial positions in trigonal bipyramidal complexes
15 Task 2 Note: The barrier for tbp to spy is very small
16 Task 1 + Task 2 σ- donation by T weakens the M-X bond, hence σ - donor strength: π - acceptors prefer equatorial positions in bpy complexes, hence π - acceptor series:
17 Conclusion Both σ- donors and π-acceptors are expected to be strong trans-directing ligands
18 Both σ- donors and π-acceptors are expected to be strong trans-directing ligands Important notes: a) Information about σ-donation is obtained from isolated complexes. b) Information about π-acceptance is obtained from isolated complexes. c) Information about preferred occupation in tbp complexes is obtained from isolated complexes. d) Conclusion: Information for a-c is acquired from thermodynamic data. But, information regarding trans-directing ligands is obtained from kinetic data. Remember that the transeffect is defined as The ability of a ligand (T) to labilize a ligand trans to it (X) Conclusion: a) All information acquired about the effect of ligands on thermodynamic properties of other ligands trans to them is called the trans-influence. b) Information acquired about the effect of ligands on kinetic properties of ligands trans to them is called the trans-effect.
Kinetics and reaction mechanisms in coordination compounds
Kinetics and reaction mechanisms in coordination compounds Square planar complexes Three pathways by which one ligand can replace another Nucleophilic substitutions in square planar complexes (with Y being
More informationChapter 21 Coordination chemistry: reactions of complexes
CHEM 511 chapter 21 page 1 of 7 Chapter 21 Coordination chemistry: reactions of complexes Reactions of Complexes Typically measure ligand substitution reactions in solution (usually water) Lability and
More informationAdvanced Inorganic Chemistry. Alireza Gorji Department of Chemistry, Yazd University. Introduction.
Advanced Inorganic Chemistry Alireza Gorji Department of Chemistry, Yazd University Introduction 2 1 Kinetics vs. Thermodynamics Thermodynamics Kinetics G = H -T S G = H -T S G = -RTlnK G= -RTlnk Large
More informationInorganic Chemistry with Doc M. Fall Semester, 2012 Day 21. Transition Metals Complexes V: Reaction Mechanisms
Inorganic Chemistry with Doc M. Fall Semester, 2012 Day 21. Transition Metals Complexes V: Reaction Mechanisms Name(s): Element: Topics: 1. Substitution reactions: dissociative v. associative 4. Pseudorotation
More informationStructure of Coordination Compounds
Chapter 22 COORDINATION CHEMISTRY (Part II) Dr. Al Saadi 1 Structure of Coordination Compounds The geometry of coordination compounds plays a significant role in determining their properties. The structure
More informationOrganometallic Rections 1: Reactions at the Metal
E Organometallic Rections 1: Reactions at the Metal Three major classes of reactions: 1 Ligand Substitution associative (cf. S N 2) dissociative (cf. S N 1) interchange (not dealt with in this course)
More information5.03, Inorganic Chemistry Prof. Daniel G. Nocera Lecture 15 Apr 11: Substitution Reactions and the Trans Effect
5.03, Inorganic Chemistry Prof. Daniel G. ocera Lecture 15 Apr 11: Substitution Reactions and the Trans Effect A substitution reaction is one in which an existing ligand on a metal center is replaced by
More information489--Lectures 3 and 4. Fundamentals of Inorganic Chemistry
489--Lectures 3 and 4 Fundamentals of Inorganic Chemistry (with special relevance to biological systems) Some slides courtesy of Prof. Xuan Zhao (U. Memphis) and Prof. Yi Lu (U. Illinois) Fundamentals
More informationCoordination and Special Materials Chemistry. Elective I/II: WS 2005/6 (Lecture) H.J. Deiseroth. Part 2
Coordination and Special Materials Chemistry Elective I/II: WS 2005/6 (Lecture) H.J. Deiseroth Part 2 Coordination Chemistry: Spectroscopy -microstates and spectroscopic symbols (RS and jj coupling), see
More informationCoordination 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
More informationMechanisms of Inorganic Reactions HS -26
Mechanisms of Inorganic Reactions HS -26 A. Ligand Substitution Reactions Octahedral Co(III), Cr(III) Dissociative mechanism Square Planar Pt(II) Associative mechanism trans effect in Pt(II) complexes
More informationB. Electron Deficient (less than an octet) H-Be-H. Be does not need an octet Total of 4 valence electrons
B. Electron Deficient (less than an octet) e.g. BeH 2 H-Be-H Be does not need an octet Total of 4 valence electrons Not the same as unsaturated systems that achieve the 8e - (octet) through the formation
More informationLecture 12 Octahedral Substitution Reactions
2P32 Principles of Inorganic Chemistry Dr. M. Pilkington ecture 12 Octahedral Substitution Reactions The most extensively studied reactions of coordination compounds Measuring rates of water exchange in
More informationCoordination compounds - Isomerism
Coordination compounds - Isomerism K.Sridharan Dean School of Chemical & Biotechnology SASTRA University Thanjavur 613 401 Page 1 of 9 Table of Contents 1 Types of isomerism... 3 1.1 Types of isomerism...
