CHAPTER 6 Chemical Bonding
|
|
|
- Imogen Ross
- 7 years ago
- Views:
Transcription
1 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 why most chemical bonding is neither purely ionic or purley 5. Classify bonding type according to electronegativity differences. SECTION 2 Covalent Bonding and Molecular Compounds OBJECTIVES 1. Define molecule and molecular formula. 2. Explain the relationships among potential energy, distance between approaching atoms, bonds length and bond energy. 3. State the octet rule. 4. List the six basic steps used in writing Lewis dot Structures. 5. Explain how to determine Lewis structures for molecules containing single bonds, multiple bonds or both. 6. Explain why scientists use resonance structures to represent some molecules. SECTION 3 Ionic Bonding and Ionic compounds OBJECTIVES 1. Compare and contrast the chemical formula for a molecular compound wit one for an ionic compound. 2. Discuss the arrangements of ions in crystals. 3. Define lattice energy and explain its significance. 4. List and compare the distinctive properties of ionic and molecular compounds. 5. Write the Lewis structure for a polyatomic ion given the identity of the atoms combined and other appropriate information. Modern Chemistry 1 Chemical Bonding
2 SECTION 4 Metallic Bonding OBJECTIVES 1. Describe the electron-sea model of metallic bonding, and explain why metals are good electrical conductors. 2. Explain why metal surfaces are shinny. 3. Explain why metals are malleable and ductile but ionic crystalline compounds are not. SECTION 5 Molecular Geometry OBJECTIVES 1. Explain VSEPR theory. 2. Predict the shapes of molecules or polyatomic ionis using VSEPR theory. 3. Explain how the shapes of molecules are accounted for by hybridization theory. 4. Describe dipole dipole forces, hydrogen bonding, induced dipoles and London Dispersion Forces and their effects on properties such as boiling point and melting point. 5. Explain what determines molecular polarity. Modern Chemistry 2 Chemical Bonding
3 Chapter 6 Vocabulary Chemical Bonding Sec 6-1 Introduction to Chemical Bonding Chemical bond Nonpolar covalent bond Ionic bonding Polar Covalent bonding Polar covalent bond Sec 6-2 Covalent Bonding and Molecular Compounds Molecule Electron dot notation Molecular compound Lewis structure Chemical formula Single bond Molecular formula Multiple bond Bond energy resonance Sec 6-3 Ionic Bonding and Ionic Compounds Ionic compound Lattice energy Formula unit Polyatomic ion Sec 6-4 Metallic Bonding Metallic bonding Malleability ductility Sec 6-5 Molecular Geometry VSEPR theory Hybridization hybrid orbitals Intramolecular force Intermolecular force dipole hydrogen bonding London dispersion forces Modern Chemistry 3 Chemical Bonding
4 Modern Chemistry 4 Chemical Bonding
5 CHAPTER 6 STUDY GUIDE Chemical Bonding SECTION 1 INTRODUCTION TO CHEMICAL BONDING SHORT ANSWER Answer the following questions in the space provided. 1. A chemical bond between atoms results from the attraction between the valence electrons and of different atoms. (a) nuclei (c) isotopes (b) inner electrons (d) Lewis structures 2. A covalent bond consists of (a) a shared electron. (b) a shared electron pair. (c) two different ions. (d) an octet of electrons. 3. If two covalently bonded atoms are identical, the bond is identified as (a) nonpolar covalent. (c) ionic. (b) polar covalent. (d) dipolar. 4. A covalent bond in which there is an unequal attraction for the shared electrons is (a) nonpolar. (c) ionic. (b) polar. (d) dipolar. 5. Atoms with a strong attraction for electrons they share with another atom exhibit (a) zero electronegativity. (c) high electronegativity. (b) low electronegativity. (d) Lewis electronegativity. 6. Bonds that possess between 5 and 50 ionic character are considered to be (a) ionic. (c) polar covalent. (b) pure covalent. (d) nonpolar covalent. 7. The greater the electronegativity difference between two atoms bonded together, the greater the bond s percentage of (a) ionic character. (c) metallic character. (b) nonpolar character. (d) electron sharing. 8. The electrons involved in the formation of a chemical bond are called. 9. A chemical bond that results from the electrostatic attraction between positive and ionic bond negative ions is called a(n). Modern Chemistry 5 Chemical Bonding
