M- M bonds and Cluster chemistry
|
|
- Charla Gaines
- 5 years ago
- Views:
Transcription
1 M- M bonds and Cluster chemistry Defini&on: "a finite group of metal atoms that are held together mainly, or at least to a significant extent, by bonds directly between metal atoms, even though some non- metal atoms may also be in&mately associated with the cluster" F.A. Co)on 1
2 Two extreme types of metal clusters: Molecular clusters are composed of 3 or more metal atoms stabilized by small molecules acang as ligands, and characterized by metal- metal bonds, either localized or delocalized over the metal framework. 2
3 "Naked clusters" - have no ligands, electronically unsaturated, naked metal paracles formed in atomic beams; are extremely reacave unless stabilized by a support or an inert matrix, e.g. [Pb5]2-. In this part of the course, we focus on transiaon metal clusters with 2 or more M- M bonds, and, paracularly, late TM clusters with CO ligands. 3
4 Importance: (a) EvoluAon of properaes as cluster size increases (e.g. structure, magneac behaviour, ionizaaon potenaal): Transi&on from molecular bulk metal domain. metal- ligand charge transfer interacaons are limited to the metal atoms which are at the surface of the metal cluster; inner- core metal atoms behave as a metal paracle. properaes of a solid gradually evolve as atoms are brought together to form increasingly larger units. 4
5 (b) InterpretaAon of data obtained from metal surfaces which are acave heterogeneous catalysis sites (cluster- surface analogy). models for chemi- and physi- sorpaon of small molecules onto metallic surfaces - e.g. fluxionality of the coordinated fragments, mechanism of hydrogen diffusion inside a metallic network, the distoraons in metal close- packing induced by intersaaal heteroatoms, etc. 5
6 6
7 chemical reac&vity of coordinated ligands in molecular metal clusters has been used for studying the reacaon mechanisms at the metal centres, and for mimicking elementary processes relevant to homogeneous and heterogeneous catalysts. 7
8 c) FascinaAng structures (!). first reports of organometallic transiaon metal clusters: Fe2(CO)9 (1905), Fe3(CO)12 (1907) and Co2(CO)8 (1910) computer analysis of X- ray crystallographic data novel structural features 8
9 variety of metal frame shapes, bonding modes for any given ligand and stereochemistry observed was only possible in the presence of several metal atoms solid state chemists and physicists also became interested clusters as par&culate metals enclosed in a ligand sphere. 9
10 1000s of examples of ligated metal clusters have been reported. Most common clusters are formed by: - early transiaon metals stabilized by halide or oxygen atoms (aggregates) - metals of group 6-10 stabilized by CO molecules - transiaon or post- transiaon metals having halogen atoms, phosphine groups, and main group elements as ligands primary analyacal tool is X- ray diffrac&on, bond lengths which are shorter than the sum of the covalent radii being a reliable indicaaon of M- M bonding. 10
11 one of the first reported X- ray structural determina&ons of TMCCs was of Fe2(CO)9 (1939), revealed CO ligands bridging the M- M bond. 11
12 historically, first unsupported M M bonds were found in the analogous complexes Re2(CO)10 and Mn2(CO)10 (1957). Confirmed the existence of unsupported M- M bonds. 12
13 also very early on, the structure of the pentacoordinate Fe5(μ5- C)(CO)15 (1962) and [Re2Cl8]2-. Interes&ng structures s&mulated research; lack of syntheses frustrated research. Recent systema&c syntheses have led to the explosion in cluster chemistry. 13
14 STRUCTURE AND BONDING (1)TYPES OF CLUSTERS (i) π- Donor clusters: early transi&on metals (oxida&on state +2 or +3) with π- donor ligands (O2, S2, Cl, Br, I, OR, etc.). Typically triangular or octahedral geometries. 14
15 Electron dona&ng characteris&cs of common π- donor bridging ligands 15
