Section 14.2: 13, 15, 18, 20, 21
Section 14.3: 24, 25, 28, 32, 34
Section 14.4: 35, 36, 37, 40, 43, 46
Section 14.5: 48, 50, 52, 53, 55, 57, 59
Section 14.6: 61, 62, 63, 65, 68, 69, 70
Section 14.7: 71, 72, 74, 76, 78, 81
Additional and Integrative Exercises: 85, 86, 88, 90, 94, 96, 99, 102, 105, 107, 110
Monday, January 31, 2011
Monday, January 31st, 2011
Before we started Chapter 14, I covered the topics from Exp #16. In this lab you will need to determine the molecular weight of an unknown by calculating its freezing point depression.
Chapter 14 is titled Chemical Kinetics, which analyze how fast (or how slow) a reaction occurs. We discussed Section 14.1, 14.2 and part of 14.3. Section 14.1 outlines why kinetics are important and 14.2 discusses rates of reactions in terms of reaction stoichiometry. One thing to note is that rate is not a constant. It varies as the reaction progresses. Since these rates are exponential we use the instantaneous rate of change, or slope of the tangent line to calculate an instantaneous rate.
We also need to know how to set up a rate law expression for each reaction and from experimental data, know how to calculate the overall order of a particular reaction and the order with respect to each reactant.
We will continue with the rate laws on Wednesday.
Chapter 14 is titled Chemical Kinetics, which analyze how fast (or how slow) a reaction occurs. We discussed Section 14.1, 14.2 and part of 14.3. Section 14.1 outlines why kinetics are important and 14.2 discusses rates of reactions in terms of reaction stoichiometry. One thing to note is that rate is not a constant. It varies as the reaction progresses. Since these rates are exponential we use the instantaneous rate of change, or slope of the tangent line to calculate an instantaneous rate.
We also need to know how to set up a rate law expression for each reaction and from experimental data, know how to calculate the overall order of a particular reaction and the order with respect to each reactant.
We will continue with the rate laws on Wednesday.
Friday, January 28th, 2011
Today I covered all the material that will be on the 1st exam. The solution process was discussed further and then the Pressure Effects of Solubility were analyzed, as Henry's Law and the concepts from Lab #15 (Temperature Effects on Solubility) were covered. Be sure to look over Table 13.3 and see how polar groups influence miscibility. Section 13.5 covers Colligative properties and we covered Vapor Pressure lowering, Boiling Point elevation, Freezing Point depression, and Osmosis. For each of these colligative properties by manipulating the equations the molecular weight can be determined.
Exam #1 will cover all of Chapter 10, all of Chapter 11, and 13.1-13.5 (topics from 13.5 that were covered in class).
Exam #1 will cover all of Chapter 10, all of Chapter 11, and 13.1-13.5 (topics from 13.5 that were covered in class).
Wednesday, January 26, 2011
Chapter 13 Homework Problems
Section 13.1: 14, 15, 16, 17, 19, 20
Section 13.2 and 13.3: 22, 24, 27, 29, 33
Section 13.4: 36, 37, 39, 42, 44, 46, 48, 50, 52,
Section 13.5: 57, 60, 61, 63, 65, 67, 70, 71, 73, 74, 76, 77, 79, 80
Section 13.6: 81, 84
Additional/Integrative Exercises: 87, 90, 93, 94, 96, 99, 100, 101, 102, 106, 108, 112
Section 13.2 and 13.3: 22, 24, 27, 29, 33
Section 13.4: 36, 37, 39, 42, 44, 46, 48, 50, 52,
Section 13.5: 57, 60, 61, 63, 65, 67, 70, 71, 73, 74, 76, 77, 79, 80
Section 13.6: 81, 84
Additional/Integrative Exercises: 87, 90, 93, 94, 96, 99, 100, 101, 102, 106, 108, 112
Wednesday, January 26th, 2011
Chapter 13 covers Properties of Solution into a bit more detail. We briefly talked about intermolecular forces in liquids, but now we will consider how these IMF impact the properties of solutions.
A solution is formed when one substance disperses uniformly throughout another. The solvent is the major substance present, and the solute is the substance(s) dissolved in the solvent.