6 SECTION 1 continued 10. If electrons involved in bonding spend most of the time closer to one atom rather than the other, the bond is. 11. If a bond s character is more than 50 ionic, then the bond is called a(n). 12. A bond s character is more than 50 ionic if the electronegativity difference between the two atoms is greater than. 13. Write the formula for an example of each of the following compounds: Answers will vary. a. nonpolar covalent compound b. polar covalent compound c. ionic compound 14. Describe how a covalent bond holds two atoms together. 15. What property of the two atoms in a covalent bond determines whether or not the bond will be polar? 16. How can electronegativity be used to distinguish between an ionic bond and a covalent bond? 17. Describe the electron distribution in a polar-covalent bond and its effect on the partial charges of the compound. Modern Chemistry 6 Chemical Bonding
7 CHAPTER 6 STUDY GUIDE Chemical Bonding SECTION 2 COVALENT BONDING AND MOLECULAR COMPOUNDS SHORT ANSWER Answer the following questions in the space provided. 1. Use the concept of potential energy to describe how a covalent bond forms between two atoms. 2. Name two elements that form compounds that can be exceptions to the octet rule. 3. Explain why resonance structures are used instead of Lewis structures to correctly model certain molecules. 4. Bond energy is related to bond length. Use the data in the tables below to arrange the bonds listed in order of increasing bond length, from shortest bond to longest. a. Bond Bond energy (kj/mol) H F 569 H I 299 H Cl 432 H Br 366 Modern Chemistry 7 Chemical Bonding
8 SECTION 2 continued b. Bond Bond energy (kj/mol) C C 346 C C 835 C C Draw Lewis structures to represent each of the following formulas: a. NH 3 b. H 2 O c. CH 4 d. C 2 H 2 e. CH 2 O Modern Chemistry 8 Chemical Bonding
9 CHAPTER 6 STUDY GUIDE Chemical Bonding SECTION 3 IONIC BONDING AND IONIC COMPOUNDS SHORT ANSWER Answer the following questions in the space provided. 1. The notation for sodium chloride, NaCl, stands for one (a) formula unit. (c) crystal. (b) molecule. (d) atom. 2. In a crystal of an ionic compound, each cation is surrounded by a number of (a) molecules. (c) dipoles. (b) positive ions. (d) negative ions. 3. Compared with the neutral atoms involved in the formation of an ionic compound, the crystal lattice that results is (a) higher in potential energy. (c) equal in potential energy. (b) lower in potential energy. (d) unstable. 4. The lattice energy of compound A is greater in magnitude than that of compound B. What can be concluded from this fact? (a) Compound A is not an ionic compound. (b) It will be more difficult to break the bonds in compound A than those in compound B. (c) Compound B has larger crystals than compound A. (d) Compound A has larger crystals than compound B. 5. The forces of attraction between molecules in a molecular compound are generally (a) stronger than the attractive forces among formula units in ionic bonding. (b) weaker than the attractive forces among formula units in ionic bonding. (c) approximately equal to the attractive forces among formula units in ionic bonding. (d) equal to zero. 6. Describe the force that holds two ions together in an ionic bond. 7. What type of energy best represents the strength of an ionic bond? Modern Chemistry 9 Chemical Bonding
10 SECTION 3 continued 8. What types of bonds are present in an ionic compound that contains a polyatomic ion? 9. Arrange the ionic bonds in the table below in order of increasing strength from weakest to strongest. Ionic bond NaCl 787 CaO 3384 KCl 715 MgO 3760 LiCl 861 Lattice energy (kj/mol) 10. Draw Lewis structures for the following polyatomic ions: a. NH 4 b. 2 SO Draw the two resonance structures for the nitrite anion, NO 2. Modern Chemistry 10 Chemical Bonding