16 Examples: [Nb6Cl12]2+, [Ta6Cl12]2+ octahedral M6, edge- bridging Cl (1) [Mo6Cl8]4+, [W6Cl8]4+ octahedral M6, face- capping Cl (2) [Re3Cl12]3- triangular Re3, 3 x μ- Cl, 9 x terminal Cl (3) 16
17 17
18 COs frequency as a ligand for stabilizing low oxidaaon state clusters arises because of its flexibility - coordinaaon as terminal, μ- and μ3- are all common and, because they are all 2e donors (unlike Cl), intramolecular exchange processes frequently have very low acavaaon energies. H- is not a π- acceptor ligand, but there are many carbonyl clusters that also have H- as a ligand, so these clusters are usually considered together. 18
19 Ligand bonding modes see more extensive discussion on bonding modes of CO, hydrido and acetylenic ligands (later in course). Cl ligand is a 1 e donor when terminal, or uses a lone pair to become a 3e donor when edge- bridging, or a 5e donor using an addiaonal lone pair when face bridging. 19
20 Bonding modes and electron count for some common ligands 20
21 (2) CLUSTER GEOMETRY high symmetry - usually define regular polyhedra as triangle, tetrahedra, octahedra, etc metal posiaons usually define deltahedra, i.e. Triangular faces; other arrangements, e.g. square- planar, trigonal prismaac, square anaprisms occur to lesser extent 21
22 many represent fragments of close- packed arrays of metal atoms, hcp ccp or bcc 22
23 form inters&&al complexes containing hydrogen, carbon, nitrogen, sulfur, phosphorus, and arsenic, as well as other metal atoms in the case of high- nuclearity clusters, in the intersaces 23
24 3 metal atom clusters great majority are triangular. Structural differences require only small changes in total energies of molecules e.g. Fe3(μ- CO)2(CO)10 and Ru3(CO)12. linear e.g [Mn3(CO)14]- or bent. Bond opening on a triangular cluster results in a linear geometry 24
25 4 metal atom clusters: many are tetrahedral with 6 M M bonds, e.g. CpWIr3(CO)11 25
26 bu)erflies can be regarded as resulang from a bond opening on the tetrahedron e.g. CpWIr3(CO)8(F3CC CCF3)2 26
27 interplanar angle in bu)erflies can be near 180, as in [Re4(CO)16] 2- Fe4(μ4- C)(μ- CO)(CO)12 contains a carbide atom in the middle of the cluster, approximately colinear with the wing- Ap atoms, providing an excellent model for a carbon atom on a metal surface. 27
28 square- planar geometries - for carbonyl clusters, onen contain a capping ligand e.g. Fe4(μ4- NEt)(μ3- η2- ONEt)(μ- CO)3(CO)8 28
29 bond rupture in a bu)erfly arrangement leads to a spiked triangle geometry, as in Re4(μ- H)3H(CO)15 29
30 30
31 31
32 32
33 33
34 34
35 35
36 36
37 37
38 38
39 39
40 40
41 41
42 42
43 43
44 Examples of prepara&ons 44
45 45
46 46
47 47
48 48
49 49
50 50
51 51
52 52
53 Ouch! 53
54 54
55 55
56 56
57 57
58 58
59 .. 59
60 60
61 61
62 62
63 63
64 64
65 65
66 66
67 67
68 68
69 69
70 n+1 n+1 n+1 70
71 71
72 72
73 73
74 74
75 75
76 76
77 77
78 78
79 79
80 80
81 81
82 82
83 83
84 Os 6 (CO) 18 84
85 85
86 EAN PSPET n = 3 18x3 = 54-6 = (12x3) = 12 à 6 pairs (arachno) 4 18x4 = = (12x4) = 12à 6 pairs (nido) 5 18x5 = = (12x5) = 12 à 6 pairs (closo) 6 18x6 = = 84 n + 2 7
87 87
88 88
89 89
90 90
91 91
92 92
93 93
94 94
95 95
96 96
97 97
98 CHEM 3032 Cluster Chemistry 98
99 99
100 100
101 101
102 102
103 103
104 104
105 105
106 106
107 107
108 108
109 109
110 110
111 111
112 112
113 113
114 114
115 115
116 116
117 117
118 118
119 119
120 120
121 121
122 122
123 123
124 124
125 125
126 126
127 127
128
129
130
131
132
133
134
135
136
11, Inorganic Chemistry III (Metal π-complexes and Metal Clusters) Module 32: Polynuclear metal carbonyls and their structure
1 Subject Paper No and Title Module No and Title Module Tag Chemistry 11, Inorganic Chemistry III (Metal π-complexes and Module 32: Polynuclear metal carbonyls and their structure CHE_P11_M32 2 TABLE OF
More informationFINAL EXAMINATION 12/17/93.
