# ACE PRACTICE TEST Chapter 8, Quiz 3

Size: px
Start display at page:

## Transcription

1 ACE PRACTICE TEST Chapter 8, Quiz 3 1. Using bond energies, calculate the heat in kj for the following reaction: CH F 2 CF HF. Use the following bond energies: CH = 414 kj/mol, F 2 = 155 kj/mol, CF = 485 kj/mol, HF = 565 kj/mol A B. 510 C D E Using bond energies, calculate the heat liberated in kj when one mole of methane is combusted as shown in the following reaction: CH O 2 CO H 2 O. Bond energies: CH = 414 kj/mol, O 2 = 494 kj/mol, CO = 799 kj/mol, HO = 460 kj/mol A. 126 B C. 5 D E The interhalogen compound, chlorine trifluoride, is prepared by reacting chlorine directly with fluorine as shown in the reaction: Cl F 2 2 ClF 3. The heat of reaction is -803 kj/mol of chlorine reacted. Calculate the F-F bond energy in kj. Bond energies: ClCl = 238 kj/mol, ClF = 251 kj/mol A. 500 B. 205 C D. 155 E What is the shape of a molecule that has the formula AX 2 with two nonbonding pairs of electrons on the central atom? A. linear B. angular C. tetrahedral D. square planar E. seesaw 5. What are the bond angles in a molecule that has the formula AX 3 with no lone pairs of electrons on the central atom? A. 60 degrees B degrees C. 90 degrees D. 150 degrees E. 120 degrees

2 6. What is the shape of a molecule that has the formula AX 5 with no nonbonding electrons on the central atom? A. square pyramidal B. pentagonal planar C. trigonal bipyramidal D. distorted tetrahedron E. octahedral 7. What is the shape of a molecule that has the formula AX 5 with one pair of nonbonding electrons on the central atom? A. square pyramidal B. pentagonal planar C. trigonal bipyramidal D. distorted tetrahedron E. octahedral 8. What are the bond angles in a molecule that has a trigonal bipyramidal shape? A. 120 degrees B. 90 degrees C. 180 degrees D. 60 degrees and 90 degrees E. 90 degrees, 120 degrees and 180 degrees 9. What is the shape of a molecule that has the formula AX 3 with two lone pairs of electrons on the central atom? A. trigonal bipyramidal B. square pyramidal C. pentagonal planar D. T-shaped E. octahedral 10. What are the bond angles in a molecule that has the shape of an octahedron? A. 90 degrees and 120 degrees B. 90 degrees and 180 degrees C degrees D. 60 degrees E. 120 degrees 11. When a molecule of POCl reacts with a molecule of chlorine, a molecule of POCl 3 is produced. What is the shape of POCl 3? A. square planar B. pyramidal C. seesaw D. tetrahedral E. trigonal planar

3 12. How many faces and how many vertexes, or corners, are in an octahedron? A. 6, 10 B. 8, 6 C. 6, 12 D. 8, 10 E. 8, Both BF 3 and NH 3 molecules consist of a central atom bonded to three other atoms. What are the bond angles in BF 3 and NH 3, respectively? A. 120 degrees, 120 degrees B. 120 degrees, 90 degrees C. 120 degrees, 107 degrees D. 90 degrees, 120 degrees E. 120 degrees, 180 degrees 14. What respective shape or shapes do the molecules Cl 2 O and CS 2 have? A. linear, linear B. angular, angular C. linear, angular D. angular, linear E. trigonal planar, angular 15. In the molecule AsF 2 Br 3, the fluorine atoms are found to be located 180 degrees apart. What positions must the fluorine atoms occupy? A. one axial and one equatorial B. both equatorial C. both axial 16. What are the bond angles in NH 3 and [NH 4 ] +, respectively? A. 120 degrees, 90 degrees B. 107 degrees, 109 degrees C. 107 degrees, 90 degrees D. 120 degrees, 109 degrees E. 90 degrees, 109 degrees 17. What shapes do NH 3 and BF 3 have, respectively? A. both angular B. pyramidal, angular C. angular, pyramidal D. trigonal pyramidal, trigonal planar E. both trigonal planar

