Molecular Modeling of Covalent Compounds
|
|
- Baldric Hudson
- 7 years ago
- Views:
Transcription
1 CHEM 121L General Chemistry Laboratory Revision 1.5 Molecular Modeling of Covalent Compounds To learn about the geometry of covalently bound molecules. To learn about VSEPR theory. To learn about Isomerism. To learn about Molecular Polarity. In this laboratory exercise we will build models of some simple molecules that are in accordance with the geometries suggested by the Valence Shell Electron Pair Repulsion (VSEPR) Theory. We will note the influence Lone Pairs of electrons and Multiple Bonds have upon the geometry of these molecules. We will also note the overall polarity of the molecules modeled. VSEPR theory provides a simple extension of Lewis bonding theory; predicting molecular geometries for covalently bound molecules, polyatomic ions and networks. This theory assumes the shape of a molecule is influenced by the number of electron pairs about each central atom in the molecule. Although largely accurate in predicting molecular geometries, it is a bit superficial and must be supplemented with Valence Bond Theory in order to provide a more accurate picture of the orbital structure of said electron pairs. In any case, both VSEPR and Valence Bond Theory are being supplanted by the more robust, although more computationally demanding, Molecular Orbital Theory to describe both the electronic structure and geometry of simple molecules. The basic idea underlying VESPR is that each valence shell electron pair around an atom will mutually repel all the other valence shell electron pairs about that atom. Therefore, the electron pairs and covalent bonds will find a geometric arrangement which minimizes these repulsions. These arrangements, for the common cases, are: Num. Electron Domains Geometry Angle Between Domains 2 Linear 180 o 3 Trigonal Planar 120 o 4 Tetrahedral o 5 Trigonal Bipyramidal 120 o (equatorial) & 90 o (axial) 6 Octahedral 90 o This Electronic Geometry defines the type of Molecular Geometry possible. For each type of Electronic Geometry, there is a subset of Molecular Geometries which depend on the number of atoms covalently bound to the central atom, as well as the number of Lone Pairs about that atom. As an example, each of the following molecules, CH 4, NH 3, H 2 O and HF, is tetrahedral in its Electronic Geometry; each has four electron domains about the central atom. However, they each exhibit different Molecular Geometries. CH 4 is tetrahedral but NH 3 is trigonal pyramidal;
2 P a g e 2 CH 4 has 4 bonding atoms about the C atom, whereas NH 3 has only 3, with the fourth electron pair being a Lone Pair. When determining Molecular Geometries, Lone Pairs of electrons are not considered. The Lone Pairs influence the Molecular Geometry, but do not participate in it. A list of possible Molecular Geometries for 2-6 electron pairs about a central atom E is provided below:
3 P a g e 3 Several points need to be considered when identifying Molecular Geometries: i) Double and triple bonds count as a single VSEPR domain. This is because a second covalent bond between two atoms shortens and strengthens the overall bonding, but it does not change the geometry of the bonding. For the series CH 3 CH 3, CH 2 CH 2, CHCH, the Carbon-Carbon bond length gets progressively shorter, simply bringing the Carbon atoms closer together. In the example below, the central Carbon atom has three VSEPR domains and so is trigonal planar in its geometry.
4 P a g e 4 ii) Lone Pair Lone Pair interactions are more unfavorable than Lone Pair Bonding Pair interactions. Likewise, these last are more unfavorable than Bonding Pair - Bonding Pair interactions. So, Xenon Tetrafluoride (XeF 4 ), which has 4 Bonding Pairs and 2 Lone Pairs about the central Xenon atom, adopts a Square Planar molecular geometry. iii) Molecules with multiple central atoms will have multiple geometries. So, CH 3 SH has two central atoms; the carbon and sulfur. Thus, it has two specified geometries. It is tetrahedral about the carbon (4 Bonding Pairs) and bent about the sulfur (2 Bonding Pairs and 2 Lone Pairs). iv) The bond angles in a molecule are determined, primarily, by the Electronic Geometry. So, both CH 4 and NH 3 have approximate bond angles of o. It is true, the Lone Pair in NH 3 requires more space than the Bonding Pairs; the measured bond angle in NH 3 is 107 o. However, as a first approximation, we can take the bond angles to be those specified by the electron domains listed above.
