Chapter 9. Chemical Bonding I: Lewis Theory
|
|
- Andra Moody
- 7 years ago
- Views:
Transcription
1 Student Objectives 9.1 Bonding Models and AIDS Drugs Know that X ray crystallography was used to characterize the structure of HIV protease, a biomolecule critical to the reproduction of HIV. Know that Lewis structures are simple predictors of how atoms combine to form ionic compounds and molecules. 9.2 Types of Chemical Bonds Know and understand that chemica l bonds form because they lower the potential energy between the charged particles in the constituent atoms. Define and understand ionic bond, covalent bond, and metallic bonding. 9.3 Representing Valence Electrons with Dots Know that valence electrons can be represented with dots around an element symbol. Identify and draw atoms with their valence electrons represented as dots. Know that Lewis theory involves the sharing or transfer of electrons. Define and know the octet rule. 9.4 Ionic Bonding: Lewis Structures and Lattice Energies Draw Lewis structures of ionic compounds containing main group elements. Understand that the formation of an ionic compound from neutral atoms is exothermic the amount of energy released is largely due to lattice energy. Know that the Born Haber cycle is a way of accounting for the energetics of each of the steps in the formation of an ionic compound from its constituent elements. Use a Born Haber cycle to calculate the lattice energy of an ionic compound. Know that lattice energy decreases for larger ions and increases with increasing charge. Understand why ionic solids are poor electrical conductors while ionic liquids and aqueous solutions of ionic compounds are good electrical conductors. 9.5 Covalent Bonding: Lewis Structures Know that most nonmetal atoms prefer to be surrounded by eight valence electrons, but hydrogen requires only two. Understand that in Lewis theory, a pair of electrons, one from each of two atoms, forms a bond or bonding pair that helps each atom achieve an octet. The two atoms can also share two pairs of electrons (a double bond) or three pairs of electrons (triple bond). Identify and draw covalent compounds with single, double, and triple bonds between constituent atoms. 124
2 9.6 Electronegativity and Bond Polarity Know and understand that a pair of electrons does not have to be shared equally between two atoms. Unequal sharing results in a polar covalent bond. Define electronegativity and know its periodic trends. Understand that bonds can range from a nonpolar covalent bond to a polar covalent bond to an ionic bond depending on the difference in electronegativity between the two atoms. Define dipole moment and percent ionic character. 9.7 Lewis Structures of Molecular Compounds and Polyatomic Ions Draw Lewis structures for molecular compounds and polyatomic ions. 9.8 Res onance and Formal Charge Define resonance structures and understand how Lewis structures represent the individual and the hybrid structures. Define formal charge and understand how to calculate it for the atoms in a Lewis structure. 9.9 Exceptions to the Octet Rule: Odd Electron Species, Incomplete Octets, and Expanded Octets Draw Lewis structures for odd electron species. Draw Lewis structures for molecules containing atoms with incomplete octets. Draw Lewis structures for molecules containing atoms with expanded octets. Understand why the second period elements cannot have expanded octets Bond Energies and Bond Lengths Define bond energy. Estimate reaction enthalpies using average bond energies for all bonds broken and formed in a chemical reaction. Understand the inverse relationship between bond length and bond strength Bonding in Metals: The Electron Sea Model Understand how the electron sea model accounts for the general macroscopic properties of metals. Section Summaries Lecture Outline Terms, Concepts, Relationships, Skills Figures, Tables, and Solved Examples Teaching Tips Suggestions and Examples Misconceptions and Pitfalls 125
3 Lecture Outline T erms, Concepts, Relationships, Skills Figures, Tables, and Solved Examples 9.1 Bonding Models and AIDS Drugs X ray crystallography o structure of HIV protease Bonding theory o Lewis theory o Lewis structure Intro figure: HIV protease and Indinavir unnumbered figure: photo of G. N. Lewis 9.2 Types of Chemical Bonds Types of bonds o ionic o covalent o metallic Electrons in bonds o transferred (ionic) o shared (covalent) o pooled (metallic) unnumbered table: types of bonds Figure 9.1 Ionic, Covalent, and Metallic Bonding Figure 9.2 Possible Configurations of One Negatively Charged Particle and Two Positively Charged Ones 9.3 Representing Valence Electrons with Dots Lewis structure o elemental symbol surrounded by valence electrons o octet rule Chemical bond o sharing electrons o octet rule: complete octet by sharing unnumbered figures: Lewis dot structures of period 2 elements 126
4 Teaching Tips S uggestions and Examples Misconceptions and Pitfalls 9.1 Bonding Models and AIDS Drugs Proteins are complex molecules, but building models of them starts with a single bond. Student understanding of X ray crystallography can start with a gross simplification that begins with an analogy to X rays in radiology. In protein structures, X rays diffract as a result of the nuclei of atoms. Lewis structures were proposed in a J. Am. Chem. Soc. paper in 1916 and have served as a simple but effective bonding model since. 9.2 Types of Chemical Bonds A brief review of electrostatic potential energy should point out that the energy is proportional to the magnitude of the charges and inversely proportional to the distance between them. Figure 9.2 shows the possibilities of one negative charge and two positive charges. Ask the students to imagine possibilities for two negative charges and two positive charges. 9.3 Representing Valence Electrons with Dots The placement of the electrons in the Lewis dot structures for the period 2 elements gives a starting point for students in terms of the number of bonds often formed by these elements. The students will realize with more study that these are not always the case. 127
