CHEMICAL BONDING. Chemical Bonds. Ionic Bonding. Lewis Symbols
|
|
- Mary Morrison
- 6 years ago
- Views:
Transcription
1 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 which wants 2 electrons around it). Ionic Bonding Electron Configurations of Ions
2 Sizes of Ions Ex 1 Which of the following atoms and ions is largest: (a) S 2, S, O 2 (b) Rb +, Sr 2+, Y 3+ Covalent Bonding Elements which are neither highly electropositive nor highly electronegative are less likely to form ionic compounds. Consider CH 4, methane; carbon and hydrogen have similar electronegativities. It would be inappropriate to describe the bonds between carbon and hydrogen in methane as ionic. Instead, the bonding between these two atoms involves a sharing of electrons (not an electron transfer) and is termed a covalent bond. Lewis Structures Multiple Bonds
3 Ex 2 (a) H 2 O (b) PH 3 (c) CH 4 (d) CO 2 (e) N 2 Bond Polarity Electronegativity is defined as the ability of an atom in a molecule to attract electrons to itself. Electronegativity and Bond Polarity Ex 3 Which bond is more polar: S Cl, S Br, Se Cl, or Se Br?
4 Dipole Moments Drawing Lewis Structures Lewis structures help to explain or predict trends in chemical reactivity. Procedure for drawing a Lewis Structure (from your text): 1. Count up total number of valence electrons from all atoms. If the species is an ion, either add the negative charge to A (for anion) or subtract the positive charge from A (for cation). 2. Draw a skeleton structure. 3. Complete the octets of the atoms bonded to the central atom. 4. Place any leftover electrons on the central atom, even if that means giving the central atom more than an octet of electrons. 5. If not enough electrons to give central atom an octet, try using multiple bonds. Alternative procedure for drawing a Lewis Structure: 1. Count up total number of valence ele ctrons available (A). If the species is an ion, either add the negative charge to A (for anion) or subtract the positive charge from A (for cation). 2. Calculate total number of electrons needed (N) to give each atom an octet (8 # non-hydrogen atoms + 2 # hydrogen atoms) 3. Calculate the number of bonding electrons (S): S = N - A 4. Draw a molecular skeleton for the substance and then assign two bonding electrons to each connection between atoms. (Note that when constructing a molecular skeleton, H and F are always terminal atoms.) 5. If any bonding electrons are left over, use them for double or triple bonds. Double bonds form only between carbon, nitrogen, oxygen, and sulfur. Triple bonds are usually restricted to carbon and nitrogen. 6. Distribute remaining electrons around atoms to complete their octets. (All atoms want an octet except H.) 7. Determine the formal charge on each atom, and write it next to the atom. Check to see that the formal charges add up to the overall charge on the molecule or ion. (See below)
5 Ex 4 Draw Lewis structures for the following: (a) POCl 3 (b) SOCl 2 (c) ClO (d) CH 2 O Formal charge Unequal sharing of electrons between atoms leads to partial charges on some of the atoms in a molecule. Determination of the formal charge on atoms in a molecule can serve as a check of the reasonableness of the Lewis structure we have drawn. Formal charge = group number # e in lone pairs 1/2(# of shared e ) Ex. 5 Compute the formal charges on the atoms in the following Lewis structure for the - azide ion N 3. [: N = N = N :]
6 Resonance Structures Some molecules may have two or more equivalent Lewis structures. These are known as resonance structures. This does not mean that the molecule jumps back and forth between these structures. In reality, the true structure of the molecule will lie somewhere in between these resonance structures. Ex 6 Draw the Lewis structures (including any resonance structures) for the following: (a) SO 2 (b) SO 3 (c) NO 3 Exceptions to the Octet Rule Odd Number of Electrons Electron Deficient Molecules
7 Expanded Valence Shapes of Molecules Lewis structures give us a picture of how atoms are connected to each other, but they don t tell us the actual shapes of the molecules. Molecules are three-dimensional. We need an extension to Lewis theory to help us predict the arrangement of the atoms in space. VSEPR Theory (Valence Shell Electron Pair Repulsion) Lone pairs occupy more space than bonding pairs Repulsive forces among valences pairs diminish in the following order: lone pair vs. lone pair > lone pair vs. bond pair > bond pair vs. bond pair Lone pairs prefer equatorial positions to axial positions in trigonal bipyramid. Ex. 7 Predict the structures of the following: (a) water (b) SO 2 (c) ClO 3 + (d) IF 5
