3. (5%) Use the molecular orbital energy-level diagram for O 2 to show that the following Lewis structure corresponds to an excited state:
|
|
|
- Jonathan Bailey
- 7 years ago
- Views:
Transcription
1 University Chemistry Quiz /11/6 1. (10%) Explain why the bond order of N 2 is greater than that of N 2, but the bond order of 2 is less than that of 2. In forming the N 2 from N 2, an electron is removed from the sigma bonding molecular orbital. Consequently, the bond order decreases to 2.5 from 3.0. In forming the 2 ion from 2, an electron is removed from the pi antibonding molecular orbital. Consequently, the bond order increases to 2.5 from (10%) Draw three resonance structures for the chlorate ion, - 3. Show formal charges. Strategy: We follow the procedure for drawing Lewis structures outlined in Section 3.4 of the text. After we complete the Lewis structure, we draw the resonance structures. Solution: Following the procedure in Section 3.4 of the text, we come up with the following Lewis structure for 3. We can draw two more equivalent Lewis structures with the double bond between and a different oxygen atom. The resonance structures with formal charges are as follows: 3. (5%) Use the molecular orbital energy-level diagram for 2 to show that the following Lewis structure corresponds to an excited state: The Lewis structure shows 4 pairs of electrons on the two oxygen atoms. From Table 3.4 of the text, we see that these 8 valence electrons are placed in the σ 2px, p 2py, p 2pz, p 2py, and p 2pz orbitals. For all the electrons to be paired, energy is
2 needed to flip the spin in one of the antibonding molecular orbitals ( π 2πy or π 2πz ). According to und s rule, this arrangement is less stable than the ground-state configuration shown in Table 3.4, and hence the Lewis structure shown actually corresponds to an excited state of the oxygen molecule. 4. (10%) A reasonable Lewis structure for carbon monoxide (C) is :C : Sketch the orbital overlap in the VB description corresponding to this Lewis structure. In this description, where do the long pair reside? The bonding orbitals, depicted below, are due to the overlap of the p-orbitals. The lone pairs of electrons remain in the 2s orbitals on each atoms (not shown in the illustration below). 5. (5%) Four atoms are arbitrarily labeled D, E, F and G. Their electronegativities are as follows: D = 3.8, E = 3.3, F = 2.8 and G = 1.3. If the atoms of these elements form the molecules DE, DG, EG and DF, how would you arrange these molecules in order of increasing covalent bond character? The smaller the electronegativity difference between the atoms, the more covalent character the bonds have. Remember that the difference in electronegativity (Dc) is always positive. Below the bonds are listed in order of increasing covalent character: D G < E G < D F < D E χ= 2.5 χ= 2.0 χ= 1.0 χ= 0.5
3 6. (10%) The dipole moment of F is 1.92 D. Given that the F bond length is 91.7 pm, calculate the separated charge q, assuming the point charge model. (1D =3.336 x C m) For the point charge model, the dipole moment is equal to the size of the charge times the distance between the charges (Equation 4.1). ence, the charge is equal to the dipole moment divided by the distance between the charges. For this problem we also have to know that 1 Debye equals x C m and that a pm equals m. 30 µ x 1 m q = = = 6.98x10 12 r 91.7 m Which is equal to 44% the charge of an electron. So, of the two bonding electrons, 22% stays on the fluorine giving the fluorine atom a negative charge, 22% is missing from the hydrogen, giving it a positive charge. 7. (10%) In 1998 scientists using a special type of electron microscope were able to measure the force needed to break a single chemical bond. If 2.0 x 10-9 N was needed to break a C Si bond, estimate the bond dissociation energy in kj mol -1. Assume that the bond had to be stretched by a distance of 2 Å (2 x m) before it was broken. Work done = force distance = ( N) ( m) = N m = J to break one bond Expressing the bond enthalpy in kj mol -1 : J 1 kj bonds = 1 bond 1000 J 1 mol kjol 8. (10%) Compare the M theory description for the 2 molecule given by Equation
4 3.10 with the VB theory treatment given in Equation 3.1. Under what condition do they become identical? (Equation 3.1: ψ VB = N[ φa, (1) φb, (2) φb, (1) φa, (2)] 1 Equation 3.10: ψ s 1) s (2) = [ φ (1) φ (1) ] [ φ (2) φ (2)] ( A, B, A, B, 1 ) 2 2 s The wavefunction determined from molecular orbital (M) theory contains the same terms as the wavefunction determined from valence bond (VB) theory. The wavefunction determined from M theory also contains terms corresponding to both electrons being on the same atom. If the likelihood of the two electrons being on the same atom is negligible (such as for a homonuclear diatomic molecule), then the wavefunctions from the two theories are identical. 9. (5%) The species 3 is the simplest polyatomic ion. The geometry of the ion is that of an equilateral triangle. Draw three resonance structures to represent the ion. 10. (5%) Which of the following molecules has the shortest nitrogen to-nitrogen bond: N 2 4, N 2, N 2, and N 2 4. Explain. nly N 2 has a triple bond. Therefore, it has the shortest bond length. 11. (10%) Write three resonance structures for (a) the cyanate ion (NC - ) and (b) the isocyanate ion (CN - ). In each case, rank the resonance structures in order of increasing importance. The resonance structures are: (a) N C N C 2 N C (b) 2 3 C N C N C N In both cases, the most likely structure is on the left and the least likely structure is on the right.