4 18. What is the shape of the SeCl 4 molecule? A. seesaw B. square planar C. tetrahedral D. octahedral E. square pyramidal 19. Which of the following molecules would be expected to have the largest dipole moment? A. HCl B. HI C. HF D. HBr E. HAt 20. Which one of the following molecules would be expected to have a dipole moment of zero? A. CO B. SO 2 C. Cl 2 O D. HCl E. CS Which one of the following molecules is nonpolar? A. CCl 3 F B. CCl 2 F 2 C. CCl 3 H D. CCl 2 H 2 E. CF Which one of the following molecules is polar? A. CO 2 B. PCl 3 C. BF 3 D. BeF 2 E. SiCl Which of the following molecules is expected to be nonpolar based on its geometry? A. IF 5 B. SO 2 C. PCl 5 D. SF 4 E. NH 3

5 24. Which of the following molecules is polar? A. CCl 4 B. PCl 5 C. PCl 4 F D. CO 2 E. CS Which one of the following molecules is polar? A. BF 3 B. CF 4 C. XeF 4 D. ClF 3 E. BeF The dipole moment in a molecule with the formula AX 6 A. is always zero B. can be nonzero C. is always nonzero 27. A molecule with the formula AX 4 is found to be nonpolar. Which of the following shapes could it have? A. tetrahedral B. seesaw C. square planar D. either tetrahedral or square planar E. any of the above shapes

6 Key D 2. D 3. D 4. B 5. E 6. C 7. A 8. E 9. D 10. B 11. D 12. B 13. C 14. D 15. C 16. B 17. D 18. A 19. C 20. E 21. E 22. B 23. C 24. C 25. D 26. A 27. D

### 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,

### 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

### 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

### 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.

### Vocabulary: VSEPR. 3 domains on central atom. 2 domains on central atom. 3 domains on central atom NOTE: Valence Shell Electron Pair Repulsion Theory

Vocabulary: VSEPR Valence Shell Electron Pair Repulsion Theory domain = any electron pair, or any double or triple bond is considered one domain. lone pair = non-bonding pair = unshared pair = any electron

### VSEPR Model. The Valence-Shell Electron Pair Repulsion Model. Predicting Molecular Geometry

VSEPR Model The structure around a given atom is determined principally by minimizing electron pair repulsions. The Valence-Shell Electron Pair Repulsion Model The valence-shell electron pair repulsion

### 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

### 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

### 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

### Structures and Properties of Substances. Introducing Valence-Shell Electron- Pair Repulsion (VSEPR) Theory

Structures and Properties of Substances Introducing Valence-Shell Electron- Pair Repulsion (VSEPR) Theory The VSEPR theory In 1957, the chemist Ronald Gillespie and Ronald Nyholm, developed a model for

### CH101/105, GENERAL CHEMISTRY LABORATORY

CH101/105, GENERAL CHEMITRY LABORATORY LABORATORY LECTURE 5 EXPERIMENT 5: LEWI TRUCTURE AND MOLECULAR HAPE Lecture topics I. LEWI TRUCTURE a) calculation of the valence electron numbers; b) choosing the

### 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

### Chapter 9. Chemical reactivity of molecules depends on the nature of the bonds between the atoms as well on its 3D structure

Chapter 9 Molecular Geometry & Bonding Theories I) Molecular Geometry (Shapes) Chemical reactivity of molecules depends on the nature of the bonds between the atoms as well on its 3D structure Molecular

### Chapter 10 Molecular Geometry and Chemical Bonding Theory

Chem 1: Chapter 10 Page 1 Chapter 10 Molecular Geometry and Chemical Bonding Theory I) VSEPR Model Valence-Shell Electron-Pair Repulsion Model A) Model predicts Predicts electron arrangement and molecular

### 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

### Polarity. Andy Schweitzer

Polarity Andy Schweitzer What does it mean to be polar? A molecule is polar if it contains + and somewhere in the molecule. Remember: Protons can not move. So for a molecule to get a +/- it must somehow

### C has 4 valence electrons, O has six electrons. The total number of electrons is 4 + 2(6) = 16.

129 Lewis Structures G. N. Lewis hypothesized that electron pair bonds between unlike elements in the second (and sometimes the third) row occurred in a way that electrons were shared such that each element