INORGANIC CHEMISTRY 413/571 FINAL EXAMINATION 12/17/93. DR. J. SHERIDAN Write all answers in the answer book. WRITE NEATLY. This will help me to understand your answers and maybe get you a few more points!
More informationPAPER No. : 11 and Inorganic Chemistry MODULE No.3 : and Structure of metal carbonyls and 18-electron rule applied to them. Paper No and Title
Subject Chemistry Paper No and Title Module No and Title Module Tag 11 : Inorganic Chemistry 3 : Structure of metal carbonyls and 18-electron rule applied to them CHE_P11_M3 TABLE OF CONTENTS 1. Learning
More information(for tutoring, homework help, or help with online classes)
www.tutor-homework.com (for tutoring, homework help, or help with online classes) Question 1 An atom loses an electron to another atom. Is this an example of a physical or chemical change? Question 2 Physical
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 informationAt the end of this lesson, students should be able to :
At the end of this lesson, students should be able to : (a) Explain Valence Shell Electron Pair Repulsion theory (VSEPR) (b) Draw the basic molecular shapes: linear, planar, tetrahedral, and octahedral.
More informationLearning Guide 2C Small Molecules Chem What are the two most common types of physical changes that we encounter in chemistry?
Review Learning Guide 2C Small Molecules Chem 1010 What are the two most common types of physical changes that we encounter in chemistry? 1) 2) What are the three most common types of nuclear changes,
More informationReview questions CHAPTER 5. Practice exercises 5.1 F F 5.3
CHAPTER 5 Practice exercises 5.1 S 5.3 5.5 Ethane is symmetrical, so does not have a dipole moment. However, ethanol has a polar H group at one end and so has a dipole moment. 5.7 xygen has the valence
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 informationCheck Your Solution A comparison with the figures in Figure 4.31 on page 234 of the student textbook confirms the results.
Predicting the Shape of a Molecule (Student textbook page 236) 11. What molecular shape is represented by each of the following VSEPR notations? a. AX 3 b. AX 5 E You need to assign a molecular shape that
More informationChemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Linear Trigonal 180 o planar 120 o Tetrahedral 109.5 o Trigonal Bipyramidal 120 and 90 o Octahedral 90 o linear Linear
More informationLecture 4! ü Review on atom/ion size! ü Crystal structure (Chap 4 of Nesseʼs book)!
Lecture 4! ü Review on atom/ion size! ü Crystal structure (Chap 4 of Nesseʼs book)! 15 C 4+ 42 Si 4+ Size of atoms! Hefferan and O Brien, 2010; Earth Materials Force balance! Crystal structure (Chap. 4)!