5 P a g e 5 Thus, the process for determining the Molecular Geometry of a covalently bound compound is: Write the Lewis Structure for the molecule. Determine the Electronic Geometry of the molecule. Determine the Molecular Geometry. An example is in order. Consider the compound Nitrogen Trichloride, NCl 3. A valid Lewis Structure for this compound is: The central Nitrogen atom has four electron domains; three Bonding Pairs and one Lone Pair. This gives rise to a Tetrahedral Electronic Geometry. Four electron domains with one Lone Pair, as can be seen in the Table above, gives rise to a Trigonal Pyramidal Molecular Geometry. Finally, the molecular geometry plays an important role in determining if the molecule is Polar. For instance, both BF 3 and GeF 2 have very polar bonds. (This is because Fluorine is very Electronegative and the metalloids B and Ge are somewhat Electropositive.) However, BF 3, because of its symmetric Trigonal Planar structure, is non-polar, whereas GeF 2, adopting an asymmetric Bent structure, is polar.
6 P a g e 6 In this laboratory exercise, we will build models of molecules for several compounds. This will help us visualize the three dimensional structure of these molecules. It should be emphasized, chemical reactions occur in three dimensions and so inherently depend on the three dimensional structure of the reactants. This is especially important in biochemistry, where enzymes are specifically designed for chemical substrates with a particular three dimensional structure.
7 P a g e 7 Pre-Lab Questions 1. Draw Lewis Structures for each of the molecules and ions in the Procedure section of the lab. You may skip the Lewis Structure for Morphine. (If you do this now, your time spent in the lab will be much shorter.)
8 P a g e 8 Procedure We will use two different model kits for the following exercises. The Prentice-Hall Molecular Model Set for General and Organic Chemistry will be used for simpler cases involving atoms that adopt Tetrahedral, Trigonal Planar and Linear Electronic Geometries. It will also be used for molecules that contain multiple geometric centers. For molecules containing Trigonal Bipyramidal and Octahedral centers, the Indigo Instruments Model Kit will be used. For the following cases, check-out and use the Prentice-Hall Molecular Model Set for General and Organic Chemistry. Simple Molecules and Ions For each case below: i) Draw the Lewis Structure of the molecule/ion. ii) Use the molecular modeling kits provided to build a model of the molecule/ion. Use the generally accepted color codes for given elements, as listed on the model kit. Each model must be checked by the instructor. iii) Sketch the Electronic Geometry about the central atom. iv) Sketch the Molecular Geometry about the central atom. v) Label the geometry and bond angles. vi) Determine if the molecule is Polar. (You do not need to do this for the Polyatomic Ions.) Note: Your sketches must use the wedge and dash notation used in the sketches above. SiH 4, PH 3, H 2 S, HCl COCl 2 (Phosgene), HCN (Hydrogen Cyanide) CO 2, CO, NO 2, NO NH + - 4, ClO 4 Molecules with Multiple Centers For each case below, where the molecule contains multiple centers: i) Draw the Lewis Structure of the molecule. ii) Use the molecular modeling kits provided to build a model of the molecule. Use the
9 P a g e 9 generally accepted color codes for given elements, as listed on the model kit. Each model must be checked by the instructor. iii) Sketch the Molecular Geometry about each central atom. iv) Label the geometry and bond angles. Note: Your sketches must use the wedge and dash notation used in the sketches above. CH 3 OH, CH 3 NH 2 CH 3 CH 3, CH 2 CH 2, CHCH Penicillin (R-C 9 H 11 N 2 O 4 S) i) This structure is as pictured below. Each point in the picture is a Carbon atom. Bonds to Carbon not explicitly shown are to Hydrogen. ii) In this structure, "R" represents a variable group which is different from one type of Penicillin to another. For our purposes, we can take R = Hydrogen.