### 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,

### Name: Class: Date: 3) The bond angles marked a, b, and c in the molecule below are about,, and, respectively.

Name: Class: Date: Unit 9 Practice Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The basis of the VSEPR model of molecular bonding is. A) regions of

### SHAPES OF MOLECULES (VSEPR MODEL)

1 SAPES MLEULES (VSEPR MDEL) Valence Shell Electron-Pair Repulsion model - Electron pairs surrounding atom spread out as to minimize repulsion. - Electron pairs can be bonding pairs (including multiple

### 7.14 Linear triatomic: A-----B-----C. Bond angles = 180 degrees. Trigonal planar: Bond angles = 120 degrees. B < B A B = 120

APTER SEVEN Molecular Geometry 7.13 Molecular geometry may be defined as the three-dimensional arrangement of atoms in a molecule. The study of molecular geometry is important in that a molecule s geometry

### Chapter10 Tro. 4. Based on the Lewis structure, the number of electron domains in the valence shell of the CO molecule is A) 1 B) 2 C) 3 D) 4 E) 5

Chapter10 Tro 1. All of the geometries listed below are examples of the five basic geometries for molecules with more than 3 atoms except A) planar triangular B) octahedral C) tetrahedral D) trihedral

### 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.

### 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

### We 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,

### CHAPTER 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.

### CHEM 1301 SECOND TEST REVIEW. Covalent bonds are sharing of electrons (ALWAYS valence electrons). Use Lewis structures to show this sharing.

CEM 1301 SECOND TEST REVIEW Lewis Structures Covalent bonds are sharing of electrons (ALWAYS valence electrons). Use Lewis structures to show this sharing. Rules OCTET RULE an atom would like to have 8

### CHAPTER 10 THE SHAPES OF MOLECULES

ATER 10 TE AE MLEULE 10.1 To be the central atom in a compound, the atom must be able to simultaneously bond to at least two other atoms. e,, and cannot serve as central atoms in a Lewis structure. elium

### Geometries and Valence Bond Theory Worksheet

Geometries and Valence Bond Theory Worksheet Also do Chapter 10 textbook problems: 33, 35, 47, 49, 51, 55, 57, 61, 63, 67, 83, 87. 1. Fill in the tables below for each of the species shown. a) CCl 2 2

### 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 10 THE SHAPES OF MOLECULES

ATER 10 TE AE MLEULE 10.1 To be the central atom in a compound, the atom must be able to simultaneously bond to at least two other atoms. e,, and cannot serve as central atoms in a Lewis structure. elium

### 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

### Molecular Structure and Polarity

OpenStax-CNX module: m51053 1 Molecular Structure and Polarity OpenStax College This work is produced by OpenStax-CNX and licensed under the Creative Commons Attribution License 4.0 By the end of this

### 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

### 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

### 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

### Covalent Bonding & Molecular Compounds Multiple Choice Review PSI Chemistry

Covalent Bonding & Molecular Compounds Multiple Choice Review PSI Chemistry Name 1) Which pair of elements is most apt to form a molecular compound with each other? A) aluminum, oxygen B) magnesium, iodine

### 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.

### 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.

### Chemistry 105, Chapter 7 Exercises

hemistry 15, hapter 7 Exercises Types of Bonds 1. Using the periodic table classify the bonds in the following compounds as ionic or covalent. If covalent, classify the bond as polar or not. Mg2 4 i2 a(3)2

### Exam. Name. 1) Chlorine (atomic number = 17) has the electronic configuration:. E) 1s22s22d103s2

Exam Name 1) Chlorine (atomic number = 17) has the electronic configuration:. A) 1s22s22p62d63s1 B) 1s22s22p63s23d5 C) 1s22s22p62d53s2 D) 1s22s22p63s23p5 E) 1s22s22d103s2 2) The complete electron configuration

### 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,

### Covalent Bonding and Molecular Geometry

Name Section # Date of Experiment Covalent Bonding and Molecular Geometry When atoms combine to form molecules (this also includes complex ions) by forming covalent bonds, the relative positions of the

### Molecular Geometry and Bonding Theories

9 Molecular Geometry and Bonding Theories We saw in hapter 8 that Lewis structures help us understand the compositions of molecules and their covalent bonds. owever, Lewis structures do not show one of