More informationName. Molecular Models
Name Molecular Models Lab Day Introduction: The atom and molecule are truly small; 6 10 23 carbon atoms occupy about 4 cm 3, or each atom has a volume of about 6 10 24 cm 3. Molecules, though larger than
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 informationChapter 12 Structures and Characteristics of Bonds Objectives
Objectives 1. To learn about ionic and covalent bonds and explain how they are formed - what holds compounds together? 2. To learn about the polar covalent bond are all covalent bonds equal? 3. To understand
More informationFind the difference in electronegativity between the hydrogen and chlorine atoms
Answers Questions 16.2 Molecular polarity 1. Write a dot diagram for the HCl molecule. Find the difference in electronegativity between the hydrogen and chlorine atoms Difference in electronegativity =
More informationChemical Bonds, Molecular Models, and Molecular Shapes
Chemical Bonds, Molecular Models, and Molecular Shapes PRELAB ASSINGMENT Read the entire laboratory write up and answer the following questions before coming to lab. Read the entire laboratory write up
More informationChemistry of the Main Group Elements: Boron through the Pnictogens
Chemistry of the Main Group Elements: Boron through the Pnictogens Sections 8.5-8.7 and 15.4.1 Friday, November 6, 2015 Group IIIA (13): B, Al, Ga, In, and Tl Diverse group of elements with three valence
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 informationChemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Valence shell electron
More informationChemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals
Chemical Bonding II: and ybridization of Atomic rbitals Chapter 10 Valence shell electron pair repulsion (VSEPR) model: Predict the geometry of the molecule from the electrostatic repulsions between the
More information1) H2 2) O2 3) N2. 4) HCl 5) H2O CHEMISTRY LAB MODELING COVALENT MOLECULES BOND TYPE(S) LEWIS STRUCTURE POLARITY OF MOLECULE ELECTRONIC SHAPE
CHEMISTRY LAB MODELING COVALENT S NAME: PER: FORMULA MOLECULAR 1) H2 hydrogen gas 2) O2 oxygen gas 3) N2 nitrogen gas 4) HCl hydrochloric acid 5) H2O dihydrogen oxide FORMULA MOLECULAR 6) CO2 carbon dioxide
More informationMetals - Homework solutions
Metals - Homework solutions Q Ex 1,2,3,6,8,10,12,13,14,17,20 and Prob. 8 8.1 a) Melting point decreases down the groups Melting point increases on going left to right b) The radii increase on going down
More informationCSIR-UGC-NET/JRF GATE CHEMISTRY TEST : ORGANOMETALLIC COMPOUNDS
1 CSIR-UGC-NET/JRF GATE CHEMISTRY TEST : ORGANOMETALLIC MPOUNDS Time 00 : Hour Date : 1-10-2017 M.M. : 0 INSTRUCTION : 1. There are Two Parts. Part-A contains 10 objective type questions, each question
More informationLewis Structures and Molecular Shapes
Lewis Structures and Molecular Shapes Drawing Lewis Structures Determine from formula if ionic or covalent Count the electrons If ionic : add valence # to charge if (-), subtract if (+) - = 7+1 electrons;
More information(A) 1 bonding pair (B) 1 bonding pair and 1 lone pair (C) 2 bonding pairs (D) 2 bonding pairs and 2 lone pairs
AP Chemistry - Problem Drill 13: Lewis Structures and VSPER No. 1 of 10 1. Lewis structure is used to model covalent bonds of a molecule or ion. Covalent bonds are a type of chemical bonding formed by
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 informationChapter 12. Molecular Structure
Chapter 12 Molecular Structure Chapter Map Models Advantages and Disadvantages (1) They help us to visualize, explain, and predict chemical changes. Because a model is a simplified version of what we think
More information5 Polyatomic molecules
s manual for Burrows et.al. Chemistry 3 Third edition 5 Polyatomic molecules Answers to worked examples WE 5.1 Formal charges in N 2 (on p. 221 in Chemistry 3 ) Use formal charges to decide whether oxygen
More informationValence Shell Electron Pair repulsion
Molecular Geometry Valence Shell Electron Pair repulsion The valence shell electron pair repulsion model (VSEPR model) assumes that electron pairs repel one another. (VSEPR) model gives helps determine
More informationChemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 1
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 1 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. How to get the book of
More informationChapter 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
More informationResearch Report by Dr. Kirill Yu. Monakhov
Research Report by Dr. Kirill Yu. Monakhov Anorganisch-Chemisches Institut, Universität Heidelberg, Im Neuenheimer Feld 270, D-69120 Heidelberg, Germany, Fax: +49-6221-546617. Supervisor: Gerald Linti
More informationCovalent Bonding and Molecular Structures
CHAPTERS 9 AND 10 Covalent Bonding and Molecular Structures Objectives You will be able to: 1. Write a description of the formation of the covalent bond between two hydrogen atoms to form a hydrogen molecule.
