10-1 Experimental Evidence for Electronic Structures Four- and Six-Coordinate Preferences
|
|
|
- Rolf Golden
- 7 years ago
- Views:
Transcription
1 Chapter 10 Coordination Chemistry II: Bonding 10-1 Experimental Evidence for Electronic Structures 10-2 Theories of Electronic Structure 10-3 Ligand Field Theory 10-4 Angular Overlap 10-5 The Jahn-Teller Effect 10-6 Four- and Six-Coordinate Preferences 10-7 Other Shapes Inorganic Chemistry Third Ed. Gary L. Miessler, Donald A. Tarr, 2004, Pearson Prentice Ha
2 Experimental Evidence for Electronic Structures Thermodynamic Data Magnetic Susceptibility Electronic Spectra Coordination Numbers and Molecular Shapes
3 Experimental Evidence for Electronic Structures; Thermodynamic Data One of the primary goal of a bonding theory is to explain the energy of compound. The energy is openly not determined directly by experiment. Thermodynamic measurements of enthalpies and free energies of reaction are used to compare. onding strength Stability constants(formation constants
4 Experimental Evidence for Electronic Structures; Thermodynamic Data What is the stability constants? The equilibrium constants for formation of coordination complex.
5 Experimental Evidence for Electronic Structures; Thermodynamic Data Stability constants HSAB concepts Thermodynamic values Prediction of properties, structures
6 Experimental Evidence for Electronic Structures; Thermodynamic Data HSAB concepts The gist of this theory is that soft acids react faster and form stronger bonds with soft bases, whereas hard acids react faster and form stronger bonds with hard bases, all other factors being equal. The classification in the original work was mostly based on equilibrium constants for reaction of two Lewis bases competing for a Lewis acid. Hard acids and hard bases tend to have: small size high oxidation state low polarizability high electronegativity energy low-lying HOMO (bases) or energy high-lying LUMO (acids).
7 Experimental Evidence for Electronic Structures; Thermodynamic Data HSAB concepts
8 Experimental Evidence for Electronic Structures; Thermodynamic Data Chelating Ligands Entropy Effect Chelate Effect Five or six membered ring en vs methyl amine Figure in head. Stability.
9 Experimental Evidence for Electronic Structures; Magnetic Susceptibility The magnetic properties of a coordination compound can provide indirect evidence of the orbital energy level. und s rule the max. # of unpaired e -. iamagnetic: all e - paried repelled by a magnetic field aramagnetic: all e - paried attracted into a magnetic field Magnetic Susceptibility: Measuring Magnetism
10 Experimental Evidence for Electronic Structures; Magnetic Susceptibility Magnetic Susceptibility Gouy method A sample that is to be tested is suspended from a balance between the poles of a magnet. The balance measures the apparent change in the mass of the sample as it is repelled or attracted by the magnetic field.
11 Experimental Evidence for Electronic Structures; Magnetic Susceptibility In physics and applied disciplines such as electrical engineering, the magnetic susceptibility is the degree of magnetization of a material in response to an applied magnetic field. Electron spin Spin magnetic moment (m s ) Total spin magnetic moment Spin quantum # S (sum of m Isolated oxygen atom 1s 2 2s 2 p 4 S = +1/2 +1/2 +1/2-1/2 = 1 Electron spin Orbital magnetic moment (m l ) Total orbital magnetic moment Orbital quantum # L (sum of m l ) Max. L for the p 4
12 Experimental Evidence for Electronic Structures; Magnetic Susceptibility Two sources of magnetic moment spin (S) and Angular (L) motions of electrons Spin quantum number Angular momentum quantum number The equation for the magnetic moment Contribution from L is small in first transition series
13 Experimental Evidence for Electronic Structures; Electronic Spectra Give a direct evidence of orbital energy level Give an information for geometry of complexes
14 Theories of Electronic Structure Valence bond theory Crystal field theory Ligand field theory Angular overlap method
15 Theories of Electronic Structure; Valence bond theory Hybridization ideas Octahedral: d 2 sp 3 d orbitals could be 3d or 4d for the first-row transition metals. (hyperligated, hypoligated)
16 Theories of Electronic Structure; Valence bond theory Fe(III) Isolated ion; 5 unpaired e - In O h compound; 1 or 5 unpaired e - Co(II) Low spin Low spin High spin High spin
17 Theories of Electronic Structure; Crystal field theory Crystal field theory (CFT) is a model that describes the electronic structure of transition metal compounds, all of which can be considered coordination complexes. CFT successfully accounts for some magnetic properties, colours, hydration enthalpies, and spinel structures of transition metal complexes, but it does not attempt to describe bonding. CFT was developed by physicists Hans Bethe and John Hasbrouck van Vleck in the 1930s. CFT was subsequently combined with molecular orbital theory to form the more realistic and complex ligand field theory (LFT), which delivers insight into the process of chemical bonding in transition metal complexes.
18 Theories of Electronic Structure; Crystal field theory Repulsion between d-orbital electrons and ligand electrons Splitting of energy levels of d-orbitals
19 Theories of Electronic Structure; Crystal field theory
20 Theories of Electronic Structure; Crystal field theory
21 Theories of Electronic Structure; Crystal field theory Electrostatic approach In an Octahedral field of ligand e - pairs; any e - in them are repelled by the field. Crystal field stabilization energy (CFSE); the actual distribution vs the uniform field. Good for the concept of the repulsion of orbitals by the ligands but no explanation for bonding in coordination complexes.