We went through examples of the units used in describing solutions and be sure to check out Section 13.4 as well as the example problems to become familiar with how to manipulate unit conversions. We then came back to Section 13.1 and discussed the Solution Process. We need to consider stability and energy in these processes and this brings us back to a discussion on thermodynamics. We considered the forces needed to break down the reactants and form products, as well as the forces gained when the products form a mixture. Before coming to class on Friday, take a look at Figure 13.4, as it summarizes the equations given in class today.
The PhET simulation shown in class today can be found here.
Song Played Before Class:
Stevie Ray Vaughan - Pride and Joy
Power-Kanye West ft. Dwele
A solution is formed when one substance disperses uniformly throughout another. The solvent is the major substance present, and the solute is the substance(s) dissolved in the solvent.
We went through examples of the units used in describing solutions and be sure to check out Section 13.4 as well as the example problems to become familiar with how to manipulate unit conversions. We then came back to Section 13.1 and discussed the Solution Process. We need to consider stability and energy in these processes and this brings us back to a discussion on thermodynamics. We considered the forces needed to break down the reactants and form products, as well as the forces gained when the products form a mixture. Before coming to class on Friday, take a look at Figure 13.4, as it summarizes the equations given in class today.
The PhET simulation shown in class today can be found here.
Song Played Before Class:
Stevie Ray Vaughan - Pride and Joy
Power-Kanye West ft. Dwele
Monday, January 24th, 2011
The discussion of solids continued with close packed arrangements of spheres. Particles in solids pack in the most efficient manner to minimize empty space. To illustrate this I used material from the Structures of Solids lab, which is posted on Carmen. Be sure to look through these figures and try to envision the structures in 3 dimensions. Be sure to highlight the sections I pointed in class in your preparation for the exam. In terms of the various packing arrangements I summarized all pertinent information in a table. Be sure to see how these formulas and numbers are derived from the packing of atoms/ions in a structure. Section 11.8 touches on the unit cells of ionic compounds and compares and contrasts the different bonding interactions in solids and the structures resulting from this bonding. At the end of lecture I discussed Lab #15.
An Excellent tutorial on the structures of solids can be found here. Be sure to check it out to gain a deeper appreciation for the 3-Dimensionality of the structures of solids.
An Excellent tutorial on the structures of solids can be found here. Be sure to check it out to gain a deeper appreciation for the 3-Dimensionality of the structures of solids.
Friday, January 21st, 2011
Now that all the phases of a substance have been studied we need to come up with a convenient way to represent all of this information. A phase diagram is a graphical representation used to depict which phase(s) is/are present during certain pressures and temperatures.
The last part of Chapter 11 deals with solids. The functional components in smart phones, laptops, and flat screen tv's consist of solids and modern materials. In order to improve the functionality of these devices we must have a common knowledge of the bonding in solids.
There are two general types of solids, amorphous and crystalline. In crystalline solids the particles order in a well-defined repeating pattern and we can analyze how the atoms/ions pack in these solids. After defining unit cells and crystal lattices, three types of cubic unit cells were investigated and this information can be used to determine density and Avagadros number.
The last part of Chapter 11 deals with solids. The functional components in smart phones, laptops, and flat screen tv's consist of solids and modern materials. In order to improve the functionality of these devices we must have a common knowledge of the bonding in solids.
There are two general types of solids, amorphous and crystalline. In crystalline solids the particles order in a well-defined repeating pattern and we can analyze how the atoms/ions pack in these solids. After defining unit cells and crystal lattices, three types of cubic unit cells were investigated and this information can be used to determine density and Avagadros number.
Wednesday, January 19th, 2011
Lecture on the 19th continued with a discussion of intermolecular forces. In some cases, such as water, a more extreme dipole-dipole interaction is observed. Since this is a special case, the term "hydrogen bonding" was coined. In this case hydrogen must be directly bonded to O, N, or F. At the end of this section I compared the relative strengths of the intermolecular forces and stressed that these effects are additive in molecules. We will come back to intermolecular forces in Chapter 13 when we study solutions, so be sure to know them.
Section 11.3 lists some other properties of liquids such as viscosity and surface tension. Each of these properties is dependent upon intermolecular forces.
Sections 11.4 and 11.5 go hand in hand with Experiment #13. When a substance changes phase from a solid to a liquid to a gas heat is required to facilitate this change. But the heat needed is not a simple linear increase. When one phase is converted to another there is a certain amount of energy required to change phase. When a solid melts becoming a liquid, this energy is referred to as heat of fusion and heat of vaporization is the heat required to convert a liquid to a vapor.