More informationCHEMICAL BONDING. Chemical Bonds. Ionic Bonding. Lewis Symbols
CHEMICAL BONDING Chemical Bonds Lewis Symbols Octet Rule whenever possible, valence electrons in covalent compounds distribute so that each main-group element is surrounded by 8 electrons (except hydrogen
More informationCHEMISTRY - MCMURRY 7E CH.7 - COVALENT BONDING AND ELECTRON DOT STRUCTURES
!! www.clutchprep.com CONCEPT: ELECTRONIC GEOMETRY When drawing a compound you have to take into account two different systems of geometrical shape. The simpler system known as electronic geometry or shape
More informationPAPER No.11: Inorganic Chemistry-III MODULE No.29: Metal- metal bonds and their evidences
1 Subject Chemistry Paper No and Title Module No and Title Module Tag 11: Inorganic Chemistry-III (Metal π-complexes and Metal Clusters) 29: Metal-metal bonds and their evidences CHE_P11_M29 2 TABLE OF
More informationShapes of Molecules. Lewis structures are useful but don t allow prediction of the shape of a molecule.
Shapes of Molecules Lewis structures are useful but don t allow prediction of the shape of a molecule. H O H H O H Can use a simple theory based on electron repulsion to predict structure (for non-transition
More informationIntroduction. A1.1 (a) Shell number and number of subshells 1. A1.1 (b) Orbitals 2. A1.1 (c ) Orbital shapes (s, p & d) 2
Preface Table of Contents Introduction i A1.1 (a) Shell number and number of subshells 1 A1.1 (b) Orbitals 2 A1.1 (c ) Orbital shapes (s, p & d) 2 A1.1 (d) Relative energies of s,p,d,f sub-shells 4 A 1.1
More informationSection 12: Lewis Structures
Section 12: Lewis Structures The following maps the videos in this section to the Texas Essential Knowledge and Skills for Science TAC 112.35(c). 12.01 Electronegativity Chemistry (5)(C) 12.02 Electron
More informationCovalent Compounds: Bonding Theories and Molecular Structure
CHM 123 Chapter 8 Covalent Compounds: Bonding Theories and Molecular Structure 8.1 Molecular shapes and VSEPR theory VSEPR theory proposes that the geometric arrangement of terminal atoms, or groups of
More informationMolecular Geometry and Bonding Theories. Chapter 9
Molecular Geometry and Bonding Theories Chapter 9 Molecular Shapes CCl 4 Lewis structures give atomic connectivity; The shape of a molecule is determined by its bond angles VSEPR Model Valence Shell Electron
More informationCh 13: Covalent Bonding
Ch 13: Covalent Bonding Section 13: Valence-Shell Electron-Pair Repulsion 1. Recall the rules for drawing Lewis dot structures 2. Remember the special situations: - Resonance structures - ormal charges
More information4.2.7 & Shapes, and bond angles for molecules with two, three and four negative charge centers
4.2.7 & 4.2.8 Shapes, and bond angles for molecules with two, three and four negative charge centers The shape of a molecule has an important part to play in determining its chemical (e.g. reactivity and
More informationCovalent Bonds: overlap of orbitals σ-bond π-bond Molecular Orbitals
Covalent Bonding What is covalent bonding? Covalent Bonds: overlap of orbitals σ-bond π-bond Molecular Orbitals Hybrid Orbital Formation Shapes of Hybrid Orbitals Hybrid orbitals and Multiple Bonds resonance
More informationExperiment #2. Lewis Structures
Experiment #2. Lewis Structures A Lewis structure shows how the valence electrons are arranged and indicates the bonding between atoms in a molecule. We represent the elements by their symbols. The shared
More informationSKILL-BUILDING EXERCISE
4. O and H Solution 1. Carbon has an electronegativity of 2.5, while the value for hydrogen is 2.1. The difference is 0.3, which is rather small. The C H bond is therefore considered nonpolar. 2. Both
More information11, Inorganic Chemistry III (Metal π-complexes and Metal Clusters) Module 31: Preparation and reactions of metal clusters
1 Subject Paper No and Title Module No and Title Module Tag Chemistry 11, Inorganic Chemistry III (Metal π-complexes and Module 31: Preparation and reactions of metal clusters CHE_P11_M31 2 TABLE OF CONTENTS
More informationChapter 12. Chemical Bonding