5 12. (5%) Explain in molecular orbital terms the changes in internuclear distance that occur as the molecular 2 is ionized first to 2 and then to 2 2. The molecular orbital electron configuration and bond order of each species is shown below bond order = 1 bond order = 1 2 bond order = 0 The internuclear distance in the 1 ion should be greater than that in the neutral hydrogen molecule. The distance in the 2 ion will be very large because there is no bond (bond order zero). 13. (5%) Which of the following species are tetrahedral? Si 4, SeF 4, XeF 4, CI 4, or Cd 2-4. Si 4, CI 4, and Cd 2-4 would all be tetrahedral.
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.
Sample 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
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
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
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
Sample 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
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
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
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
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
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 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
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
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 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.
Questions on Chapter 8 Basic Concepts of Chemical Bonding
Questions on Chapter 8 Basic Concepts of Chemical Bonding Circle the Correct Answer: 1) Which ion below has a noble gas electron configuration? A) Li 2+ B) Be 2+ C) B2+ D) C2+ E) N 2-2) Of the ions below,
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
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
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
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,
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
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
: : 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
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 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
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
Ionic 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
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
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
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
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.
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
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
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
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
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
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
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
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
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
Chapter 6 Assessment. Name: Class: Date: ID: A. Multiple Choice Identify the choice that best completes the statement or answers the question.
Name: Class: Date: ID: A Chapter 6 Assessment Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When an atom loses an electron, it forms a(n) a. anion. c.
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
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
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
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
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.
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
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
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.
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,
CHAPTER 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.
How To Write A Periodic Table
Spring 2008 hemistry 2000 Midterm #1A / 50 marks INSTRUTINS 1) Please read over the test carefully before beginning. You should have 5 pages of questions and a periodic table. 2) If you need extra space,
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
Worksheet 14 - Lewis structures. 1. Complete the Lewis dot symbols for the oxygen atoms below
Worksheet 14 - Lewis structures Determine the Lewis structure of 2 oxygen gas. 1. omplete the Lewis dot symbols for the oxygen atoms below 2. Determine the number of valence electrons available in the
List the 3 main types of subatomic particles and indicate the mass and electrical charge of each.
