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The Chemistry Workshop   

 

Remember the victims -- September 11, 2001

The Chemistry Workshop          Honors Chemistry          Last Homework Study Guide

Friday, May 22 & over the long weekend--Read 16.2 and 16.3 and answer these questions.

29. (a) What is the hybridization around the carbons in ethane, C2H6?     

(b) Hybrid orbitals only make single bonds. Where does the double bond in ethane come from?    

(c) Where do the double and triple bonds in acetylene come from?

30. Study figures 16.18 & 16.19.  Describe the σ  and π overlap in (a) ethane and      (b) acetylene

31. Explain the difference between non-polar covalent bonds and polar covalent bonds.

32. What does electronegativity have to do with the polarity of a covalent bond?

33. What does the Greek letter δ stand for in the illustrations on page 461?

34. Study Table 16.4, sample problem 16-4, and Table 14.2 on page 405.  Use this information to rate these bonds as "non-polar covalent", "moderately polar covalent", "very polar covalent", or "ionic". 

      a)   H-Br     b) K-Cl     c) C-O     d) Cl-F     e) Li-O     f) Br-Br     g) H-Cl     h) H-Br     i) H-S     j) H-C     k) F-F

35. (a) What is a dipole?    

(b) What makes a molecule polar?    

(c) Why are some molecules non-polar even though they have polar bonds?

Tuesday, May 26--Read 16.3 and answer these questions.

36. (a) Name the two types of van der Waals forces.  (b) Give descriptions of the two types of forces named in (a).

37. Why are intermolecular forces important?

38. (a) What are Hydrogen Bonds?    

(b) What causes hydrogen bonds?    

      (c) Compare the strength of a hydrogen bond to the strength of a covalent bond.    

(d) Why are hydrogen bonds important?

39. Molecular & ionic compounds frequently have big differences in their physical properties due to the differences in the forces between the atoms/molecules/ions that make up the substance. 

      Explain the following in terms of intermolecular/interionic/interatomic forces.  

      (a) Molecular compounds typically melt at much lower temperatures than Ionic compounds.

      (b) Ionic compounds are typically soluble in water, but many Molecular substances are not.

40. (a) What is a Network Solid?    

(b) Why do they have extremely high melting points, compared to "regular" molecular solids?

Review:

41. CHCl3 is a polar molecule, but CCl4 is not.  Explain.  (A Dot Structure would be helpful here)

42. How many sigma and pi bonds are in the molecule HCN.  (Hint: you must do the dor structure)

43. Which of the following molecules is polar?  Explain why.  (a) BF3    (b) CO2    (c) H2S     (d) SO2

 

Wednesday, May 27--Complete Chapter 16 Review (page 470) #27, #28, #29, #32, #33, #36, #37, #40, #41, #45

 

Thursday, May 28--Complete Chapter 16 Review (pp 470 & 471) #47, #48, #49, #50, #51, #52, #53, #54, #55, #56

 

Friday, May 29 & over the weekend--Complete these Chapter 16 Review questions:

(page 471) #57, #58, #59, #61, #62, #63, #64, #65, #66, #67
Chapter 16 "Standardized Test Prep" (page 473) #1, #3, #5, #6, #7, #8, #9 (Please write out both the question & answer if you wish to receive credit!) AND #14, #15, #16, #17 (Please explain why each one is true or false if you wish to receive credit!)

