Chem 11 Practice Questions for Ch. 8

Similar documents
2. Atoms with very similar electronegativity values are expected to form

ch9 and 10 practice test

EXPERIMENT 9 Dot Structures and Geometries of Molecules

SOME TOUGH COLLEGE PROBLEMS! .. : 4. How many electrons should be shown in the Lewis dot structure for carbon monoxide? N O O

EXPERIMENT 17 : Lewis Dot Structure / VSEPR Theory

ACE PRACTICE TEST Chapter 8, Quiz 3

Questions on Chapter 8 Basic Concepts of Chemical Bonding

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

Self Assessment_Ochem I

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

Chapter 7. Comparing Ionic and Covalent Bonds. Ionic Bonds. Types of Bonds. Quick Review of Bond Types. Covalent Bonds

Theme 3: Bonding and Molecular Structure. (Chapter 8)

5. Which of the following is the correct Lewis structure for SOCl 2

Chemistry Workbook 2: Problems For Exam 2

AP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts

: : Solutions to Additional Bonding Problems

CHEMISTRY Practice Exam #5 - SPRING 2014 (KATZ)

Molecular Geometry and Chemical Bonding Theory

Sample Exercise 8.1 Magnitudes of Lattice Energies

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

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

Health Science Chemistry I CHEM-1180 Experiment No. 15 Molecular Models (Revised 05/22/2015)

CHEMISTRY BONDING REVIEW

Chemistry 105, Chapter 7 Exercises

Sample Exercise 8.1 Magnitudes of Lattice Energies

We emphasize Lewis electron dot structures because of their usefulness in explaining structure of covalent molecules, especially organic molecules.

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

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

A pure covalent bond is an equal sharing of shared electron pair(s) in a bond. A polar covalent bond is an unequal sharing.

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

Chapter 8 Basic Concepts of the Chemical Bonding

Question 4.2: Write Lewis dot symbols for atoms of the following elements: Mg, Na, B, O, N, Br.

A REVIEW OF GENERAL CHEMISTRY: ELECTRONS, BONDS AND MOLECULAR PROPERTIES

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

2. 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+

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

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

Molecular Geometry and VSEPR We gratefully acknowledge Portland Community College for the use of this experiment.

CHAPTER 10 THE SHAPES OF MOLECULES

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

Ionic and Covalent Bonds

Covalent Bonding & Molecular Compounds Multiple Choice Review PSI Chemistry

CHAPTER 10 THE SHAPES OF MOLECULES

CHAPTER 6 Chemical Bonding

Laboratory 11: Molecular Compounds and Lewis Structures

Molecular Geometry & Polarity

CHAPTER 10 THE SHAPES OF MOLECULES

Bonding Practice Problems

pre -TEST Big Idea 2 Chapters 8, 9, 10

Chapter 8 Concepts of Chemical Bonding

DCI for Electronegativity. Data Table:

Exercises Topic 2: Molecules

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

CHAPTER 12: CHEMICAL BONDING

We will not be doing these type of calculations however, if interested then can read on your own

Ionization energy _decreases from the top to the bottom in a group. Electron affinity increases from the left to the right within a period.

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

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

Which substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s)

Geometries and Valence Bond Theory Worksheet

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

CH101/105, GENERAL CHEMISTRY LABORATORY

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

SHAPES OF MOLECULES (VSEPR MODEL)

Bonding & Molecular Shape Ron Robertson

Chem 121 Problem Set V Lewis Structures, VSEPR and Polarity

Unit 3: Quantum Theory, Periodicity and Chemical Bonding

5. Structure, Geometry, and Polarity of Molecules

Chapter 10 Molecular Geometry and Chemical Bonding Theory

Exam 2 Chemistry 65 Summer Score:

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

A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together is called a(n)

3.091 Fall Term 2002 Homework #4 Solutions

REVIEW QUESTIONS Chapter 8

CHAPTER 6 REVIEW. Chemical Bonding. Answer the following questions in the space provided.

Name period Unit 3 worksheet

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

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

In the box below, draw the Lewis electron-dot structure for the compound formed from magnesium and oxygen. [Include any charges or partial charges.