5 Lecture Outline T erms, Concepts, Relationships, Skills Figures, Tables, and Solved Examples 9.4 Ionic Bonding: Lewis Structures and Lattice Energies Lewis structures of ionic compounds o complete octet by addition or subtraction of electrons Energetics o Lattice energy o Born Haber cycle o trends ion size ion charge Electrical Conductivity unnumbered figures: Lewis dot structures of KCl and Na 2 S Example 9.1 Using Lewis Structures to Predict the Chemical Formula of an Ionic Compound Figure 9.3 Lattice Energy Figure 9.4 Born Haber Cycle for Sodium Chloride unnumbered figure: bond lengths of the group 1A metal chlorides unnumbered figures: bond lengths of NaF and CaO Example 9.2 Predicting Relative Lattice Energies unnumbered figure: melting of NaCl unnumbered figures: electrical conductivity of NaCl(s) and NaCl(aq) Chemistry and Medicine: Ionic Compounds in Medicine 9.5 Covalent Bonding: Lewis Structures Lewis structures of covalent compounds o bonding pairs o lone pairs o single bonds o double, triple bonds Covalent bonds (intramolecular) versus intermolecular forces unnumbered figures: Lewis structures for H 2 O unnumbered figures: Lewis structures for Cl 2 and H 2 unnumbered figures: Lewis structures for O 2, N 2 unnumbered figures: Lewis structures for H 3 O + and H 2 O 2 Figure 9.5 Intermolecular and Intramolecular Forces 128
6 Teaching Tips S uggestions and Examples Misconceptions and Pitfalls 9.4 Ionic Bonding: Lewis Structures and Lattice Energies The electron configuration of K + but not K demonstrates a complete octet. Lattice energy cannot be measured directly in the laboratory but is obtained through a thermodynamic cycle. Ion size and ion charge discussions about the trend in lattice energy are an application of Coulomb s law. The reality section brings focus on the electrical conductivity of ionic compounds. Electricity can be conducted only when the charged particles can move. Conceptual Connection 9.1 Melting Points of Ionic Solids Despite especially the group 1A and group 2A elements willingness to ionize, that ionization still is endothermic. Lattice energy is the main reason that ionic solids form from their elements. 9.5 Covalent Bonding: Lewis Structures Introduce the idea of the common numbers of bonds, e.g. 2 for O, 3 for N, 4 for C, etc. It may be useful to use colors or other symbols to differentiate electrons as you assign them in the first few Lewis structure examples. The discussion of intramolecular (microscopic) versus intermolecular (macroscopic) forces is an important one. The latter are always much weaker than bond energies (Section 9.10). Conceptual Connection 9.2 Energy and the Octet Rule Lewis structures and octets are simple schemes to understand how atoms combine to form molecules. They are neither the forces nor the justification for why they do. The overall lower energy of the molecule drives its formation. 129
7 Lecture Outline T erms, Concepts, Relationships, Skills Figures, Tables, and Solved Examples 9.6 Electronegativity and Bond Polarity Covalent bonds o nonpolar covalent o polar covalent Electronegativity o Pauling values o bond polarity, EN covalent, EN = polar covalent, EN = ionic, EN = 2.0+ Dipole moment o = qr o percent ionic character Figure 9.6 Orientation of Gaseous Hydrogen Fluoride in an Electric Field Figure 9.7 Electron Density Plot for the HF Molecule Figure 9.8 Electronegativities of the Elements unnumbered figures: molecular models of Cl 2, NaCl, and HCl Table 9.1 The Effect of Electronegativity Difference on Bond Type Figure 9.9 Electronegativity Difference (EN) and Bond Type Table 9.2 Dipole Moments of Several Molecules in the Gas Phase Figure 9.10 Percent Ionic Character versus Electronegativity Difference for Some Compounds Example 9.3 Classifying Compounds as Pure Covalent, Polar Covalent, or Ionic 9.7 Lewis Structures of Molecular Compounds and Polyatomic Ions Skeletal structure Total number of valence electrons Distribution of electrons to satisfy octet rule Multiple bonds Example 9.4 Writing Lewis Structures: Write a Lewis Structure for CO 2 Example 9.5 Writing Lewis Structures: Write a Lewis Structure for NH 3 Example 9.6 Writing Lewis Structures for Polyatomic Ions 9.8 Resonance and Formal Charge Resonance o equivalent Lewis structures o hybrid structure Formal charge o calculation o minimization o negative formal charges on electronegative atoms unnumbered figure: Lewis structure of O 3 Figure 9.11 Hybridization Example 9.7 Writing Resonance Structures unnumbered figures: formal charges of HCN and HNC Example 9.8 Assigning Formal Charges Example 9.9 Drawing Resonance Structures and Assigning Formal Charge for Organic Compounds 130
8 Teaching Tips S uggestions and Examples Misconceptions and Pitfalls 9.6 Electronegativity and Bond Polarity Polar bonds in diatomic molecules can be detected by placing the molecules in an electric field. Electronegativity has several predictive uses, but differences in electronegativity and the resulting bonds must not be too rigid, particularly values between two types, e.g. 1.9 and 2.0. Conceptual Connection 9.3 Periodic Trends in Electronegativity A dipole moment is a physical measurement, so comparison with the predictions from EN is instructive. Conceptual Connection 9.4 Percent Ionic Character Bonds can be described as a continuum ranging from equal sharing of a pair of electrons between two atoms through degrees of polar covalent bonds to an ionic bond in which the electrons are completely transferred. 