; (c) [Li] [: O :] [Li]. 5a. The electrostatic potential map that corresponds to IF is the one with the most red in it. ... C C H
|
|
- Juliet Newman
- 5 years ago
- Views:
Transcription
1 hapter 10 Answers ractice Examples 1a Mg 1b n, Ge, [: Br :], K, : e: + 2 : : +, [Tl ] +, 2 : : [] 2a (a) [a] [ ] [a] ; (b) [Mg] [: :] [Mg] [: :] [Mg] b (a) [: I :] [a] [: I :] 2+ 2 ; (b) [Ba] [::] ; (c) [Li] [: :] [Li] 3a :Br Br:,, l : :I I: 3b, : I :, 4a and l bonds are the most polar of the four bonds cited 4b The bond is the most polar of the four bonds cited 5a The electrostatic potential map that corresponds to I is the one with the most red in it 5b The electrostatic potential map that corresponds to 3 is the one with the most red in it 6a (a) : : ; (b) : ; (c) : ( l :) 2 6b (a) ; (b) 7a (a) ; (b) (c) 2- opyright 2011 earson anada Inc 1
2 7b (a) B ; (b) ; (c) tructure 1 tructure 2 tructure 3 l 8a is much poorer than the one derived in Example 10-8 because it has a positive formal charge on oxygen, which is the most electronegative atom in the molecule 8b and structures because it has no formal charges The first structure is the better of the two 9a b Resonance ybrid 10a Trigonal pyramidal 10b Tetrahedral 11a Linear 11b Linear opyright 2011 earson anada Inc 2
3 12a The bond angles are ~1095º, as are the bond angles Around the there are two bonding pairs of electrons and two lone pairs, resulting in a tetrahedral electron-group geometry and a bent molecular shape around the atom, with a bond angle of slightly less than b The bond angle and the bond angles are almost the tetrahedral angle of 1095, made a bit smaller by the lone pair The angles, the angle and the angles all are very close to1095 The bond angle is made somewhat smaller than 1095 by the presence of two lone pairs on Three electron groups surround the right-hand, making its electron-group and molecular geometries trigonal planar The bond angle and the bond angles all are very close to120 13a In 2 2, the molecular geometry around each atom is bent; the bond moments do not cancel 2 2 is polar 13b l 5 as the only nonpolar species; it is a highly symmetrical molecule in which individual bond dipoles cancel out 14a rom Table 102, the length of a bond is 110 pm The length of a Br bond is not given in the table A reasonable value is the average of the and Br Br bond lengths = 195pm 14b, linear 15a 486 kj/mol 15b kj/mol 3 16a Exothermic 16b Endothermic Integrative Example A l 1655 kj/mol ince the geometries of the two molecules differ, the orbital overlap between and the surrounding l atoms will be different and therefore the l bonds in these two compounds will also be slightly different opyright 2011 earson anada Inc 3
4 B (a)ormamide: 2, bond energy = 2233 kj/mol ; ormaldoxime: 2, bond energy = 2129 kj / mol ince BE of formamide is greater than that of formaldoxime, it is more stable, and its conversion endothermic 124 o (b) 109 o Exercises 1a 1b 1c 1d 1e Kr Ge Ga As 1f Rb 3a l 3b I I 3c opyright 2011 earson anada Inc 4
5 3d 3e Te 5a s Br b 5b l 5c l B l 5d s l Li 5e 2- Li 5f I l 7 2, B 3, 6 9a as two bonds (4 electrons) to the second hydrogen, and only six electrons around the nitrogen 9b It is improperly written as a covalent Lewis structure a is actually an ionic compound 11 The answer is (c) The flaws with the other answers are as follows: (a) does not have an octet of electrons; (b) either has an octet of electrons and the total number of valence electrons is incorrect; (c) The total number of valence electrons is incorrect 2+ 13a [: l :] [a] [: l :] b [Ba] [::] opyright 2011 earson anada Inc 5
6 13c [Li] [: :] [Li] d [a] [::] 15a [Li] [: :] [Li] b [a] [::] 2+ 15c [: I :] [a] [: I :] 3+ [: l [: l :] :] [c] [: l :] 15d 17a 17b c = 0 ( 2) 1 0 (7) 0 side (2) 0 central or instance, there are cases where atoms of the same type with the same oxidation state have different formal charges, such as oxygen in ozone, 3 Another is that formal charges are used to decide between alternative Lewis structures, while oxidation state is used in balancing equations and naming compounds Also, the oxidation state in a compound is invariant, while the formal charge can change The most significant difference, though, is that whereas the oxidation state of an element in its compounds is usually not zero, its formal charge usually is 21a +1 21b -1 21c 0 21d -2 21e 0 opyright 2011 earson anada Inc 6