11 CHAPTER 6 STUDY GUIDE Chemical Bonding SECTION 4 METALLIC BONDING SHORT ANSWER Answer the following questions in the space provided. 1. In metals, the valence electrons are considered to be (a) attached to particular positive ions. (c) immobile. (b) shared by all surrounding atoms.(d) involved in covalent bonds. 2. The fact that metals are malleable and ionic crystals are brittle is best explained in terms of their (a) chemical bonds. (c) enthalpies of vaporization. (b) London forces. (d) polarity. 3. As light strikes the surface of a metal, the electrons in the electron sea (a) allow the light to pass through. (b) become attached to particular positive ions. (c) fall to lower energy levels. (d) absorb and re-emit the light. 4. Mobile electrons in the metallic bond are responsible for (a) luster. (c) electrical conductivity. (b) thermal conductivity. (d) All of the above. 5. In general, the strength of the metallic bond moving from left to right on any row of the periodic table. (a) increases (c) remains the same (b) decreases (d) varies 6. When a metal is drawn into a wire, the metallic bonds (a) break easily. (c) do not break. (b) break with difficulty. (d) become ionic bonds. 7. Use the concept of electron configurations to explain why the number of valence electrons in metals tends to be less than the number in most nonmetals. Modern Chemistry 11 Chemical Bonding
12 SECTION 4 continued 8. How does the behavior of electrons in metals contribute to the metal s ability to conduct electricity and heat? 9. What is the relationship between the enthalpy of vaporization of a metal and the strength of the bonds that hold the metal together? 10. Draw two diagrams of a metallic bond. In the first diagram, draw a weak metallic bond; in the second, show a metallic bond that would be stronger. Be sure to include nuclear charge and number of electrons in your illustrations. a. b. Note: In the strong bond, the charge on the nucleus and the number of electrons must be greater than in the weak bond. 11. Complete the following table: Components Overall charge Conductive in the solid state Melting point Hardness Malleable Ductile Metals Ionic Compounds Modern Chemistry 12 Chemical Bonding
13 CHAPTER 6 STUDY GUIDE Chemical Bonding SECTION 5 MOLECULAR GEOMETRY SHORT ANSWER Answer the following questions in the space provided. 1. Identify the major assumption of the VSEPR theory, which is used to predict the shape of atoms. 2. In water, two hydrogen atoms are bonded to one oxygen atom. Why isn t water a linear molecule? 3. What orbitals combine together to form sp 3 hybrid orbitals around a carbon atom? 4. What two factors determine whether or not a molecule is polar? 5. Arrange the following types of attractions in order of increasing strength, with 1 being the weakest and 4 the strongest. hydrogen bonding ionic dipole-dipole London dispersion 6. How are dipole-dipole attractions, London dispersion forces, and hydrogen bonding similar? Modern Chemistry 13 Chemical Bonding
14 SECTION 5 continued 7. Complete the following table: Formula Lewis structure Geometry Polar H 2 S CCl 4 BF 3 H 2 O PCl 5 BeF 2 SF 6 Modern Chemistry 14 Chemical Bonding
15 CHAPTER 6 STUDY GUIDE Chemical Bonding MIXED REVIEW SHORT ANSWER Answer the following questions in the space provided. 1. Name the type of energy that is a measure of strength for each of the following types of bonds: a. ionic bond b. covalent bond c. metallic bond 2. Use the electronegativity values shown in Figure 20, on page 161 of the text, to determine whether each of the following bonds is nonpolar covalent, polar covalent, or ionic. a. H b. Na c. H O F Cl d. H e. H f. H 3. How is a hydrogen bond different from an ionic or covalent bond? 4. H 2 S and H 2 O have similar structures and their central atoms belong to the same group. Yet H 2 S is a gas at room temperature and H 2 O is a liquid. Use bonding principles to explain why this is. Modern Chemistry 15 Chemical Bonding H C N
16 MIXED REVIEW continued 5. In what way is a polar-covalent bond similar to an ionic bond? 6. Draw a Lewis structure for each of the following formulas. Determine whether the molecule is polar or nonpolar. a. H 2 S b. COCl 2 c. PCl 3 d. CH 2 O. Modern Chemistry 16 Chemical Bonding
CHAPTER 6 REVIEW. Chemical Bonding. Answer the following questions in the space provided.