22 Theories of Electronic Structure; Crystal field theory
23 Theories of Electronic Structure; Crystal field theory
24 Theories of Electronic Structure; Crystal field theory
25 Theories of Electronic Structure; Crystal field theory
26 Theories of Electronic Structure; Crystal field theory
27 Theories of Electronic Structure; Crystal field theory
28 Theories of Electronic Structure; Crystal field theory Why are complexes formed in crystal field theory? Crystal Field Stabilization Energy (CFSE) Or Ligand Field Stabilization Energy (LFSE) the stabilization of the d orbitals because of metal-ligand environments
29 Theories of Electronic Structure; Crystal field theory E = strong field weak field E > 0 weak field E < 0 strong field
30 Theories of Electronic Structure; Crystal field theory hat determine? epends on the relative energies f the metal ions and ligand rbitals and on the degree of verlap.
31 Theories of Electronic Structure; Crystal field theory Spectrochemical Series for Metal Ions Oxidation # Small size & higher charge Only low spin aqua comple Pt 4+ > Ir 3+ > Pd 4+ > Ru 3+ > Rh 3+ >Mo 3+ > Mn 4+ > Co 3+ > Fe 3+ > V 2+ > Fe 2+ Co 2+ > Ni 2+ > Mn 2+
32 Ligand field theory; Molecular orbitals for Octahedral complexes CFT & MO were combined The d x2-y2 and d z2 orbitals can form bonding orbitals with the ligand orbitals, but d xy, d xz, and d yz orbitals cannot form bonding orbitals
33 Ligand field theory; Molecular orbitals for Octahedral complexes The combination of the ligand and metal orbitals (4s, 4p x, 4p y, 4p z, 3d z2, and 3d x2-y2 ) form six bonding and six antibonding with a 1g, e g, t 1u symmetries. The metal T 2g orbitals do Electron not have in bonding appropriate orbitals provide symmetry the - nonbonding potential energy that holds molecules together
34 Ligand field theory; Orbital Splitting and Electron Spin Strong-field ligand Ligands whose orbitals interact strongly with the metal orbitals large o Weak-field ligand. d 0 ~d 3 and d 8 ~d 10 only one electron configuration possible no difference in the net spin Strong fields lead to low-spin complexes Weak fields lead to high-spin complexes
35 Ligand field theory; Orbital Splitting and Electron Spin hat determine? epends on the relative nergies of the metal ions nd ligand orbitals and on he degree of overlap.
36 Ligand field theory; Orbital Splitting and Electron Spin Spectrochemical Series for Metal Ions Oxidation # Small size & higher charge Pt 4+ > Ir 3+ > Pd 4+ > Ru 3+ > Rh 3+ >Mo 3+ > Mn 4+ > Co 3+ > Fe 3+ > V 2+ > Fe 2+ Co 2+ > Ni 2+ > Mn 2+
37 Ligand field theory; Ligand field Stabilization Energy
38 Ligand field theory; Orbital Splitting and Electron Spin Orbital configuration of the complex is determined by o, π c, and π e In general o for 3 + ions is larger than o for 2 + ions with the same # of e -. o > π low-spin o < π high-spin For low-spin configuration Require a strong field ligand
39 Ligand field theory; Ligand field Stabilization Energy
40 Ligand field theory; Orbital Splitting and Electron Spin The position of the metal in the periodic table Second and third transition series form lowspin more easily than metals form the first transition series -The greater overlap between the larger 4d and 5d orbitals and the ligand orbitals -A decreased pairing energy due to the larger volume available for electrons
41 Ligand field theory; Pi-Bonding The reducible representation is
42 Ligand field theory; Pi-Bonding LUMO orbitals:can be used for π bonding with metal HOMO
43 Ligand field theory; Pi-Bonding metal-to-ligand π bonding or π back-bonding -Increase stability -Low-spin configuration -Result of transfer of negative charge away from the metal ion Ligand-to metal π bondin -decrease stability -high-spin configuration
44 Ligand field theory; Square planar Complexes; Sigma bonding
45 Ligand field theory; Square planar Complexes; Sigma bonding ll e - from metal 16 e - 8 e -
46 Ligand field theory; Tetrahedral Complexes; Sigma bonding The reducible representation is A 1 and T 2
47 Ligand field theory; Tetrahedral Complexes; Pi bonding The reducible representation i E, T 1 and T 2
48 Angular Overlap LFT No explicit use of the energy change that results Difficult to use other than octahedral, square planar, tetrahedral. Deal with a variety of possible geometries and with a mixture of ligand. Angular Overlap Model The strength of interaction between individual ligand orbitals and metal d orbitals based on the overlap between them.
49 Angular Overlap: Sigma-Donor Interactions The strongest σ interaction There are no examples of complexes with e - in the antibonding orbitals from s and p orbitals, and these high-energy antibonding orbitals are not significant in describing the spectra of complexes. we will not consider them further.