Exp #13 compares the heat of vaporization for alcohols and alkanes and relates them back to intermolecular forces. The Clausius-Clapeyron equation graphically shows the relationship between vapor pressure, temperature, and the heat of vaporization.
Section 11.3 lists some other properties of liquids such as viscosity and surface tension. Each of these properties is dependent upon intermolecular forces.
Sections 11.4 and 11.5 go hand in hand with Experiment #13. When a substance changes phase from a solid to a liquid to a gas heat is required to facilitate this change. But the heat needed is not a simple linear increase. When one phase is converted to another there is a certain amount of energy required to change phase. When a solid melts becoming a liquid, this energy is referred to as heat of fusion and heat of vaporization is the heat required to convert a liquid to a vapor.
Exp #13 compares the heat of vaporization for alcohols and alkanes and relates them back to intermolecular forces. The Clausius-Clapeyron equation graphically shows the relationship between vapor pressure, temperature, and the heat of vaporization.
Sunday, January 16, 2011
Chapter 11 Homework Problems
Section 11.1: 10
Section 11.2: 13, 16, 19, 24, 26, 27, 28
Section 11.3: 30, 32
Section 11.4: 34, 36, 39, 41
Section 11.5: 43, 46, 50
Section 11.6: 52, 54
Section 11.7: 57, 59, 62, 64, 65, 66, 67, 68
Section 11.8: 69, 71, 72, 76, 78
Additional/Integrated Exercises: 81, 82, 83, 86, 88, 89, 95, 97, 98, 99, 102, 106, 108, 111, 112, 116, 12o
Keep in mind that these are only suggested exercises and the quiz/exam questions will be most similar to the Additional/Integrated exercises.
Section 11.2: 13, 16, 19, 24, 26, 27, 28
Section 11.3: 30, 32
Section 11.4: 34, 36, 39, 41
Section 11.5: 43, 46, 50
Section 11.6: 52, 54
Section 11.7: 57, 59, 62, 64, 65, 66, 67, 68
Section 11.8: 69, 71, 72, 76, 78
Additional/Integrated Exercises: 81, 82, 83, 86, 88, 89, 95, 97, 98, 99, 102, 106, 108, 111, 112, 116, 12o
Keep in mind that these are only suggested exercises and the quiz/exam questions will be most similar to the Additional/Integrated exercises.
Friday, January 14, 2011
Friday, January 14th, 2011
Today we briefly finished Chapter 10 by defining effusion and went over an example problem comparing the rates of effusion of ammonia an and unknown gas.
In the first part of Chapter 11 we are investigating the properties of liquids and before we do so, intermolecular forces must be discussed. The four main IMF are ion-dipole interactions, dipole-dipole interactions, London Dispersion forces, and hydrogen bonding. We will discuss these forces in detail and relate them to the physical properties of liquids and gases. Be sure to read the first two sections of Ch 11 over the weekend.
In class today I also highlighted the Martin Luther King Day of Service. This year's MLK Day of Service is taking place on Monday, January 17, 2011. Registration will begin at 8am in the Archie Griffin Ballroom in the Ohio Union.
For MLK Day of Service specific questions, please contact Rosie Holmes, Coordinator of Community Service, or call the SERV Team office at 614-292-SERV (7378).
Inspirational Quote of the Day:
"...He who is greatest among you shall be a servant. That's the new definition of greatness…Everyone can be great because everyone can serve."
Dr. Martin Luther King, Jr.
Songs Played Before Class:
The Cars - You Might Think
Queen - Bohemian Rhapsody
In the first part of Chapter 11 we are investigating the properties of liquids and before we do so, intermolecular forces must be discussed. The four main IMF are ion-dipole interactions, dipole-dipole interactions, London Dispersion forces, and hydrogen bonding. We will discuss these forces in detail and relate them to the physical properties of liquids and gases. Be sure to read the first two sections of Ch 11 over the weekend.
In class today I also highlighted the Martin Luther King Day of Service. This year's MLK Day of Service is taking place on Monday, January 17, 2011. Registration will begin at 8am in the Archie Griffin Ballroom in the Ohio Union.
For MLK Day of Service specific questions, please contact Rosie Holmes, Coordinator of Community Service, or call the SERV Team office at 614-292-SERV (7378).