10 P a g e 10 Isomers Isomers are substances that have the same chemical formula, but are different compounds; i.e., each has its own set of physical and chemical properties. An example is the isomerism exhibited by compounds with the chemical formula C 4 H 8. Two isomers with this formula are: 1-Butene H 3 C-CH 2 -CH=CH 2 2-Butene H 3 C-CH=CH-CH 3 In the case of 1-Butene, the Carbon-Carbon double bond is between Carbons 1 and 2. For 2-Butene it is between Carbons 2 and 3. Each of these compounds has distinctly different Boiling Points, Melting Points, Densities, etc. This type of Isomerism is a Structural Isomerism; the bonding between the atoms is different from one isomer to another. Other types of isomerism will be covered in your Organic and Inorganic chemistry courses. Build models of the following two structural isomers. Sketch each structure. (Use the standard wedge and dash notation in each sketch.) CH 3 CH 2 OH (Grain Alcohol) CH 3 OCH 3 (Dimethyl Ether) For the following cases, check-out and use the Indigo Instruments Model Kit. (Parts are contained in a Red Cup.) Expanded Octets For each case below: i) Draw the Lewis Structure of the molecule/ion. ii) Use the molecular modeling kits provided to build a model of the molecule/ion. Use the generally accepted color codes for given elements, as listed on the model kit. Each model must be checked by the instructor. iv) Sketch the Molecular Geometry about the central atom. Note: Your sketches must use the wedge and dash notation used in the sketches above. PCl 5 SF 4 Build both possibilities. Explicitly include the Lone Pairs. Which Geometry is better?
11 P a g e 11 XeF 4 Build both possibilities. Explicitly include the Lone Pairs. Which Geometry is better? Resonance Structures In many cases, Lewis Structures do not adequately describe the bonding between atoms in a molecule. This is frequently due to delocalization of the bonding. And, in many cases, this delocalized bonding is due to overlap of unhybridized atomic p-orbitals. The bonding in these cases is usually represented by the use of Resonance Structures. The Indigo Instruments Model Kit contains lobes that can be used to represent p- orbitals. So, for a molecule like Ethene (CH 2 =CH 2 ), where each Carbon is sp 2 hybridized, the unhybridized p-orbitals overlap and form a -bond between the Carbon atoms. CH 2 =CH 2 Build a model of this molecule that explicitly shows the p-orbitals used to construct the -bond. O 3 First draw the two resonance structures for this molecule. Then build a model of this molecule that explicitly shows the p-orbitals involved in the delocalized bonding.
12 P a g e 12 Post Lab Questions 1. Part of the reasoning that led van't Hoff and Le Bel to propose a tetrahedral shape for Methane, CH 4, was based on the number of compounds that are theoretically possible for substituted Methanes; that is, compounds in which one or more hydrogens have been replaced by some other group. For example, only one compound of the type CH 2 X 2 has ever been found. Is this consistent with a tetrahedral shape? With a square planar shape? Provide an explanation for each answer using appropriate diagrams. 2. For H 2 O, the H-O-H bond angle is o and the measure dipole moment is 1.85 Debye. What is the magnitude of the O-H bond dipole moment for H 2 O? Estimate the bond angle in H 2 S given that the H-S bond dipole moment is 0.67 Debye and the resultant molecular dipole moment is 0.95 Debye. 3. There has been some back-and-forth concerning the correct Lewis Structure for the Sulfate Ion; SO At one extreme, the Lewis Structure of SO 4 2- can be represented using a strict adherence to the octet rule. At the other extreme, Sulfur s valence shell is expanded to allow for a minimization of atomic Formal Charges. Draw the Lewis Structures for Sulfate using both of these extremes. Include Formal Charges for each atom. What geometry is predicted for each of these structures? Some interesting computational results are presented in Common Textbook and Teaching Misrepresentations of Lewis Structures by Lalia Suidan, Jay K. Badenhoop, Eric. D. Glendening, and Frank Weinhold Journal of Chemical Education 72 (1995) 583.