50 Angular Overlap: Sigma-Donor Interactions
51 Angular Overlap: Sigma-Donor Interactions Stabilization is 12e σ
52 Angular Overlap: Pi-Acceptor Interactions Because of the overlap for these orbitals is smaller than the σ overlap, e π < e σ. The strongest π interaction is considered to be between a metal d xy orbitals and a ligand π* orbital.
53 Angular Overlap: Pi-Acceptor Interactions
54 Angular Overlap: Pi-Acceptor Interactions
55 Angular Overlap: Pi-Donor Interactions In general, in situations involving ligands that can behave as both π acceptors and π donors (such as CO, CN - ), the π acceptor nature predominates.
56 Angular Overlap: Pi-Donor Interactions
57 Angular Overlap: Pi-Acceptor Interactions
58 Angular Overlap: Types of the ligands and the spectrochemical series Spectrochemical Series for Ligands CO > CN - > PPh 3 > NO 2- > phen > bipy > en NH 3 > py > CH 3 CN > NCS - > H 2 O > C 2 O 4 2- OH - > RCO 2- > F - > N 3- > NO 3- > Cl - > SCN - S 2- > Br - > I - σ donor on π acceptor (strong field ligand) π donor(weak field ligand)
59 Angular Overlap: Magnitudes of e σ eπ and Metal and ligand
60 Angular Overlap: Magnitudes of e σ eπ and Angular overlap parameters derived from electronic spectra e σ is always larger than e π. overlap isoelectronic The magnitudes of both the σ and π parameters with size and electronegativity of the halide ions. overlap
61 Angular Overlap: Magnitudes of e σ eπ and Can describe the electronic energy of complexes with different shapes or with combinations of different liagnds. The magnitude of o Magnetic properties and visible spectrum.
62 Angular Overlap: The Jahn-Teller Effect There cannot be unequal occupation of orbitals with identical orbitals. To avoid such unequal occupation, the molecule distorts so that these orbitals no longer degenerate. In other words, if the ground electron configuration of a nonlinear complex is orbitally degenerate, the complex will distort to remove the degeneracy and achieve a lower energy.
63 Angular Overlap: The Jahn-Teller Effect
64 Angular Overlap: Four- and Six-Coordinate Preference Angular overlap calculations Only σ bonding is considered Low-spin square planar Large # of bonds formed in the octahedral complexes.
65 Angular Overlap: Four- and Six-Coordinate Preference
66 Angular Overlap: Four- and Six-Coordinate Preference How accurate are these predictions? Their success is variable, because of there are other differences between metals and between ligands. In addition, bond lengths for the same ligand-metal pair depend on the geometry of the complex. The interactions of the s and p orbitals. The formation enthalpy for complexes also becomes more negative with increasing atomic number and increasing ionization energy. By careful selection of ligands, many of the transition metal ions can form compounds with geometries other than octahedral.
67 Angular Overlap: Other shapes Strength of σ interaction /4 9/8 9/8 0 0
68 Angular Overlap: Other shapes Trigonal-bipyramidal ML 5 (D 3h ) σ-donor only
Covalent Bonding & Molecular Orbital Theory
Covalent Bonding & Molecular Orbital Theory Chemistry 754 Solid State Chemistry Dr. Patrick Woodward Lecture #16 References - MO Theory Molecular orbital theory is covered in many places including most
Chapter 10 Molecular Geometry and Chemical Bonding Theory
Chem 1: Chapter 10 Page 1 Chapter 10 Molecular Geometry and Chemical Bonding Theory I) VSEPR Model Valence-Shell Electron-Pair Repulsion Model A) Model predicts Predicts electron arrangement and molecular
TRANSITION METALS AND COORDINATION CHEMISTRY
CHAPTER TWENTY-ONE TRANSITION METALS AND COORDINATION CHEMISTRY For Review 1. Chromium ([Ar]:4s 0 3d 5 ) and copper [Ar]:4s 1 3d 10 ) have electron configurations which are different from that predicted
SHAPES OF MOLECULES (VSEPR MODEL)
1 SAPES MLEULES (VSEPR MDEL) Valence Shell Electron-Pair Repulsion model - Electron pairs surrounding atom spread out as to minimize repulsion. - Electron pairs can be bonding pairs (including multiple
Chapter 9 - Covalent Bonding: Orbitals
Chapter 9 - Covalent Bonding: Orbitals 9.1 Hybridization and the Localized Electron Model A. Hybridization 1. The mixing of two or more atomic orbitals of similar energies on the same atom to produce new
Name: Class: Date: 3) The bond angles marked a, b, and c in the molecule below are about,, and, respectively.
Name: Class: Date: Unit 9 Practice Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The basis of the VSEPR model of molecular bonding is. A) regions of
AP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts
AP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts 8.1 Types of Chemical Bonds A. Ionic Bonding 1. Electrons are transferred 2. Metals react with nonmetals 3. Ions paired have lower energy
Bonding Models. Bonding Models (Lewis) Bonding Models (Lewis) Resonance Structures. Section 2 (Chapter 3, M&T) Chemical Bonding
Bonding Models Section (Chapter, M&T) Chemical Bonding We will look at three models of bonding: Lewis model Valence Bond model M theory Bonding Models (Lewis) Bonding Models (Lewis) Lewis model of bonding
A pure covalent bond is an equal sharing of shared electron pair(s) in a bond. A polar covalent bond is an unequal sharing.