8 Shapes of Molecules with Bond Pairs ONLY, No Electron Pairs AX 2 AX 3 AX 4 Linear Trigonal Tetrahedral Planar Planar (CO 2 ) (BF 3 ) (CH 4 ) AX 5 AX 6 Trigonal Octahedral Bipyramidal (PCl 5 ) (SF 6 )
9 Shapes of Molecules with... Three Electron Pairs Cl B Cl Ge No Lone Pairs Trigonal Planar One Lone Pair Bent (BCl 3 ) (GeCl 2 ) Four Electron Pairs C N H O No Lone Pairs One Lone Pair Two Lone Pairs Tetrahedral Pyramidal Bent (CCl 4 ) (NH 3 ) (H 2 O)
10 Polarity of Polyatomic Molecules Ex. 8 Predict whether the following have a dipole moment: (a) NH 3 (b) SF 6 Some general rules of thumb regarding dipole moments: a central atom with no lone pairs on it, surrounded by other atoms of all the same type will NOT have a dipole moment (e.g. CH 4, CO 2, SF 6 ) a central atom with no lone pairs surrounded by other atoms of not all the same type WILL usually have a dipole moment (e.g. CH 3 Cl, NO 2 Cl, OCN) a central atom with lone pairs on it, surrounded by other atoms of any type WILL almost always have a dipole moment (e.g. H 2 O, NH 3, ICl 3 ) a diatomic molecule containing the same atoms will NOT have a dipole moment (e.g. O 2 ); a diatomic molecule containing different atoms WILL have a dipole moment (e.g. CO)
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 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 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 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 informationChemical Bonds. Chapter 6
Chemical Bonds Chapter 6 1 Ch. 6 Chemical Bonding I. How and Why Atoms Bond A. Vocabulary B. Chemical Bonds - Basics C. Chemical Bonds Types D. Chemical Bonds Covalent E. Drawing Lewis Diagrams F. Bond
More informationMolecular Models: The shape of simple molecules and ions
Molecular Models: The shape of simple molecules and ions Background The shape of a molecule is very important when investigating its properties and reactivity. For example, compare CO 2 and SO 2. Carbon
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 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 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 informationCHEM 101: CHAPTER 11: CHEMICAL BONDS: THE FORMATION OF COMPOUNDS FROM ATOMS
1 CHEM 101: CHAPTER 11: CHEMICAL BONDS: THE FORMATION OF COMPOUNDS FROM ATOMS PERIODIC TRENDS: See pages 214-216, 221 Table 11.3, and 227 + 228 of text. Lewis Structures of Atoms: The Lewis Dot Diagram
More informationIntroduction to VSEPR Theory 1
1 Class 8: Introduction to VSEPR Theory Sec 10.2 VSEPR Theory: The Five Basic Shapes Two Electron Groups: Linear Geometry Three Electron Groups: Trigonal Planar Geometry Four Electron Groups: Tetrahedral
More informationCOVALENT BONDING CHEMICAL BONDING I: LEWIS MODEL. Chapter 7
Chapter 7 P a g e 1 COVALENT BONDING Covalent Bonds Covalent bonds occur between two or more nonmetals. The two atoms share electrons between them, composing a molecule. Covalently bonded compounds are
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 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 informationCP Covalent Bonds Ch. 8 &
CP Covalent Bonds Ch. 8 & 9 2015-2016 Why do atoms bond? Atoms want stability- to achieve a noble gas configuration ( ) For bonds there is a transfer of electrons to get an octet of electrons For covalent
More informationChapter 9 Molecular Geometries. and Bonding Theories
Chapter 9 Molecular Geometries and Bonding Theories Coverage of Chapter 9 9.1 All 9.2 All 9.3 All 9.4 All 9.5 Omit Hybridization Involving d Orbitals 9.6 All 9.7 and 9.8 Omit ALL MOLECULAR SHAPES The shape
More informationCovalent Bonds Ch. Why do atoms bond? Atoms want noble gas configuration ( ) For bonds there is a transfer of electrons to get an octet of electrons
Covalent Bonds Ch. Why do atoms bond? Atoms want noble gas configuration ( ) For bonds there is a transfer of electrons to get an octet of electrons For covalent bonds there is a of electrons to get an
More informationMolecular Geometry. Valence Shell Electron Pair. What Determines the Shape of a Molecule? Repulsion Theory (VSEPR) Localized Electron Model
Molecular Geometry 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 Electron
More informationLewis structures show the number and type of bonds between atoms in a molecule or polyatomic ion.