13 P a g e 13 Addendum The Polarity of Water Molecules The shape of the molecules which comprise a substance have a profound effect on the chemical and physical properties of that substance. Certain chemical reactions can depend as heavily on the three dimensional structure of the molecules involved as on the nature of the chemical bonds which must break and reform during the reaction. Additionally, the boiling point, melting point, density, and other physical properties of the substance will depend on the three dimensional structure of the substance's molecules. As a case in point, consider the structure of Water molecules. As we have seen, the molecules which comprise a sample of water have a Bent geometry. This bent structure imparts a strong polarity on the molecule because the polar O-H bonds: contribute to an overall dipole moment for the molecule. These molecular dipole moments, representing a separation of positive and negative electric charge, can be oriented along the field lines emanating from a charged object, such as a charged rod. The resulting Polarization will cause the water sample will be attracted to the charged object.
14 P a g e 14 There are a few subtleties here,however. First, the orientation of the water molecules due to the presence of the charged object is not complete. Overall, only a few percent of the total number of molecules in the sample will be oriented along the electric field. The polarization is more a skewing of the molecule's orientation along the electric field lines. Second, the polarization of a sample is not limited to those substances with polar molecules. The electron clouds of molecules can polarize when in the presence of an external electric field. This electron cloud polarization generates an induced dipole moment within the molecule. This induced dipole can give rise to Polarization of the sample. However, this polarization is typically much weaker than the polarization that occurs in a sample comprised of polar molecules. In this exercise, we will observe the polarization of Water by bringing a charged object near a narrow stream of water. This will be compared with the rather weak polarization of the nonpolar compound Cyclhexane, C 6 H 12. Procedure 1. A pair of burets, one filled with Water and the other filled with Cyclohexane (C 6 H 12 ), are available. Water is composed of polar molecules, while Cyclohexane molecules are nonpolar Arrange these so they drain into a large beaker. 2. Allow a stream of Water to flow from the buret into the beaker. 3. Charge a glass rod by briskly rubbing it in your hair or on a woolen garment. This will Charge the rod by Friction; electric charge is transferred from your hair/garment to the rod. (Does it matter what charge is imparted to the rod?) 4. Bring the rod near the stream of Water. Observe the results. 5. Do the same with a buret filled with the non-polar liquid Cyclohexane. 6. Refill the burets with the liquid from the beakers when you are done.
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,
More informationEXPERIMENT 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
More informationChemical 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
More informationChapter 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
More informationMolecular 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
More informationChapter 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
More informationLaboratory 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
More informationChemistry 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.
More informationHealth 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
More informationChapter10 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
More information5. 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
More informationVocabulary: 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
More informationTheme 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,
More information2. 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
More informationch9 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
More informationChapter 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
More informationBonding 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
More information5. 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
More informationStructures 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
More informationSurvival Organic Chemistry Part I: Molecular Models
Survival Organic Chemistry Part I: Molecular Models The goal in this laboratory experience is to get you so you can easily and quickly move between empirical formulas, molecular formulas, condensed formulas,
More informationMolecular 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
More informationSHAPES 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
More informationName: 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
More informationCHEMISTRY 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.
More informationVSEPR 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
More informationA 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
More information7.14 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
More informationAP 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
More informationChemistry 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
More informationQuestion 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
More informationEXPERIMENT 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
More informationSOME TOUGH COLLEGE PROBLEMS! .. : 4. How many electrons should be shown in the Lewis dot structure for carbon monoxide? N O O
SME TUGH CLLEGE PRBLEMS! LEWIS DT STRUCTURES 1. An acceptable Lewis dot structure for 2 is (A) (B) (C) 2. Which molecule contains one unshared pair of valence electrons? (A) H 2 (B) H 3 (C) CH 4 acl 3.
