1.15 Bonding in Methane and Orbital Hybridization
|
|
|
- Pamela Tate
- 9 years ago
- Views:
Transcription
1 1.15 Bonding in Methane and Orbital Hybridization
2 Structure of Methane tetrahedral bond angles = bond distances = 110 pm but structure seems inconsistent with electron configuration of carbon
3 Electron configuration of carbon 2p only two unpaired electrons should form σ bonds to only two hydrogen atoms 2s bonds should be at right angles to one another
4 sp 3 Orbital Hybridization 2p Promote an electron from the 2s 2 to the 2p2 orbital 2s
5 sp 3 Orbital Hybridization 2p 2p 2s 2s
6 sp 3 Orbital Hybridization 2p Mix together (hybridize) the 2s 2 orbital and the three 2p2 orbitals 2s
7 sp 3 Orbital Hybridization 2p 2 sp 3 4 equivalent half-filled filled orbitals are consistent with four bonds and tetrahedral geometry 2s
8 Shapes of orbitals p s
9 Nodal properties of orbitals p + s +
10 Shape of sp 3 hybrid orbitals p + take the s orbital and place it on top of the p orbital s +
11 Shape of sp 3 hybrid orbitals s + p + + reinforcement of electron wave in regions where sign is the same destructive interference in regions of opposite sign
12 Shape of sp 3 hybrid orbitals sp hybrid + orbital shown is sp hybrid analogous procedure using three s orbitals and one p orbital gives sp 3 hybrid shape of sp 3 hybrid is similar
13 Shape of sp 3 hybrid orbitals sp hybrid + hybrid orbital is not symmetrical higher probability of finding an electron on one side of the nucleus than the other leads to stronger bonds
14 The C H C σ Bond in Methane In-phase overlap of a half-filled filled 1s1 orbital of hydrogen with a half-filled filled sp 3 hybrid orbital of carbon: s + H + C sp 3 gives a σ bond. H C σ H + C
15 Justification for Orbital Hybridization consistent with structure of methane allows for formation of 4 bonds rather than 2 bonds involving sp 3 hybrid orbitals are stronger than those involving s-s overlap or p-p overlap
16 1.16 sp 3 Hybridization and Bonding in Ethane
17 Structure of Ethane C 2 H 6 CH 3 CH 3 tetrahedral geometry at each carbon C H H bond distance = 110 pm C C C bond distance = 153 pm
18 The C C C σ Bond in Ethane In-phase overlap of half-filled filled sp 3 hybrid orbital of one carbon with half-filled filled sp 3 hybrid orbital of another. Overlap is along internuclear axis to give a σ bond.
19 The C C C σ Bond in Ethane In-phase overlap of half-filled filled sp 3 hybrid orbital of one carbon with half-filled filled sp 3 hybrid orbital of another. Overlap is along internuclear axis to give a σ bond.
20 1.17 sp 2 Hybridization and Bonding in Ethylene
21 Structure of Ethylene C 2 H 4 H 2 C=CH 2 planar bond angles: close to 120 bond distances: C H H = 110 pm C=C = 134 pm
22 sp 2 Orbital Hybridization 2p Promote an electron from the 2s 2 to the 2p2 orbital 2s
23 sp 2 Orbital Hybridization 2p 2p 2s 2s
24 sp 2 Orbital Hybridization 2p Mix together (hybridize) the 2s 2 orbital and two of the three 2p2 orbitals 2s
25 sp 2 Orbital Hybridization 2p 2 sp 2 3 equivalent half-filled filled sp 2 hybrid orbitals plus 1 p orbital left unhybridized 2s
26 sp 2 Orbital Hybridization p 2 of the 3 sp 2 orbitals 2 sp 2 are involved in σ bonds to hydrogens; the other is involved in a σ bond to carbon
27 sp 2 Orbital Hybridization p σ σ 2 sp 2 σ σ σ
28 π Bonding in Ethylene p 2 sp 2 the unhybridized p orbital of carbon is involved in π bonding to the other carbon
29 π Bonding in Ethylene π Bonding in Ethylene p 2 sp 2 each carbon has an unhybridized 2 p orbital axis of orbital is perpendicular to the plane of the σ bonds
30 π Bonding in Ethylene π Bonding in Ethylene p 2 sp 2 side-by-side overlap of half-filled p orbitals gives a π bond double bond in ethylene has a σ component and a π component
31 1.18 sp Hybridization and Bonding in Acetylene
32 Structure of Acetylene C 2 H 2 HC CH linear bond angles: 180 bond distances: C H H = 106 pm CC = 120 pm
33 sp Orbital Hybridization 2p Promote an electron from the 2s 2 to the 2p2 orbital 2s
34 sp Orbital Hybridization 2p 2p 2s 2s
35 sp Orbital Hybridization 2p Mix together (hybridize) the 2s 2 orbital and one of the three 2p2 orbitals 2s
36 sp Orbital Hybridization 2 p 2p 2 sp 2 equivalent half-filled filled sp hybrid orbitals plus 2 p orbitals left unhybridized 2s
37 sp Orbital Hybridization 2 p 2 sp 1 of the 2 sp orbitals is involved in a σ bond to hydrogen; the other is involved in a σ bond to carbon
38 sp Orbital Hybridization 2 p σ σ 2 sp σ
39 π Bonding in Acetylene 2 p the unhybridized p orbitals of carbon are involved in separate π bonds to the other carbon 2 sp