VSEPR & Geometry Lewis structures show the number and type of bonds between atoms in a molecule or polyatomic ion. Lewis structures are not intended to show the 3-dimensional structure (i.e. shape or geometry)
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 informationOFB Chapter 3 Chemical Periodicity and the Formation of Simple Compounds
OFB hapter 3 hemical Periodicity and the Formation of Simple ompounds 3-1 Groups of Elements 3-2 The Periodic Table 3-3 Ions and Ionic ompounds 3-4 ovalent Bonding and Lewis Structures 3-5 3-6 Naming ompounds
More informationShapes of Molecules and Hybridization
Shapes of Molecules and Hybridization A. Molecular Geometry Lewis structures provide us with the number and types of bonds around a central atom, as well as any NB electron pairs. They do not tell us the
More informationMolecular Geometry. Objectives N H H. The objectives of this laboratory are to:
Objectives The objectives of this laboratory are to: Molecular Geometry Write Lewis structure representations of the bonding and valence electrons in molecules. Use the VSEPR model to predict the molecular
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 informationSubtopic 4.2 MOLECULAR SHAPE AND POLARITY
Subtopic 4.2 MOLECULAR SHAPE AND POLARITY 1 LEARNING OUTCOMES (covalent bonding) 1. Draw the Lewis structure of covalent molecules (octet rule such as NH 3, CCl 4, H 2 O, CO 2, N 2 O 4, and exception to
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 informationStructures, Shapes and Polarity. of Molecules. Level 2 recap: - Polar and non polar bonds - Lewis diagrams - Lone pairs - Shapes - Polarity
Structures, Shapes and Polarity Level 2 recap: - Polar and non polar bonds - Lewis diagrams - Lone pairs - Shapes - Polarity of Molecules Do now: Brainstorm what you know/remember about these L2 concepts
More information(A) 1 bonding pair (B) 1 bonding pair and 1 lone pair (C) 2 bonding pairs (D) 2 bonding pairs and 2 lone pairs
AP Chemistry - Problem Drill 13: Lewis Structures and VSPER No. 1 of 10 1. Lewis structure is used to model covalent bonds of a molecule or ion. Covalent bonds are a type of chemical bonding formed by
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 informationHonors Chemistry Unit 6 ( )
Honors Chemistry Unit 6 (2017-2018) Lewis Dot Structures VSEPR Structures 1 We are learning to: 1. Represent compounds with Lewis structures. 2. Apply the VSEPR theory to determine the molecular geometry
More informationChemistry and the material world Lecture 3
Chemistry and the material world 123.102 Lecture 3 Electronic bookkeeping we need a way of finding out in which proportions two or more atoms make up a molecule is it CH 3 or CH 4 or CH 5? counting valence
More informationbond energy- energy required to break a chemical bond -We can measure bond energy to determine strength of interaction
bond energy- energy required to break a chemical bond -We can measure bond energy to determine strength of interaction ionic compound- a metal reacts with a nonmetal Ionic bonds form when an atom that
More informationAdapted from CHM 130 Maricopa County, AZ Molecular Geometry and Lewis Dot Formulas Introduction
Adapted from CHM 130 Maricopa County, AZ Molecular Geometry and Lewis Dot Formulas Introduction A chemical bond is an intramolecular (within the molecule) force holding two or more atoms together. Covalent
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 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 informationOFB Chapter 3 Chemical Periodicity and the Formation of Simple Compounds
OFB hapter 3 hemical Periodicity and the Formation of Simple ompounds 3-1 Groups of Elements 3-2 The Periodic Table 3-3 Ions and Ionic ompounds 3-4 ovalent Bonding and Lewis Structures 3-5 Drawing Lewis
More informationCHAPTER 12 CHEMICAL BONDING
Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 12 CHEMICAL BONDING Day Plans for the day Assignment(s) for the day 1 Begin Chapter
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 informationSKILL-BUILDING EXERCISE
4. O and H Solution 1. Carbon has an electronegativity of 2.5, while the value for hydrogen is 2.1. The difference is 0.3, which is rather small. The C H bond is therefore considered nonpolar. 2. Both