9.7 Lewis Structures of Molecular Compounds and Polyatomic Ions Students learn best how to draw Lewis structures from seeing and also working through lots of examples. Common errors in writing good Lewis structures include omitting lone pairs and omitting added or removed electrons in polyatomic ions. 9.8 Resonance and Formal Charge Resonance forms indicate that the actual structure can be represented by several equivalent Lewis structures. The analogy of resonance forms to dogs in Figure 9.11 is one that overcomes the urge to think of the Lewis structures as rapidly changing forms. Formal charges enable students to discriminate among different Lewis structures for a given molecule to determine which is better. Resonance does not arise from two or more interconverting forms. Two or more forms indicate a special situation in which the hybrid structure has special stability or properties, e.g. the different properties of benzene from other alkenes. Formal charges on constituent atoms in a Lewis structure can be confused with oxidation numbers. 131
9 Lecture Outline T erms, Concepts, Relationships, Skills Figures, Tables, and Solved Examples 9.9 Exceptions to the Octet Rule: Odd Electron Species, Incomplete Octets, and Expanded Octets Odd electron species o radicals or free radicals Incomplete octet o especially Be, B Expanded octet o 10, 12, or even 14 electrons around the central atom o impossible for 2nd period elements unnumbered figures: Lewis structures of NO and NO 2 Chemistry and the Environment: Free Radicals and the Atmospheric Vacuum Cleaner unnumbered figures: Lewis structures of BF 3, BH 3, NH 3, and BF 3 NH 3 unnumbered figures: Lewis structures of AsF5, SF6, and H 2 SO 4 Example 9.10 Writing Lewis Structures for Compounds Having Expanded Octets 9.10 Bond Energies and Bond Lengths Bond energies o breaking bonds: endothermic o forming bonds: exothermic o higher for mu ltiple bonds o average bond energy o estimation of H rxn Bond lengths o center to center distance between nuclei o shorter for multiple bonds unnumbered table: carbon carbon bond energies Table 9.3 Average Bond Energies Figure 9.12 Estimating Hrxn from Bond Energies Example 9.11 Calculating H rxn from Bond Energies Table 9.4 Average Bond Lengths unnumbered figures: molecular models, bond lengths of halogens unnumbered table: carbon carbon bond lengths unnumbered table: nitrogen halogen bond lengths 9.11 Bonding in Metals: The Electron Sea Model Microscopic properties o low ionization energies o electrons not attached to particular atoms Macroscopic properties o thermal and electrical conductivity o malleability o ductility Figure 9.13 The Electron Sea Model for Sodium Chemistry in the Environment: The Lewis Structure of Ozone unnumbered figure: photo of ductility of Cu 132
10 Teaching Tips S uggestions and Examples Misconceptions and Pitfalls 9.9 Exceptions to the Octet Rule: Odd Electron Species, Incomplete Octets, and Expanded Octets Conceptual Connection 9.5 Odd Electron Species Many radicals exist, especially if one considers organic examples. Incomplete octets are common for boron compounds, but the formal charge for boron when it makes three bonds is 0. Expanded octets are common for structures with P and S as well as for oxyanions of the halogens. Conceptual Connection 9.6 Expanded Octets 9.10 Bond Energies and Bond Lengths Average bond energies are useful for providing approximate values for H rxn. A bond energy for a bond being broken is positive, while that for a bond being formed is negative. Conceptual Connection 9.7 Bond Energies and H rxn Expanded octets apply only to central atoms and never to terminal atoms. When estimating H rxn, students are sometimes tempted to use products minus reactants as they did using enthalpies of formation Bonding in Metals: The Electron Sea Model Metals require a unique bonding model to account for many of their macroscopic properties, e.g. electrical conductivity. 133
11 Additional Problem for Classifying Bonds as Pure Covalent, Polar Covalent, or Ionic (Example 9.3) Determine whether the bond between each pair of atoms will be pure covalent, polar covalent or ionic: a) S and O b) Al and F c) C and Br d) Mg and Cl Solution Find the electronegativity values in Figure 9.10: S = 2.5 O = 3.5 Solution Find the electronegativity values in Figure 9.10: Al = 1.5 F = 4.0 Solution Find the electronegativity values in Figure 9.10: C = 2.5 Br = 2.8 Solution Find the electronegativity values in Figure 9.10: Mg = 1.2 Cl = 3.0 EN = 1.0 polar covalent EN = 2.5 ionic EN = 0.3 pure covalent EN = 1.8 polar covalent, near ionic 134
12 Additional Problem for Writing Lewis Structures (Examples 9.4, 9.5) Correct Skeletal Structure Write the correct skeletal structure for the molecule. Write a Lewis structure for CS 2. C is the same electronegativity as S but we put it in the center since there are two S. Write a Lewis structure for CH 3 Cl. C is less electronegative than Cl; H is always terminal. Number of Electrons Calculate the total number of electrons for the Lewis structure by summing the valence electrons of each atom in the molecule. Distribute Electrons Distribute the electrons among the atoms, giving octets (or duets for H) to as many atoms as possible. Begin with the bonding electrons and proceed to lone pairs on the central atom. C = 4 S = 6 S = 6 total = 16 First, bonding electrons. Next, lone pairs. C = 4 H = 1 H = 1 H = 1 Cl = 7 total = 14 First, bonding electrons. Next, lone pairs. Form Double of Triple Bonds If any atom lacks an octet, form double or triple bonds as necessary to give them octets. Move lone pairs from S to C. All H have duets. All other atoms have octets. The structure above is complete. 135