7 23 Based on formal charge rules alone, we must conclude that structures (A) and (B) are equally plausible 25a 25b l 25c 25d 25e 2-27a 27b c 27d opyright 2011 earson anada Inc 7
8 29 31a l 31b 33a 33b 35a Group 16, b Group 16 except oxygen, l 35c Group 17 except fluorine, opyright 2011 earson anada Inc 8
9 B 35d Group 13, 37 Br a l K 39a 4% 39b 5% 39c 60% 39d 33% 43 2 = is represented on the left, while 2 = is represented on the right 45 The molecular formulas for the compounds are 4 and i 4 The electrostatic potential map on the right is for i 4 47 [ ] - [ ] - 49 The molecule seems best represented as a resonance hybrid of (a) and (b) A 0 0 B 51a A B b opyright 2011 earson anada Inc 9
10 A B , etc 51c 0 A B d 53a 53b 53c l or l 55a Diamagnetic 55b aramagnetic 55c aramagnetic 55d Diamagnetic 55e Diamagnetic 55f aramagnetic 57 4 and Il 3 require expanded octets The others do not 59a Linear 59b Linear 59c Tetrahedral 59d Trigonal lanar 59e Bent opyright 2011 earson anada Inc 10
11 61a Bent 61b lanar 61c Linear 61d ctahedral 61e Tetrahedral a = =, linear 65b l 65c l l, trigonal planar 67a Tetrahedral 67b Tetrahedral 67c ctahedral 67d Linear 69 Tetrahedral 71 Looking at the structures, the molecular angle/shape depends on the number of valence electron pairs on the central atom The more pairs there are, the more acute the angle becomes 73a l, trigonal bipyramidal, linear 73b l, trigonal bipyramidal, t-shaped 73c l, octahedral, square planar opyright 2011 earson anada Inc 11
12 73d l, octahedral, square pyramidal 75 A m aximum of 5 atom s can be in the sam e p l a n e b c 77 are 120 a all angles ~1095 except c --, b =-, and b =- c which 109 o 109 o 120 o 109 o 120 o 79 81a Bent, polar 81b Trigonal pyramidal, polar 81c Bent, polar 81d lanar, nonpolar 81e ctahedral, nonpolar 81f Tetrahedral, polar 83 It cannot be linear 85 Br 2 possess the longest bond ingle bonds are generally longer than multiple bonds 87a 233 pm opyright 2011 earson anada Inc 12
13 87b 172 pm 87c 149 pm 87d 191 pm pm 91 Endothermic kj/mol 95a f o = 39 kj / mol o 95b =99 kj f kj/mol kj/mol Integrative and Advanced Exercises kj/mol g/mol, , either is completely linear 109, 110 Bent kj kj 120 = , l = , Br = , I = EA ~ -260 kj/mol EA for At : ~ -260 kj/mol opyright 2011 earson anada Inc 13
14 127, The bond is not linear 128a 91 kj/mol 128b E = c 23% 129a 149 D 129b Approximately c 976 elf-assessment Exercises 134 The answer is (b) 135 The answer is (c) 136 The answer is (a) 137 The answer is (a) 138 The answer is (b) 139 The answer is (c) 140a l 140b 2-140c opyright 2011 earson anada Inc 14
15 140d Br 141a Bent 141b Trigonal pyramidal 141c Tetrahedral 142 Bi 143 Bond Bond Energy (kj/mol) Bond Length (pm) = l VER theory is valence shell electron pair repulsion theory It is based on the premise that electron pairs assume orientations about an atom to minimize electron pair repulsions 145 ince there are 4 electron pairs around the central atom, the way to maximize the distance between them is to set up a tetrahedral electron group geometry owever, since there are only three atoms bonding to the central atom, the molecular geometry is trigonal pyramidal 146 A pyramidal geometry is observed when an atom has one lone pair and is bonded to three other atoms (AX 3 E) A bent geometry is observed when an atom has two lone pairs and is bonded to two other atoms (AX 2 E 2 ) or both, the bond angles will be approximately (usually smaller than) opyright 2011 earson anada Inc 15
CHAPTER 10 CHEMICAL BONDING I: BASIC CONCEPTS
APTER 10 EMIAL BDIG I: BAI EPT PRATIE EXAMPLE 1A 1B 2A 2B (E) Mg is in group 2(2A), and thus has 2 valence electrons and 2 dots in its Lewis symbol. Ge is in group 14(4A), and thus has 4 valence electrons
More informationChapter 10: Molecular Structure and Bonding Theories
hapter 10: Molecular Structure and Bonding Theories 10.1 See Section 10.1. The main premise of the VSEPR model is that the electron pairs within the valence shell of an atom repel each other and determine
More informationCHAPTER 8 BONDING: GENERAL CONCEPTS Ionic solids are held together by strong electrostatic forces that are omnidirectional.