Name Date lass APTER 6 REVIEW hemical Bonding SETIN 1 SRT ANSWER Answer the following questions in the space provided. 1. a A chemical bond between atoms results from the attraction between the valence
A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together is called a(n)
Chemistry I ATOMIC BONDING PRACTICE QUIZ Mr. Scott Select the best answer. 1) A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together is
Bonding 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
CHEMISTRY BONDING REVIEW
Answer the following questions. CHEMISTRY BONDING REVIEW 1. What are the three kinds of bonds which can form between atoms? The three types of Bonds are Covalent, Ionic and Metallic. Name Date Block 2.
Which substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s)
BONDING MIDTERM REVIEW 7546-1 - Page 1 1) Which substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s) 2) The bond between hydrogen and oxygen in
Chapter 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,
In the box below, draw the Lewis electron-dot structure for the compound formed from magnesium and oxygen. [Include any charges or partial charges.
Name: 1) Which molecule is nonpolar and has a symmetrical shape? A) NH3 B) H2O C) HCl D) CH4 7222-1 - Page 1 2) When ammonium chloride crystals are dissolved in water, the temperature of the water decreases.
AP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts
AP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts 8.1 Types of Chemical Bonds A. Ionic Bonding 1. Electrons are transferred 2. Metals react with nonmetals 3. Ions paired have lower energy
Chapter 4: Structure and Properties of Ionic and Covalent Compounds
Chapter 4: Structure and Properties of Ionic and Covalent Compounds 4.1 Chemical Bonding o Chemical Bond - the force of attraction between any two atoms in a compound. o Interactions involving valence
POLAR 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
CHAPTER 12: CHEMICAL BONDING
CHAPTER 12: CHEMICAL BONDING Active Learning Questions: 3-9, 11-19, 21-22 End-of-Chapter Problems: 1-36, 41-59, 60(a,b), 61(b,d), 62(a,b), 64-77, 79-89, 92-101, 106-109, 112, 115-119 An American chemist
Bonding & Molecular Shape Ron Robertson
Bonding & Molecular Shape Ron Robertson r2 n:\files\courses\1110-20\2010 possible slides for web\00bondingtrans.doc The Nature of Bonding Types 1. Ionic 2. Covalent 3. Metallic 4. Coordinate covalent Driving
A pure covalent bond is an equal sharing of shared electron pair(s) in a bond. A polar covalent bond is an unequal sharing.
CHAPTER EIGHT BNDING: GENERAL CNCEPT or Review 1. Electronegativity is the ability of an atom in a molecule to attract electrons to itself. Electronegativity is a bonding term. Electron affinity is the
Chapter 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
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.