More informationMolecular 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:
More information: : 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
More informationChapter 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
More informationACE 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,
More informationCHAPTER 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
More informationBonding & 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
More informationExercises 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
More informationCHAPTER 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
More informationC 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
More informationMolecular Geometry & Polarity
Name AP Chemistry Molecular Geometry & Polarity Molecular Geometry A key to understanding the wide range of physical and chemical properties of substances is recognizing that atoms combine with other atoms
More informationCHAPTER 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
More informationValence 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
More informationGeometries 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
More informationCH101/105, 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
More informationCovalent 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
More informationCHEMISTRY 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
More informationChapter 4 Lecture Notes
Chapter 4 Lecture Notes Chapter 4 Educational Goals 1. Given the formula of a molecule, the student will be able to draw the line-bond (Lewis) structure. 2. Understand and construct condensed structural
More informationSelf 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.
More informationCHAPTER 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
More informationThe 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.
More informationWe 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,
More informationA 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
More informationMolecular Structure and Polarity
OpenStax-CNX module: m51053 1 Molecular Structure and Polarity OpenStax College This work is produced by OpenStax-CNX and licensed under the Creative Commons Attribution License 4.0 By the end of this
More informationSample Exercise 8.1 Magnitudes of Lattice Energies
Sample Exercise 8.1 Magnitudes of Lattice Energies Without consulting Table 8.2, arrange the ionic compounds NaF, CsI, and CaO in order of increasing lattice energy. Analyze From the formulas for three
More informationA 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
More informationSample Exercise 8.1 Magnitudes of Lattice Energies
Sample Exercise 8.1 Magnitudes of Lattice Energies Without consulting Table 8.2, arrange the following ionic compounds in order of increasing lattice energy: NaF, CsI, and CaO. Analyze: From the formulas
More informationCHEMISTRY 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)
More informationCHAPTER 10 THE SHAPES OF MOLECULES
ATER 10 TE AE MLEULE EMIAL ETI BED READIG RBLEM B10.1 lan: Examine the Lewis structure, noting the number of regions of electron density around the carbon and nitrogen atoms in the two resonance structures.
More informationPOLARITY 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
More informationChem 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
More informationChapter 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
More informationCovalent Bonding & Molecular Compounds Multiple Choice Review PSI Chemistry
Covalent Bonding & Molecular Compounds Multiple Choice Review PSI Chemistry Name 1) Which pair of elements is most apt to form a molecular compound with each other? A) aluminum, oxygen B) magnesium, iodine
More informationSection Activity #1: Fill out the following table for biology s most common elements assuming that each atom is neutrally charged.
LS1a Fall 2014 Section Week #1 I. Valence Electrons and Bonding The number of valence (outer shell) electrons in an atom determines how many bonds it can form. Knowing the number of valence electrons present
More informationPOLAR COVALENT BONDS Ionic compounds form repeating. Covalent compounds form distinct. Consider adding to NaCl(s) vs. H 2 O(s):
POLAR COVALENT BONDS Ionic compounds form repeating. Covalent compounds form distinct. Consider adding to NaCl(s) vs. H 2 O(s): Sometimes when atoms of two different elements form a bond by sharing an
More information4.2. 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
More informationDCI 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
More informationCHAPTER 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
More information3) 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.
More informationUnit 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
More informationUnit 3: Quantum Theory, Periodicity and Chemical Bonding. Chapter 10: Chemical Bonding II Molecular Geometry & Intermolecular Forces
onour Chemistry Unit 3: Quantum Theory, Periodicity and Chemical Bonding Chapter 10: Chemical Bonding II Molecular Geometry & Intermolecular orces 10.1: Molecular Geometry Molecular Structure: - the three-dimensional
More informationPolarity. Andy Schweitzer
Polarity Andy Schweitzer What does it mean to be polar? A molecule is polar if it contains + and somewhere in the molecule. Remember: Protons can not move. So for a molecule to get a +/- it must somehow
More informationThe 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
More informationChapter 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
More informationAP* 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.