13 Additional Problem for Writing Lewis Structures for Polyatomic Ions (Example 9.6) Correct Skeletal Structure Write the correct skeletal structure for the molecule. Write a Lewis structure for NO 2. N is lower electronegativity than O and is at the center. Number of Electrons Calculate the total number of electrons for the Lewis structure by summing the valence electrons of each atom in the molecule. Distribute Electrons N = 5 O = 6 O = 6 charge = 1 total = 18 First, bonding electrons. Distribute the electrons among the atoms, giving octets (or duets for H) to as many atoms as possible. Begin with the bonding electrons and proceed to lone pairs on the central atom. Next, lone pairs. Form Double or Triple Bonds Move lone pairs from O to N. If any atom lacks an octet, form double or triple bonds as necessary to give them octets. 136
14 Additional Problem for Calculating H rxn from Bond Energies (Example 9.10) Hydrogen is considered an optimal fuel since it burns without forming any carbon dioxide. 2 H 2 (g) + O 2 (g) 2 H 2 O(g) Use bond energies to calculate H rxn. Equation Begin by writing the reaction using the Lewis structures of the molecules involved. Bonds Broken Determine which bonds are broken in the reaction and sum the bond energies of these. H H + H H + O=O H O H + H O H Bond broken, H 2 H H = 2(436 kj) 1 O=O = 1(498 kj) = 1370 kj Bonds Formed Determine which bonds are formed in the reaction and sum the negatives of the bond energies of these. Bond formed, H 4 H O = 4(464 kj) = 1856 kj Result Find H rxn by summing the results of the previous two steps. H rxn = = 486 kj 137
CHAPTER 6 Chemical Bonding
CHAPTER 6 Chemical Bonding SECTION 1 Introduction to Chemical Bonding OBJECTIVES 1. Define Chemical bond. 2. Explain why most atoms form chemical bonds. 3. Describe ionic and covalent bonding.. 4. Explain
More informationChapter 8 Concepts of Chemical Bonding
Chapter 8 Concepts of Chemical Bonding Chemical Bonds Three types: Ionic Electrostatic attraction between ions Covalent Sharing of electrons Metallic Metal atoms bonded to several other atoms Ionic Bonding
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 4: Structure and Properties of Ionic and Covalent Compounds
Chapter 4: Structure and Properties of Ionic and Covalent Compounds 4.1 Chemical Bonding o Chemical Bond - the force of attraction between any two atoms in a compound. o Interactions involving valence
More informationSample Exercise 8.1 Magnitudes of Lattice Energies
Sample Exercise 8.1 Magnitudes of Lattice Energies Without consulting Table 8.2, arrange the ionic compounds NaF, CsI, and CaO in order of increasing lattice energy. Analyze From the formulas for three
More informationIonic and Covalent Bonds
Ionic and Covalent Bonds Ionic Bonds Transfer of Electrons When metals bond with nonmetals, electrons are from the metal to the nonmetal The becomes a cation and the becomes an anion. The between the cation
More informationBonding & Molecular Shape Ron Robertson
Bonding & Molecular Shape Ron Robertson r2 n:\files\courses\1110-20\2010 possible slides for web\00bondingtrans.doc The Nature of Bonding Types 1. Ionic 2. Covalent 3. Metallic 4. Coordinate covalent Driving
More informationA pure covalent bond is an equal sharing of shared electron pair(s) in a bond. A polar covalent bond is an unequal sharing.
CHAPTER EIGHT BNDING: GENERAL CNCEPT or Review 1. Electronegativity is the ability of an atom in a molecule to attract electrons to itself. Electronegativity is a bonding term. Electron affinity is the
More informationWhich substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s)
BONDING MIDTERM REVIEW 7546-1 - Page 1 1) Which substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s) 2) The bond between hydrogen and oxygen in
More informationSample Exercise 8.1 Magnitudes of Lattice Energies
Sample Exercise 8.1 Magnitudes of Lattice Energies Without consulting Table 8.2, arrange the following ionic compounds in order of increasing lattice energy: NaF, CsI, and CaO. Analyze: From the formulas
More informationQuestions on Chapter 8 Basic Concepts of Chemical Bonding
Questions on Chapter 8 Basic Concepts of Chemical Bonding Circle the Correct Answer: 1) Which ion below has a noble gas electron configuration? A) Li 2+ B) Be 2+ C) B2+ D) C2+ E) N 2-2) Of the ions below,
More informationChapter 8 Basic Concepts of the Chemical Bonding
Chapter 8 Basic Concepts of the Chemical Bonding 1. There are paired and unpaired electrons in the Lewis symbol for a phosphorus atom. (a). 4, 2 (b). 2, 4 (c). 4, 3 (d). 2, 3 Explanation: Read the question
More information3/5/2014. iclicker Participation Question: A. MgS < AlP < NaCl B. MgS < NaCl < AlP C. NaCl < AlP < MgS D. NaCl < MgS < AlP
Today: Ionic Bonding vs. Covalent Bonding Strengths of Covalent Bonds: Bond Energy Diagrams Bond Polarities: Nonpolar Covalent vs. Polar Covalent vs. Ionic Electronegativity Differences Dipole Moments
More informationIn the box below, draw the Lewis electron-dot structure for the compound formed from magnesium and oxygen. [Include any charges or partial charges.
Name: 1) Which molecule is nonpolar and has a symmetrical shape? A) NH3 B) H2O C) HCl D) CH4 7222-1 - Page 1 2) When ammonium chloride crystals are dissolved in water, the temperature of the water decreases.
More informationch9 and 10 practice test
1. Which of the following covalent bonds is the most polar (highest percent ionic character)? A. Al I B. Si I C. Al Cl D. Si Cl E. Si P 2. What is the hybridization of the central atom in ClO 3? A. sp
More informationCHEMISTRY BONDING REVIEW
Answer the following questions. CHEMISTRY BONDING REVIEW 1. What are the three kinds of bonds which can form between atoms? The three types of Bonds are Covalent, Ionic and Metallic. Name Date Block 2.
More informationBonding Practice Problems
NAME 1. When compared to H 2 S, H 2 O has a higher 8. Given the Lewis electron-dot diagram: boiling point because H 2 O contains stronger metallic bonds covalent bonds ionic bonds hydrogen bonds 2. Which
More informationCHAPTER 6 REVIEW. Chemical Bonding. Answer the following questions in the space provided.