CAPTER 8 BDIG: GEERAL CCEPTS 1 CAPTER 8 BDIG: GEERAL CCEPTS Questions 15. a. This diagram represents a polar covalent bond as in. In a polar covalent bond, there is an electron rich region (indicated by
More informationChapter 11 Answers. Practice Examples
hapter Answers Practice Examples a. There are three half-filled p orbitals on, and one half-filled 5p orbital on I. Each halffilled p orbital from will overlap with one half-filled 5p orbital of an I.
More informationChemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals
Chemical Bonding II: and ybridization of Atomic rbitals Chapter 10 Valence shell electron pair repulsion (VSEPR) model: Predict the geometry of the molecule from the electrostatic repulsions between the
More informationReview questions CHAPTER 5. Practice exercises 5.1 F F 5.3
CHAPTER 5 Practice exercises 5.1 S 5.3 5.5 Ethane is symmetrical, so does not have a dipole moment. However, ethanol has a polar H group at one end and so has a dipole moment. 5.7 xygen has the valence
More information18. Ionic solids are held together by strong electrostatic forces that are omnidirectional.
APTER 8 BDIG: GEERAL EPTS Questions 15. In 2 and, the bonding is covalent in nature, with the bonding electrons pair shared between the atoms. In 2, the two atoms are identical, so the sharing is equal;
More informationCHAPTER 8 BONDING: GENERAL CONCEPTS. Questions
APTER 8 BDIG: GEERAL EPTS Questions 15. a. This diagram represents a polar covalent bond as in. In a polar covalent bond, there is an electron rich region (indicated by the red color) and an electron poor
More informationChemical Bonding polarity & Dipole Moments. Chapter 8 Part III
Chemical Bonding polarity & Dipole Moments Chapter 8 Part III Exercise Arrange the following bonds from most to least polar: a) N F O F C F b) C F N O Si F c) Cl Cl B Cl S Cl Exercise a) C F, N F, O F
More information: Bond Order = 1.5 CHAPTER 5. Practice Questions
CAPTER 5 Practice Questions 5.1 5.3 S 5.5 Ethane is symmetrical, so does not have a dipole moment. owever, ethanol has a polar group at one end and so has a dipole moment. 5.7 xygen has the valence electron
More informationChapter 13: Phenomena
Chapter 13: Phenomena Phenomena: Scientists measured the bond angles of some common molecules. In the pictures below each line represents a bond that contains 2 electrons. If multiple lines are drawn together
More informationChemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals 1 Chemical Bonding II Molecular Geometry (10.1) Dipole Moments (10.2) Valence Bond Theory (10.3) Hybridization of Atomic Orbitals
More informationREVIEW ANSWERS EXAM 3 GENERAL CHEMISTRY I Do not hesitate to contact the instructor should you have any questions.
REVIEW ANSWERS EXAM 3 GENERAL CEMISTRY I Do not hesitate to contact the instructor should you have any questions. 1) Predict which of the following has the largest atomic radius: potassium (K) OR selenium
More information2. Write the electron configuration notation and the electron dot notation for each: (a) Ni atom (b) Ni 2+ ion (c) Ni 3+ ion
EXTRA HOMEWORK 2A 1. Predict whether each of the following types of matter will be bonded with ionic, covalent, or metallic bonds, and identify whether each will be composed of atoms, ions, or molcules
More informationChemical Bonding Chapter 8
Chemical Bonding Chapter 8 Get your Clicker, 2 magnets, goggles and your handouts Nov 15 6:15 PM Recall that: Ionic-Involves the transfer of electrons - forms between a metal and a nonmetal Covalent-Involves
More informationOrganic Chemistry. Review Information for Unit 1. VSEPR Hybrid Orbitals Polar Molecules
rganic hemistry Review Information for Unit 1 VSEPR ybrid rbitals Polar Molecules VSEPR The valence shell electron pair repulsion model (VSEPR) can be used to predict the geometry around a particular atom
More informationCHEMICAL BONDING. Chemical Bonds. Ionic Bonding. Lewis Symbols
CHEMICAL BONDING Chemical Bonds Lewis Symbols Octet Rule whenever possible, valence electrons in covalent compounds distribute so that each main-group element is surrounded by 8 electrons (except hydrogen
More informationCHAPTER EIGHT BONDING: GENERAL CONCEPTS. For Review
APTER EIGT BDIG: GEERAL EPTS 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 energy
More information2. If an atom moving 7.50 x 10 5 m/s has a wavelength of 9.53 x m associated with it, what element is it? a. Re b. Fe c. He d. Ne e.