More informationpre -TEST Big Idea 2 Chapters 8, 9, 10
Name: AP Chemistry Period: Date: R.F. Mandes, PhD, NBCT Complete each table with the appropriate information. Compound IMF Compound IMF 1 NiCl 3 7 ClCH 2 (CH 2 ) 3 CH 3 2 Fe 8 H 2 CF 2 3 Ar 9 H 2 NCH 2
More informationMolecular 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
More information3/5/2014. 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
More informationIonic and Covalent Bonds
Ionic and Covalent Bonds Ionic Bonds Transfer of Electrons When metals bond with nonmetals, electrons are from the metal to the nonmetal The becomes a cation and the becomes an anion. The between the cation
More informationChapter 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
More informationCHEM 1301 SECOND TEST REVIEW. Covalent bonds are sharing of electrons (ALWAYS valence electrons). Use Lewis structures to show this sharing.
CEM 1301 SECOND TEST REVIEW Lewis Structures Covalent bonds are sharing of electrons (ALWAYS valence electrons). Use Lewis structures to show this sharing. Rules OCTET RULE an atom would like to have 8
More informationChapter 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
More information7) How many electrons are in the second energy level for an atom of N? A) 5 B) 6 C) 4 D) 8
HOMEWORK CHEM 107 Chapter 3 Compounds Putting Particles Together 3.1 Multiple-Choice 1) How many electrons are in the highest energy level of sulfur? A) 2 B) 4 C) 6 D) 8 2) An atom of phosphorous has how
More informationPRACTICE 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.
More informationBonding Practice Problems
NAME 1. When compared to H 2 S, H 2 O has a higher 8. Given the Lewis electron-dot diagram: boiling point because H 2 O contains stronger metallic bonds covalent bonds ionic bonds hydrogen bonds 2. Which
More informationChapter 8: Covalent Bonding and Molecular Structure
hapter 8 ovalent Bonding and Molecular Structure 8-1 hapter 8: ovalent Bonding and Molecular Structure hapter 8 8.1 Interactions Between Particles: oulomb s Law 8.2 ovalent Bonding Basics 8.3 Lewis Structures
More informationMolecular 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
More informationStart: 26e Used: 6e Step 4. Place the remaining valence electrons as lone pairs on the surrounding and central atoms.
Section 4.1: Types of Chemical Bonds Tutorial 1 Practice, page 200 1. (a) Lewis structure for NBr 3 : Step 1. The central atom for nitrogen tribromide is bromine. 1 N atom: 1(5e ) = 5e 3 Br atoms: 3(7e
More informationCHEM 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
More informationChapter 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
More informationExam. 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
More informationChem 112 Intermolecular Forces Chang From the book (10, 12, 14, 16, 18, 20,84,92,94,102,104, 108, 112, 114, 118 and 134)
Chem 112 Intermolecular Forces Chang From the book (10, 12, 14, 16, 18, 20,84,92,94,102,104, 108, 112, 114, 118 and 134) 1. Helium atoms do not combine to form He 2 molecules, What is the strongest attractive
More informationWhich 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
More informationIntroduction to Chemistry. Course Description
CHM 1025 & CHM 1025L Introduction to Chemistry Course Description CHM 1025 Introduction to Chemistry (3) P CHM 1025L Introduction to Chemistry Laboratory (1) P This introductory course is intended to introduce
More informationThe 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
More informationOCTET RULE Generally atoms prefer electron configurations with 8 valence electrons. - Filled s and p subshells
TYPES EMIAL BDIG 1 Ionic Bonding - Bond between ions whose charges attract each other - ne atom gives electrons and one atom takes electrons. Example a + l - ionic bond ovalent Bonding - two atoms each
More informationCHEM 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
More informationCHEMISTRY 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
More informationName: Date: Period: Presentation #4. Covalent compounds continued practice with drawing them. Modeling covalent compounds in 3D
Homework Activities Name: Date: Period: This week we will practice creating covalent compounds through drawings and 3D models. We will also look at polar and non-polar molecules to see how their structures
More information