Honors Chemistry Spring 2009 Final Exam Study Guide

Chapter 10 Terms:

Kinetic Energy                      Kinetic Molecular Theory                                  Gas Pressure                                         Vacuum 

Atmospheric Pressure         Barometer                                                              Pascal                                                     Atmosphere

mm Hg                                    STP                                                                         Kinetic Energy Distribution               Vaporization

Evaporation                          Vapor Pressure                                                     "Normal" Boiling Point                       Boiling Point

Intermolecular Force            Vapor Pressure/Temperature Graph                  Melting Point                                        Crystal

Unit Cell                 Allotrope                                                               Crystalline Solid                                   Amorphous Solid

Glasses                                  Phase Diagram                                                      Triple Point                                           Critical Point

Sublimation                           Equilibrium                                                            Dynamic Equilibrium                           Greenhouse Gases

CFCs                                      Change of State                                                    Freezing                                                 Condensing

Chapter 10 calculations & other stuff to know:

·         Know how and why a barometer works

·         Know how T, P, V, n changes will affect a gas in a container.  Know how & why.

·         Know how kinetic energy relationships work in gases.

·         Know about solid-liquid-gas relationships work in substances.

·         Know about the crystal structures found in solids.

·         Know how to work with phase diagrams. 

·         Study the chapter 10 figures & tables--Go through Chapter 10 and be sure you understand each table and picture/illustration.

 

Chapter 11 Terms:

Calorie                                                    Calorimetry                                            Chemical Potential Energy                  Endothermic

Exothermic                                             Enthalpy                                                Heat of Combustion                            Heat

Heat Capacity                                       Heat of Reaction                                  Hess's Law of Heat Summation         Joule

Heat of Solution                                   Heat of Condensation                         Heat of Vaporization                            Specific Heat

Heat of Solidification                           Thermochemical Equation                  Standard Heat of Formation               Surroundings

Energy                                                   Heat Flow                                              Heat of Fusion                                      System

Chapter 11 calculations & other stuff to know:

·         Know about heat transfer between a system & its surroundings & how endothermic & exothermic affect this.

·         Know about specific heat and how to do specific calculations C = q/m x DT  (see sample problem 11-1 & practice problems 1-3).

·         Know how to do calorimetry problems q = m x C x DT  (see sample problem 11-2 & practice problems 11 & 12).

·         Know how to read, interpret, & do calculations with Thermochemical equations (see sample problem 11-3 &                practice problems 13 & 14)

·         Know how to do heat of fusion/vaporization calculations (see sample problems 11-4 & 11-5 and  practice problems 20-23).

·         Know how to do heat of solution problems (see sample problem 11-6 & practice problems 24 & 25).

·         Know how to do Hess's Law problems.

·         Know how to do calculate DHreaction using Heats of formation (see sample problem 11-7 & practice problems 30-31).

·         Study the chapter 11 figures & tables--Go through Chapter 11 and be sure you understand each table and picture/illustration.

 

Chapter 12 Terms:

Avogadro's Hypothesis                                     Boyle's Law                           Charles's Law                        Combined Gas Law

Dalton's Law of Partial Pressures                      Compressibility                    Diffusion                               Effusion

Graham's Law of Effusion                                   Gay-Lussac's Law                Ideal Gas Law                       Ideal Gas Constant, "R"

Partial Pressure                                                     kPa, atm, mm Hg                   K = °C + 273

Chapter 12 calculations & other stuff to know:

·         Review the Kinetic Molecular Theory of Gases

·         Know how T, P, V, n changes will affect a gas in a container.  Know how & why.

·         Know how kinetic energy relationships work in gases.

·         Know how to do Boyle's Law calculations  (see sample problem 12-1 & practice problems 10 & 11).

·         Know how to do Charles's Law calculations  (see sample problem 12-2 & practice problems 12 & 13).

·         Know how to do Gay-Lussac's Law calculations  (see sample problem 12-3 & practice problem 15).

·         Know how to do Combined Gas Law calculations  (see sample problem 12-4 & practice problems 16 & 17).

·         Know how to do Ideal Gas Law calculations  (see sample problems 12-5 & 12-6 and  practice problems 22-25).

·         Know how and why gases deviate from ideal behavior.

·         Know how to use Avogadro's hypothesis in calculations  Law calculations  (see sample problems 12-7 -- 12-9 & practice problems 31-36).