Chapter 12 Chemical Bonding Chemical Bond Concept Recall that an atom has core and valence electrons. Core electrons are found close to the nucleus. Valence electrons are found in the most distant s and
More informationChemical Bonding and Molecular Models
25 Chemical Bonding and Molecular Models A chemical bond is a force that holds groups of two or more atoms together and makes them function as a unit. Bonding involves only the valence (outer shell) electrons
More informationLearning 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
More informationCH 222 Chapter Seven Concept Guide
CH 222 Chapter Seven Concept Guide 1. Lewis Structures Draw the Lewis Dot Structure for cyanide ion, CN -. 1 C at 4 electrons = 4 electrons 1 N at 5 electrons = 5 electrons -1 charge = + 1 electron Total
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 informationCOVALENT BONDING CHEMICAL BONDING I: LEWIS MODEL. Chapter 7
Chapter 7 P a g e 1 COVALENT BONDING Covalent Bonds Covalent bonds occur between two or more nonmetals. The two atoms share electrons between them, composing a molecule. Covalently bonded compounds are
More informationHybridization of Orbitals
Hybridization of Orbitals Structure & Properties of Matter 1 Atomic Orbitals and Bonding Previously: Electron configurations Lewis structures Bonding Shapes of molecules Now: How do atoms form covalent
More informationChem Spring, 2018 Assignment 1 - Solutions
Chem 370 - Spring, 2018 Assignment 1 - Solutions 2.15 a. The possible values are shown in the following table. rbital l m l 5d 2-2, -1, 0, +1, +2 4f 3-3, -2, -1, 0, +1, +2, +3 7g 4-4, -3, -2, -1, 0, +1,
More informationMolecular Geometry and Electron Domain Theory *
OpenStax-CNX module: m12594 1 Molecular Geometry and Electron Domain Theory * John S. Hutchinson This work is produced by OpenStax-CNX and licensed under the Creative Commons Attribution License 2.0 1
More information8.3 Bonding Theories > Chapter 8 Covalent Bonding. 8.3 Bonding Theories. 8.1 Molecular Compounds 8.2 The Nature of Covalent Bonding
Chapter 8 Covalent Bonding 8.1 Molecular Compounds 8.2 The Nature of Covalent Bonding 8.3 Bonding Theories 8.4 Polar Bonds and Molecules 1 Molecular Shape What information does a structural formula give
More information: Bond Order = 1.5 CHAPTER 5. Practice Questions
CAPTER 5 Practice Questions 5.1 5.3 S 5.5 Ethane is symmetrical, so does not have a dipole moment. owever, ethanol has a polar group at one end and so has a dipole moment. 5.7 xygen has the valence electron
More informationChemical 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 4.3 Covalent structures
More informationPAPER No.11 : Inorganic Chemistry-II MODULE No.1 : Π-acceptor ligand, metal carbonyls, bonding modes of CO, classification of metal carbonyls
Subject Paper No and Title Module No and Title Module Tag 11: INORGANIC CHEMISTRY-III (METAL π- COMPLEXES AND METAL CLUSTERS) 1: π-acidity, Metal carbonyls, their classification and general features CHE_P11_M1
More informationSHAPES OF EXPANDED VALENCE MOLECULES
228 SHAPES OF EXPANDED VALENCE MOLECULES There are five atoms bonded to the central phosphorus atom, and they will attempt to get as far apart as possible from one another! The top and bottom atoms are
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 informationA DOT STRUCTURE FOR A LARGER MOLECULE ETHANOL! Count valence electrons
212 A DOT STRUCTURE FOR A LARGER MOLECULE Count valence electrons Pick central atom and draw skeletal structure - central atom is usually the one that needs to gain the most electrons! - skeletal structure
More informationChemical 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
More informationCovalent bonding occurs in nonmetal compounds. Use the highlighter to select the compounds that are covalently bonded. HCl
Covalent bonding occurs in nonmetal compounds. Use the highlighter to select the compounds that are covalently bonded. 2 C 2 Cl Li NaF Mg C 4 N NaCl 3 Drag this to the target to reveal the answers. Properties
More informationChapter 9: Chemical Bonding I: Lewis Theory. Lewis Theory: An Overview
Chapter 9: Chemical Bonding I: Lewis Theory Dr. Chris Kozak Memorial University of ewfoundland, Canada Lewis Theory: An verview Valence e - play a fundamental role in chemical bonding. e - transfer leads