Inspirational Quote of the Day:
"...He who is greatest among you shall be a servant. That's the new definition of greatness…Everyone can be great because everyone can serve."
Dr. Martin Luther King, Jr.
Songs Played Before Class:
The Cars - You Might Think
Queen - Bohemian Rhapsody
Wednesday, January 12, 2011
Wednesday, January 12th, 2011
Quiz #2 is now posted up on Mastering Chemistry. For each quiz you are permitted one submission of your answer and you have an unlimited time to complete the quiz. It is due on Sunday, January 16th, at 11:00 pm. There are three versions of the quiz posted (A, B, and C) and your highest grade will be recorded as your Quiz #2 score. Each quiz is 10 questions totaling 10 points.
To this point in lecture we have only discussed pure gases, but in reality gases readily exist as mixtures. Gas Mixtures and Partial Pressures were discussed today starting with Dalton's Law of Partial Pressures. Manipulation of the ideal gas law allows us to use a mole fraction relationship to analyze mixtures of gases. A common experiment of collecting gas over water was described and a calculation was performed showing how the mass of a solid reactant can be calculated from the volume of a gas collected.
I used the gas properties PhET simulation from the Chapter 10 Section 10.1 - 10.4 Ungraded Practice Quiz Problems assignment to illustrate Kinetic Molecular Theory. Be sure to use that tutorial with the statements from the Kinetic Molecular Theory (page 414) to see how these statements come to life.
I was finishing up the chapter with gas speeds, diffusion and effusion when the bell rang. I'll start class on Friday with the following example:
The rate of effusion of an unknown gas is 2.91 times faster than that of NH3. What is the molecular weight of the gas?
If you are keeping up with the material you should be finishing up all of the Chapter 10 problems, which will prepare you for the quiz.
Inspirational Quote of the Day:
"Concern for man and his fate must form the chief interest of all technical endeavors… Never forget that in the midst of your diagrams and equations."
-Albert Einstein
Songs Played Before Class:
Journey - Don't Stop Believing
Counting Crows - Mr. Jones
To this point in lecture we have only discussed pure gases, but in reality gases readily exist as mixtures. Gas Mixtures and Partial Pressures were discussed today starting with Dalton's Law of Partial Pressures. Manipulation of the ideal gas law allows us to use a mole fraction relationship to analyze mixtures of gases. A common experiment of collecting gas over water was described and a calculation was performed showing how the mass of a solid reactant can be calculated from the volume of a gas collected.
I used the gas properties PhET simulation from the Chapter 10 Section 10.1 - 10.4 Ungraded Practice Quiz Problems assignment to illustrate Kinetic Molecular Theory. Be sure to use that tutorial with the statements from the Kinetic Molecular Theory (page 414) to see how these statements come to life.
I was finishing up the chapter with gas speeds, diffusion and effusion when the bell rang. I'll start class on Friday with the following example:
The rate of effusion of an unknown gas is 2.91 times faster than that of NH3. What is the molecular weight of the gas?
If you are keeping up with the material you should be finishing up all of the Chapter 10 problems, which will prepare you for the quiz.
Inspirational Quote of the Day:
"Concern for man and his fate must form the chief interest of all technical endeavors… Never forget that in the midst of your diagrams and equations."
-Albert Einstein
Songs Played Before Class:
Journey - Don't Stop Believing
Counting Crows - Mr. Jones
Monday, January 10, 2011
Monday, January 10th, 2011
Today's lecture focused on the content of Lab #11, which is Sections 10.5 and 10.9 of the text. Many useful physical properties of gases can be determined by manipulating the ideal gas law and we covered a few example problems involving density, molar mass, empirical formulas, and molecular formulas. Be sure to review Sections 3.4 and 3.5 in the text as the content from these sections will show up again in lecture and the lab.
Johannes van der Waal recognized that the ideal gas equation could be modified to take into account the volume and attractive forces in real gases. He developed the van der Waal equation, which you will observe in lab this week.
After Lecture today, you should read Sections 10.5 and 10.9 and perform the following homework problems:
Section 10.5: 46, 50, 52, 54, 57
Section 10.9: 83, 86, 88
Songs Played Before Class:
Chris Young - Voices
Flo Rida - Club Can't Handle Me (feat. David Guetta)
Johannes van der Waal recognized that the ideal gas equation could be modified to take into account the volume and attractive forces in real gases. He developed the van der Waal equation, which you will observe in lab this week.
