Chemistry 162:  Exam #2 Study Guide

Instructor: Ken Marr

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Exam #2 covers the material in chapters 9-11 and labs 4-7 

The exam will be combination of multiple choice questions and short answer/essay questions. BRING A SCANTRON CARD, NUMBER 2 PENCIL and a GOOD ERASER.

Stuff to concentrate on while reviewing for Exam 2

• Understand These Concepts. Chapter 9: 1-15 on page 356 (#16-17 will be covered in class when we do ALE 19); Chapter 10: 1-8 on page 388; Chapter 11: 1-10 on page 413. 

• Master These Skills. Chapter 9:  1-6 on page 356; Chapter 10: 1-5 on page 388; Chapter 11: 1-4 on page 413. 

• Key Equations and Relationships: Chapter 9: 1-2 on page 356; Chapter 10: 1-2 on page 388. Chapter 11: 1 on p. 413.

• All ALE's for Chapters 9, 10 and 11 (i.e. ALE's 8 -16)

 Exam 2 Practice Questions

• Have a go at this Practice Exam. ( NOTE:  This practice exam is intended to give you an idea of the kind of questions to expect. The actual exam given WILL differ from this one!

• IR Sprectra Analysis Practice Questions

• Here are some good multiple choice Practice Questions: focus on the questions for chapters 9-11 from the Silberberg Online Learning Center http://highered.mcgraw-hill.com/sites/0072396814/student_view0/index.html. These questions are intended to give you an idea of the kind of questions to expect and to help you identify areas of strength and areas where further review is needed. The actual exam will be a combination of multiple choice questions and short answer/essay questions. Questions given WILL differ slightly from the practice questions!

Bonding & Molecular Structure Practice Questions

Study Cards:  See "AP5"   Study Questions [Word | Acrobat] Lewis Dot Practice [Word | Acrobat] and Answers (.GIF) [Page 1 | Page 2] Lewis Structures Practice [Word | Acrobat] and Answers (.GIF)  Correction:  the phosphate ion, PO43- should have one dbl bond and three single bonds and has 4 resonance structures!! More Lewis Structure Practice [Word | Acrobat] and Answers (.GIF) [Page 1 | Page 2 | Page 3 | Page 4]                                   Correction:  the sulfate ion, SO42- should have two dbl bonds and two single bonds and has 6 resonance structures!! Bond Energy Practice [Word | Acrobat] Electronegativity Practice [Word | Acrobat] Practice Test:  Bonding and Molecular Structure [Word | Acrobat] and Answers (.GIF) [Page 1 | Page 2 | Page 3]

Study Guide for Chapters 9-11 (Silberberg) 

1. Terms/Concepts

   1. Valence electrons

   2. The octet rule, and the exceptions of (1) molecules with an electron deficiency, (2) an odd number of electrons, and (3) an expanded valence shell

   3. Bonding and non–bonding pairs
   4. Lewis dot symbols for atoms
   5. Electronegativity
   6. Bond length, bond energy and bond order
   7. Single, double, and triple bonds
   8. Polarity
   9. Formal charge
   10. Resonance, delocalized electrons and resonance hybrids
   11. Free radical
   12. Valence bond theory and hybrid orbitals
   13. Molecular orbital theory and electron delocalization
2. Skills/Background Knowledge
   1. The models for ionic, covalent, and metallic bonds, and the continuum of bonding
   2. Trends in electronegativity on the periodic chart
   3. Ranking bond polarity
   4. Use Lewis dot structures to diagram molecular bonding, including molecules with more than one central atom
   5. Draw resonance structures
   6. Valence–Shell Electron–Pair Repulsion (VESPR)
      1. Know the name and geometry for 2, 3, 4, 5, and 6 electron pairs
      2. Draw each of the shapes for molecules with 2–6 electron pairs
      3. Use the AX_mE_n notation
   7. Describe the shape of the orbital, geometry about the central atom, and bond angles for sp, sp², sp³, sp³d, and sp³d² hybrid orbitals
   8. Describe/draw the valence bond model for s and p bonds
   9. Describe/draw the energy, shape and orientation about the central atoms of s_s, s_s*, s_p, s_p*, p_p, and p_p* molecular orbitals in diatomic substances
   10. Use molecular orbital diagrams to determine the bond order and molecular orbital electronic structure of diatomic substances
3. Problem Solving Abilities & Application of Principles
   1. Explain physical and chemical properties based on the models for ionic, covalent, and metallic bonds
   2. Predict trends in bond lengths and bond strengths
   3. Predict the direction of polarity of a bond and molecular dipoles
   4. Explain molecular properties based on dipoles
   5. Use the VSEPR model to predict:
      1. The geometry of molecules
      2. The placement of nonbonding pairs
      3. Bond angles, including the effect of non–bonding pairs
   6. Calculate enthalpy changes from bond energies
   7. Determine which hybrid orbitals are present on the central atoms of covalent molecules
   8. Use molecular orbital diagrams to predict bond orders, and relative strengths and lengths of bonds in diatomic substances
   9. Apply the valence bond and molecular orbital models to demonstrate an understanding of resonance

© Kenneth R. Marr 2001