EMTRY 103 ractice roblems #3 hapters 5 (5.45.13), 6 (6.16.2, 6.46.10), 7 (7.17.2d, 7.37.5), and 6.12 **Do the appropriate topics for your lecture** repared by Dr. Tony Jacob http://www.chem.wisc.edu/areas/clc
More informationCH 222 Chapter Seven Concept Guide
CH 222 Chapter Seven Concept Guide 1. Lewis Structures Draw the Lewis Dot Structure for cyanide ion, CN -. 1 C at 4 electrons = 4 electrons 1 N at 5 electrons = 5 electrons -1 charge = + 1 electron Total
More informationChemical Bonding II. Molecular Geometry Valence Bond Theory Phys./Chem. Properties Quantum Mechanics Sigma & Pi bonds Hybridization MO theory
Chemical Bonding II Molecular Geometry Valence Bond Theory Phys./Chem. Properties Quantum Mechanics Sigma & Pi bonds ybridization MO theory 1 Molecular Geometry 3-D arrangement of atoms 2 VSEPR Valence-shell
More informationChapters 9&10 Structure and Bonding Theories
Chapters 9&10 Structure and Bonding Theories Ionic Radii Ions, just like atoms, follow a periodic trend in their radii. The metal ions in a given period are smaller than the non-metal ions in the same
More informationQuestion 1. Electron Configurations Noble Gases and The Rule of Eight. Chapter 1. What is the electronic configuration of carbon?
hapter ~. nm Electronic Structure and Bonding Anders Jöns Ångström (84-874) Å = picometers =. nanometers = -4 microns = -8 centimeters Acids and Bases nm = Å An atom vs. a nucleus ~, x larger ucleus =
More informationH-H bond length Two e s shared by two Hs: covalent bonding. Coulomb attraction: Stronger attraction for e Fractional charge A dipole
8 Bonding: General Concepts Types of chemical bonds Covalent bonding Ex. 2 E (kj/mol) Repulsions of nucleus and e s r 0 458 0.074 r (nm) Zero interaction at long distance - bond length Two e s shared by
More informationAP Chemistry- Practice Bonding Questions for Exam
AP Chemistry- Practice Bonding Questions for Exam Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which of the following is a correct Lewis structure for
More informationWhat Do Molecules Look Like?
What Do Molecules Look Like? The Lewis Dot Structure approach provides some insight into molecular structure in terms of bonding, but what about 3D geometry? Recall that we have two types of electron pairs:
More informationForm J. Test #4 Last Name First Name Zumdahl, Chapters 8 and 9 November 23, 2004
Form J Chemistry 1441-023 Name (please print) Test #4 Last Name First Name Zumdahl, Chapters 8 and 9 November 23, 2004 Instructions: 1. This exam consists of 27 questions. 2. No scratch paper is allowed.
More informationChemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 1
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 1 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. How to get the book of
More informationA Simple Model for Chemical Bonds
A Simple Model for hemical Bonds Multiple hoice 1. Modern organic chemistry a. is the study of carbon-containing compounds. b. is the study of compounds from living organisms. c. deals exclusively with
More information1. There are paired and unpaired electrons in the Lewis symbol for a phosphorus atom. a. 4, 2 b. 2, 4 c. 2, 3 d. 4, 3 e. 0, 3
Name: Score: 0 / 42 points (0%) [2 open ended questions not graded] C8&9Practice Multiple Choice Identify the choice that best completes the statement or answers the question. 1. There are paired and unpaired
More informationFill in the chart below to determine the valence electrons of elements 3-10
Chemistry 11 Atomic Theory IV Name: Date: Block: 1. Lewis Diagrams 2. VSEPR Lewis Diagrams Lewis diagrams show the bonding between atoms of a molecule. Only the outermost electrons of an atom (called electrons)
More informationCH 222 Sample Exam Exam I Name: Lab Section:
222 Sample Exam Exam I Name: Lab Section: Part I: Multiple hoice Questions (100 Points) Use a scantron sheet for Part I. There is only one best answer for each question. 1. Which of the following statements
More information13 Bonding: General Concepts. Types of chemical bonds. Covalent bonding Ex. H 2. Repulsions of nuclei and e s. Zero interaction at long distance
13 Bonding: General Concepts Types of chemical bonds Covalent bonding Ex. 2 E (kj/mol) epulsions of nuclei and e s r 0 458 0.074 r (nm) - bond length Two e s shared by two s: covalent bonding Zero interaction
More informationVersion 188 Exam 2 mccord (51600) 1
Version 188 Exam 2 mccord (51600) 1 This print-out should have 35 questions. Multiple-choice questions may continue on the next column or page find all choices before answering. l I l l 001 3.0 points
More informationTest Review # 4. Chemistry: Form TR4.11A
Chemistry: Form TR4.11 REVIEW Name Date Period Test Review # 4 Bonding. The electrons of one atom are attracted to the protons of another. When atoms combine, there is a tug of war over the valence electrons.