More information- an approach to bonding that is useful for making estimates of E of orbitals in coordination complexes
10.4 Angular Overlap - an approach to bonding that is useful for making estimates of E of orbitals in coordination complexes - estimate the strength of interaction b/w ligand orbitals & metal d orbitals
More informationHow to identify types of transition in experimental spectra
17 18 19 How to identify types of transition in experimental spectra 1. intensity 2. Band width 3. polarization Intensities are governed by how well the selection rules can be applied to the molecule under
More informationBonding in Octahedral and Tetrahedral Metal Complexes. Predict how the d orbitals are affected by the Metal- Ligand Bonding
Bonding in Octahedral and Tetrahedral Metal Complexes 327 Molecular Orbital Theory and Crystal Field/Ligand Field Theory Predict how the d orbitals are affected by the Metal- Ligand Bonding d z 2, d x
More informationCoordination Chemistry: Bonding Theories. Molecular Orbital Theory. Chapter 20
Coordination Chemistry: Bonding Theories Molecular Orbital Theory Chapter 20 Review of the Previous Lecture 1. Discussed magnetism in coordination chemistry and the different classification of compounds
More information(1) Solvent interactions Water is a ligand itself so it can become involved in the chemistry: Overall reaction: [L 5 MX] + Y [L 5 MY] + X
(1) Solvent interactions Water is a ligand itself so it can become involved in the chemistry: Overall reaction: [L 5 MX] + Y [L 5 MY] + X 270 1.(slow) [L 5 MX] + H 2 O [L 5 M(H 2 O)] + X 2. (fast) [L 5
More informationMolecular Geometry and Bonding Theories. Molecular Shapes. Molecular Shapes. Chapter 9 Part 2 November 16 th, 2004
Molecular Geometry and Bonding Theories Chapter 9 Part 2 November 16 th, 2004 8 Molecular Shapes When considering the geometry about the central atom, we consider all electrons (lone pairs and bonding
More informationMITOCW ocw lec33
MITOCW ocw-5.112-lec33 The following content is provided by MIT OpenCourseWare under a Creative Commons license. Additional information about our license and MIT OpenCourseWare in general is available
More informationSchedule. Lecture 7: M-M bonds δ-bonds and bonding in metal clusters
Schedule Lecture 7: M-M bonds δ-bonds and bonding in metal clusters Lecture 8: Rates of reaction Ligand-exchange reactions, labile and inert metal ions Lecture 9: Redox reactions Inner and outer-sphere
More informationMolecular Orbital Theory (MOT)
Molecular Orbital Theory (MOT) In this section, There are another approach to the bonding in metal complexes: the use of molecular orbital theory (MOT). In contrast to crystal field theory, the molecular
More informationChapter 25 Transition Metals and Coordination Compounds Part 2
Chapter 25 Transition Metals and Coordination Compounds Part 2 Bonding in Coordination Compounds Valence Bond Theory Coordinate covalent bond is between: completely filled atomic orbital and an empty atomic
More informationElectronic 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
More informationCoordination Chemistry: Bonding Theories. Crystal Field Theory. Chapter 20
Coordination Chemistry: Bonding Theories Crystal Field Theory Chapter 0 Review of the Previous Lecture 1. We discussed different types of isomerism in coordination chemistry Structural or constitutional
More informationLecture 11 Reaction Types and Mechanisms for Inorganic Complexes
2P32 Principles of Inorganic Chemistry Dr. M. Pilkington Lecture 11 Reaction Types and Mechanisms for Inorganic Complexes Variations in reactivity Reaction types substitution, dissociation, addition and
More informationHydrogen Bond 1. The states of hybridization of boron and oxygen atoms in boric acid (H BO ) are reectively (A) and (B) and (C) and (D) and. The correct order of the hybridization of the central atom in
More informationIntroduction to VSEPR Theory 1
1 Class 8: Introduction to VSEPR Theory Sec 10.2 VSEPR Theory: The Five Basic Shapes Two Electron Groups: Linear Geometry Three Electron Groups: Trigonal Planar Geometry Four Electron Groups: Tetrahedral
More informationFill in the chart below to determine the valence electrons of elements 3-10
Chemistry 11 Atomic Theory IV Name: Date: Block: 1. Lewis Diagrams 2. VSEPR Lewis Diagrams Lewis diagrams show the bonding between atoms of a molecule. Only the outermost electrons of an atom (called electrons)