·         Know how to do Dalton's Law calculations  (see sample problem 12-10 & practice problems 37 & 38).

·         Know how to do Graham's Law calculations (see page 353).

·         Study the chapter 12 figures & tables--Go through Chapter 12 and be sure you understand each table and picture/illustration.

 

Chapter 13 & 14 Terms:

        Emission Spectrum                      Hund's Rule                                          Noble Gases                                          Frequency

        Atomic Orbital                              Pauli Exclusion Principle                     Representative Elements                    Photon

        Aufbau Principle                          Photoelectric Effect                             Transition Metals                                                Lanthanides

        Electromagnetic Radiation          Electron Configuration                        Ionization Energy                                 Actinides

        Alkali Metals                                Valence Electrons                                Alkaline Earth Metals                          Electronegativity

        Ground State                                 Atomic Radius                                      Electron Affinity                                  Energy Level

Chapter 13 & 14 calculations & other stuff to know:

Know what each of these pioneers did: John Dalton, J. J. Thomson, Ernest Rutherford, Niels Bohr, Albert Einstein, Max Planck, Werner Heisenberg, Louis de Broglie, Erwin Schrodinger, Dmitri Mendeleev.
Know what atomic orbitals are and what s, p, & d orbitals look like.
Be able to do electron configurations and energy diagrams for atoms and ions.
Know about the measurable properties of light (wavelength & frequency).
Be able to convert between wavelength and frequency (see sample problem 13-2 and practice problems 11 &12).
Have a rough idea of where each type of light, radio waves, visible, X-rays, etc. is in the electromagnetic spectrum (see figure 13.10)
Be able to do energy calculations with Planck's constant, λ, & υ  (see sample problem 13-3 and practice problems 13 & 14).
Know the various groups of elements, alkali metals, noble gases, etc.
Know how to determine the number of valence electrons in an atom.
Know the trends in atomic size, ionic size, ionization energy, electron affinity, electronegativity and WHY they are what they are.
Study the chapters 13 & 14 figures & tables--Go through both chapters and be sure you understand each table and picture/illustration.

 

Chapter 15 & 16 Terms:

        Coordination Number                  Electron Dot Structure                        Ionic Bond                            Metallic Bond

        Valence electron                           Octet Rule                                             Antibonding Orbital            Bond Dissociation Energy

        Bonding Orbital                            Dipole                                                    Dipole Interaction                Dispersion Force

        Hybridization                                Hydrogen Bond                                   Molecular Orbital                 Network Solid

        Nonpolar Covalent Bond            Pi Bond                                                  Polar Covalent Bond           Polar Molecule

        Resonance Structure                   Sigma Bond                                           Structural Formula               Lone Pair

        VSEPR                                            van der Waals force

Chapter 15 & 16 stuff to know:

Be able to determine the number of valence electrons in any atom.
Be able to do electron configurations for atoms & ions as dot structures or energy diagrams.
Be able to visualize molecules as electron dot structures, ball-and-stick structures, or space-filling models.
Be able to describe ionic bonds and discuss their properties.
Be able to discuss the properties of ionic compounds.
Be able to discuss metallic bonds, the structure of metallic solids and alloys, and metallic properties in general.
Be able to discuss covalent bonds and describe details regarding molecular compounds.
Be able to draw dot structures of molecular compounds and molecular ions and describe the following features:

Bond angles, bond strength (bond dissociation energy), hybridization, molecular geometry, bond or molecular polarity, resonance, exceptions to the octet rule, bond length, intermolecular interactions, and hydrogen bonding.

·         Be able to compare atomic orbitals to molecular orbitals.

·         Be able to discuss and apply Molecular Orbital Theory, VSEPR Theory, and Hybridization Theory

·         Study the chapter 15 & chapter 16 figures & tables and be sure you understand each table and picture/illustration.

 

 

 

Questions?? Comments?? Feel free to e-mail Mr. Polsinelli

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