; (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

Size: px
Start display at page:

Download "; (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"

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

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 information

Chapter 10: Molecular Structure and Bonding Theories

Chapter 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 information

CHAPTER 8 BONDING: GENERAL CONCEPTS Ionic solids are held together by strong electrostatic forces that are omnidirectional.

CHAPTER 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 information

Chapter 11 Answers. Practice Examples

Chapter 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 information

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals

Chemical 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 information

Review questions CHAPTER 5. Practice exercises 5.1 F F 5.3

Review 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 information

18. Ionic solids are held together by strong electrostatic forces that are omnidirectional.

18. 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 information

CHAPTER 8 BONDING: GENERAL CONCEPTS. Questions

CHAPTER 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 information

Chemical Bonding polarity & Dipole Moments. Chapter 8 Part III

Chemical 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

: 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 information

Chapter 13: Phenomena

Chapter 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 information

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals

Chemical 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 information

REVIEW ANSWERS EXAM 3 GENERAL CHEMISTRY I Do not hesitate to contact the instructor should you have any questions.

REVIEW 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 information

2. Write the electron configuration notation and the electron dot notation for each: (a) Ni atom (b) Ni 2+ ion (c) Ni 3+ ion

2. 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 information

Chemical Bonding Chapter 8

Chemical 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 information

Organic Chemistry. Review Information for Unit 1. VSEPR Hybrid Orbitals Polar Molecules

Organic 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 information

CHEMICAL BONDING. Chemical Bonds. Ionic Bonding. Lewis Symbols

CHEMICAL 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 information

CHAPTER EIGHT BONDING: GENERAL CONCEPTS. For Review

CHAPTER 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 information

2. 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.

2. 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 information

CH 222 Chapter Seven Concept Guide

CH 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 information

Chemical 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 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 information

Chapters 9&10 Structure and Bonding Theories

Chapters 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 information

Question 1. Electron Configurations Noble Gases and The Rule of Eight. Chapter 1. What is the electronic configuration of carbon?

Question 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 information

H-H bond length Two e s shared by two Hs: covalent bonding. Coulomb attraction: Stronger attraction for e Fractional charge A dipole

H-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 information

AP Chemistry- Practice Bonding Questions for Exam

AP 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 information

What Do Molecules Look Like?

What 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 information

Form J. Test #4 Last Name First Name Zumdahl, Chapters 8 and 9 November 23, 2004

Form 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 information

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 1

Chemical 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 information

A Simple Model for Chemical Bonds

A 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 information

1. 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

1. 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 information

Fill in the chart below to determine the valence electrons of elements 3-10

Fill 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 information

CH 222 Sample Exam Exam I Name: Lab Section:

CH 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 information

13 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. 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 information

Version 188 Exam 2 mccord (51600) 1

Version 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 information

Test Review # 4. Chemistry: Form TR4.11A

Test 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 information

Lewis Structures and Molecular Shapes

Lewis 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 information

VSEPR. Valence Shell Electron Pair Repulsion Theory

VSEPR. 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 information

CHEM 110 Exam 2 - Practice Test 1 - Solutions

CHEM 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 information

Section 12: Lewis Structures

Section 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 information

Lewis Structure. Lewis Structures & VSEPR. Octet & Duet Rules. Steps for drawing Lewis Structures

Lewis 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 information

Homework #7. Chapter 14. Covalent Bonding Orbitals

Homework #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 information

Hour Exam 3 on Chap 6, 7, and 8 is this Friday 11/12. A practice exam is posted on the course website.

Hour 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 information

Chemical Bonding AP Chemistry Ms. Grobsky

Chemical 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 information

Lecture 17 - Covalent Bonding. Lecture 17 - VSEPR and Molecular Shape. Lecture 17 - Introduction. Lecture 17 - VSEPR and Molecular Shape

Lecture 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 information

Valence Bond Theory - Description

Valence 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 information

REVIEW: VALENCE ELECTRONS CHEMICAL BONDS: LEWIS SYMBOLS: CHEMICAL BONDING. What are valence electrons?

REVIEW: 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 information

Lewis Structure and Electron Dot Models

Lewis 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 information

Experiment #2. Lewis Structures

Experiment #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 information

Name AP CHEM / / Chapter 8 Outline Bonding: General Concepts

Name 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 information

Name Unit Three MC Practice March 15, 2017

Name 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 information

Molecular Geometry and intermolecular forces. Unit 4 Chapter 9 and 11.2

Molecular 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 information

Chapter 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 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 information

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals

Chemical 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 information

Bonding: 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. (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 information

General and Inorganic Chemistry I.