More informationLewis Structures and Molecular Shapes
Lewis Structures and Molecular Shapes Drawing Lewis Structures Determine from formula if ionic or covalent Count the electrons If ionic : add valence # to charge if (-), subtract if (+) - = 7+1 electrons;
More informationVSEPR. Valence Shell Electron Pair Repulsion Theory
VSEPR Valence Shell Electron Pair Repulsion Theory Vocabulary: domain = any electron pair or bond (single, double or triple) is considered one domain. bonding pair = shared pair = any electron pair that
More informationCHEM 110 Exam 2 - Practice Test 1 - Solutions
CHEM 110 Exam 2 - Practice Test 1 - Solutions 1D 1 has a triple bond. 2 has a double bond. 3 and 4 have single bonds. The stronger the bond, the shorter the length. 2A A 1:1 ratio means there must be the
More informationSection 12: Lewis Structures
Section 12: Lewis Structures The following maps the videos in this section to the Texas Essential Knowledge and Skills for Science TAC 112.35(c). 12.01 Electronegativity Chemistry (5)(C) 12.02 Electron
More informationLewis Structure. Lewis Structures & VSEPR. Octet & Duet Rules. Steps for drawing Lewis Structures
Lewis Structure Lewis Structures & VSEPR Lewis Structures shows how the are arranged among the atoms of a molecule There are rules for Lewis Structures that are based on the formation of a Atoms want to
More informationHomework #7. Chapter 14. Covalent Bonding Orbitals
omework #7 hapter 14 ovalent Bonding rbitals 7. Both M theory and LE model use quantum mechanics to describe bonding. In the LE model, wavefunctions on one atom are mixed to form hybridized orbitals. In
More informationHour Exam 3 on Chap 6, 7, and 8 is this Friday 11/12. A practice exam is posted on the course website.
11/8/2010 1 Chem 105 Monday 11 Nov 2010 Bond length qualitative Polarity Polarity and geometry Bond energy our Exam 3 on Chap 6, 7, and 8 is this riday 11/12. A practice exam is posted on the course website.
More informationChemical Bonding AP Chemistry Ms. Grobsky
Chemical Bonding AP Chemistry Ms. Grobsky What Determines the Type of Bonding in Any Substance? Why do Atoms Bond? The key to answering the first question are found in the electronic structure of the atoms
More informationLecture 17 - Covalent Bonding. Lecture 17 - VSEPR and Molecular Shape. Lecture 17 - Introduction. Lecture 17 - VSEPR and Molecular Shape
Chem 103, Section F0F Unit VI - Compounds Part II: Covalent Compounds Lecture 17 Using the Valence-Shell Electron-Pair Repulsion (VSEPR) Theory to predict molecular shapes Molecular shape and polarity
More informationValence Bond Theory - Description
Bonding and Molecular Structure - PART 2 - Valence Bond Theory and Hybridization 1. Understand and be able to describe the Valence Bond Theory description of covalent bond formation. 2. Understand and
More informationREVIEW: VALENCE ELECTRONS CHEMICAL BONDS: LEWIS SYMBOLS: CHEMICAL BONDING. What are valence electrons?
REVIEW: VALENCE ELECTRONS 13 CHEMICAL BONDING What are valence electrons? Which groups on the periodic table readily give up electrons? What group readily accepts electrons? CHEMICAL BONDS: What are chemical
More informationLewis Structure and Electron Dot Models
Lewis Structure and Electron Dot Models The Lewis Structure is a method of displaying the electrons present in any given atom or compound. Steps: 1. Make a skeleton structure 2. Count all e- available
More informationExperiment #2. Lewis Structures
Experiment #2. Lewis Structures A Lewis structure shows how the valence electrons are arranged and indicates the bonding between atoms in a molecule. We represent the elements by their symbols. The shared
More informationName AP CHEM / / Chapter 8 Outline Bonding: General Concepts
Name AP CHEM / / Chapter 8 Outline Bonding: General Concepts Types of Chemical Bonds Information about the strength of a bonding interaction is obtained by measuring the bond energy, which is the energy
More informationName Unit Three MC Practice March 15, 2017
Unit Three: Bonding & Molecular Geometry Name Unit Three MC Practice March 15, 2017 1. What is the hybridization of the oxygen atom in water? a) sp b) sp 2 c) sp 3 d) It is not hybridized 2. When a double
More informationMolecular Geometry and intermolecular forces. Unit 4 Chapter 9 and 11.2
1 Molecular Geometry and intermolecular forces Unit 4 Chapter 9 and 11.2 2 Unit 4.1 Chapter 9.1-9.3 3 Review of bonding Ionic compound (metal/nonmetal) creates a lattice Formula doesn t tell the exact
More informationChapter 10 Molecular Geometry and Chemical Bonding Theory. Copyright Cengage Learning. All rights reserved. 10 1
Chapter 10 Molecular Geometry and Chemical Bonding Theory Copyright Cengage Learning. All rights reserved. 10 1 Molecular geometry is the general shape of a molecule, as determined by the relative positions
More informationChemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Valence shell electron
More informationBonding: Part Two. Three types of bonds: Ionic Bond. transfer valence e - Metallic bond. (NaCl) (Fe) mobile valence e - Covalent bond
Bonding: Part Two Three types of bonds: Ionic Bond transfer valence e - Metallic bond mobile valence e - Covalent bond (NaCl) (Fe) shared valence e - (H 2 O) 1 Single Covalent Bond H + H H H H-atoms H
More informationGeneral and Inorganic Chemistry I.