Name Date lass APTER 6 REVIEW hemical Bonding SETIN 1 SRT ANSWER Answer the following questions in the space provided. 1. a A chemical bond between atoms results from the attraction between the valence
More informationA mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together is called a(n)
Chemistry I ATOMIC BONDING PRACTICE QUIZ Mr. Scott Select the best answer. 1) A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together is
More informationLewis Dot Notation Ionic Bonds Covalent Bonds Polar Covalent Bonds Lewis Dot Notation Revisited Resonance
Lewis Dot Notation Ionic Bonds Covalent Bonds Polar Covalent Bonds Lewis Dot Notation Revisited Resonance Lewis Dot notation is a way of describing the outer shell (also called the valence shell) of an
More informationDCI for Electronegativity. Data Table:
DCI for Electronegativity Data Table: Substance Ionic/covalent EN value EN Value EN NaCl ionic (Na) 0.9 (Cl) 3.0 2.1 KBr (K) 0.8 (Br) 2.8 MgO (Mg) 1.2 (O) 3.5 HCl (H) 2.1 (Cl) 3.0 HF (H) 2.1 (F) 4.0 Cl
More informationQuestion 4.2: Write Lewis dot symbols for atoms of the following elements: Mg, Na, B, O, N, Br.
Question 4.1: Explain the formation of a chemical bond. A chemical bond is defined as an attractive force that holds the constituents (atoms, ions etc.) together in a chemical species. Various theories
More informationCHAPTER 12: CHEMICAL BONDING
CHAPTER 12: CHEMICAL BONDING Active Learning Questions: 3-9, 11-19, 21-22 End-of-Chapter Problems: 1-36, 41-59, 60(a,b), 61(b,d), 62(a,b), 64-77, 79-89, 92-101, 106-109, 112, 115-119 An American chemist
More informationChapter 7. Comparing Ionic and Covalent Bonds. Ionic Bonds. Types of Bonds. Quick Review of Bond Types. Covalent Bonds
Comparing Ionic and Covalent Bonds Chapter 7 Covalent Bonds and Molecular Structure Intermolecular forces (much weaker than bonds) must be broken Ionic bonds must be broken 1 Ionic Bonds Covalent Bonds
More informationEXPERIMENT 9 Dot Structures and Geometries of Molecules
EXPERIMENT 9 Dot Structures and Geometries of Molecules INTRODUCTION Lewis dot structures are our first tier in drawing molecules and representing bonds between the atoms. The method was first published
More informationBonds. Bond Length. Forces that hold groups of atoms together and make them function as a unit. Bond Energy. Chapter 8. Bonding: General Concepts
Bonds hapter 8 Bonding: General oncepts Forces that hold groups of atoms together and make them function as a unit. Bond Energy Bond Length It is the energy required to break a bond. The distance where
More informationWe will not be doing these type of calculations however, if interested then can read on your own
Chemical Bond Lattice Energies and Types of Ions Na (s) + 1/2Cl 2 (g) NaCl (s) ΔH= -411 kj/mol Energetically favored: lower energy Like a car rolling down a hill We will not be doing these type of calculations
More informationPOLAR COVALENT BONDS Ionic compounds form repeating. Covalent compounds form distinct. Consider adding to NaCl(s) vs. H 2 O(s):
POLAR COVALENT BONDS Ionic compounds form repeating. Covalent compounds form distinct. Consider adding to NaCl(s) vs. H 2 O(s): Sometimes when atoms of two different elements form a bond by sharing an
More informationB) atomic number C) both the solid and the liquid phase D) Au C) Sn, Si, C A) metal C) O, S, Se C) In D) tin D) methane D) bismuth B) Group 2 metal
1. The elements on the Periodic Table are arranged in order of increasing A) atomic mass B) atomic number C) molar mass D) oxidation number 2. Which list of elements consists of a metal, a metalloid, and
More informationChapter 2 Polar Covalent Bonds: Acids and Bases
John E. McMurry www.cengage.com/chemistry/mcmurry Chapter 2 Polar Covalent Bonds: Acids and Bases Modified by Dr. Daniela R. Radu Why This Chapter? Description of basic ways chemists account for chemical
More informationLaboratory 11: Molecular Compounds and Lewis Structures
Introduction Laboratory 11: Molecular Compounds and Lewis Structures Molecular compounds are formed by sharing electrons between non-metal atoms. A useful theory for understanding the formation of molecular
More informationChapter 6 Assessment. Name: Class: Date: ID: A. Multiple Choice Identify the choice that best completes the statement or answers the question.
Name: Class: Date: ID: A Chapter 6 Assessment Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When an atom loses an electron, it forms a(n) a. anion. c.
More informationMolecular Geometry and VSEPR We gratefully acknowledge Portland Community College for the use of this experiment.
Molecular and VSEPR We gratefully acknowledge Portland ommunity ollege for the use of this experiment. Objectives To construct molecular models for covalently bonded atoms in molecules and polyatomic ions
More informationTheme 3: Bonding and Molecular Structure. (Chapter 8)
Theme 3: Bonding and Molecular Structure. (Chapter 8) End of Chapter questions: 5, 7, 9, 12, 15, 18, 23, 27, 28, 32, 33, 39, 43, 46, 67, 77 Chemical reaction valence electrons of atoms rearranged (lost,
More informationChapter 13 - LIQUIDS AND SOLIDS
Chapter 13 - LIQUIDS AND SOLIDS Problems to try at end of chapter: Answers in Appendix I: 1,3,5,7b,9b,15,17,23,25,29,31,33,45,49,51,53,61 13.1 Properties of Liquids 1. Liquids take the shape of their container,
More informationA PREVIEW & SUMMMARY of the 3 main types of bond:
Chemical Bonding Part 1 Covalent Bonding Types of Chemical Bonds Covalent Bonds Single Polar Double NonPolar Triple Ionic Bonds Metallic Bonds Other Bonds InterMolecular orces first A PREVIEW & SUMMMARY
More informationEXPERIMENT # 17 CHEMICAL BONDING AND MOLECULAR POLARITY
EXPERIMENT # 17 CHEMICAL BONDING AND MOLECULAR POLARITY Purpose: 1. To distinguish between different types of chemical bonds. 2. To predict the polarity of some common molecules from a knowledge of bond
More informationChemistry 1050 Chapter 13 LIQUIDS AND SOLIDS 1. Exercises: 25, 27, 33, 39, 41, 43, 51, 53, 57, 61, 63, 67, 69, 71(a), 73, 75, 79
Chemistry 1050 Chapter 13 LIQUIDS AND SOLIDS 1 Text: Petrucci, Harwood, Herring 8 th Edition Suggest text problems Review questions: 1, 5!11, 13!17, 19!23 Exercises: 25, 27, 33, 39, 41, 43, 51, 53, 57,
More information4.5 Physical Properties: Solubility
4.5 Physical Properties: Solubility When a solid, liquid or gaseous solute is placed in a solvent and it seems to disappear, mix or become part of the solvent, we say that it dissolved. The solute is said
More informationType of Chemical Bonds
Type of Chemical Bonds Covalent bond Polar Covalent bond Ionic bond Hydrogen bond Metallic bond Van der Waals bonds. Covalent Bonds Covalent bond: bond in which one or more pairs of electrons are shared
More informationChemistry 11 Some Study Materials for the Final Exam
Chemistry 11 Some Study Materials for the Final Exam Prefix Abbreviation Exponent giga G 10 9 mega M 10 6 kilo k 10 3 hecto h 10 2 deca da 10 1 deci d 10-1 centi c 10-2 milli m 10-3 micro µ 10-6 nano n
More informationName Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question.