More informationChem 121 Exam 4 Practice Exam
Chem 121 Exam 4 Practice Exam 1. What is the correct electron configuration for bromine? b. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 9 4s 2 4p 6 c. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 5 d. 1s 2 2s 2 2p 6 3s 2 3p
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 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 informationhttps://cuvillier.de/de/shop/publications/766
Jelena Jenter (Autor) Nitrogen Donor Ligands in the Coordination Chemistry of the are Earth and Alkaline Earth Metals Synthesis - Structures - Catalysis https://cuvillier.de/de/shop/publications/766 Copyright:
More informationCHAPTER 6 CHEMICAL BONDING TEXT BOOK EXERCISE Q.1. Select the correct statement. i. An ionic compound A + B - is most likely to be formed when ii. iii. a. the ionization energy of A is high and electron
More informationChapters 9&10 Structure and Bonding Theories
Chapters 9&10 Structure and Bonding Theories Ionic Radii Ions, just like atoms, follow a periodic trend in their radii. The metal ions in a given period are smaller than the non-metal ions in the same
More informationCHAPTER 6 CHEMICAL BONDING SHORT QUESTION WITH ANSWERS Q.1 Dipole moments of chlorobenzene is 1.70 D and of chlorobenzene is 2.5 D while that of paradichlorbenzene is zero; why? Benzene has zero dipole
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 informationDiamond. There are four types of solid: -Hard Structure - Tetrahedral atomic arrangement. What hybrid state do you think the carbon has?
Bonding in Solids Bonding in Solids There are four types of solid: 1. Molecular (formed from molecules) - usually soft with low melting points and poor conductivity. 2. Covalent network - very hard with
More informationChem 1075 Chapter 12 Chemical Bonding Lecture Outline. Chemical Bond Concept
Chem 1075 Chapter 12 Chemical Bonding Lecture Outline Slide 2 Chemical Bond Concept Recall that an atom has and electrons. Core electrons are found to the nucleus. Valence electrons are found in the s
More informationThere are four types of solid:
Bonding in Solids There are four types of solid: 1. Molecular (formed from molecules) - usually soft with low melting points and poor conductivity. 2. Covalent network - very hard with very high melting
More informationChemical Bonding II. Molecular Geometry Valence Bond Theory Phys./Chem. Properties Quantum Mechanics Sigma & Pi bonds Hybridization MO theory
Chemical Bonding II Molecular Geometry Valence Bond Theory Phys./Chem. Properties Quantum Mechanics Sigma & Pi bonds ybridization MO theory 1 Molecular Geometry 3-D arrangement of atoms 2 VSEPR Valence-shell
More informationDo now: Brainstorm how you would draw the Lewis diagram for: H 2 O CO 2
Do now: Brainstorm how you would draw the Lewis diagram for: 2 O CO 2 Shapes of molecules C 4 N 3 2 O C 2 O CO 2 Shapes of molecules Shapes of molecules are determined by the number of bonding and non-bonding
More informationEPIC LIGAND SURVEY: CARBON MONOXIDE
EPIC LIGAND SURVEY: CARBON MONOXIDE As a young, growing field, organometallic chemistry may be taught in many ways. Some professors (e.g., Shaugnessy) spend a significant chunk of time discussing ligands,
More informationCovalent Bonding. In nature, only the noble gas elements exist as uncombined atoms. All other elements need to lose or gain electrons
In nature, only the noble gas elements exist as uncombined atoms. They are monatomic - consist of single atoms. All other elements need to lose or gain electrons To form ionic compounds Some elements share
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 11 Introduction to Organic Chemistry Based on Material Prepared by Andrea D. Leonard University of Louisiana at Lafayette
Chapter 11 Introduction to Organic Chemistry Based on Material Prepared by Andrea D. Leonard University of Louisiana at Lafayette Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction
More informationMultiple Choice Identify the letter of the choice that best completes the statement or answers the question.