CHAPTER EIGHT BNDING: GENERAL CNCEPT or Review 1. Electronegativity is the ability of an atom in a molecule to attract electrons to itself. Electronegativity is a bonding term. Electron affinity is the
UV-Vis spectroscopy Basic theory
UV-Vis spectroscopy Basic theory Dr. Davide Ferri Empa, Lab. for Solid State Chemistry and Catalysis 044 823 46 09 davide.ferri@empa.ch Importance of UV-Vis in catalysis IR Raman NMR XAFS UV-Vis EPR 0
Theme 3: Bonding and Molecular Structure. (Chapter 8)
Theme 3: Bonding and Molecular Structure. (Chapter 8) End of Chapter questions: 5, 7, 9, 12, 15, 18, 23, 27, 28, 32, 33, 39, 43, 46, 67, 77 Chemical reaction valence electrons of atoms rearranged (lost,
Hybrid Molecular Orbitals
Hybrid Molecular Orbitals Last time you learned how to construct molecule orbital diagrams for simple molecules based on the symmetry of the atomic orbitals. Molecular orbitals extend over the entire molecule
CHEM 1211K Test IV. MULTIPLE CHOICE (3 points each)
CEM 1211K Test IV MULTIPLE COICE (3 points each) 1) ow many single covalent bonds must a silicon atom form to have a complete octet in its valence shell? A) 4 B) 3 C) 1 D) 2 E) 0 2) What is the maximum
Chemistry Workbook 2: Problems For Exam 2
Chem 1A Dr. White Updated /5/1 1 Chemistry Workbook 2: Problems For Exam 2 Section 2-1: Covalent Bonding 1. On a potential energy diagram, the most stable state has the highest/lowest potential energy.
Topics. Coordination Compounds. Lewis Acid/Base Adducts Definitions complexes, ligands, coordination number
Topics Introduction Molecular Structure and Bonding Molecular Symmetry Coordination Compounds Electronic Spectra of Complexes Reactions of Metal Complexes Organometallic Chemistry Coordination Compounds
18 electron rule : How to count electrons
18 electron rule : How to count electrons The rule states that thermodynamically stable transition metal organometallic compounds are formed when the sum of the metal d electrons and the electrons conventionally
The Lewis structure is a model that gives a description of where the atoms, charges, bonds, and lone pairs of electrons, may be found.
CEM110 Week 12 Notes (Chemical Bonding) Page 1 of 8 To help understand molecules (or radicals or ions), VSEPR shapes, and properties (such as polarity and bond length), we will draw the Lewis (or electron
Molecular Geometry and VSEPR We gratefully acknowledge Portland Community College for the use of this experiment.
Molecular and VSEPR We gratefully acknowledge Portland ommunity ollege for the use of this experiment. Objectives To construct molecular models for covalently bonded atoms in molecules and polyatomic ions
Chapter 9. Chemical reactivity of molecules depends on the nature of the bonds between the atoms as well on its 3D structure
Chapter 9 Molecular Geometry & Bonding Theories I) Molecular Geometry (Shapes) Chemical reactivity of molecules depends on the nature of the bonds between the atoms as well on its 3D structure Molecular
AP* Bonding & Molecular Structure Free Response Questions page 1
AP* Bonding & Molecular Structure ree Response Questions page 1 (1) AP is a registered trademark of the ollege Board. The ollege Board was not involved in the production of and does not endorse this product.
Question 4.2: Write Lewis dot symbols for atoms of the following elements: Mg, Na, B, O, N, Br.
Question 4.1: Explain the formation of a chemical bond. A chemical bond is defined as an attractive force that holds the constituents (atoms, ions etc.) together in a chemical species. Various theories
Chapter10 Tro. 4. Based on the Lewis structure, the number of electron domains in the valence shell of the CO molecule is A) 1 B) 2 C) 3 D) 4 E) 5
Chapter10 Tro 1. All of the geometries listed below are examples of the five basic geometries for molecules with more than 3 atoms except A) planar triangular B) octahedral C) tetrahedral D) trihedral
Chemistry 105, Chapter 7 Exercises
hemistry 15, hapter 7 Exercises Types of Bonds 1. Using the periodic table classify the bonds in the following compounds as ionic or covalent. If covalent, classify the bond as polar or not. Mg2 4 i2 a(3)2
CHEM 340 CHEMICAL BONDING - in General Lect-07 IONIC COVALENT METAL COVALENT NETWORK
CHEM 340 CHEMICAL BONDING in General Lect07 BONDING between atoms classified as belonging to one of the following types: IONIC COVALENT METAL COVALENT NETWORK or each bond type, the valence shell electrons
5. Which of the following is the correct Lewis structure for SOCl 2
Unit C Practice Problems Chapter 8 1. Draw the lewis structures for the following molecules: a. BeF 2 b. SO 3 c. CNS 1- d. NO 2. The correct Lewis symbol for ground state carbon is a) b) c) d) e) 3. Which
Molecular Geometry and Chemical Bonding Theory
Chapter 10 Molecular Geometry and Chemical Bonding Theory Concept Check 10.1 An atom in a molecule is surrounded by four pairs of electrons, one lone pair and three bonding pairs. Describe how the four
CHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH
1. Is H 3 O + polar or non-polar? (1 point) a) Polar b) Non-polar CHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH 2. The bond strength is considerably greater in HF than in the other three hydrogen halides
Covalent Bonding and Molecular Geometry
Name Section # Date of Experiment Covalent Bonding and Molecular Geometry When atoms combine to form molecules (this also includes complex ions) by forming covalent bonds, the relative positions of the
CHAPTER 6 REVIEW. Chemical Bonding. Answer the following questions in the space provided.