### 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

### 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

### 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.

### Chemical Bonding: Covalent Systems Written by Rebecca Sunderman, Ph.D Week 1, Winter 2012, Matter & Motion

Chemical Bonding: Covalent Systems Written by Rebecca Sunderman, Ph.D Week 1, Winter 2012, Matter & Motion A covalent bond is a bond formed due to a sharing of electrons. Lewis structures provide a description

### Chem 121 Problem Set V Lewis Structures, VSEPR and Polarity

hemistry 121 Problem set V olutions - 1 hem 121 Problem et V Lewis tructures, VEPR and Polarity AWER 1. pecies Elecronegativity difference in bond Bond Polarity Mp 3 E = 3.0-3.0 = 0 for - very weakly polar

### Molecular Structures. Chapter 9 Molecular Structures. Using Molecular Models. Using Molecular Models. C 2 H 6 O structural isomers: .. H C C O..

John W. Moore onrad L. Stanitski Peter. Jurs http://academic.cengage.com/chemistry/moore hapter 9 Molecular Structures Stephen. oster Mississippi State University Molecular Structures 2 6 structural isomers:

### 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

### 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

### CHEMISTRY 113 EXAM 4(A)

Summer 2003 1. The molecular geometry of PF 4 + ion is: A. bent B. trigonal planar C. tetrahedral D. octahedral CHEMISTRY 113 EXAM 4(A) 2. The Cl-C-Cl bond angle in CCl 2 O molecule (C is the central atom)

### 5. 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

### 4.2. Molecular Shape and Polarity. Lewis Structures for Molecules and Polyatomic Ions

Molecular Shape and Polarity 4.2 molecule is a discrete chemical entity, in which atoms are held together by the electrostatic attractions of covalent bonds. In previous chemistry courses, you used Lewis

### 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

### Chapter 8: Covalent Bonding and Molecular Structure

hapter 8 ovalent Bonding and Molecular Structure 8-1 hapter 8: ovalent Bonding and Molecular Structure hapter 8 8.1 Interactions Between Particles: oulomb s Law 8.2 ovalent Bonding Basics 8.3 Lewis Structures

### 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

### The Lewis structure is a model that gives a description of where the atoms, charges, bonds, and lone pairs of electrons, may be found.

CEM110 Week 12 Notes (Chemical Bonding) Page 1 of 8 To help understand molecules (or radicals or ions), VSEPR shapes, and properties (such as polarity and bond length), we will draw the Lewis (or electron

### CHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH

1. Is H 3 O + polar or non-polar? (1 point) a) Polar b) Non-polar CHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH 2. The bond strength is considerably greater in HF than in the other three hydrogen halides

### 3.091 Fall Term 2002 Homework #4 Solutions

3.091 all Term 2002 omework #4 olutions 5-5. We imply that sodium is a better electron donor than lithium. Evidence for this can be found in the lower value of AVEE which for these two elements is equivalent

### CHEM 1211K Test IV. MULTIPLE CHOICE (3 points each)

CEM 1211K Test IV MULTIPLE COICE (3 points each) 1) ow many single covalent bonds must a silicon atom form to have a complete octet in its valence shell? A) 4 B) 3 C) 1 D) 2 E) 0 2) What is the maximum

### 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

### 3) Of the following, radiation has the shortest wavelength. A) X-ray B) radio C) microwave D) ultraviolet E) infrared Answer: A

1) Which one of the following is correct? A) ν + λ = c B) ν λ = c C) ν = cλ D) λ = c ν E) νλ = c Answer: E 2) The wavelength of light emitted from a traffic light having a frequency of 5.75 1014 Hz is.

### MOLECULAR GEOMETRY AND BONDING THEORIES

u MOLECULAR GEOMETRY AND BONDNG TEORES TE ANTCANCER DRUG TAXOL was originally isolated from the bark of the Pacific yew tree. Chemists have now learned how to synthesize this important pharmaceutical in

### 7) How many electrons are in the second energy level for an atom of N? A) 5 B) 6 C) 4 D) 8

HOMEWORK CHEM 107 Chapter 3 Compounds Putting Particles Together 3.1 Multiple-Choice 1) How many electrons are in the highest energy level of sulfur? A) 2 B) 4 C) 6 D) 8 2) An atom of phosphorous has how