After Lecture today, you should read Sections 10.5 and 10.9 and perform the following homework problems:
Section 10.5: 46, 50, 52, 54, 57
Section 10.9: 83, 86, 88
Songs Played Before Class:
Chris Young - Voices
Flo Rida - Club Can't Handle Me (feat. David Guetta)
Saturday, January 8, 2011
Friday, January 7th, 2011
The first two lectures covered the theory from Sections 10.1-10.4, but we did not perform many example problems. Today I went through various example problems illustrating the gas laws we learned about earlier in the week. Over the weekend you should complete all assignments covering Sections 10.1-10.4, which are the practice quiz questions on MC and the following problems from the end of the Chapter (which are also posted on MC)
Section 10.2: 12, 13, 16, 19, 24
Section 10.3: 26, 27, 28
Section 10.4: 30, 32 34, 36, 39, 41, 43
On Monday we will continue with the Further Applications of the Ideal Gas Law (10.5), Gas Mixtures and Partial Pressures (10.6) and will discuss the content of the lab this week. It would be helpful for you to bring your lab manual to class on Monday. Have a great weekend everyone.
Inspirational Quote:
"To give anything less than your best is to sacrifice the gift."
-Steve Prefontaine
Songs Played Before Class:
Sugarland - Stuck Like Glue
I Made It - Cash Money Heroes
Section 10.2: 12, 13, 16, 19, 24
Section 10.3: 26, 27, 28
Section 10.4: 30, 32 34, 36, 39, 41, 43
On Monday we will continue with the Further Applications of the Ideal Gas Law (10.5), Gas Mixtures and Partial Pressures (10.6) and will discuss the content of the lab this week. It would be helpful for you to bring your lab manual to class on Monday. Have a great weekend everyone.
Inspirational Quote:
"To give anything less than your best is to sacrifice the gift."
-Steve Prefontaine
Songs Played Before Class:
Sugarland - Stuck Like Glue
I Made It - Cash Money Heroes
Thursday, January 6, 2011
Tips for Success in Chemistry 122
Everyone has their own unique learning style and part of college is figuring out which learning style works best for you. Chemistry 122 will continue to build on fundamental chemistry concepts from 121 and as we progress through the book the concepts keep building on each other. It is imperative that you build a solid foundation and more importantly, keep up with all the assigned readings and assignments this quarter.
When I lecture, I will include the section # from the book for the topics that we will cover. Right now in lecture we just started Section 10.4, so any assignments from Sections 10.2-10.3 should be completed. You should also be reading the sections of the textbook either before or after class as we go along.
On Mastering Chemistry I will post the due dates for all the assignments for when you should be completing them if you are keeping up with the material. You still have access to these assignments after they are due, but this way you will know if you are on top of things or falling behind.
Doing the homework problems correctly, keeping up with the homework and readings, and understanding all the content from the tutorials will lead to success on the exams. There are a ton of problems posted, but as I said the first day in class, if you are too busy to do all the assigned reading and homework problems, you are too busy to be a college student.
You may not be able to control how smart you are, but you can control how hard you work. Don't let anyone outwork you.
When I lecture, I will include the section # from the book for the topics that we will cover. Right now in lecture we just started Section 10.4, so any assignments from Sections 10.2-10.3 should be completed. You should also be reading the sections of the textbook either before or after class as we go along.
On Mastering Chemistry I will post the due dates for all the assignments for when you should be completing them if you are keeping up with the material. You still have access to these assignments after they are due, but this way you will know if you are on top of things or falling behind.
Doing the homework problems correctly, keeping up with the homework and readings, and understanding all the content from the tutorials will lead to success on the exams. There are a ton of problems posted, but as I said the first day in class, if you are too busy to do all the assigned reading and homework problems, you are too busy to be a college student.
You may not be able to control how smart you are, but you can control how hard you work. Don't let anyone outwork you.
Mastering Chemistry Homework Assignments
As we progress through the quarter I will be posting various Mastering Chemistry Assignments relating to the material covered in lecture. There are two types of MC problems: tutorial based problems (which are not included in the text book) and end of chapter problems (identical to the back of the book, but some contain hints and math help). I will be assigning both types of problems on Mastering as we progress through the material.
Practice Quiz Questions will contain the tutorial problems. Practice Problems are exactly the same as they are in the back of the textbook. Neither of these are graded, but you are responsible for the content of these questions on quizzes and exams.