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
Unit 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
Type 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
CHEMISTRY 1710 - Practice Exam #5 - SPRING 2014 (KATZ)
CHEMISTRY 1710 - Practice Exam #5 - SPRING 2014 (KATZ) Name: Score: This is a multiple choice exam. Choose the BEST answer from the choices which are given and write the letter for your choice in the space
Lewis Dot Notation Ionic Bonds Covalent Bonds Polar Covalent Bonds Lewis Dot Notation Revisited Resonance
Lewis Dot Notation Ionic Bonds Covalent Bonds Polar Covalent Bonds Lewis Dot Notation Revisited Resonance Lewis Dot notation is a way of describing the outer shell (also called the valence shell) of an
Laboratory 11: Molecular Compounds and Lewis Structures
Introduction Laboratory 11: Molecular Compounds and Lewis Structures Molecular compounds are formed by sharing electrons between non-metal atoms. A useful theory for understanding the formation of molecular
Ionic and Covalent Bonds
Ionic and Covalent Bonds Ionic Bonds Transfer of Electrons When metals bond with nonmetals, electrons are from the metal to the nonmetal The becomes a cation and the becomes an anion. The between the cation
ch9 and 10 practice test
1. Which of the following covalent bonds is the most polar (highest percent ionic character)? A. Al I B. Si I C. Al Cl D. Si Cl E. Si P 2. What is the hybridization of the central atom in ClO 3? A. sp
Chapter 7. Comparing Ionic and Covalent Bonds. Ionic Bonds. Types of Bonds. Quick Review of Bond Types. Covalent Bonds
Comparing Ionic and Covalent Bonds Chapter 7 Covalent Bonds and Molecular Structure Intermolecular forces (much weaker than bonds) must be broken Ionic bonds must be broken 1 Ionic Bonds Covalent Bonds
3/5/2014. 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
SOME TOUGH COLLEGE PROBLEMS! .. : 4. How many electrons should be shown in the Lewis dot structure for carbon monoxide? N O O
SME TUGH CLLEGE PRBLEMS! LEWIS DT STRUCTURES 1. An acceptable Lewis dot structure for 2 is (A) (B) (C) 2. Which molecule contains one unshared pair of valence electrons? (A) H 2 (B) H 3 (C) CH 4 acl 3.
A REVIEW OF GENERAL CHEMISTRY: ELECTRONS, BONDS AND MOLECULAR PROPERTIES
A REVIEW OF GENERAL CEMISTRY: ELECTRONS, BONDS AND MOLECULAR PROPERTIES A STUDENT SOULD BE ABLE TO: 1. Draw Lewis (electron dot and line) structural formulas for simple compounds and ions from molecular
EXPERIMENT 9 Dot Structures and Geometries of Molecules
EXPERIMENT 9 Dot Structures and Geometries of Molecules INTRODUCTION Lewis dot structures are our first tier in drawing molecules and representing bonds between the atoms. The method was first published
Theme 3: Bonding and Molecular Structure. (Chapter 8)
Theme 3: Bonding and Molecular Structure. (Chapter 8) End of Chapter questions: 5, 7, 9, 12, 15, 18, 23, 27, 28, 32, 33, 39, 43, 46, 67, 77 Chemical reaction valence electrons of atoms rearranged (lost,
Chapter 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.
4.5 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
Unit 3: Quantum Theory, Periodicity and Chemical Bonding. Chapter 10: Chemical Bonding II Molecular Geometry & Intermolecular Forces
onour Chemistry Unit 3: Quantum Theory, Periodicity and Chemical Bonding Chapter 10: Chemical Bonding II Molecular Geometry & Intermolecular orces 10.1: Molecular Geometry Molecular Structure: - the three-dimensional
Self Assessment_Ochem I
UTID: 2013 Objective Test Section Identify the choice that best completes the statement or answers the question. There is only one correct answer; please carefully bubble your choice on the scantron sheet.
Chemistry 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,
Question 4.2: Write Lewis dot symbols for atoms of the following elements: Mg, Na, B, O, N, Br.
Question 4.1: Explain the formation of a chemical bond. A chemical bond is defined as an attractive force that holds the constituents (atoms, ions etc.) together in a chemical species. Various theories
Section Activity #1: Fill out the following table for biology s most common elements assuming that each atom is neutrally charged.