General and Inorganic Chemistry I. Lecture 1 István Szalai Eötvös University István Szalai (Eötvös University) Lecture 1 1 / 29 Outline István Szalai (Eötvös University) Lecture 1 2 / 29 Lewis Formulas
More informationBonding: Part Two. Three types of bonds: Ionic Bond. transfer valence e - Metallic bond. (NaCl) (Fe) mobile valence e - Covalent bond
Bonding: Part Two Three types of bonds: Ionic Bond transfer valence e - Metallic bond mobile valence e - Covalent bond (NaCl) (Fe) shared valence e - (H 2 O) 1 Single Covalent Bond H + H H H H-atoms H
More informationFor more info visit Chemical bond is the attractive force which holds various constituents together in a molecule.
Chemical bond:- Chemical bond is the attractive force which holds various constituents together in a molecule. There are three types of chemical bonds: Ionic Bond, Covalent Bond, Coordinate Bond. Octet
More informationCh 13: Covalent Bonding
Ch 13: Covalent Bonding Section 13: Valence-Shell Electron-Pair Repulsion 1. Recall the rules for drawing Lewis dot structures 2. Remember the special situations: - Resonance structures - ormal charges
More informationChapter 10: Chemical Bonding II: Molecular Shapes; VSEPR, Valence Bond and Molecular Orbital Theories
C h e m i s t r y 1 A : C h a p t e r 1 0 P a g e 1 Chapter 10: Chemical Bonding II: Molecular Shapes; VSEPR, Valence Bond and Molecular Orbital Theories Homework: Read Chapter 10: Work out sample/practice
More informationMolecular Geometry and Chemical Bonding Theory
Molecular Geometry and Chemical Bonding Theory The Valence -Shell Electron -Pair Repulsion (VSEPR) Model predicts the shapes of the molecules and ions by assuming that the valence shell electron pairs
More informationChemistry 121: Topic 4 - Chemical Bonding Topic 4: Chemical Bonding
Topic 4: Chemical Bonding 4.0 Ionic and covalent bonds; Properties of covalent and ionic compounds 4.1 Lewis structures, the octet rule. 4.2 Molecular geometry: the VSEPR approach. Molecular polarity.
More informationA DOT STRUCTURE FOR A LARGER MOLECULE ETHANOL! Count valence electrons
212 A DOT STRUCTURE FOR A LARGER MOLECULE Count valence electrons Pick central atom and draw skeletal structure - central atom is usually the one that needs to gain the most electrons! - skeletal structure
More informationExample: Write the Lewis structure of XeF 4. Example: Write the Lewis structure of I 3-. Example: Select the favored resonance structure of the PO 4
Expanded valence shells (extended octets) more than 8e - around a central atom Extended octets are formed only by atoms with vacant d-orbitals in the valence shell (p-elements from the third or later periods)
More informationChapters 8 and 9. Octet Rule Breakers Shapes
Chapters 8 and 9 Octet Rule Breakers Shapes Bond Energies Bond Energy (review): The energy needed to break one mole of covalent bonds in the gas phase Breaking bonds consumes energy; forming bonds releases
More informationChapter 6 Chemical Bonding
Chapter 6 Chemical Bonding Section 6-1 Introduction to Chemical Bonding Chemical Bonds Valence electrons are attracted to other atoms, and that determines the kind of chemical bonding that occurs between
More informationCHAPTER TEN MOLECULAR GEOMETRY MOLECULAR GEOMETRY V S E P R CHEMICAL BONDING II: MOLECULAR GEOMETRY AND HYBRIDIZATION OF ATOMIC ORBITALS
CHAPTER TEN CHEMICAL BONDING II: AND HYBRIDIZATION O ATOMIC ORBITALS V S E P R VSEPR Theory In VSEPR theory, multiple bonds behave like a single electron pair Valence shell electron pair repulsion (VSEPR)
More informationCHEM PRACTICE EXAM IV CLASS - SPRING 2017 ANSWER KEY
CHEM 1031 - PRACTICE EXAM IV CLASS - SPRING 2017 ANSWER KEY 1. When Group 1A (except for H) and Group 17 (7A) elements react with each other, they are most likely to form: A. Covalent or ionic bonds B.