If you happen to prefer working out your problems with a pen and paper rather than look at a computer screen, here are the Chapter 10 Practice Problems from the Textbook:
Section 10.2: 12, 13, 16, 19, 24
Section 10.3: 26, 27, 28
Section 10.4: 30, 32 34, 36, 39, 41, 43,
Section 10.5: 46, 50, 52, 54, 57,
Section 10.6: 59, 62, 64, 65, 66, 67, 68, 69,
Sections 10.7 & 10.8: 71, 72, 76, 78, 81, 82
Section 10.9: 83, 86, 88,
Additional Exercises: 89, 95, 97, 98, 99, 102, 106, 108, 111
Integrative Exercises: 112, 116, 120
The practice quiz tutorial assignments are not included in the text book.
There will also be graded homework assignments throughout the quarter in the Mastering Chemistry program, which will be announced in class.
Practice Quiz Questions will contain the tutorial problems. Practice Problems are exactly the same as they are in the back of the textbook. Neither of these are graded, but you are responsible for the content of these questions on quizzes and exams.
If you happen to prefer working out your problems with a pen and paper rather than look at a computer screen, here are the Chapter 10 Practice Problems from the Textbook:
Section 10.2: 12, 13, 16, 19, 24
Section 10.3: 26, 27, 28
Section 10.4: 30, 32 34, 36, 39, 41, 43,
Section 10.5: 46, 50, 52, 54, 57,
Section 10.6: 59, 62, 64, 65, 66, 67, 68, 69,
Sections 10.7 & 10.8: 71, 72, 76, 78, 81, 82
Section 10.9: 83, 86, 88,
Additional Exercises: 89, 95, 97, 98, 99, 102, 106, 108, 111
Integrative Exercises: 112, 116, 120
The practice quiz tutorial assignments are not included in the text book.
There will also be graded homework assignments throughout the quarter in the Mastering Chemistry program, which will be announced in class.
Lecture #2 Wednesday, January 5th
The first three topics we will cover in this class are the properties of gases, liquids, and solids. Section 10.1 sets the foundation for the next three chapters and outlines the general properties and differences of solids liquids and gases. The rest of Chapter 10 focuses on gases, starting with Pressure in Section 10.2. From the early 1600's to the 1800's, many chemists studied the properties of gases and as more empirical observations were made several Gas Laws (Section 10.3) were developed.
Robert Boyle studied the relationship between Pressure and Volume in what is now known as Boyle's Law. About 100 years later Jacques Charles looked into the relationship of Temperature and Volume to form Charles's Law. 20 years later Amedeo Avagadro proposed Avagadro's Law which relates Volume and the number of moles of a gas.
All of these law's help form the combined gas law which led to the ideal gas equation. We will go over several example problems of everything we talked about to this point Friday in lecture.
If you are keeping up with the material at this point you should read sections 10.1 - 10.5 by the time you come to lecture on Friday and you should also complete the 8 tutorials posted on Mastering Chemistry. All the quiz questions will be taken from the content of the Mastering Chemistry assignments.
Inspirational Quote of the Day:
"Take a moment to write down the following personal characteristics: confidence, poise, imagination, initiative, tolerance, humility, love, cheerfulness, faith, enthusiasm, courage, honesty, serenity.
Circle all of the characteristics you possess. I hope you circled them all because they are all within us."
-John Wooden
Song Played Before Class:
Tom Petty - Free Falling
The Killers - All These Things That I've Done
Robert Boyle studied the relationship between Pressure and Volume in what is now known as Boyle's Law. About 100 years later Jacques Charles looked into the relationship of Temperature and Volume to form Charles's Law. 20 years later Amedeo Avagadro proposed Avagadro's Law which relates Volume and the number of moles of a gas.
All of these law's help form the combined gas law which led to the ideal gas equation. We will go over several example problems of everything we talked about to this point Friday in lecture.
If you are keeping up with the material at this point you should read sections 10.1 - 10.5 by the time you come to lecture on Friday and you should also complete the 8 tutorials posted on Mastering Chemistry. All the quiz questions will be taken from the content of the Mastering Chemistry assignments.
Inspirational Quote of the Day:
"Take a moment to write down the following personal characteristics: confidence, poise, imagination, initiative, tolerance, humility, love, cheerfulness, faith, enthusiasm, courage, honesty, serenity.