More informationReductive Elimination
Reductive Elimination Reductive elimination, the reverse of oxidative addition, is most often seen in higher oxidation states because the formal oxidation state of the metal is reduced by two units in
More informationChemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Chang & Goldsby Modified by Dr. Juliet Hahn Copyright McGraw-Hill Education. All rights reserved. No reproduction
More informationRDCH 702 Lecture 4: Orbitals and energetics
RDCH 702 Lecture 4: Orbitals and energetics Molecular symmetry Bonding and structure Molecular orbital theory Crystal field theory Ligand field theory Provide fundamental understanding of chemistry dictating
More informationChemistry 3211 Coordination Chemistry Part 3 Ligand Field and Molecular Orbital Theory
Chemistry 3211 Coordination Chemistry Part 3 Ligand Field and Molecular Orbital Theory Electronic Structure of Six and Four-Coordinate Complexes Using Crystal Field Theory, we can generate energy level
More informationDrawing Lewis Structures
Chapter 2 - Basic Concepts: molecules Bonding models: Valence-Bond Theory (VB) and Molecular Orbital Theory (MO) Lewis acids and bases When both of the electrons in the covalent bond formed by a Lewis
More informationModule 10 : Reaction mechanism. Lecture 1 : Oxidative addition and Reductive elimination. Objectives. In this lecture you will learn the following
Module 10 : Reaction mechanism Lecture 1 : Oxidative addition and Reductive elimination Objectives In this lecture you will learn the following The oxidative addition reactions. The reductive elimination
More informationElectron Geometry Hybrid Orbitals
Molecular Shape and Hybridized Orbitals CH2000: Introduction to General Chemistry, Plymouth State University Introduction: In chemistry, the three dimensional shape of a molecule is as important as the
More informationRecommended Reading: 23, 29 (3rd edition); 22, 29 (4th edition) Ch 102 Problem Set 7 Due: Thursday, June 1 Before Class. Problem 1 (1 points) Part A
Recommended Reading: 23, 29 (3rd edition); 22, 29 (4th edition) Ch 102 Problem Set 7 Due: Thursday, June 1 Before Class Problem 1 (1 points) Part A Kinetics experiments studying the above reaction determined
More informationMolecular Geometry. Valence Shell Electron Pair. What Determines the Shape of a Molecule? Repulsion Theory (VSEPR) Localized Electron Model
Molecular Geometry Learn Shapes you will Because the physical and chemical properties of compounds are tied to their structures, the importance of molecular geometry can not be overstated. Localized Electron
More informationName CHM 4610/5620 Fall 2016 December 15 FINAL EXAMINATION SOLUTIONS
Name CHM 4610/5620 Fall 2016 December 15 FINAL EXAMINATION SOLUTIONS I. (80 points) From the literature... A. The synthesis and properties of copper(ii) complexes with ligands containing phenanthroline
More informationReductive Elimination
Reductive Elimination Reductive elimination, the reverse of oxidative addition, is most often seen in higher oxidation states because the formal oxidation state of the metal is reduced by two units in
More informationElectron Geometry Hybrid Orbitals
Molecular Shape and Hybridized Orbitals CH2000: Introduction to General Chemistry, Plymouth State University, Fall 2014 Introduction: In chemistry, the three dimensional shape of a molecule is as important
More informationπ donor L L L π acceptor has empty π orbitals on ligand in to which d e- from M can be donated
Name KEY D# Chemistry 350 Fall 2005 Exam #4, November 18, 2005 50 minutes CCM 100 points on 4 pages + a useful page 5 1. Consider the molecular orbital diagram shown for M N. (16 pts) a) Indicate the following:
More informationValence Bond Theory - Description
Bonding and Molecular Structure - PART 2 - Valence Bond Theory and Hybridization 1. Understand and be able to describe the Valence Bond Theory description of covalent bond formation. 2. Understand and
More informationOrbitals and energetics
Orbitals and energetics Bonding and structure Molecular orbital theory Crystal field theory Ligand field theory Provide fundamental understanding of chemistry dictating radionuclide complexes Structure
More information1. Draw the molecular geometry and indicate any deviations from ideal VSEPR coordination angles. Give the point group for each molecule.