More informationChapter 9: Chemical Bonding I: Lewis Theory. Lewis Theory: An Overview
Chapter 9: Chemical Bonding I: Lewis Theory Dr. Chris Kozak Memorial University of ewfoundland, Canada Lewis Theory: An verview Valence e - play a fundamental role in chemical bonding. e - transfer leads
More informationm measured m if 100%ionic
μ = q r %ionic character = 1 Debye = 3.34 x 10 30 C m m measured m if 100%ionic 100% Scoring: Six points each for questions 1 through 23; two points each for questions 24 through 32. Directions: n the
More informationValence Shell Electron Pair Repulsion Model
Activity 22 Valence hell Electron Pair Repulsion Model Why? Molecules adopt a shape that minimizes their energy. In many cases it is possible to predict the geometry of a molecule simply by considering
More informationChapter 9 Molecular Geometry and Bonding Theories
Lecture Presentation Chapter 9 Geometry James F. Kirby Quinnipiac University Hamden, CT Shapes Lewis Structures show bonding and lone pairs, but do not denote shape. However, we use Lewis Structures to
More informationChapter 6 PRETEST: Chemical Bonding
Chapter 6 PRETEST: Chemical In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1.The charge on an ion is a. always positive.
More informationName. CHM 115 EXAM #2 Practice KEY. a. N Cl b. N F c. F F d. I I e. N Br. a. K b. Be c. O d. Al e. S
Name CHM 115 EXAM #2 Practice KEY Circle the correct answer. (numbers 1-8, 2.5 points each) 1. Which of the following bonds should be the most polar? a. N Cl b. N F c. F F d. I I e. N Br 2. Choose the
More informationCHAPTER 9 COVALENT BONDING: ORBITALS. Questions
APTER 9 VALET BDIG: RBITALS Questions 11. In hybrid orbital theory, some or all of the valence atomic orbitals of the central atom in a molecule are mixed together to form hybrid orbitals; these hybrid
More informationChapter 9. Chemical Bonding II: Molecular Geometry and Bonding Theories
Chapter 9 Chemical Bonding II: Molecular Geometry and Bonding Theories Topics Molecular Geometry Molecular Geometry and Polarity Valence Bond Theory Hybridization of Atomic Orbitals Hybridization in Molecules
More informationLewis Theory of Shapes and Polarities of Molecules
Lewis Theory of Shapes and Polarities of Molecules Sulfanilamide Lewis Structures and the Real 3D-Shape of Molecules Molecular Shape or Geometry The way in which atoms of a molecule are arranged in space
More informationUnit 6: Molecular Geometry
Unit 6: Molecular Geometry Molecular Geometry [6-5] the polarity of each bond, along with the geometry of the molecule determines Molecular Polarity. To predict the geometries of more complicated molecules,
More information1. What is the phenomenon that occurs when certain metals emit electrons when illuminated by particular wavelengths of light? a.
CHEMISTRY 123-07 Midterm #3 solution key December 02, 2010 Statistics: Average: 77 p (77%); Highest: 100 p (100%); Lowest: 33 p (33%) Number of students performing at or above average: 54 (52%) Number
More informationBonding/Lewis Dots Lecture Page 1 of 12 Date. Bonding. What is Coulomb's Law? Energy Profile: Covalent Bonds. Electronegativity and Linus Pauling
Bonding/Lewis Dots Lecture Page 1 of 12 Date Bonding What is Coulomb's Law? Energy Profile: Covalent Bonds Electronegativity and Linus Pauling 2.1 H 1.0 Li 0.9 Na 0.8 K 0.8 Rb 0.7 Cs 0.7 Fr 1.5 Be 1.2
More informationCh 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules
Fructose Water Ch 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules Carbon Dioxide Ammonia Title and Highlight TN Ch 10.1 Topic: EQ: Right Side NOTES
More informationMolecular Structures. Using Molecular Models. Using Molecular Models. Predicting Molecular Shapes: VSEPR. Predicting Molecular Shapes: VSEPR
Molecular Structures Two 2 6 structural isomers: hapter 9: Molecular Structures ethanol dimethyl ether m.p./ -114.1-141.5 b.p./ 78.3-24.8 Molecular shape is important! Small structural changes cause large
More informationChapter 10 Shapes of Molecules. Dr. Sapna Gupta
Chapter 10 Shapes of Molecules Dr. Sapna Gupta Shapes of Molecules - Importance All molecules have a 3D orientations; even the diatomic ones because atoms have a volume. In case of tri atomic or polyatomic
More informationChapter 7 Chemical Bonding and Molecular Structure
Chapter 7 Chemical Bonding and Molecular Structure Three Types of Chemical Bonding (1) Ionic: formed by electron transfer (2) Covalent: formed by electron sharing (3) Metallic: attraction between metal
More information4/25/2017. VSEPR Theory. Two Electron Groups. Shapes of Molecules. Two Electron Groups with Double Bonds. Three Electron Groups.
Chapter 10 Lecture Chapter 10 Bonding and Properties of Solids and Liquids 10.3 Shapes of Molecules and Ions (VSEPR Theory) Learning Goal Predict the three-dimensional structure of a molecule or a polyatomic
More informationChapter 9: Molecular Geometries and Bonding Theories Learning Outcomes: Predict the three-dimensional shapes of molecules using the VSEPR model.