CHAPTER 4 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. A substance is a brittle crystal that conducts electricity in molten liquid state
More informationINTRODUCTORY CHEMISTRY Concepts and Critical Thinking
INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Sixth Edition by Charles H. Corwin Chapter 12 Chemical Bonding by Christopher Hamaker 2011 Pearson Education, Inc. Chapter 12 1 Chemical Bond Concept
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 informationChapter 25: The Chemistry of Life: Organic and Biological Chemistry
Chemistry: The Central Science Chapter 25: The Chemistry of Life: Organic and Biological Chemistry The study of carbon compounds constitutes a separate branch of chemistry known as organic chemistry The
More information1. I can use Collision Theory to explain the effects of concentration, particle size, temperature, and collision geometry on reaction rates.
Chemical Changes and Structure Learning Outcomes SECTION 1 Controlling the Rate. Subsection (a) Collision Theory 1. I can use Collision Theory to explain the effects of concentration, particle size, temperature,
More informationINTRODUCTORY CHEMISTRY Concepts and Critical Thinking Seventh Edition by Charles H. Corwin
Lecture INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Seventh Edition by Charles H. Corwin Chemical Bonding by Christopher G. Hamaker Illinois State University Chemical Bond Concept Recall that
More informationAP Chemistry- Practice Bonding Questions for Exam
AP Chemistry- Practice Bonding Questions for Exam Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which of the following is a correct Lewis structure for
More informationbond energy- energy required to break a chemical bond -We can measure bond energy to determine strength of interaction
bond energy- energy required to break a chemical bond -We can measure bond energy to determine strength of interaction ionic compound- a metal reacts with a nonmetal Ionic bonds form when an atom that
More informationCHAPTER 6: CHEMICAL NAMES AND FORMULAS CHAPTER 16: COVALENT BONDING
CHAPTER 6: CHEMICAL NAMES AND FORMULAS CHAPTER 16: COVALENT BONDING 6.1 Introduction to Chemical Bonding A chemical bond is a mutual electrical attraction between the nuclei and valence electrons of different
More information1. Which is the most electronegative atom in the compound below?
1. Which is the most electronegative atom in the compound below? A) Carbon C) Oxygen B) Nitrogen D) Bromine 2. Which of the following correctly describes the electrons of a carbon atom in its ground state?
More informationDEFINITION. 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
More informationHour Exam 3 on Chap 6, 7, and 8 is this Friday 11/12. A practice exam is posted on the course website.
11/8/2010 1 Chem 105 Monday 11 Nov 2010 Bond length qualitative Polarity Polarity and geometry Bond energy our Exam 3 on Chap 6, 7, and 8 is this riday 11/12. A practice exam is posted on the course website.
More informationReview for Chapter 4: Structures and Properties of Substances
Review for Chapter 4: Structures and Properties of Substances You are responsible for the following material: 1. Terms: You should be able to write definitions for the following terms. A complete definition
More informationPaper No and Title. Module No and Title CHEMISTRY
1 Subject Paper No and Title Module No and Title Module Tag Chemistry 11, Inorganic Chemistry III (Metal π-complexes and Metal Module 33: Preparation, structure and bonding of compounds CHE_P11_M33 2 TABLE
More informationTest Review # 4. Chemistry: Form TR4.11A
Chemistry: Form TR4.11 REVIEW Name Date Period Test Review # 4 Bonding. The electrons of one atom are attracted to the protons of another. When atoms combine, there is a tug of war over the valence electrons.
More informationValence Shell Electron Pair Repulsion Model
Activity 22 Valence hell Electron Pair Repulsion Model Why? Molecules adopt a shape that minimizes their energy. In many cases it is possible to predict the geometry of a molecule simply by considering
More information