40 π Bonding in Acetylene π Bonding in Acetylene 2 p 2 sp one π bond involves one of the p orbitals on each carbon there is a second π bond perpendicular to this one
41 π Bonding in Acetylene π Bonding in Acetylene 2 p 2 sp
42 π Bonding in Acetylene π Bonding in Acetylene 2 p 2 sp
43 1.19 Which Theory of Chemical Bonding is Best?
44 Lewis Three Models most familiar easiest to apply Valence-Bond (Orbital Hybridization) provides more insight than Lewis model ability to connect structure and reactivity to hybridization develops with practice Molecular Orbital potentially the most powerful method but is the most abstract requires the most experience to use effectively
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
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
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
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
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
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
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
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
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.
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
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
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
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
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:
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
Chapter 1 Benzene Blues 27
hapter 1 Benzene Blues 27 The ybridization Model of Atoms in Molecules An important question facing chemists about 80 years ago, was, ow does one go from recently invented atomic orbitals to rationalizing
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,
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
Valence Bond Theory: Hybridization
Exercise 13 Page 1 Illinois Central College CEMISTRY 130 Laboratory Section: Valence Bond Theory: ybridization Name: Objectives To illustrate the distribution of electrons and rearrangement of orbitals
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
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.
CHEM 101 Exam 4. Page 1
CEM 101 Exam 4 Form 1 (White) November 30, 2001 Page 1 Section This exam consists of 8 pages. When the exam begins make sure you have one of each. Print your name at the top of each page now. Show your
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
Molecular-Orbital Theory
Molecular-Orbital Theory 1 Introduction Orbitals in molecules are not necessarily localized on atoms or between atoms as suggested in the valence bond theory. Molecular orbitals can also be formed the
CHEMISTRY 113 EXAM 4(A)
Summer 2003 1. The molecular geometry of PF 4 + ion is: A. bent B. trigonal planar C. tetrahedral D. octahedral CHEMISTRY 113 EXAM 4(A) 2. The Cl-C-Cl bond angle in CCl 2 O molecule (C is the central atom)
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.
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
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
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.
Where Is My Lone Pair?
Where Is My Lone Pair? Goal: In this tutorial we'll learn how to determine which orbital contains a lone pair. This is important for resonance, conjugation, and aromaticity. To master this subject you'll
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
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
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
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
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
Molecular Geometry and Bonding Theories
9 Molecular Geometry and Bonding Theories We saw in hapter 8 that Lewis structures help us understand the compositions of molecules and their covalent bonds. owever, Lewis structures do not show one of
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
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
VSEPR Model. The Valence-Shell Electron Pair Repulsion Model. Predicting Molecular Geometry
VSEPR Model The structure around a given atom is determined principally by minimizing electron pair repulsions. The Valence-Shell Electron Pair Repulsion Model The valence-shell electron pair repulsion
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
Molecular Orbital Theory
Molecular Orbital Theory To date, we have looked at three different theories of molecular boning. They are the VSEPR Theory (with Lewis Dot Structures), the Valence Bond Theory (with hybridization) and
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
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.