1 Inorganic Chemistry 411/511 115 minutes; 200 points total Show your work for partial credit. Final Exam 1. Draw the molecular geometry and indicate any deviations from ideal VSEPR coordination angles.
More informationThe VSEPR Model applied to Steric Numbers 2 through 4. (VSEPR Part 3)
This work is licensed by Shawn Shields under a Creativ e Commons Attribution-NonCommercial-ShareAlike 4.0 International License. The VSPR Model applied to Steric Numbers 2 through 4. (VSPR Part 3) By Shawn
More informationChapter 10 Shapes of Molecules. Dr. Sapna Gupta
Chapter 10 Shapes of Molecules Dr. Sapna Gupta Shapes of Molecules - Importance All molecules have a 3D orientations; even the diatomic ones because atoms have a volume. In case of tri atomic or polyatomic
More informationV.2 Synthesis of nickel complexes
V.2 Synthesis of nickel complexes Introduction: The nickel ion in nickel(ii)-complexes exists in the coordination number of 4, 5 and 6. Its octahedral, trigonal-bipyramidal, quadratic-pyramidal and tetrahedral
More informationChapter Molecules are 3D. Shapes and Bonds. Chapter 9 1. Chemical Bonding and Molecular Structure
Chapter 9 Chemical Bonding and Molecular Structure 1 Shape 9.1 Molecules are 3D Angle Linear 180 Planar triangular (trigonal planar) 120 Tetrahedral 109.5 2 Shapes and Bonds Imagine a molecule where the
More informationSection 6 Questions from Shriver and Atkins
Section 6 Questions from Shriver and tkins 4.35 Remember, softness increases as you go down a group, and both Zn and Hg are in Group 12. Hg 2+ is a very soft acid, so it is only realistically able to form
More informationCHEM Core Chemistry 3. Inorganic Reaction Mechanisms
CHEM3012 - Core Chemistry 3 Inorganic Reaction Mechanisms 5. Mechanisms of electron transfer between metal ions This section of the course is concerned with the mechanisms of electron transfer reactions,
More informationσ Bonded ligands: Transition Metal Alkyls and Hydrides
σ Bonded ligands: Transition Metal Alkyls and Hydrides Simplest of organo-transitionmetal species Rare until and understanding of their stability in the 60 s and 70 s Metal alkyls can be considered as
More informationLewis structures show the number and type of bonds between atoms in a molecule or polyatomic ion.
VSEPR & Geometry Lewis structures show the number and type of bonds between atoms in a molecule or polyatomic ion. Lewis structures are not intended to show the 3-dimensional structure (i.e. shape or geometry)
More informationCHM151LL: VSEPR and Molecular Geometry Tables
CHM151LL: VSEPR and Molecular Geometry Tables VSEPR Model VALENCE-SHELL ELECTRON-PAIR REPULSION (VSEPR) MODEL Lewis structures show the two-dimensional distribution of atoms and electrons. The molecular
More informationDownloaded from
1 Class XII: Chemistry Chapter 9: Coordination Compounds 1. Difference between coordination compound and double bond: Coordination compound A coordination compound contains a central metal atom or ion
More informationChapter 9. Lewis Theory-VSEPR Valence Bond Theory Molecular Orbital Theory
Chapter 9 Lewis Theory-VSEPR Valence Bond Theory Molecular Orbital Theory Problems with Lewis Theory Lewis theory generally predicts trends in properties, but does not give good numerical predictions.