LS1a Fall 2014 Section Week #1 I. Valence Electrons and Bonding The number of valence (outer shell) electrons in an atom determines how many bonds it can form. Knowing the number of valence electrons present
EXPERIMENT # 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
Intermolecular Forces
Intermolecular Forces: Introduction Intermolecular Forces Forces between separate molecules and dissolved ions (not bonds) Van der Waals Forces 15% as strong as covalent or ionic bonds Chapter 11 Intermolecular
Questions on Chapter 8 Basic Concepts of Chemical Bonding
Questions on Chapter 8 Basic Concepts of Chemical Bonding Circle the Correct Answer: 1) Which ion below has a noble gas electron configuration? A) Li 2+ B) Be 2+ C) B2+ D) C2+ E) N 2-2) Of the ions below,
Ionic 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
Name 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
KINETIC MOLECULAR THEORY OF MATTER
KINETIC MOLECULAR THEORY OF MATTER The kinetic-molecular theory is based on the idea that particles of matter are always in motion. The theory can be used to explain the properties of solids, liquids,
EXPERIMENT 17 : Lewis Dot Structure / VSEPR Theory
EXPERIMENT 17 : Lewis Dot Structure / VSEPR Theory Materials: Molecular Model Kit INTRODUCTION Although it has recently become possible to image molecules and even atoms using a high-resolution microscope,
Chapter 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
Sample Exercise 8.1 Magnitudes of Lattice Energies
Sample Exercise 8.1 Magnitudes of Lattice Energies Without consulting Table 8.2, arrange the ionic compounds NaF, CsI, and CaO in order of increasing lattice energy. Analyze From the formulas for three
Molecular Geometry and VSEPR We gratefully acknowledge Portland Community College for the use of this experiment.
Molecular and VSEPR We gratefully acknowledge Portland ommunity ollege for the use of this experiment. Objectives To construct molecular models for covalently bonded atoms in molecules and polyatomic ions
Bonding 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,
Chapter 2. Atomic Structure and Interatomic Bonding
Chapter 2. Atomic Structure and Interatomic Bonding Interatomic Bonding Bonding forces and energies Primary interatomic bonds Secondary bonding Molecules Bonding Forces and Energies Considering the interaction
AP CHEMISTRY 2009 SCORING GUIDELINES
AP CHEMISTRY 2009 SCORING GUIDELINES Question 6 (8 points) Answer the following questions related to sulfur and one of its compounds. (a) Consider the two chemical species S and S 2. (i) Write the electron
H 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
Structure, 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
Unit 11 Practice. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question.
Name: Class: Date: Unit 11 Practice Multiple Choice Identify the choice that best completes the statement or answers the question. 1) Crystalline solids. A) have their particles arranged randomly B) have
Exercises Topic 2: Molecules
hemistry for Biomedical Engineering. Exercises Topic 2 Authors: ors: Juan Baselga & María González Exercises Topic 2: Molecules 1. Using hybridization concepts and VSEPR model describe the molecular geometry
States of Matter CHAPTER 10 REVIEW SECTION 1. Name Date Class. Answer the following questions in the space provided.
CHAPTER 10 REVIEW States of Matter SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Identify whether the descriptions below describe an ideal gas or a real gas. ideal gas
2. Atoms with very similar electronegativity values are expected to form
AP hemistry Practice Test #6 hapter 8 and 9 1. Which of the following statements is incorrect? a. Ionic bonding results from the transfer of electrons from one atom to another. b. Dipole moments result
DCI 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
Chapter 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
Chapter 2 The Chemical Context of Life
Chapter 2 The Chemical Context of Life Multiple-Choice Questions 1) About 25 of the 92 natural elements are known to be essential to life. Which four of these 25 elements make up approximately 96% of living
Use the Force! Noncovalent Molecular Forces
Use the Force! Noncovalent Molecular Forces Not quite the type of Force we re talking about Before we talk about noncovalent molecular forces, let s talk very briefly about covalent bonds. The Illustrated
Chapter 10 Liquids & Solids
1 Chapter 10 Liquids & Solids * 10.1 Polar Covalent Bonds & Dipole Moments - van der Waals constant for water (a = 5.28 L 2 atm/mol 2 ) vs O 2 (a = 1.36 L 2 atm/mol 2 ) -- water is polar (draw diagram)
List the 3 main types of subatomic particles and indicate the mass and electrical charge of each.
Basic Chemistry Why do we study chemistry in a biology course? All living organisms are composed of chemicals. To understand life, we must understand the structure, function, and properties of the chemicals
AS Chemistry Revision Notes Unit 1 Atomic Structure, Bonding And Periodicity
AS Chemistry Revision Notes Unit Atomic Structure, Bonding And Periodicity Atomic Structure. All atoms have a mass number, A (the number of nucleons), and a proton number, Z (the number of protons). 2.