General 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 information

Bonding: 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. (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 information

For more info visit Chemical bond is the attractive force which holds various constituents together in a molecule.

For 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 information

Ch 13: Covalent Bonding

Ch 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 information

Chapter 10: Chemical Bonding II: Molecular Shapes; VSEPR, Valence Bond and Molecular Orbital Theories

Chapter 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 information

Molecular Geometry and Chemical Bonding Theory

Molecular 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 information

Chemistry 121: Topic 4 - Chemical Bonding Topic 4: Chemical Bonding

Chemistry 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 information

A DOT STRUCTURE FOR A LARGER MOLECULE ETHANOL! Count valence electrons

A 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 information

Example: 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

Example: 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 information

Chapters 8 and 9. Octet Rule Breakers Shapes

Chapters 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 information

Chapter 6 Chemical Bonding

Chapter 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 information

CHAPTER TEN MOLECULAR GEOMETRY MOLECULAR GEOMETRY V S E P R CHEMICAL BONDING II: MOLECULAR GEOMETRY AND HYBRIDIZATION OF ATOMIC ORBITALS

CHAPTER 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 information

CHEM PRACTICE EXAM IV CLASS - SPRING 2017 ANSWER KEY

CHEM 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 information

Chapter 9: Chemical Bonding I: Lewis Theory. Lewis Theory: An Overview

Chapter 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 information

m measured m if 100%ionic

m 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 information

Valence Shell Electron Pair Repulsion Model

Valence 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 information

Chapter 9 Molecular Geometry and Bonding Theories

Chapter 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 information

Chapter 6 PRETEST: Chemical Bonding

Chapter 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 information

Name. 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. 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 information

CHAPTER 9 COVALENT BONDING: ORBITALS. Questions

CHAPTER 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 information

Chapter 9. Chemical Bonding II: Molecular Geometry and Bonding Theories

Chapter 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 information

Lewis Theory of Shapes and Polarities of Molecules

Lewis 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 information

Unit 6: Molecular Geometry

Unit 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 information

1. What is the phenomenon that occurs when certain metals emit electrons when illuminated by particular wavelengths of light? a.

1. 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 information

Bonding/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 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 information

Ch 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules

Ch 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 information

Molecular Structures. Using Molecular Models. Using Molecular Models. Predicting Molecular Shapes: VSEPR. Predicting Molecular Shapes: VSEPR

Molecular 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 information

Chapter 10 Shapes of Molecules. Dr. Sapna Gupta

Chapter 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 information

Chapter 7 Chemical Bonding and Molecular Structure

Chapter 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 information

4/25/2017. VSEPR Theory. Two Electron Groups. Shapes of Molecules. Two Electron Groups with Double Bonds. Three Electron Groups.

4/25/2017. 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 information

Chapter 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. 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 information

Chapter 9. Molecular Geometry and Bonding Theories

Chapter 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 information

Assignment 09 A. 2- The image below depicts a seesaw structure. Which of the following has such a structure?

Assignment 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 information

Chem 105 Friday Review Lewis formulas and geometry Bond length qualitative Polarity Polarity and geometry 11/20/2009 1

Chem 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 information

Chapter 13: Phenomena

Chapter 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 information

11/14/2014. Chemical Bonding. Richard Philips Feynman, Nobel Laureate in Physics ( )

11/14/2014. 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 information

Chapter 8. Bonding: General Concepts

Chapter 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 information

Molecular Geometry & Polarity

Molecular 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 information

Lecture outline: Section 9. theory 2. Valence bond theory 3. Molecular orbital theory. S. Ensign, Chem. 1210

Lecture 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 information

CHAPTER 9 COVALENT BONDING: ORBITALS 323

CHAPTER 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 information

8.1 Types of Chemical Bonds List and define three types of bonding. chapter 8 Bonding General Concepts.notebook. September 10, 2015

8.1 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 information

Chapter 7. Chemical Bonding I: Basic Concepts

Chapter 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 information

Unit IV. Covalent Bonding

Unit 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 information

Covalent Bonding Introduction, 2. Chapter 7 Covalent Bonding. Figure 7.1 The Hydrogen Molecule. Outline. Covalent Bonding Introduction, 1. Figure 7.

Covalent 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 information

CHEMISTRY 103 Practice Problems #3 Chapters (Resource page) Prepared by Dr. Tony Jacob

CHEMISTRY 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 information

Chem 105 Friday Bond length qualitative Infrared spectroscopy Bond and molecular polarity Polarity and geometry Bond energy

Chem 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