Polarity. Andy Schweitzer

Lewis Dot Notation Ionic Bonds Covalent Bonds Polar Covalent Bonds Lewis Dot Notation Revisited Resonance

Covalent Bonding and Molecular Geometry

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

3. What would you predict for the intensity and binding energy for the 3p orbital for that of sulfur?

Name: Date: Period: Presentation #4. Covalent compounds continued practice with drawing them. Modeling covalent compounds in 3D

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

LEWIS DIAGRAMS. by DR. STEPHEN THOMPSON MR. JOE STALEY

A PREVIEW & SUMMMARY of the 3 main types of bond:

Chapter 2 Polar Covalent Bonds; Acids and Bases

Chapter 8: Covalent Bonding and Molecular Structure

Unit 3: Quantum Theory, Periodicity and Chemical Bonding. Chapter 10: Chemical Bonding II Molecular Geometry & Intermolecular Forces

Chemistry 151 Final Exam

EXPERIMENT 1: Survival Organic Chemistry: Molecular Models

3/5/2014. iclicker Participation Question: A. MgS < AlP < NaCl B. MgS < NaCl < AlP C. NaCl < AlP < MgS D. NaCl < MgS < AlP

Chapter 4: Structure and Properties of Ionic and Covalent Compounds

CHEM 101 Exam 4. Page 1

OCTET RULE Generally atoms prefer electron configurations with 8 valence electrons. - Filled s and p subshells

Bonds. Bond Length. Forces that hold groups of atoms together and make them function as a unit. Bond Energy. Chapter 8. Bonding: General Concepts

Molecular Structure and Polarity

Transcription:

Chem 11 Practice Questions for Ch. 8 1. Atoms having equal or nearly equal electronegativities are expected to form A) no bonds B) polar covalent bonds C) nonpolar covalent bonds D) ionic bonds E) covalent bonds 2. For the elements Cs, F, and Cl, the order of increasing electronegativity is: A) F < Cl < Cs B) Cs < Cl < F C) Cl < Cs < F D) F < Cs < Cl E) none of these 3. Based on electronegativity differences, which of the following is most likely to be ionic? A) CaF 2 B) Br 2 C) BH 3 D) NO E) CF 4 4. Which of the following bonds would be the most polar without being considered ionic? A) Mg-O B) C-O C) O-O D) Si-O E) N-O 5. Which of these is an isoelectronic series? A) Na +, K +, Rb +, Cs + B) K +, Ca 2+, Ar, S 2 C) Na +, Mg 2+, S 2, Cl D) Li, Be, B, C E) none of these (A-D) 1

6. Using the following bond energies: Bond Bond Energy (kj/mol) C C 839 C H 413 O=O 495 C=O 799 O H 467 estimate the heat of combustion for one mole of acetylene: C 2 H 2 (g) + 5 2 O 2(g) 2CO 2 (g) + H 2 O(g) A) 1228 kj B) 1228 kj C) 447 kj D) +447 kj E) +365 kj 7. In the Lewis structure for elemental nitrogen there is (are) A) a single bond between the nitrogens B) a double bond between the nitrogens C) a triple bond between the nitrogens D) three unpaired electrons E) none of the above Consider the compound crotonaldehyde, whose skeleton is: 8. How many electrons must be shown (as bonding or nonbonding electrons) in the Lewis structure of this molecule? A) 12 B) 18 C) 24 D) 28 E) 32 9. How many nonbonding electrons appear in the Lewis structure of this molecule? A) 2 B) 4 C) 6 D) 8 E) 10 2

10. Which carbon in this molecule has tetrahedral bonding? A) 1 B) 2 C) 3 D) 4 E) all 11. Which of the following Lewis structures best describes BF 3? A) B) C) D) E) 12. Which of the following has an incomplete octet in its Lewis structure? A) SO 2 B) ICl C) CO 2 D) F 2 E) NO 3

13. Which of the following is not a valid resonance structure for N 3? A) B) C) D) E) all are correct 14. Select the molecule from the following that has a dipole moment. A) CO 2 B) SeO 3 C) XeF 4 D) SF 4 E) BeCl 2 15. If a compound has a number of individual dipoles, then: I. It is polar overall. II. There is an electronegativity difference between the bonded atoms. III. it is ionic. IV. It doesn't have resonance. A) II only B) II, IV C) I, II, IV D) I, III E) All of the above statements are correct. 16. The Cl Kr Cl bond angle in KrCl 4 is closest to A) 90 B) 109 C) 120 D) 150 E) 360 4