Circle all of the characteristics you possess. I hope you circled them all because they are all within us."
-John Wooden
Song Played Before Class:
Tom Petty - Free Falling
The Killers - All These Things That I've Done
Wednesday, January 5, 2011
Lecture #1 January 3rd, 2010
Hello everyone and welcome to Chemistry 122. I am looking forward to a great quarter. In Monday's lecture we went over the syllabus and course requirements/expectations. Both the syllabus and a pdf of the powerpoint from the first lecture are posted on Carmen.
This quarter we will be using two on-line assessment programs. The registration information for My Math Test and Mastering Chemistry is posted on the content section of Carmen under the Lecture Material subheading. Your first quiz is worth 10 points and needs to be completed using the My Math Test program. The reason we are using this program is to help refresh everyone with their math skills. It has been shown that students who struggle with fundamental algebra/trigonometry have a very tough time in Chemistry 122. After completing the assessment test in My Math Test you will be given an individualized study plan containing practice problems to help solidify your foundation for the math aspect of the course. This study plan will vary based on how many questions you answered correctly in the initial assessment. You have unlimited attempts to complete the first quiz, but it designed to enhance your understanding of some key concepts so use the study plan and complete some practice problems and watch the lecture videos to maximize the benefit of the program.
I'd also like you to register for Mastering Chemistry. Your first graded Mastering assignment will not be due until next week, but it would be great to get everyone registered and ready to go. I have posted an ungraded Thermochemistry Practice Quiz Questions assignment, as the first recitation quiz will focus on Experiment #11: Calorimetry and Hess's Law. This week's recitation should be devoted to review some aspects of Chapter 5 dealing with the first lab. If you happened to forget some of the Thermochemistry principles from last quarter (or the last time you took Chem 121), be sure to read sections 5.4, 5.5, and 5.6 and work out Sample Exercise 5.6, which directly relates to the lab.
We will start with the content in Chapter 10 on Wednesday.
Today's Inspirational Quote:
"Make the most of this time; it will not come again … make each day count. This is the place to expand your horizons to any and all opportunities.”
E. Gordon Gee
I'd also like to post an inspirational quote each day before class starts, so please e-mail any of your favorites.
Song Played Before Class:
Bruce Springsteen - Glory Days
Lil Wayne - Right Above It feat. Drake
Also feel free to send your song requests.
Ohio State 31 - Arkansas 26
Go Bucks!
This quarter we will be using two on-line assessment programs. The registration information for My Math Test and Mastering Chemistry is posted on the content section of Carmen under the Lecture Material subheading. Your first quiz is worth 10 points and needs to be completed using the My Math Test program. The reason we are using this program is to help refresh everyone with their math skills. It has been shown that students who struggle with fundamental algebra/trigonometry have a very tough time in Chemistry 122. After completing the assessment test in My Math Test you will be given an individualized study plan containing practice problems to help solidify your foundation for the math aspect of the course. This study plan will vary based on how many questions you answered correctly in the initial assessment. You have unlimited attempts to complete the first quiz, but it designed to enhance your understanding of some key concepts so use the study plan and complete some practice problems and watch the lecture videos to maximize the benefit of the program.
I'd also like you to register for Mastering Chemistry. Your first graded Mastering assignment will not be due until next week, but it would be great to get everyone registered and ready to go. I have posted an ungraded Thermochemistry Practice Quiz Questions assignment, as the first recitation quiz will focus on Experiment #11: Calorimetry and Hess's Law. This week's recitation should be devoted to review some aspects of Chapter 5 dealing with the first lab. If you happened to forget some of the Thermochemistry principles from last quarter (or the last time you took Chem 121), be sure to read sections 5.4, 5.5, and 5.6 and work out Sample Exercise 5.6, which directly relates to the lab.
We will start with the content in Chapter 10 on Wednesday.
Today's Inspirational Quote:
"Make the most of this time; it will not come again … make each day count. This is the place to expand your horizons to any and all opportunities.”
E. Gordon Gee
I'd also like to post an inspirational quote each day before class starts, so please e-mail any of your favorites.
Song Played Before Class:
Bruce Springsteen - Glory Days
Lil Wayne - Right Above It feat. Drake
Also feel free to send your song requests.
Ohio State 31 - Arkansas 26
Go Bucks!
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