Name Date lass APTER 6 REVIEW hemical Bonding SETIN 1 SRT ANSWER Answer the following questions in the space provided. 1. a A chemical bond between atoms results from the attraction between the valence
CHAPTER 5: MOLECULAR ORBITALS
Chapter 5 Molecular Orbitals 5 CHAPTER 5: MOLECULAR ORBITALS 5. There are three possible bonding interactions: p z d z p y d yz p x d xz 5. a. Li has a bond order of. (two electrons in a bonding orbital;
3) Of the following, radiation has the shortest wavelength. A) X-ray B) radio C) microwave D) ultraviolet E) infrared Answer: A
1) Which one of the following is correct? A) ν + λ = c B) ν λ = c C) ν = cλ D) λ = c ν E) νλ = c Answer: E 2) The wavelength of light emitted from a traffic light having a frequency of 5.75 1014 Hz is.
7.14 Linear triatomic: A-----B-----C. Bond angles = 180 degrees. Trigonal planar: Bond angles = 120 degrees. B < B A B = 120
APTER SEVEN Molecular Geometry 7.13 Molecular geometry may be defined as the three-dimensional arrangement of atoms in a molecule. The study of molecular geometry is important in that a molecule s geometry
LCAO-MO Correlation Diagrams
LCAO-MO Correlation Diagrams (Linear Combination of Atomic Orbitals to yield Molecular Orbitals) For (Second Row) Homonuclear Diatomic Molecules (X 2 ) - the following LCAO-MO s are generated: LCAO MO
Summer Holidays Questions
Summer Holidays Questions Chapter 1 1) Barium hydroxide reacts with hydrochloric acid. The initial concentration of the 1 st solution its 0.1M and the volume is 100ml. The initial concentration of the
EXPERIMENT 17 : Lewis Dot Structure / VSEPR Theory
EXPERIMENT 17 : Lewis Dot Structure / VSEPR Theory Materials: Molecular Model Kit INTRODUCTION Although it has recently become possible to image molecules and even atoms using a high-resolution microscope,
Geometries and Valence Bond Theory Worksheet
Geometries and Valence Bond Theory Worksheet Also do Chapter 10 textbook problems: 33, 35, 47, 49, 51, 55, 57, 61, 63, 67, 83, 87. 1. Fill in the tables below for each of the species shown. a) CCl 2 2
Vocabulary: VSEPR. 3 domains on central atom. 2 domains on central atom. 3 domains on central atom NOTE: Valence Shell Electron Pair Repulsion Theory
Vocabulary: VSEPR Valence Shell Electron Pair Repulsion Theory domain = any electron pair, or any double or triple bond is considered one domain. lone pair = non-bonding pair = unshared pair = any electron
C has 4 valence electrons, O has six electrons. The total number of electrons is 4 + 2(6) = 16.
129 Lewis Structures G. N. Lewis hypothesized that electron pair bonds between unlike elements in the second (and sometimes the third) row occurred in a way that electrons were shared such that each element
AP CHEMISTRY 2009 SCORING GUIDELINES
AP CHEMISTRY 2009 SCORING GUIDELINES Question 6 (8 points) Answer the following questions related to sulfur and one of its compounds. (a) Consider the two chemical species S and S 2. (i) Write the electron
A. Essentially the order of Pt II affinity for these ligands (their Lewis basicity or nucleophilicity)
(c) Entering Ligand Effects 284 The second order rate constant k 2 in square planar complexes in the rate law below that we just discussed is strongly dependent on the nature of Y, the entering ligand
Symmetry and group theory
Symmetry and group theory or How to Describe the Shape of a Molecule with two or three letters Natural symmetry in plants Symmetry in animals 1 Symmetry in the human body The platonic solids Symmetry in
EXPERIMENT 9 Dot Structures and Geometries of Molecules
EXPERIMENT 9 Dot Structures and Geometries of Molecules INTRODUCTION Lewis dot structures are our first tier in drawing molecules and representing bonds between the atoms. The method was first published
CHEMISTRY BONDING REVIEW
Answer the following questions. CHEMISTRY BONDING REVIEW 1. What are the three kinds of bonds which can form between atoms? The three types of Bonds are Covalent, Ionic and Metallic. Name Date Block 2.