More informationCrystal Field Theory History
Crystal Field Theory History 1929 Hans Bethe - Crystal Field Theory (CFT) Developed to interpret color, spectra, magnetism in crystals 1932 J. H. Van Vleck - CFT of Transition Metal Complexes Champions
More informationLewis Structure. Lewis Structures & VSEPR. Octet & Duet Rules. Steps for drawing Lewis Structures
Lewis Structure Lewis Structures & VSEPR Lewis Structures shows how the are arranged among the atoms of a molecule There are rules for Lewis Structures that are based on the formation of a Atoms want to
More informationChemistry Instrumental Analysis Lecture 11. Chem 4631
Chemistry 4631 Instrumental Analysis Lecture 11 Molar Absorptivities Range 0 to 10 5 Magnitude of e depends on capture cross section of the species and probability of the energy-absorbing transition. e
More informationInorganic Chemistry Laboratory
Inorganic Chemistry Laboratory Lab 8 Experiment 12 (p.117) The Paramagnetic Complex Mn(acac) 3 1 N 2 2s 2 2p 3 Electron Configurations 2 2s 2 2p 4 What are some consequences of the different electron configurations?
More informationChapter 9 practice questions
Class: Date: Chapter 9 practice questions Multiple Choice Identify the choice that best completes the statement or answers the question. 1. All of the following statements concerning valence bond (VB)
More informationPREDICTING THE GEOMETRY OF ORGANOMETALLIC COMPLEXES
PREDICTING THE GEOMETRY OF ORGANOMETALLIC COMPLEXES An important issue that we ve glossed over until now concerns what organometallic complexes actually look like: what are their typical geometries? Can
More informationSTEREOCHEMISTRY AND STEREOELECTRONICS NOTES
- 1 - STEREOCHEMISTRY AND STEREOELECTRONICS NOTES Stereochemistry in Organic Molecules Conventions used in drawing molecules Also, Fischer projections can sometimes be useful for acyclic molecules with
More informationCBSE Class-12 Chemistry Quick Revision Notes Chapter-09: Co-ordination Compounds
CBSE Class-12 Chemistry Quick Revision Notes Chapter-09: Co-ordination Compounds Co-ordination compounds: a) A coordination compound contains a central metal atom or ion surrounded by number of oppositely
More informationInorganic Chemistry GARY L. MIESSLER DONALD A. TARR. St. Olaf College Northfield, Minnesota
Inorganic Chemistry GARY L. MIESSLER DONALD A. TARR St. Olaf College Northfield, Minnesota Contents PREFACE xiii 1 INTRODUCTION TO INORGANIC CHEMISTRY 1 1-1 What Is Inorganic Chemistry? 1 1-2 Contrasts
More informationChapter 9. Molecular Geometries and Bonding Theories. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 9 Theories John D. Bookstaver St. Charles Community College Cottleville, MO Shapes The shape of a molecule plays an important role in its reactivity. By noting the number of
More informationInorganic Chemistry Laboratory
Inorganic Chemistry Laboratory Lab 8 Experiment 12 (p.117) The Paramagnetic Complex Mn(acac) 3 1 N 2 2s 2 2p 3 Electron Configurations 2 2s 2 2p 4 What are some consequences of the different electron configurations?
More informationCoordination Number Six
Coordination Number Six 241 Octahedral is a very important geometry. It is the starting point for the shapes of most transition metal complexes. 1. Regular octahedron all distances are EQUIVALENT 2. Distorted
More informationChapter 10 Theories of Covalent Bonding
Chapter 10 Theories of Covalent Bonding 1 Atomic Orbitals Molecules Bonding and 2 Molecular Structure Questions How are molecules held together? Why is O 2 paramagnetic? And how is this property connected
More informationCHAPTER TEN MOLECULAR GEOMETRY MOLECULAR GEOMETRY V S E P R CHEMICAL BONDING II: MOLECULAR GEOMETRY AND HYBRIDIZATION OF ATOMIC ORBITALS
CHAPTER TEN CHEMICAL BONDING II: AND HYBRIDIZATION O ATOMIC ORBITALS V S E P R VSEPR Theory In VSEPR theory, multiple bonds behave like a single electron pair Valence shell electron pair repulsion (VSEPR)
More informationAP Chemistry - Problem Drill 15: Lewis Structures and VSEPR Theory
AP Chemistry - Problem Drill 15: Lewis Structures and VSEPR Theory No. 1 of 10 1. Which shape would have sp 3 hybridization? (A) Linear (B) Bent (C) Tetrahedron (D) Trigonal planar (E) Octahedron C. Correct.