More informationChapter 10. Valence Electrons. Lewis dot symbols. Chemical Bonding
Chapter 10 Chemical Bonding Valence Electrons Recall: the outer electrons in an atom are valence electrons. Valence electrons are related to stability Valence electrons can be represented with dots in
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 informationChapter 11 Chemical Bonds: The Formation of Compounds from Atoms Advanced Chemistry Periodic Trends in Atomic Properties Learning Objective
Chapter 11 Chemical Bonds: The Formation of Compounds from Atoms Advanced Chemistry 11.1 Periodic Trends in Atomic Properties Discuss the atomic trends Metals are located on the left side of the periodic
More informationHelpful Hints Lewis Structures Octet Rule For Lewis structures of covalent compounds least electronegative
Helpful Hints Lewis Structures Octet Rule Lewis structures are a basic representation of how atoms are arranged in compounds based on bond formation by the valence electrons. A Lewis dot symbol of an atom
More informationWhat is a Bond? Chapter 8. Ionic Bonding. Coulomb's Law. What about covalent compounds?
Chapter 8 What is a Bond? A force that holds atoms together. Why? We will look at it in terms of energy. Bond energy- the energy required to break a bond. Why are compounds formed? Because it gives the
More informationTest Bank for Introductory Chemistry Essentials 5th Edition by Tro
Test Bank for Introductory Chemistry Essentials 5th Edition by Tro Sample Introductory Chemistry, 5e (Tro) Chapter 10 Chemical Bonding 10.1 True/False Questions 1) Bonding theories are used to predict
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 informationMOLECULAR MODELS OBJECTIVES
MOLECULAR MODELS OBJECTIVES 1. To learn to draw Lewis structures for common compounds 2. To identify electron pairs as bonding pairs or lone pairs 3. To use electron pair repulsion theory to predict electronic
More informationChapter 9 Molecular Geometry. Lewis Theory-VSEPR Valence Bond Theory Molecular Orbital Theory
Chapter 9 Molecular Geometry Lewis Theory-VSEPR Valence Bond Theory Molecular Orbital Theory Sulfanilamide Lewis Structures and the Real 3D-Shape of Molecules Lewis Theory of Molecular Shape and Polarity
More informationCHEMICAL BONDING. Valence Electrons. Chapter Ten
CHEMICAL BONDING Chapter Ten Valence Electrons! The electrons occupying the outermost energy level of an atom are called the valence electrons; all other electrons are called the core electrons.! The valence
More informationHey, Baby. You and I Have a Bond...Ch. 8
I. IONIC BONDING FUNDAMENTALS A. They form between... 1. A and a a. A to become b. A to become B. How it happens (Let s first focus on two atoms): 1. When a metal and a nonmetal meet, electrons get transferred
More informationAP Chemistry. Unit #7. Chemical Bonding & Molecular Shape. Zumdahl Chapters 8 & 9 TYPES OF BONDING BONDING. Discrete molecules formed
AP Chemistry Unit #7 Chemical Bonding & Molecular Shape Zumdahl Chapters 8 & 9 TYPES OF BONDING BONDING INTRA (Within (inside) compounds) STRONG INTER (Interactions between the molecules of a compound)
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 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 informationLewis Dot Formulas and Molecular Shapes
Lewis Dot Formulas and Molecular Shapes Introduction A chemical bond is an intramolecular (within the molecule) force holding two or more atoms together. Covalent chemical bonds are formed by valence electrons
More informationExperiment 21 Lewis structures and VSEPR Theory
Experiment 21 Lewis structures and VSEPR Theory Introduction 1. Lewis Structures and Formal Charge LG.N. Lewis, at the University of California at Berkeley devised a simple way to understand the nature
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 informationChapter 12 Structures and Characteristics of Bonds Objectives
Objectives 1. To learn about ionic and covalent bonds and explain how they are formed - what holds compounds together? 2. To learn about the polar covalent bond are all covalent bonds equal? 3. To understand
More informationChapter 12. Chemical Bonding