Basic Chemistry Why do we study chemistry in a biology course? All living organisms are composed of chemicals. To understand life, we must understand the structure, function, and properties of the chemicals
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
Bonds. Bond Length. Forces that hold groups of atoms together and make them function as a unit. Bond Energy. Chapter 8. Bonding: General Concepts
Bonds hapter 8 Bonding: General oncepts Forces that hold groups of atoms together and make them function as a unit. Bond Energy Bond Length It is the energy required to break a bond. The distance where
Molecular 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
Chapter 8 Basic Concepts of the Chemical Bonding
Chapter 8 Basic Concepts of the Chemical Bonding 1. There are paired and unpaired electrons in the Lewis symbol for a phosphorus atom. (a). 4, 2 (b). 2, 4 (c). 4, 3 (d). 2, 3 Explanation: Read the question
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
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
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
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
Formal Charges. Step 2. Assign the formal charge to each atom. Formal charge is calculated using this formula: H O H H
Formal harges Discussion: Ions bear a positive or negative charge. If the ion is polyatomic (is constructed of more than on atom), we might ask which atom(s) of the ion carry the charge? Knowledge of charge
Order of Filling Subshells
Bonding: General Concepts Ionic Bonds Sections 13.2-13.6 Covalent Bonds Section 13.7 Covalent Bond Energy & Chemical Reactions Section 13.8-13.9 Lewis Structures Sections 13.10-13.12 VSEPR Theory Section
Chapter 2 Polar Covalent Bond Covalent bond in which the electron pairs are not shared equally.
hapter 2 Polar ovalent Bond ovalent bond in which the electron pairs are not shared equally. Pure ovalent Bond (non-polar) increasing bond polarity Ionic Bond X X X Y X + Y - Electronegativity, c ability
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;
Lewis Dot Notation Ionic Bonds Covalent Bonds Polar Covalent Bonds Lewis Dot Notation Revisited Resonance
Lewis Dot Notation Ionic Bonds Covalent Bonds Polar Covalent Bonds Lewis Dot Notation Revisited Resonance Lewis Dot notation is a way of describing the outer shell (also called the valence shell) of an
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,
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
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
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
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
1.15 Bonding in Methane and Orbital Hybridization
1.15 Bonding in Methane and Orbital Hybridization Structure of Methane tetrahedral bond angles = 109.5 bond distances = 110 pm but structure seems inconsistent with electron configuration of carbon Electron
Chapter 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
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
OCTET 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
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
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
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
(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.
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 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
Section 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
Modelling Compounds. 242 MHR Unit 2 Atoms, Elements, and Compounds
6.3 Figure 6.26 To build the Michael Lee-Chin Crystal at the Royal Ontario Museum, models were used at different stages to convey different types of information. Modelling Compounds The Michael Lee-Chin
In the box below, draw the Lewis electron-dot structure for the compound formed from magnesium and oxygen. [Include any charges or partial charges.
Name: 1) Which molecule is nonpolar and has a symmetrical shape? A) NH3 B) H2O C) HCl D) CH4 7222-1 - Page 1 2) When ammonium chloride crystals are dissolved in water, the temperature of the water decreases.
SOME 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.
Resonance Structures Arrow Pushing Practice
Resonance Structures Arrow Pushing Practice The following is a collection of ions and neutral molecules for which several resonance structures can be drawn. For the ions, the charges can be delocalized
Chapter 4: Structure and Properties of Ionic and Covalent Compounds
Chapter 4: Structure and Properties of Ionic and Covalent Compounds 4.1 Chemical Bonding o Chemical Bond - the force of attraction between any two atoms in a compound. o Interactions involving valence
A PREVIEW & SUMMMARY of the 3 main types of bond:
Chemical Bonding Part 1 Covalent Bonding Types of Chemical Bonds Covalent Bonds Single Polar Double NonPolar Triple Ionic Bonds Metallic Bonds Other Bonds InterMolecular orces first A PREVIEW & SUMMMARY
CHEM 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
O P O O. This structure puts the negative charges on the more electronegative element which is preferred. Molecular Geometry: O Xe O
hemistry& 141 lark ollege Exam 4 olution 1. Draw the Lewis structures for the following molecules and ions. Include formal charges and resonance structures, where appropriate. Fill out the table for the
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
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
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
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 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
Ionization energy _decreases from the top to the bottom in a group. Electron affinity increases from the left to the right within a period.
hem 150 Answer Key roblem et 2 1. omplete the following phrases: Ionization energy _decreases from the top to the bottom in a group. Electron affinity increases from the left to the right within a period.