Chapter 7. Comparing Ionic and Covalent Bonds. Ionic Bonds. Types of Bonds. Quick Review of Bond Types. Covalent Bonds
Comparing Ionic and Covalent Bonds Chapter 7 Covalent Bonds and Molecular Structure Intermolecular forces (much weaker than bonds) must be broken Ionic bonds must be broken 1 Ionic Bonds Covalent Bonds
ACE PRACTICE TEST Chapter 8, Quiz 3
ACE PRACTICE TEST Chapter 8, Quiz 3 1. Using bond energies, calculate the heat in kj for the following reaction: CH 4 + 4 F 2 CF 4 + 4 HF. Use the following bond energies: CH = 414 kj/mol, F 2 = 155 kj/mol,
Laboratory 11: Molecular Compounds and Lewis Structures
Introduction Laboratory 11: Molecular Compounds and Lewis Structures Molecular compounds are formed by sharing electrons between non-metal atoms. A useful theory for understanding the formation of molecular
Self Assessment_Ochem I
UTID: 2013 Objective Test Section Identify the choice that best completes the statement or answers the question. There is only one correct answer; please carefully bubble your choice on the scantron sheet.
2. Atoms with very similar electronegativity values are expected to form
AP hemistry Practice Test #6 hapter 8 and 9 1. Which of the following statements is incorrect? a. Ionic bonding results from the transfer of electrons from one atom to another. b. Dipole moments result
Use the Force! Noncovalent Molecular Forces
Use the Force! Noncovalent Molecular Forces Not quite the type of Force we re talking about Before we talk about noncovalent molecular forces, let s talk very briefly about covalent bonds. The Illustrated
Chapter 2 Polar Covalent Bonds; Acids and Bases
John E. McMurry http://www.cengage.com/chemistry/mcmurry Chapter 2 Polar Covalent Bonds; Acids and Bases Javier E. Horta, M.D., Ph.D. University of Massachusetts Lowell Polar Covalent Bonds: Electronegativity
CHAPTER 6 Chemical Bonding
CHAPTER 6 Chemical Bonding SECTION 1 Introduction to Chemical Bonding OBJECTIVES 1. Define Chemical bond. 2. Explain why most atoms form chemical bonds. 3. Describe ionic and covalent bonding.. 4. Explain
Unit 3: Quantum Theory, Periodicity and Chemical Bonding
Selected Honour Chemistry Assignment Answers pg. 9 Unit 3: Quantum Theory, Periodicity and Chemical Bonding Chapter 7: The Electronic Structure of Atoms (pg. 240 to 241) 48. The shape of an s-orbital is
5. Structure, Geometry, and Polarity of Molecules
5. Structure, Geometry, and Polarity of Molecules What you will accomplish in this experiment This experiment will give you an opportunity to draw Lewis structures of covalent compounds, then use those
We emphasize Lewis electron dot structures because of their usefulness in explaining structure of covalent molecules, especially organic molecules.
Chapter 10 Bonding: Lewis electron dot structures and more Bonding is the essence of chemistry! Not just physics! Chemical bonds are the forces that hold atoms together in molecules, in ionic compounds,
ch9 and 10 practice test
1. Which of the following covalent bonds is the most polar (highest percent ionic character)? A. Al I B. Si I C. Al Cl D. Si Cl E. Si P 2. What is the hybridization of the central atom in ClO 3? A. sp
H 2O gas: molecules are very far apart
Non-Covalent Molecular Forces 2/27/06 3/1/06 How does this reaction occur: H 2 O (liquid) H 2 O (gas)? Add energy H 2O gas: molecules are very far apart H 2O liquid: bonding between molecules Use heat
Bonding & Molecular Shape Ron Robertson
Bonding & Molecular Shape Ron Robertson r2 n:\files\courses\1110-20\2010 possible slides for web\00bondingtrans.doc The Nature of Bonding Types 1. Ionic 2. Covalent 3. Metallic 4. Coordinate covalent Driving
Elements in the periodic table are indicated by SYMBOLS. To the left of the symbol we find the atomic mass (A) at the upper corner, and the atomic num
. ATOMIC STRUCTURE FUNDAMENTALS LEARNING OBJECTIVES To review the basics concepts of atomic structure that have direct relevance to the fundamental concepts of organic chemistry. This material is essential
Magnetic susceptibility measurements of transition metal containing compounds
Magnetic susceptibility measurements of transition metal containing compounds Introduction: Measurements of magnetic properties have been used to characterize a wide range of systems from oxygen, metallic
Visualizing Molecular Orbitals: A MacSpartan Pro Experience
Introduction Name(s) Visualizing Molecular Orbitals: A MacSpartan Pro Experience In class we have discussed Lewis structures, resonance, VSEPR, hybridization and molecular orbitals. These concepts are
Chapter 8 Concepts of Chemical Bonding
Chapter 8 Concepts of Chemical Bonding Chemical Bonds Three types: Ionic Electrostatic attraction between ions Covalent Sharing of electrons Metallic Metal atoms bonded to several other atoms Ionic Bonding
3/5/2014. iclicker Participation Question: A. MgS < AlP < NaCl B. MgS < NaCl < AlP C. NaCl < AlP < MgS D. NaCl < MgS < AlP
Today: Ionic Bonding vs. Covalent Bonding Strengths of Covalent Bonds: Bond Energy Diagrams Bond Polarities: Nonpolar Covalent vs. Polar Covalent vs. Ionic Electronegativity Differences Dipole Moments
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
CHEM 101/105 BONDING (continued) Lect-16
CHEM 0/05 BONDING (continued) Lect6 A Second covalent bonding theory, MOLECULAR ORBITAL THEORY accounts for covalent bonding by... before looking at MO, return for a moment to the individual unbonded atom
INFRARED SPECTROSCOPY (IR)
INFRARED SPECTROSCOPY (IR) Theory and Interpretation of IR spectra ASSIGNED READINGS Introduction to technique 25 (p. 833-834 in lab textbook) Uses of the Infrared Spectrum (p. 847-853) Look over pages
Molecular Structures. Chapter 9 Molecular Structures. Using Molecular Models. Using Molecular Models. C 2 H 6 O structural isomers: .. H C C O..