Assessment Chapter Test A Chapter: States of Matter In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. The kinetic-molecular
More informationIntroduction to Chemistry. Course Description
CHM 1025 & CHM 1025L Introduction to Chemistry Course Description CHM 1025 Introduction to Chemistry (3) P CHM 1025L Introduction to Chemistry Laboratory (1) P This introductory course is intended to introduce
More informationSOME TOUGH COLLEGE PROBLEMS! .. : 4. How many electrons should be shown in the Lewis dot structure for carbon monoxide? N O O
SME TUGH CLLEGE PRBLEMS! LEWIS DT STRUCTURES 1. An acceptable Lewis dot structure for 2 is (A) (B) (C) 2. Which molecule contains one unshared pair of valence electrons? (A) H 2 (B) H 3 (C) CH 4 acl 3.
More informationEXPERIMENT 17 : Lewis Dot Structure / VSEPR Theory
EXPERIMENT 17 : Lewis Dot Structure / VSEPR Theory Materials: Molecular Model Kit INTRODUCTION Although it has recently become possible to image molecules and even atoms using a high-resolution microscope,
More informationName Class Date. What is ionic bonding? What happens to atoms that gain or lose electrons? What kinds of solids are formed from ionic bonds?
CHAPTER 1 2 Ionic Bonds SECTION Chemical Bonding BEFORE YOU READ After you read this section, you should be able to answer these questions: What is ionic bonding? What happens to atoms that gain or lose
More informationCHAPTER 10: INTERMOLECULAR FORCES: THE UNIQUENESS OF WATER Problems: 10.2, 10.6,10.15-10.33, 10.35-10.40, 10.56-10.60, 10.101-10.
CHAPTER 10: INTERMOLECULAR FORCES: THE UNIQUENESS OF WATER Problems: 10.2, 10.6,10.15-10.33, 10.35-10.40, 10.56-10.60, 10.101-10.102 10.1 INTERACTIONS BETWEEN IONS Ion-ion Interactions and Lattice Energy
More informationChapter 2: The Chemical Context of Life
Chapter 2: The Chemical Context of Life Name Period This chapter covers the basics that you may have learned in your chemistry class. Whether your teacher goes over this chapter, or assigns it for you
More informationSurvival Organic Chemistry Part I: Molecular Models
Survival Organic Chemistry Part I: Molecular Models The goal in this laboratory experience is to get you so you can easily and quickly move between empirical formulas, molecular formulas, condensed formulas,
More informationChapter 17. How are acids different from bases? Acid Physical properties. Base. Explaining the difference in properties of acids and bases
Chapter 17 Acids and Bases How are acids different from bases? Acid Physical properties Base Physical properties Tastes sour Tastes bitter Feels slippery or slimy Chemical properties Chemical properties
More information7.4. Using the Bohr Theory KNOW? Using the Bohr Theory to Describe Atoms and Ions
7.4 Using the Bohr Theory LEARNING TIP Models such as Figures 1 to 4, on pages 218 and 219, help you visualize scientific explanations. As you examine Figures 1 to 4, look back and forth between the diagrams
More information(b) Formation of calcium chloride:
Chapter 2: Chemical Compounds and Bonding Section 2.1: Ionic Compounds, pages 22 23 1. An ionic compound combines a metal and a non-metal joined together by an ionic bond. 2. An electrostatic force holds
More informationWriting and Balancing Chemical Equations
Name Writing and Balancing Chemical Equations Period When a substance undergoes a chemical reaction, chemical bonds are broken and new bonds are formed. This results in one or more new substances, often
More informationUnit 2 Periodic Behavior and Ionic Bonding
Unit 2 Periodic Behavior and Ionic Bonding 6.1 Organizing the Elements I. The Periodic Law A. The physical and chemical properties of the elements are periodic functions of their atomic numbers B. Elements
More informationChapter 2 Polar Covalent Bonds; Acids and Bases
John E. McMurry http://www.cengage.com/chemistry/mcmurry Chapter 2 Polar Covalent Bonds; Acids and Bases Javier E. Horta, M.D., Ph.D. University of Massachusetts Lowell Polar Covalent Bonds: Electronegativity
More informationChemistry Workbook 2: Problems For Exam 2
Chem 1A Dr. White Updated /5/1 1 Chemistry Workbook 2: Problems For Exam 2 Section 2-1: Covalent Bonding 1. On a potential energy diagram, the most stable state has the highest/lowest potential energy.
More informationWe emphasize Lewis electron dot structures because of their usefulness in explaining structure of covalent molecules, especially organic molecules.