Chapter 12 Chemical Bonding Chapter 12 Introduction to Chemical Bonding Chemical Bonding Valence electrons are the electrons in the outer shell (highest energy level) of an atom. A chemical bond is a mutual
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 informationPART 3 Chemical Bonds, Valence Bond Method, and Molecular Shapes. Reference: Chapter 9 10 in textbook
PART 3 Chemical Bonds, Valence Bond Method, and Molecular Shapes Reference: Chapter 9 10 in textbook 1 Valence Electrons Valence ae Electron Define: the outer shell electrons Important for determination
More informationAP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts
AP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts 8.1 Types of Chemical Bonds A. Ionic Bonding 1. Electrons are transferred 2. Metals react with nonmetals 3. Ions paired have lower energy
More informationChapter 8. Chemical Bonding: Basic Concepts
Chapter 8. Chemical Bonding: 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 informationCHAPTER 12: CHEMICAL BONDING
CHAPTER 12: CHEMICAL BONDING Problems: 1-26, 27c, 28, 33-34, 35b, 36(a-c), 37(a,b,d), 38a, 39-40, 41-42(a,c), 43-58, 67-74 12.1 THE CHEMICAL BOND CONCEPT chemical bond: what holds atoms or ions together
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 information10-1. The Shapes of Molecules, chapter 10
10-1 The Shapes of Molecules, chapter 10 The Shapes of Molecules; Goals 10.1 Depicting Molecules and Ions with Lewis Structures 10.2 Valence-Shell Electron-Pair Repulsion (VSEPR) Theory 10.3 Molecular
More informationChapter 10. Geometry
Chapter 10 Molec cular Geometry 1 CHAPTER OUTLINE Molecular Geometry Molecular Polarity VSEPR Model Summary of Molecular Shapes Hybridization Molecular Orbital Theory Bond Angles 2 MOLECULAR GEOMETRY Molecular
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 informationAt the end of this lesson, students should be able to :
At the end of this lesson, students should be able to : (a) Explain Valence Shell Electron Pair Repulsion theory (VSEPR) (b) Draw the basic molecular shapes: linear, planar, tetrahedral, and octahedral.
More informationCHEM1101 Worksheet 6: Lone Pairs and Molecular Geometry
CHEM1101 Worksheet 6: Lone Pairs and Molecular Geometry Model 1: Oxidation numbers Oxidation numbers are a useful accountancy tool to help keep track of electrons in compounds and reactions. This is particularly
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 informationIts Bonding Time. Chemical Bonds CH 12
Its Bonding Time Chemical Bonds CH 12 What is a chemical bond? Octet Rule: Chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its
More informationCHEMISTRY Matter and Change Section 8.1 The Covalent Bond
CHEMISTRY Matter and Change Section Chapter 8: Covalent Bonding CHAPTER 8 Table Of Contents Section 8.2 Section 8.3 Section 8.4 Section 8.5 Naming Molecules Molecular Structures Molecular Shapes Electronegativity
More informationEx. 1) F F bond in F = 0 < % covalent, no transfer of electrons
#60 Notes Unit 8: Bonding Ch. Bonding I. Bond Character Bonds are usually combinations of ionic and covalent character. The electronegativity difference is used to determine a bond s character. Electronegativity
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 informationChapter 8 The Concept of the Chemical Bond
Chapter 8 The Concept of the Chemical Bond Three basic types of bonds: Ionic - Electrostatic attraction between ions (NaCl) Metallic - Metal atoms bonded to each other Covalent - Sharing of electrons Ionic
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 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 informationCopyright McGraw-Hill Education. Permission required for reproduction or display : A force that holds atoms together in a molecule or compound
: Chemical Bonding 8-1 8.1 Types of Bonds : A force that holds atoms together in a molecule or compound Two types of chemical bonds Ionic Bonds Covalent Bonds 8-2 1 8.1 Types of Bonds 8-3 8.1 Types of
More informationChem 1075 Chapter 12 Chemical Bonding Lecture Outline. Chemical Bond Concept
Chem 1075 Chapter 12 Chemical Bonding Lecture Outline Slide 2 Chemical Bond Concept Recall that an atom has and electrons. Core electrons are found to the nucleus. Valence electrons are found in the s