John W. Moore onrad L. Stanitski Peter. Jurs http://academic.cengage.com/chemistry/moore hapter 9 Molecular Structures Stephen. oster Mississippi State University Molecular Structures 2 6 structural isomers:
Health Science Chemistry I CHEM-1180 Experiment No. 15 Molecular Models (Revised 05/22/2015)
(Revised 05/22/2015) Introduction In the early 1900s, the chemist G. N. Lewis proposed that bonds between atoms consist of two electrons apiece and that most atoms are able to accommodate eight electrons
Since we will be dealing with aqueous acid and base solution, first we must examine the behavior of water.
Acids and Bases Know the definition of Arrhenius, Bronsted-Lowry, and Lewis acid and base. Autoionization of Water Since we will be dealing with aqueous acid and base solution, first we must examine the
Molecular Geometry and Hybrid Orbitals. Molecular Geometry
Molecular Geometry and ybrid Orbitals + -- bond angle 90 o Molecular Geometry Why Should I are bout Molecular Geometry? Molecular geometry (shape) influences... 3 Physical properties: 3 3 3 3 3 Pentane
: : Solutions to Additional Bonding Problems
Solutions to Additional Bonding Problems 1 1. For the following examples, the valence electron count is placed in parentheses after the empirical formula and only the resonance structures that satisfy
Chapter 1 Structure and Bonding. Modified by Dr. Daniela Radu
John E. McMurry www.cengage.com/chemistry/mcmurry Chapter 1 Structure and Bonding Modified by Dr. Daniela Radu What is Organic Chemistry? Living things are made of organic chemicals Proteins that make
Paper 1 (7405/1): Inorganic and Physical Chemistry Mark scheme
AQA Qualifications A-level Chemistry Paper (7405/): Inorganic and Physical Chemistry Mark scheme 7405 Specimen paper Version 0.5 MARK SCHEME A-level Chemistry Specimen paper 0. This question is marked
Ultraviolet Spectroscopy
Ultraviolet Spectroscopy The wavelength of UV and visible light are substantially shorter than the wavelength of infrared radiation. The UV spectrum ranges from 100 to 400 nm. A UV-Vis spectrophotometer
Why? Intermolecular Forces. Intermolecular Forces. Chapter 12 IM Forces and Liquids. Covalent Bonding Forces for Comparison of Magnitude
1 Why? Chapter 1 Intermolecular Forces and Liquids Why is water usually a liquid and not a gas? Why does liquid water boil at such a high temperature for such a small molecule? Why does ice float on water?
Lesson 3. Chemical Bonding. Molecular Orbital Theory
Lesson 3 Chemical Bonding Molecular Orbital Theory 1 Why Do Bonds Form? An energy diagram shows that a bond forms between two atoms if the overall energy of the system is lowered when the two atoms approach
Chapter 2 Polar Covalent Bonds: Acids and Bases
John E. McMurry www.cengage.com/chemistry/mcmurry Chapter 2 Polar Covalent Bonds: Acids and Bases Modified by Dr. Daniela R. Radu Why This Chapter? Description of basic ways chemists account for chemical
Chapter 2 The Chemical Context of Life
Chapter 2 The Chemical Context of Life Multiple-Choice Questions 1) About 25 of the 92 natural elements are known to be essential to life. Which four of these 25 elements make up approximately 96% of living
Exercises Topic 2: Molecules
hemistry for Biomedical Engineering. Exercises Topic 2 Authors: ors: Juan Baselga & María González Exercises Topic 2: Molecules 1. Using hybridization concepts and VSEPR model describe the molecular geometry
Chemistry 151 Final Exam
Chemistry 151 Final Exam Name: SSN: Exam Rules & Guidelines Show your work. No credit will be given for an answer unless your work is shown. Indicate your answer with a box or a circle. All paperwork must
RESONANCE, USING CURVED ARROWS AND ACID-BASE REACTIONS
RESONANCE, USING CURVED ARROWS AND ACID-BASE REACTIONS A STUDENT SHOULD BE ABLE TO: 1. Properly use curved arrows to draw resonance structures: the tail and the head of every arrow must be drawn in exactly
Chapter 2: The Chemical Context of Life
Chapter 2: The Chemical Context of Life Name Period This chapter covers the basics that you may have learned in your chemistry class. Whether your teacher goes over this chapter, or assigns it for you
Chapter 24 Chemistry of Coordination Compounds
Chapter 24 Chemistry of Coordination Compounds Transition metal compounds (demo samples) variable oxidation number colored unusual composition often contain covalent compounds bonded to the metal hydrates
AP* Atomic Structure & Periodicity Free Response Questions KEY page 1
AP* Atomic Structure & Periodicity ree Response Questions KEY page 1 1980 a) points 1s s p 6 3s 3p 6 4s 3d 10 4p 3 b) points for the two electrons in the 4s: 4, 0, 0, +1/ and 4, 0, 0, - 1/ for the three
Electron Counting in Organometallic Chemistry
Electron Counting in Organometallic Chemistry 1. The 18-Electron Rule; definition & rationalisation The constitution and structure of main group element complexes can be predicted and rationalised by a
Acids and Bases: A Brief Review
Acids and : A Brief Review Acids: taste sour and cause dyes to change color. : taste bitter and feel soapy. Arrhenius: acids increase [H ] bases increase [OH ] in solution. Arrhenius: acid base salt water.