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
POLARITY AND MOLECULAR SHAPE WITH HYPERCHEM LITE
POLARITY AND MOLECULAR SHAPE WITH HYPERCHEM LITE LAB MOD4.COMP From Gannon University SIM INTRODUCTION Many physical properties of matter, such as boiling point and melting point, are the result of the
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,
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
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
Determination of Molecular Structure by MOLECULAR SPECTROSCOPY
Determination of Molecular Structure by MOLEULAR SPETROSOPY hemistry 3 B.Z. Shakhashiri Fall 29 Much of what we know about molecular structure has been learned by observing and analyzing how electromagnetic
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
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
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
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 111 Laboratory Experiment 4: Visualizing Molecular Orbitals with MacSpartan Pro (This experiment will be conducted in OR341)
Chemistry 111 Laboratory Experiment 4: Visualizing Molecular Orbitals with MacSpartan Pro (This experiment will be conducted in OR341) Introduction In class we have discussed Lewis structures, resonance,
2/10/2011. Stability of Cycloalkanes: Ring Strain. Stability of Cycloalkanes: Ring Strain. 4.3 Stability of Cycloalkanes: Ring Strain
4.3 Stability of Cycloalkanes: Ring Strain Angle strain The strain induced in a molecule when bond angles are forced to deviate from the ideal 109º tetrahedral value (Adolf von Baeyer 1885) Stability of
Structures and Properties of Substances. Introducing Valence-Shell Electron- Pair Repulsion (VSEPR) Theory
Structures and Properties of Substances Introducing Valence-Shell Electron- Pair Repulsion (VSEPR) Theory The VSEPR theory In 1957, the chemist Ronald Gillespie and Ronald Nyholm, developed a model for
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;
: : 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
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
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
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
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.
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
1: Organic Molecules and Chemical Bonding
1: Organic Molecules and Chemical Bonding Organic Molecules Chemical Bonds Organic Chemistry Bon voyage Preview Organic chemistry describes the structures, properties, preparation, and reactions of a vast
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
Chem 121 Problem Set V Lewis Structures, VSEPR and Polarity
hemistry 121 Problem set V olutions - 1 hem 121 Problem et V Lewis tructures, VEPR and Polarity AWER 1. pecies Elecronegativity difference in bond Bond Polarity Mp 3 E = 3.0-3.0 = 0 for - very weakly polar
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
(a) What is the hybridization at each carbon atom in the molecule? (b) How many σ and how many π bonds are there in the molecule?
Read Chapter 9 and complete the following problems: 1. Figure 9.15 is listed on page 361 of the textbook and shows the potential energy of two hydrogen atoms as a function of the distance between them.
9.7 MOLECULAR ORBITALS
368 CHAPTER 9 Molecular Geometry and Bonding Theories John Barbaro, Orbital Bartending, J. Chem. Educ., Vol. 71, 1994, 1012. An analogy for orbital hybridization is suggested in this short article. Robert
1.3 STRUCTURES OF COVALENT COMPOUNDS
1.3 STRUTURES OF OVALENT OMPOUNDS 13 1.9 Draw an appropriate bond dipole for the carbon magnesium bond of dimethylmagnesium. Explain your reasoning. 3 Mg 3 dimethylmagnesium 1.3 STRUTURES OF OVALENT OMPOUNDS
ORGANIC COMPOUNDS IN THREE DIMENSIONS
(adapted from Blackburn et al., Laboratory Manual to Accompany World of hemistry, 2 nd ed., (1996) Saunders ollege Publishing: Fort Worth) Purpose: To become familiar with organic molecules in three dimensions
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 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
Composition of the Atmosphere. Outline Atmospheric Composition Nitrogen and Oxygen Lightning Homework
Molecules of the Atmosphere The present atmosphere consists mainly of molecular nitrogen (N2) and molecular oxygen (O2) but it has dramatically changed in composition from the beginning of the solar system.