Chapter 10 Bonding: Lewis electron dot structures and more Bonding is the essence of chemistry! Not just physics! Chemical bonds are the forces that hold atoms together in molecules, in ionic compounds,
More informationCHEMISTRY STANDARDS BASED RUBRIC ATOMIC STRUCTURE AND BONDING
CHEMISTRY STANDARDS BASED RUBRIC ATOMIC STRUCTURE AND BONDING Essential Standard: STUDENTS WILL UNDERSTAND THAT THE PROPERTIES OF MATTER AND THEIR INTERACTIONS ARE A CONSEQUENCE OF THE STRUCTURE OF MATTER,
More information19.1 Bonding and Molecules
Most of the matter around you and inside of you is in the form of compounds. For example, your body is about 80 percent water. You learned in the last unit that water, H 2 O, is made up of hydrogen and
More informationIonization energy _decreases from the top to the bottom in a group. Electron affinity increases from the left to the right within a period.
hem 150 Answer Key roblem et 2 1. omplete the following phrases: Ionization energy _decreases from the top to the bottom in a group. Electron affinity increases from the left to the right within a period.
More informationChapter 4 Lecture Notes
Chapter 4 Lecture Notes Chapter 4 Educational Goals 1. Given the formula of a molecule, the student will be able to draw the line-bond (Lewis) structure. 2. Understand and construct condensed structural
More informationH 2O gas: molecules are very far apart
Non-Covalent Molecular Forces 2/27/06 3/1/06 How does this reaction occur: H 2 O (liquid) H 2 O (gas)? Add energy H 2O gas: molecules are very far apart H 2O liquid: bonding between molecules Use heat
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
CHE 1401 - Fall 2013 - Chapter 8 Homework 8 (Chapter 8: Basic concepts of chemical bonding) MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Of
More informationExercises Topic 2: Molecules
hemistry for Biomedical Engineering. Exercises Topic 2 Authors: ors: Juan Baselga & María González Exercises Topic 2: Molecules 1. Using hybridization concepts and VSEPR model describe the molecular geometry
More informationList the 3 main types of subatomic particles and indicate the mass and electrical charge of each.
Basic Chemistry Why do we study chemistry in a biology course? All living organisms are composed of chemicals. To understand life, we must understand the structure, function, and properties of the chemicals
More informationExam 2 Chemistry 65 Summer 2015. Score:
Name: Exam 2 Chemistry 65 Summer 2015 Score: Instructions: Clearly circle the one best answer 1. Valence electrons are electrons located A) in the outermost energy level of an atom. B) in the nucleus of
More information2. Which one of the ions below possesses a noble gas configuration? A) Fe 3+ B) Sn 2+ C) Ni 2+ D) Ti 4+ E) Cr 3+
Chapter 9 Tro 1. Bromine tends to form simple ions which have the electronic configuration of a noble gas. What is the electronic configuration of the noble gas which the bromide ion mimics? A) 1s 2 2s
More informationEXPERIMENT 1: Survival Organic Chemistry: Molecular Models
EXPERIMENT 1: Survival Organic Chemistry: Molecular Models Introduction: The goal in this laboratory experience is for you to easily and quickly move between empirical formulas, molecular formulas, condensed
More informationPeriodic Table Questions
Periodic Table Questions 1. The elements characterized as nonmetals are located in the periodic table at the (1) far left; (2) bottom; (3) center; (4) top right. 2. An element that is a liquid at STP is
More information1.2 CLASSICAL THEORIES OF CHEMICAL BONDING
1. CLASSICAL TEORIES OF CEMICAL BONDING simply memorizing them. We ll consider some of the organic chemistry that is industrially important. Finally, we ll examine some of the beautiful applications of
More informationChapter 2 Polar Covalent Bond Covalent bond in which the electron pairs are not shared equally.
hapter 2 Polar ovalent Bond ovalent bond in which the electron pairs are not shared equally. Pure ovalent Bond (non-polar) increasing bond polarity Ionic Bond X X X Y X + Y - Electronegativity, c ability
More informationLewis Dot Structures of Atoms and Ions
Why? The chemical properties of an element are based on the number of electrons in the outer shell of its atoms. We use Lewis dot structures to map these valence electrons in order to identify stable electron
More informationHealth Science Chemistry I CHEM-1180 Experiment No. 15 Molecular Models (Revised 05/22/2015)
(Revised 05/22/2015) Introduction In the early 1900s, the chemist G. N. Lewis proposed that bonds between atoms consist of two electrons apiece and that most atoms are able to accommodate eight electrons
More information19.2 Chemical Formulas
In the previous section, you learned how and why atoms form chemical bonds with one another. You also know that atoms combine in certain ratios with other atoms. These ratios determine the chemical formula
More informationName: Date: Period: Presentation #4. Covalent compounds continued practice with drawing them. Modeling covalent compounds in 3D
Homework Activities Name: Date: Period: This week we will practice creating covalent compounds through drawings and 3D models. We will also look at polar and non-polar molecules to see how their structures
More informationSelf Assessment_Ochem I
UTID: 2013 Objective Test Section Identify the choice that best completes the statement or answers the question. There is only one correct answer; please carefully bubble your choice on the scantron sheet.