17. The bond angles about the carbon atom in the formaldehyde molecule, H 2 C=O, are about: A) 120 B) 60 C) 109 D) 180 E) 90 18. Which of the following species has a trigonal bipyramid structure? A) NH 3 B) IF 5 C) I 3 D) PCl 5 E) none of these 19. Which ion is planar? A) NH + 4 B) CO 2 3 C) SO 2 3 D) ClO 3 E) all are planar 20. Which ion is larger in each pair? i) O 2- or S 2- ii) Fe 2+ or Fe 3+ iii) S 2- or K + A) S 2-, Fe 2+, S 2- B) S 2-, Fe 3+, S 2- C) O 2-, Fe 3+, K + D) S 2-, Fe 2+, K + E) O 2-, Fe 2+, S 2-21. Calculate the lattice energy of the ionic compound MCl 2 given the information below: H f MCl 2 (s) = -342 kj/mol IE 1 of M = +600 kj/mol IE 2 of M = +1150 kj/mol Cl 2 (g) => 2 Cl(g) H = +244 kj Cl(g) + 1 e - => Cl - (g) H = -349 kj M(s) => M(g) H = +150 kj A) -2136 kj B) -2015 kj C) -1446 kj D) -1788 kj E) -1666 kj 5

ID: A Chem 11 Practice Questions for Ch. 8 Answer Section 1. ANS: C PTS: 1 DIF: Easy REF: 8.2 KEY: Chemistry general chemistry bonding covalent bonding electronegativity 2. ANS: B PTS: 1 DIF: Easy REF: 8.2 KEY: Chemistry general chemistry bonding covalent bonding electronegativity 3. ANS: A PTS: 1 DIF: Easy REF: 8.2 KEY: Chemistry general chemistry bonding covalent bonding electronegativity 4. ANS: D PTS: 1 DIF: Moderate REF: 8.2 KEY: Chemistry general chemistry bonding covalent bonding electronegativity polar covalent bond 5. ANS: B PTS: 1 DIF: Easy REF: 8.4 KEY: Chemistry general chemistry bonding ionic bonding 6. ANS: B PTS: 1 DIF: Moderate REF: 8.8 KEY: Chemistry general chemistry bonding covalent bonding bond energy MSC: Quantitative 7. ANS: C PTS: 1 DIF: Easy REF: 8.1 KEY: Chemistry general chemistry bonding covalent bonding Lewis dot formula 8. ANS: D PTS: 1 DIF: Easy REF: 8.1 KEY: Chemistry general chemistry bonding covalent bonding Lewis dot formula 9. ANS: B PTS: 1 DIF: Easy REF: 8.1 KEY: Chemistry general chemistry bonding covalent bonding Lewis dot formula 10. ANS: A PTS: 1 DIF: Easy REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry the valence-shell electron-pair repulsion model 11. ANS: A PTS: 1 DIF: Easy REF: 8.11 KEY: Chemistry general chemistry bonding covalent bonding exceptions to the octet rule 12. ANS: E PTS: 1 DIF: Easy REF: 8.11 KEY: Chemistry general chemistry bonding covalent bonding exceptions to the octet rule 13. ANS: A PTS: 1 DIF: Easy REF: 8.12 KEY: Chemistry general chemistry bonding covalent bonding resonance 1

ID: A 14. ANS: D PTS: 1 DIF: Moderate REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry dipole moment 15. ANS: A PTS: 1 DIF: Easy REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry dipole moment 16. ANS: A PTS: 1 DIF: Moderate REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry bond angle 17. ANS: A PTS: 1 DIF: Moderate REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry bond angle 18. ANS: D PTS: 1 DIF: Moderate REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry the valence-shell electron-pair repulsion model trigonal bipyramidal arrangement 19. ANS: B PTS: 1 DIF: Moderate REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry the valence-shell electron-pair repulsion model 20. ANS: A PTS: 1 DIF: Moderate REF: 8.4 KEY: Chemistry general chemistry bonding ionic bonding ionic radii 21. ANS: D PTS: 1 DIF: Difficult REF: 8.5 KEY: Chemistry general chemistry bonding ionic bonding Born-Haber cycle MSC: Quantitative 22. ANS: A PTS: 1 DIF: Moderate REF: 9.1 KEY: Chemistry general chemistry bonding bonding theories hybridization 23. ANS: C PTS: 1 DIF: Moderate REF: 9.1 KEY: Chemistry general chemistry bonding bonding theories hybridization 24. ANS: D PTS: 1 DIF: Moderate REF: 9.1 KEY: Chemistry general chemistry bonding bonding theories multiple bonding 25. ANS: D PTS: 1 DIF: Easy REF: 9.1 KEY: Chemistry general chemistry bonding bonding theories multiple bonding 2

2026 © DocPlayer.net Privacy Policy | Terms of Service | Feedback  | Do Not Sell My Personal Information