Polymers: Introduction
Chapter Outline: Polymer Structures Hydrocarbon and Polymer Molecules Chemistry of Polymer Molecules Molecular Weight and Shape Molecular Structure and Configurations Copolymers Polymer Crystals Optional
Molecular Models Experiment #1
Molecular Models Experiment #1 Objective: To become familiar with the 3-dimensional structure of organic molecules, especially the tetrahedral structure of alkyl carbon atoms and the planar structure of
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
4.2. Molecular Shape and Polarity. Lewis Structures for Molecules and Polyatomic Ions
Molecular Shape and Polarity 4.2 molecule is a discrete chemical entity, in which atoms are held together by the electrostatic attractions of covalent bonds. In previous chemistry courses, you used Lewis
CHAPTER 10 THE SHAPES OF MOLECULES
ATER 10 TE AE MLEULE 10.1 To be the central atom in a compound, the atom must be able to simultaneously bond to at least two other atoms. e,, and cannot serve as central atoms in a Lewis structure. elium
Carbon-Carbon bonds: Hybridization
Carbon-Carbon bonds: Hybridization Abstract: Gina 05/05/11 Molecular binding behavior has a large inuence on the structure of a material and their properties. As a exclusion, carbon bind themself not in
Symmetric Stretch: allows molecule to move through space
BACKGROUND INFORMATION Infrared Spectroscopy Before introducing the subject of IR spectroscopy, we must first review some aspects of the electromagnetic spectrum. The electromagnetic spectrum is composed
Chapter 6 An Overview of Organic Reactions
John E. McMurry www.cengage.com/chemistry/mcmurry Chapter 6 An Overview of Organic Reactions Why this chapter? To understand organic and/or biochemistry, it is necessary to know: -What occurs -Why and
Chemical Bonding: Covalent Systems Written by Rebecca Sunderman, Ph.D Week 1, Winter 2012, Matter & Motion
Chemical Bonding: Covalent Systems Written by Rebecca Sunderman, Ph.D Week 1, Winter 2012, Matter & Motion A covalent bond is a bond formed due to a sharing of electrons. Lewis structures provide a description
EXPERIMENT 1: Survival Organic Chemistry: Molecular Models
EXPERIMENT 1: Survival Organic Chemistry: Molecular Models Introduction: The goal in this laboratory experience is for you to easily and quickly move between empirical formulas, molecular formulas, condensed
Kinetic Molecular Theory. Chapter 5. KE AVE and Average Velocity. Graham s Law of Effusion. Chapter 7. Real Gases
hapter 5 1. Kinetic Molecular Theory. 2. Average kinetic energy and velocity. 3. Graham s Law of Effusion. 4. Real gases and the van der Waals equation. Kinetic Molecular Theory The curves below represent
Exam. Name. 1) Chlorine (atomic number = 17) has the electronic configuration:. E) 1s22s22d103s2
Exam Name 1) Chlorine (atomic number = 17) has the electronic configuration:. A) 1s22s22p62d63s1 B) 1s22s22p63s23d5 C) 1s22s22p62d53s2 D) 1s22s22p63s23p5 E) 1s22s22d103s2 2) The complete electron configuration
MOLECULAR GEOMETRY AND BONDING THEORIES
u MOLECULAR GEOMETRY AND BONDNG TEORES TE ANTCANCER DRUG TAXOL was originally isolated from the bark of the Pacific yew tree. Chemists have now learned how to synthesize this important pharmaceutical in
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
Chapter 1 Organic Molecules and Chemical Bonding
hapter 1 Organic Molecules and hemical Bonding from Organic hemistry by Robert. Neuman, Jr. Professor of hemistry, emeritus University of alifornia, Riverside [email protected]
Chapter 5 Chemical Compounds
Chapter 5 59 Chapter 5 Chemical Compounds Review Skills 5.1 Classification of Matter 5.2 Compounds and Chemical Bonds Equal and Unequal Sharing of Electrons Transfer of Electrons Summary of Covalent and
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
The elements of the second row fulfill the octet rule by sharing eight electrons, thus acquiring the electronic configuration of neon, the noble gas o
2. VALENT BNDING, TET RULE, PLARITY, AND BASI TYPES F FRMULAS LEARNING BJETIVES To introduce the basic principles of covalent bonding, different types of molecular representations, bond polarity and its
Test Bank - Chapter 4 Multiple Choice
Test Bank - Chapter 4 The questions in the test bank cover the concepts from the lessons in Chapter 4. Select questions from any of the categories that match the content you covered with students. The
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
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
CHAPTER 1 INTRODUCTION TO ORGANIC CHEMISTRY. 1.1 Historical Background of Organic Chemistry
APTER 1 INTRDUTIN T RGANI EMISTRY 1.1 istorical Background of rganic hemistry rganic chemistry is the area of chemistry that involves the study of carbon and its compounds. arbon is now known to form a
PROTEINS THE PEPTIDE BOND. The peptide bond, shown above enclosed in the blue curves, generates the basic structural unit for proteins.
Ca 2+ The contents of this module were developed under grant award # P116B-001338 from the Fund for the Improvement of Postsecondary Education (FIPSE), United States Department of Education. However, those