More informationLEWIS DIAGRAMS. by DR. STEPHEN THOMPSON MR. JOE STALEY
by DR. STEPHEN THOMPSON MR. JOE STALEY The contents of this module were developed under grant award # P116B-001338 from the Fund for the Improvement of Postsecondary Education (FIPSE), United States Department
More informationChemistry B11 Chapter 4 Chemical reactions
Chemistry B11 Chapter 4 Chemical reactions Chemical reactions are classified into five groups: A + B AB Synthesis reactions (Combination) H + O H O AB A + B Decomposition reactions (Analysis) NaCl Na +Cl
More informationBonding in Elements and Compounds. Covalent
Bonding in Elements and Compounds Structure of solids, liquids and gases Types of bonding between atoms and molecules Ionic Covalent Metallic Many compounds between metals & nonmetals (salts), e.g. Na,
More information5. Structure, Geometry, and Polarity of Molecules
5. Structure, Geometry, and Polarity of Molecules What you will accomplish in this experiment This experiment will give you an opportunity to draw Lewis structures of covalent compounds, then use those
More information6.5 Periodic Variations in Element Properties
324 Chapter 6 Electronic Structure and Periodic Properties of Elements 6.5 Periodic Variations in Element Properties By the end of this section, you will be able to: Describe and explain the observed trends
More informationA REVIEW OF GENERAL CHEMISTRY: ELECTRONS, BONDS AND MOLECULAR PROPERTIES
A REVIEW OF GENERAL CEMISTRY: ELECTRONS, BONDS AND MOLECULAR PROPERTIES A STUDENT SOULD BE ABLE TO: 1. Draw Lewis (electron dot and line) structural formulas for simple compounds and ions from molecular
More information: : Solutions to Additional Bonding Problems
Solutions to Additional Bonding Problems 1 1. For the following examples, the valence electron count is placed in parentheses after the empirical formula and only the resonance structures that satisfy
More informationPERIODIC TABLE OF THE ELEMENTS
PERIODIC TABLE OF THE ELEMENTS Periodic Table: an arrangement of elements in horizontal rows (Periods) and vertical columns (Groups) exhibits periodic repetition of properties First Periodic Table: discovered
More informationStart: 26e Used: 6e Step 4. Place the remaining valence electrons as lone pairs on the surrounding and central atoms.
Section 4.1: Types of Chemical Bonds Tutorial 1 Practice, page 200 1. (a) Lewis structure for NBr 3 : Step 1. The central atom for nitrogen tribromide is bromine. 1 N atom: 1(5e ) = 5e 3 Br atoms: 3(7e
More informationSection Activity #1: Fill out the following table for biology s most common elements assuming that each atom is neutrally charged.
LS1a Fall 2014 Section Week #1 I. Valence Electrons and Bonding The number of valence (outer shell) electrons in an atom determines how many bonds it can form. Knowing the number of valence electrons present
More informationTrends of the Periodic Table Basics
Trends of the Periodic Table Basics Trends are patterns of behaviors that atoms on the periodic table of elements follow. Trends hold true most of the time, but there are exceptions, or blips, where the
More informationName period Unit 3 worksheet
Name period Unit 3 worksheet Read chapter 8, 2.52.7 1. Explain the difference between metallic, ionic, and covalent bonding Metallic cations share a sea of electrons Ionic atoms give and take electrons
More informationIonic and Metallic Bonding
Ionic and Metallic Bonding BNDING AND INTERACTINS 71 Ions For students using the Foundation edition, assign problems 1, 3 5, 7 12, 14, 15, 18 20 Essential Understanding Ions form when atoms gain or lose
More informationChemical Equations and Chemical Reactions. Chapter 8.1
Chemical Equations and Chemical Reactions Chapter 8.1 Objectives List observations that suggest that a chemical reaction has taken place List the requirements for a correctly written chemical equation.
More informationChapter 6 An Overview of Organic Reactions
John E. McMurry www.cengage.com/chemistry/mcmurry Chapter 6 An Overview of Organic Reactions Why this chapter? To understand organic and/or biochemistry, it is necessary to know: -What occurs -Why and
More informationCHAPTER 10 THE SHAPES OF MOLECULES
ATER 10 TE AE MLEULE EMIAL ETI BED READIG RBLEM B10.1 lan: Examine the Lewis structure, noting the number of regions of electron density around the carbon and nitrogen atoms in the two resonance structures.
More informationWorksheet 14 - Lewis structures. 1. Complete the Lewis dot symbols for the oxygen atoms below
Worksheet 14 - Lewis structures Determine the Lewis structure of 2 oxygen gas. 1. omplete the Lewis dot symbols for the oxygen atoms below 2. Determine the number of valence electrons available in the
More informationSummer Holidays Questions
Summer Holidays Questions Chapter 1 1) Barium hydroxide reacts with hydrochloric acid. The initial concentration of the 1 st solution its 0.1M and the volume is 100ml. The initial concentration of the
More informationChapter 11. Electrochemistry Oxidation and Reduction Reactions. Oxidation-Reduction Reactions. Oxidation-Reduction Reactions
Oxidation-Reduction Reactions Chapter 11 Electrochemistry Oxidation and Reduction Reactions An oxidation and reduction reaction occurs in both aqueous solutions and in reactions where substances are burned
More informationStructure, Polarity & Physical Properties
tructure, Polarity & Physical Properties upplemental packet handouts 92-96 I. Lewis structure, stability, and bond energies A. ydrogen, oxygen, and nitrogen are present in the atmosphere as diatomic molecular
More informationOrder of Filling Subshells
Bonding: General Concepts Ionic Bonds Sections 13.2-13.6 Covalent Bonds Section 13.7 Covalent Bond Energy & Chemical Reactions Section 13.8-13.9 Lewis Structures Sections 13.10-13.12 VSEPR Theory Section
More informationMolecular Geometry & Polarity
Name AP Chemistry Molecular Geometry & Polarity Molecular Geometry A key to understanding the wide range of physical and chemical properties of substances is recognizing that atoms combine with other atoms
More informationChemistry. The student will be able to identify and apply basic safety procedures and identify basic equipment.
Chemistry UNIT I: Introduction to Chemistry The student will be able to describe what chemistry is and its scope. a. Define chemistry. b. Explain that chemistry overlaps many other areas of science. The
More informationTest Bank - Chapter 4 Multiple Choice
Test Bank - Chapter 4 The questions in the test bank cover the concepts from the lessons in Chapter 4. Select questions from any of the categories that match the content you covered with students. The
More information