Chapter 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
Chapter 2: The Chemical Context of Life
Chapter 2: The Chemical Context of Life Name Period This chapter covers the basics that you may have learned in your chemistry class. Whether your teacher goes over this chapter, or assigns it for you
Name 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
Chemistry. 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
We 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
KINETIC THEORY OF MATTER - molecules in matter are always in motion - speed of molecules is proportional to the temperature
1 KINETIC TERY F MATTER - molecules in matter are always in motion - speed of molecules is proportional to the temperature TE STATES F MATTER 1. Gas a) ideal gas - molecules move freely - molecules have
INTERMOLECULAR FORCES
INTERMOLECULAR FORCES Intermolecular forces- forces of attraction and repulsion between molecules that hold molecules, ions, and atoms together. Intramolecular - forces of chemical bonds within a molecule
CHEM 101 Exam 4. Page 1
CEM 101 Exam 4 Form 1 (White) November 30, 2001 Page 1 Section This exam consists of 8 pages. When the exam begins make sure you have one of each. Print your name at the top of each page now. Show your
Chapter 5 TEST: The Periodic Table name
Chapter 5 TEST: The Periodic Table name HPS # date: Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The order of elements in the periodic table is based
Chemistry Workbook 2: Problems For Exam 2
Chem 1A Dr. White Updated /5/1 1 Chemistry Workbook 2: Problems For Exam 2 Section 2-1: Covalent Bonding 1. On a potential energy diagram, the most stable state has the highest/lowest potential energy.
Sample Exercise 8.1 Magnitudes of Lattice Energies
Sample Exercise 8.1 Magnitudes of Lattice Energies Without consulting Table 8.2, arrange the following ionic compounds in order of increasing lattice energy: NaF, CsI, and CaO. Analyze: From the formulas
B) 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
Molecular Geometry and Chemical Bonding Theory
Chapter 10 Molecular Geometry and Chemical Bonding Theory Concept Check 10.1 An atom in a molecule is surrounded by four pairs of electrons, one lone pair and three bonding pairs. Describe how the four
Health Science Chemistry I CHEM-1180 Experiment No. 15 Molecular Models (Revised 05/22/2015)
(Revised 05/22/2015) Introduction In the early 1900s, the chemist G. N. Lewis proposed that bonds between atoms consist of two electrons apiece and that most atoms are able to accommodate eight electrons
BOND TYPES: THE CLASSIFICATION OF SUBSTANCES
BOND TYPES: THE CLASSIFICATION OF SUBSTANCES Every (pure) substance has a unique set of intrinsic properties which distinguishes it from all other substances. What inferences, if any can be made from a
ANSWER KEY. Energy Levels, Electrons and IONIC Bonding It s all about the Give and Take!
ANSWER KEY Energy Levels, Electrons and IONIC Bonding It s all about the Give and Take! From American Chemical Society Middle School Chemistry Unit: Chapter 4 Content Statements: Distinguish the difference
Chem 112 Intermolecular Forces Chang From the book (10, 12, 14, 16, 18, 20,84,92,94,102,104, 108, 112, 114, 118 and 134)
Chem 112 Intermolecular Forces Chang From the book (10, 12, 14, 16, 18, 20,84,92,94,102,104, 108, 112, 114, 118 and 134) 1. Helium atoms do not combine to form He 2 molecules, What is the strongest attractive
AP* Bonding & Molecular Structure Free Response Questions page 1
AP* Bonding & Molecular Structure ree Response Questions page 1 (1) AP is a registered trademark of the ollege Board. The ollege Board was not involved in the production of and does not endorse this product.