A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together is called a(n)
Chemistry I ATOMIC BONDING PRACTICE QUIZ Mr. Scott Select the best answer. 1) A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together is
DCI for Electronegativity. Data Table:
DCI for Electronegativity Data Table: Substance Ionic/covalent EN value EN Value EN NaCl ionic (Na) 0.9 (Cl) 3.0 2.1 KBr (K) 0.8 (Br) 2.8 MgO (Mg) 1.2 (O) 3.5 HCl (H) 2.1 (Cl) 3.0 HF (H) 2.1 (F) 4.0 Cl
Answer Key, Problem Set 11
Chemistry 122 Mines, Spring 2010 Answer Key, Problem Set 11 1. Write the electron configuration for each of the following atoms and ions (use the noble gas abbreviation): (a) Mn: [Ar] 4s 2 3d 5 (Note:
CH101/105, GENERAL CHEMISTRY LABORATORY
CH101/105, GENERAL CHEMITRY LABORATORY LABORATORY LECTURE 5 EXPERIMENT 5: LEWI TRUCTURE AND MOLECULAR HAPE Lecture topics I. LEWI TRUCTURE a) calculation of the valence electron numbers; b) choosing the
Ionic Bonding Pauling s Rules and the Bond Valence Method
Ionic Bonding Pauling s Rules and the Bond Valence Method Chemistry 754 Solid State Chemistry Dr. Patrick Woodward Lecture #14 Pauling Rules for Ionic Structures Linus Pauling,, J. Amer. Chem. Soc. 51,,
PRACTICE PROBLEMS, CHAPTERS 1-3
PRATIE PRBLEMS, APTERS 1-3 (overed from h. 3: Alkane and Alkyl alide nomenclature only) 1. The atomic number of boron is 5. The correct electronic configuration of boron is: A. 1s 2 2s 3 B. 1s 2 2p 3.
The Synthesis of trans-dichlorobis(ethylenediamine)cobalt(iii) Chloride
CHEM 122L General Chemistry Laboratory Revision 2.0 The Synthesis of trans-dichlorobis(ethylenediamine)cobalt(iii) Chloride To learn about Coordination Compounds and Complex Ions. To learn about Isomerism.
Which substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s)
BONDING MIDTERM REVIEW 7546-1 - Page 1 1) Which substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s) 2) The bond between hydrogen and oxygen in
CHEMISTRY 1710 - Practice Exam #5 - SPRING 2014 (KATZ)
CHEMISTRY 1710 - Practice Exam #5 - SPRING 2014 (KATZ) Name: Score: This is a multiple choice exam. Choose the BEST answer from the choices which are given and write the letter for your choice in the space
Proton Nuclear Magnetic Resonance ( 1 H-NMR) Spectroscopy
Proton Nuclear Magnetic Resonance ( 1 H-NMR) Spectroscopy Theory behind NMR: In the late 1940 s, physical chemists originally developed NMR spectroscopy to study different properties of atomic nuclei,
Electronegativity and Polarity MAIN Idea A chemical bond s character is related to each atom s
Section 8.5 Objectives Describe how electronegativity is used to determine bond type. Compare and contrast polar and nonpolar covalent bonds and polar and nonpolar molecules. Generalize about the characteristics
CHAPTER 12: CHEMICAL BONDING
CHAPTER 12: CHEMICAL BONDING Active Learning Questions: 3-9, 11-19, 21-22 End-of-Chapter Problems: 1-36, 41-59, 60(a,b), 61(b,d), 62(a,b), 64-77, 79-89, 92-101, 106-109, 112, 115-119 An American chemist
3.091 Fall Term 2002 Homework #4 Solutions
3.091 all Term 2002 omework #4 olutions 5-5. We imply that sodium is a better electron donor than lithium. Evidence for this can be found in the lower value of AVEE which for these two elements is equivalent
Lecture 22 The Acid-Base Character of Oxides and Hydroxides in Aqueous Solution
2P32 Principles of Inorganic Chemistry Dr. M. Pilkington Lecture 22 The Acid-Base Character of Oxides and Hydroxides in Aqueous Solution Oxides; acidic, basic, amphoteric Classification of oxides - oxide
Atomic Structure Ron Robertson
Atomic Structure Ron Robertson r2 n:\files\courses\1110-20\2010 possible slides for web\atomicstructuretrans.doc I. What is Light? Debate in 1600's: Since waves or particles can transfer energy, what is