More informationCHEM 101: CHAPTER 11: CHEMICAL BONDS: THE FORMATION OF COMPOUNDS FROM ATOMS
1 CHEM 101: CHAPTER 11: CHEMICAL BONDS: THE FORMATION OF COMPOUNDS FROM ATOMS PERIODIC TRENDS: See pages 214-216, 221 Table 11.3, and 227 + 228 of text. Lewis Structures of Atoms: The Lewis Dot Diagram
More informationIntroduction to Inorganic Chemistry
Introduction to Inorganic Chemistry What is inorganic chemistry? Inorganic Chemistry Organimetallic Bioinorganic Organic vs Inorganic Introduction to Inorganic Chemistry Organic vs Inorganic Introduction
More informationUNIT 9 Topic: Coordination Compounds
UNIT 9 Topic: Coordination Compounds 1. State the postulates of Werner s theory of coordination compounds. Postulates: 1. Central metal ion in a complex shows two types of valences - primary valence and
More informationCHEMISTRY 112 LECTURE EXAM II Material
CHEMISTRY 112 LECTURE EXAM II Material Part I Chemical Bonding I Lewis Theory Chapter 9 pages 376-386 A. Drawing electron dot structures HOW TO: 1. Write e- dot structure for the individual atoms. 2. a)
More informationIllinois Central College CHEMISTRY 130 Laboratory Section: To predict the shapes of molecules based on their Lewis Structures.
Exercise 12 Page 1 Illinois Central College CEMISTRY 130 Laboratory Section: Molecular Structure Name: Objectives To predict the shapes of molecules based on their Lewis Structures. Background The Valence
More informationChemistry 324 Final Examination
Chem 324 Final Examination 2008 December 11, 2008 Page 1 of 8 Chemistry 324 Final Examination Thursday, December 11, 2008 Instructor: Dave Berg Answer all questions in the booklet provided; additional
More informationChapter 9. Covalent Bonding: Orbitals. Copyright 2017 Cengage Learning. All Rights Reserved.
Chapter 9 Covalent Bonding: Orbitals Chapter 9 Table of Contents (9.1) (9.2) (9.3) (9.4) (9.5) (9.6) Hybridization and the localized electron model The molecular orbital model Bonding in homonuclear diatomic
More informationCHEM1101 Worksheet 6: Lone Pairs and Molecular Geometry
CHEM1101 Worksheet 6: Lone Pairs and Molecular Geometry Model 1: Oxidation numbers Oxidation numbers are a useful accountancy tool to help keep track of electrons in compounds and reactions. This is particularly
More informationChem 673, Problem Set 5 Due Thursday, December 1, 2005
otton, Problem 9.3 (assume D 4h symmetry) Additional Problems: hem 673, Problem Set 5 Due Thursday, December 1, 2005 (1) Infrared and Raman spectra of Benzene (a) Determine the symmetries (irreducible
More informationCrystal Field Theory
Crystal Field Theory It is not a bonding theory Method of explaining some physical properties that occur in transition metal complexes. Involves a simple electrostatic argument which can yield reasonable
More informationChapter 9. Molecular Geometry and Bonding Theories
Chapter 9 Molecular Geometry and Bonding Theories MOLECULAR SHAPES 2 Molecular Shapes Lewis Structures show bonding and lone pairs do not denote shape Use Lewis Structures to determine shapes Molecular
More informationIf you put an electron into the t 2g, like that for Ti 3+, then you stabilize the barycenter of the d orbitals by 0.4 D o.