Chapter 9: Molecular Geometries and Bonding Theories Learning Outcomes: Predict the three-dimensional shapes of molecules using the VSEPR model. Determine whether a molecule is polar or nonpolar based
More informationChapter 9. Molecular Geometry and Bonding Theories
9.1 Molecular Shapes Read Sec. 9.1 and 9.2, then complete the Sample and Practice Exercises in these sections. Sample Exercise 9.1 (p. 347) Use the VSEPR model to predict the molecular geometries of a)
More informationAssignment 09 A. 2- The image below depicts a seesaw structure. Which of the following has such a structure?
Assignment 09 A 1- Give the total number of electron domains, the number of bonding and nonbonding domains, and the molecular geometry, respectively, for the central atom of P 3. a) four electron domains,
More informationChem 105 Friday Review Lewis formulas and geometry Bond length qualitative Polarity Polarity and geometry 11/20/2009 1
hem 105 riday 11-20-09 Review Lewis formulas and geometry Bond length qualitative Polarity Polarity and geometry 11/20/2009 1 Shown below is a partial Lewis formula for hydrogen carbonate ion ( 3- ). What
More informationChapter 13: Phenomena
Chapter 13: Phenomena Phenomena: Scientists measured the bond angles of some common molecules. In the pictures below each line represents a bond that contains 2 electrons. If multiple lines are drawn together
More information11/14/2014. Chemical Bonding. Richard Philips Feynman, Nobel Laureate in Physics ( )
Chemical Bonding Lewis Theory Valence Bond VSEPR Molecular rbital Theory 1 "...he [his father] knew the difference between knowing the name of something and knowing something" Richard Philips eynman, Nobel
More informationChapter 8. Bonding: General Concepts
Chapter 8 Bonding: General Concepts Chapter 8 Table of Contents 8.1 Types of Chemical Bonds 8.3 Bond Polarity and Dipole Moments 8.5 Energy Effects in Binary Ionic Compounds 8.6 Partial Ionic Character
More informationMolecular Geometry & Polarity
Molecular Geometry & Polarity Learn Shapes you will Because the physical and chemical properties of compounds are tied to their structures, the importance of molecular geometry can not be overstated. Localized
More informationLecture outline: Section 9. theory 2. Valence bond theory 3. Molecular orbital theory. S. Ensign, Chem. 1210
Lecture outline: Section 9 Molecular l geometry and bonding theories 1. Valence shell electron pair repulsion theory 2. Valence bond theory 3. Molecular orbital theory 1 Ionic bonding Covalent bonding
More informationCHAPTER 9 COVALENT BONDING: ORBITALS 323
APTER 9 OVALET BODIG: ORBITALS 323 2 3 2 2 2 3 3 2 2 3 2 3 O * * 2 o; most of the carbons are not in the same plane since a majority of carbon atoms exhibit a tetrahedral structure (19.5 bond angles).
More information8.1 Types of Chemical Bonds List and define three types of bonding. chapter 8 Bonding General Concepts.notebook. September 10, 2015
chapter 8 Bonding General Concepts.notebook Chapter 8: Bonding: General Concepts Mar 13 11:15 AM 8.1 Types of Chemical Bonds List and define three types of bonding. Bonds are forces that hold groups of
More informationChapter 7. Chemical Bonding I: Basic Concepts
Chapter 7. Chemical Bonding I: Basic Concepts Chemical bond: is an attractive force that holds 2 atoms together and forms as a result of interactions between electrons found in combining atoms We rarely
More informationUnit IV. Covalent Bonding
Unit IV. Covalent Bonding READING ASSIGNMENT 1: Read 16.1 pp. 437-451. Complete section review questions 1-12. Lewis Theory of Covalent Bonding- The driving force of bond formation is the desire of each
More informationCovalent Bonding Introduction, 2. Chapter 7 Covalent Bonding. Figure 7.1 The Hydrogen Molecule. Outline. Covalent Bonding Introduction, 1. Figure 7.
Covalent Bonding Introduction, 2 William L. Masterton Cecile N. Hurley http://academic.cengage.com/chemistry/masterton Chapter 7 Covalent Bonding Electron density Electrons are located between nuclei Electrostatic
More informationCHEMISTRY 103 Practice Problems #3 Chapters (Resource page) Prepared by Dr. Tony Jacob
EMITRY 103 Practice Problems #3 hapters 8 10 http://www.chem.wisc.edu/areas/clc (Resource page) Prepared by Dr. Tony Jacob uggestions on preparing for a chemistry exam: 1. rganize your materials (quizzes,
More informationChem 105 Friday Bond length qualitative Infrared spectroscopy Bond and molecular polarity Polarity and geometry Bond energy
11/7/2011 1 Chem 105 Friday 11-7-11 Bond length qualitative Infrared spectroscopy Bond and molecular polarity Polarity and geometry Bond energy Hour Exam 3 on Chap 6, 7, and 8 is this Friday, 11/11/11.
More information