More informationChemical Bonding. Types of Bonds. Ionic Bonding. Resonance Structures. Molecular Geometries. VSEPR Basic Shapes 3-D Notation Hybridization (Lab)
Chemical Bonding Types of Bonds Ionic Bonding Lewis Structures Covalent Bonding Resonance Structures Octet Rule Polar Molecules Molecular Geometries VSEPR Basic Shapes 3-D Notation Hybridization (Lab)
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 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 informationUnit 9: CHEMICAL BONDING
Unit 9: CHEMICAL BONDING 1 Unit 9: Bonding: 1. Electronegativity 2. Intramolecular Bonding 3. Intermolecular Bonding 4. Drawing Lewis Structures 5. Lewis Structures for Polyatomic Ions 6. Exceptions to
More informationChapter 4. Molecular Structure and Orbitals
Chapter 4 Molecular Structure and Orbitals Chapter 4 Table of Contents (4.1) (4.2) (4.3) (4.4) (4.5) (4.6) (4.7) Molecular structure: The VSEPR model Bond polarity and dipole moments Hybridization and
More informationShapes of Molecules. Lewis structures are useful but don t allow prediction of the shape of a molecule.
Shapes of Molecules Lewis structures are useful but don t allow prediction of the shape of a molecule. H O H H O H Can use a simple theory based on electron repulsion to predict structure (for non-transition
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 informationChapter 6. The Chemical Bond
Chapter 6 The Chemical Bond Some questions Why do noble gases rarely bond to other elements? How does this relate to why the atoms of other elements do form bonds? Why do certain elements combine to form
More informationCovalent Bonding. In nature, only the noble gas elements exist as uncombined atoms. All other elements need to lose or gain electrons
In nature, only the noble gas elements exist as uncombined atoms. They are monatomic - consist of single atoms. All other elements need to lose or gain electrons To form ionic compounds Some elements share
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 informationLewis Dot Structures and Molecular Geometry
Experiment 11 Lewis Dot Structures and Molecular Geometry Pre-Lab Assignment Before coming to lab: Read the lab thoroughly. Answer the pre-lab questions that appear at the end of this lab exercise. Purpose
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 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 informationThe Shapes of Molecules. Chemistry II
The Shapes of Molecules Chemistry II Lewis Structures DEFINITIN: A structure of a molecule showing how the valence electrons are arranged. 1) nly the valence electrons appear in a Lewis structure. 2) The
More information6.1 Intro to Chemical Bonding Name:
6.1 Intro to Chemical Bonding Name: A. Chemical bond Favored by nature because: 3 main types of bonds 1. 2. 3. B. Ionic Bonds C. Covalent Bonds D. Metallic Bond E. Bond Determination RECALL: Electronegativity
More informationMolecular Geometry and Bonding Theories. Molecular Shapes. Molecular Shapes. Chapter 9 Part 2 November 16 th, 2004
Molecular Geometry and Bonding Theories Chapter 9 Part 2 November 16 th, 2004 8 Molecular Shapes When considering the geometry about the central atom, we consider all electrons (lone pairs and bonding
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 informationIonic and Covalent Bonding
1. Define the following terms: a) valence electrons Ionic and Covalent Bonding the electrons in the highest occupied energy level always electrons in the s and p orbitals maximum of 8 valence electrons
More informationCarbon and Its Compounds
Chapter 1 Carbon and Its Compounds Copyright 2018 by Nelson Education Limited 1 1.2 Organic Molecules from the Inside Out I: The Modelling of Atoms Copyright 2018 by Nelson Education Limited 2 s orbitals:
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 informationCovalent Compounds: Bonding Theories and Molecular Structure
CHM 123 Chapter 8 Covalent Compounds: Bonding Theories and Molecular Structure 8.1 Molecular shapes and VSEPR theory VSEPR theory proposes that the geometric arrangement of terminal atoms, or groups of
More information