### Chapter 9 - Covalent Bonding: Orbitals

Chapter 9 - Covalent Bonding: Orbitals 9.1 Hybridization and the Localized Electron Model A. Hybridization 1. The mixing of two or more atomic orbitals of similar energies on the same atom to produce new

### : : 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

### Bonding Models. Bonding Models (Lewis) Bonding Models (Lewis) Resonance Structures. Section 2 (Chapter 3, M&T) Chemical Bonding

Bonding Models Section (Chapter, M&T) Chemical Bonding We will look at three models of bonding: Lewis model Valence Bond model M theory Bonding Models (Lewis) Bonding Models (Lewis) Lewis model of bonding

### 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

### Molecular Geometry and Hybrid Orbitals. Molecular Geometry

Molecular Geometry and ybrid Orbitals + -- bond angle 90 o Molecular Geometry Why Should I are bout Molecular Geometry? Molecular geometry (shape) influences... 3 Physical properties: 3 3 3 3 3 Pentane

### NOTE: This practice exam contains more than questions than the real final.

NOTE: This practice exam contains more than questions than the real final 1 The wavelength of light emitted from a green laser pointer is 532 10 2 nm What is the wavelength in meters? 532 10-7 m 2 What

### 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

### Unit 3: Quantum Theory, Periodicity and Chemical Bonding

Selected Honour Chemistry Assignment Answers pg. 9 Unit 3: Quantum Theory, Periodicity and Chemical Bonding Chapter 7: The Electronic Structure of Atoms (pg. 240 to 241) 48. The shape of an s-orbital is

### 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.

### Section 3.3: Polar Bonds and Polar Molecules

Section 3.3: Polar Bonds and Polar Molecules Mini Investigation: Evidence for Polar Molecules, page 103 A. The polar liquids will all exhibit some type of bending toward charged materials. The nonpolar

### 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

### 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

### Experiment 13 Molecular Models on a Computer

Experiment 13 Models on a Computer PRE-LABORATORY QUESTIONS The following preparatory questions should be answered before coming to laboratory. They are intended to introduce you to several ideas that

### Valence Bond Theory: Hybridization

Exercise 13 Page 1 Illinois Central College CEMISTRY 130 Laboratory Section: Valence Bond Theory: ybridization Name: Objectives To illustrate the distribution of electrons and rearrangement of orbitals

### 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

### 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,

### 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

### 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

### Chemistry 2014 Scoring Guidelines

AP Chemistry 2014 Scoring Guidelines 2014 The College Board. College Board, Advanced Placement Program, AP, AP Central, and the acorn logo are registered trademarks of the College Board. Visit the College

### 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 151 Final Exam

Chemistry 151 Final Exam Name: SSN: Exam Rules & Guidelines Show your work. No credit will be given for an answer unless your work is shown. Indicate your answer with a box or a circle. All paperwork must

### 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

### Name 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

### 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

### Exam 4 Practice Problems false false

Exam 4 Practice Problems 1 1. Which of the following statements is false? a. Condensed states have much higher densities than gases. b. Molecules are very far apart in gases and closer together in liquids

### O P O O. This structure puts the negative charges on the more electronegative element which is preferred. Molecular Geometry: O Xe O

hemistry& 141 lark ollege Exam 4 olution 1. Draw the Lewis structures for the following molecules and ions. Include formal charges and resonance structures, where appropriate. Fill out the table for the

### Name: 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

### 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

### Page 1. 6. Which hydrocarbon is a member of the alkane series? (1) 1. Which is the structural formula of methane? (1) (2) (2) (3) (3) (4) (4)

1. Which is the structural formula of methane? 6. Which hydrocarbon is a member of the alkane series? 7. How many carbon atoms are contained in an ethyl group? 1 3 2 4 2. In the alkane series, each molecule

### 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?

### Ionic Bonds. Chapter 8 Chemical Bonds (+VSEPR from Chapter 9) Li Be B C N O F Ne delocalized electron sea. 3. Introduction. Types of Chemical Bonds

hapter 8: hemical Bonds (+ VSEPR) hapter bjectives: hapter 8 hemical Bonds (+VSEPR from hapter 9) Understand the principal types of chemical bonds. Understand the properties of ionic and molecular compounds.

### 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