Crystal Field Stabilization Energy Week 2-1 Octahedral Symmetry (O h ) If you put an electron into the t 2g, like that for Ti 3+, then you stabilize the barycenter of the d orbitals by 0.4 D o. Each additional
More informationLecture Notes Chem 51B S. King I. Conjugation
Lecture Notes Chem 51B S. King Chapter 16 Conjugation, Resonance, and Dienes I. Conjugation Conjugation occurs whenever p-orbitals can overlap on three or more adjacent atoms. Conjugated systems are more
More informationPAPER No.7 : Inorganic Chemistry-II MODULE No.1 : Crystal Field Theory
Subject Chemistry Paper No and Title Module No and Title Module Tag 7, Inorganic Chemistry II 1, Crystal Field Theory CHE_P7_M1 TABLE OF CONTENTS 1. Learning Outcomes 2. Introduction to Crystal Field Theory
More informationChapter 10 Molecular Geometry and Chemical Bonding Theory. Copyright Cengage Learning. All rights reserved. 10 1
Chapter 10 Molecular Geometry and Chemical Bonding Theory Copyright Cengage Learning. All rights reserved. 10 1 Molecular geometry is the general shape of a molecule, as determined by the relative positions
More informationRecapping where we are so far
Recapping where we are so far Valence bond constructions, valence, valence electron counting, formal charges, etc Equivalent neutral classification and MLX plots Basic concepts for mechanism and kinetics
More informationN-Heterocyclic Carbenes (NHCs)
N-Heterocyclic Carbenes (NHCs) In contrast to Fischer and Schrock type carbenes NHCs are extremely stable, inert ligands when complexed to a metal centre. Similar to phosphine ligands they are electronically
More informationInorganic Chemistry 411/511 Final Exam Name 115 minutes; 200 points total Show your work for partial credit.
Inorganic Chemistry 411/511 Final Exam Name 115 minutes; 200 points total Show your work for partial credit. 1 1. Draw the molecular geometry and indicate any deviations from ideal VSEPR coordination angles.
More informationVSEPR. Valence Shell Electron Pair Repulsion Theory
VSEPR Valence Shell Electron Pair Repulsion Theory Vocabulary: domain = any electron pair or bond (single, double or triple) is considered one domain. bonding pair = shared pair = any electron pair that
More informationChemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals 1 Chemical Bonding II Molecular Geometry (10.1) Dipole Moments (10.2) Valence Bond Theory (10.3) Hybridization of Atomic Orbitals
More informationCHEM 110 Exam 2 - Practice Test 1 - Solutions
CHEM 110 Exam 2 - Practice Test 1 - Solutions 1D 1 has a triple bond. 2 has a double bond. 3 and 4 have single bonds. The stronger the bond, the shorter the length. 2A A 1:1 ratio means there must be the
More informationElectronic structure / bonding in d-block complexes
LN05-1 Electronic structure / bonding in d-block complexes Many, many properties of transition metal complexes (coordination number, structure, colour, magnetism, reactivity) are very sensitive to the
More information18-Electron Rule: Myth or Reality? An NBO Perspective
18-Electron Rule: Myth or Reality? An NBO Perspective Eric CLOT UMR 5253 - CNRS, UM2, ENSCM, UM1 Interaction Experiment/Theory Experimental Chemists have Questions Where are the Nucleophilic and Electrophilic
More informationElectron Counting. It s easier to show than to explain, I think.
Electron Counting This, for some reason I ve never worked out, isn t as easy as it should be. It is, however, important. It allows us to say things about the stability of organometallic complexes and make
More informationChem 1102 Semester 2, 2011!
Chem 110 Semester, 011! How is the ligand bonded to the metal? In octahedral complexes, six d sp 3 hybrid orbitals are used by the metal. The metal-ligand bond is a two-electron covalent bond. Mix d z,
More informationChapter 9 Molecular Geometries. and Bonding Theories
Chapter 9 Molecular Geometries and Bonding Theories Coverage of Chapter 9 9.1 All 9.2 All 9.3 All 9.4 All 9.5 Omit Hybridization Involving d Orbitals 9.6 All 9.7 and 9.8 Omit ALL MOLECULAR SHAPES The shape
More informationChapter 25 Transition Metals and Coordination Compounds Part 1
Chapter 25 Transition Metals and Coordination Compounds Part 1 Introduction The transition elements are defined as: those metallic elements that have a partially but incompletely filled d subshell or easily
More informationA Summary of Organometallic Chemistry
A Summary of Organometallic Chemistry Counting valence electrons (v.e.) with the ionic model 1. Look at the total charge of the complex Ph 3 P Cl Rh Ph 3 P PPh 3 OC CO 2 Fe OC CO Co + charge:0 charge:
More information