Chapter 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
Section 11.3 Atomic Orbitals Objectives
Objectives 1. To learn about the shapes of the s, p and d orbitals 2. To review the energy levels and orbitals of the wave mechanical model of the atom 3. To learn about electron spin A. Electron Location
Bonds. Bond Length. Forces that hold groups of atoms together and make them function as a unit. Bond Energy. Chapter 8. Bonding: General Concepts
Bonds hapter 8 Bonding: General oncepts Forces that hold groups of atoms together and make them function as a unit. Bond Energy Bond Length It is the energy required to break a bond. The distance where
All about Chemical Bonding Ionic
Program Support Notes by: Peter Gribben BA BSc (Hons) PGCE Produced by: VEA Pty Ltd Commissioning Editor: Darren Gray Cert IV Training & Assessment Executive Producer: Simon Garner B.Ed, Dip Management
: : 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
7. Gases, Liquids, and Solids 7.1 Kinetic Molecular Theory of Matter
7. Gases, Liquids, and Solids 7.1 Kinetic Molecular Theory of Matter Kinetic Molecular Theory of Matter The Kinetic Molecular Theory of Matter is a concept that basically states that matter is composed
Electronegativity and Polarity MAIN Idea A chemical bond s character is related to each atom s
Section 8.5 Objectives Describe how electronegativity is used to determine bond type. Compare and contrast polar and nonpolar covalent bonds and polar and nonpolar molecules. Generalize about the characteristics
Exam 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
Why? Intermolecular Forces. Intermolecular Forces. Chapter 12 IM Forces and Liquids. Covalent Bonding Forces for Comparison of Magnitude
1 Why? Chapter 1 Intermolecular Forces and Liquids Why is water usually a liquid and not a gas? Why does liquid water boil at such a high temperature for such a small molecule? Why does ice float on water?
Molecular Geometry & Polarity
Name AP Chemistry Molecular Geometry & Polarity Molecular Geometry A key to understanding the wide range of physical and chemical properties of substances is recognizing that atoms combine with other atoms
5. Which of the following is the correct Lewis structure for SOCl 2
Unit C Practice Problems Chapter 8 1. Draw the lewis structures for the following molecules: a. BeF 2 b. SO 3 c. CNS 1- d. NO 2. The correct Lewis symbol for ground state carbon is a) b) c) d) e) 3. Which
Intermolecular and Ionic Forces
Intermolecular and Ionic Forces Introduction: Molecules are attracted to each other in the liquid and solid states by intermolecular, or attractive, forces. These are the attractions that must be overcome
Chemistry 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
LEWIS 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
pre -TEST Big Idea 2 Chapters 8, 9, 10
Name: AP Chemistry Period: Date: R.F. Mandes, PhD, NBCT Complete each table with the appropriate information. Compound IMF Compound IMF 1 NiCl 3 7 ClCH 2 (CH 2 ) 3 CH 3 2 Fe 8 H 2 CF 2 3 Ar 9 H 2 NCH 2
PERIODIC TABLE OF GROUPS OF ELEMENTS Elements can be classified using two different schemes.
1 PERIODIC TABLE OF GROUPS OF ELEMENTS Elements can be classified using two different schemes. Metal Nonmetal Scheme (based on physical properties) Metals - most elements are metals - elements on left
(1) e.g. H hydrogen that has lost 1 electron c. anion - negatively charged atoms that gain electrons 16-2. (1) e.g. HCO 3 bicarbonate anion
GS106 Chemical Bonds and Chemistry of Water c:wou:gs106:sp2002:chem.wpd I. Introduction A. Hierarchy of chemical substances 1. atoms of elements - smallest particles of matter with unique physical and
Name: Block: Date: Test Review: Chapter 8 Ionic Bonding
Name: Block: Date: Test Review: Chapter 8 Ionic Bonding Part 1: Fill-in-the-blank. Choose the word from the word bank below. Each word may be used only 1 time. electron dot structure metallic electronegativity
A PREVIEW & SUMMMARY of the 3 main types of bond:
Chemical Bonding Part 1 Covalent Bonding Types of Chemical Bonds Covalent Bonds Single Polar Double NonPolar Triple Ionic Bonds Metallic Bonds Other Bonds InterMolecular orces first A PREVIEW & SUMMMARY
(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
Test 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