CHEMISTRY A
Unit 1: Measurement and Analysis
6. Practice in Measuring Metric Volumes
If you don't have a graduated cylinder, use a Pyrex measuring cup. For question 1, record your estimates and the actual measurements for the five large containers (you may need to fill the Pyrex cup a couple of times if the containers hold more water than the Pyrex cup). For question 2 record your estimates and measurements for the five medium containers. For question 3 record your estimates and measurements for the five small containers.
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10. Project: Measuring Length with Precision
You always need to estimate your answers to one place beyond the smallest division on your ruler. For example, if your ruler has centimeters as the smallest unit, then you should estimate all answers to the nearest tenth of a centimeter (e.g. 14.1 cm). If it has millimeter markings (as most rulers do) then you must estimate to the tenth of a millimeter (e.g. 14.12 cm). If you are using the same ruler then all answers should have the same precision.
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Unit 2: How to Identify Elements, Compounds, and Mixtures
4. Experiment: Observation of a Phase Change
Open up the worksheet (see link near the bottom of the lesson). Since you can't do the graphing part of the experiment, just answer the first five questions on the worksheet and the last seven questions. If you watch the video carefully and review the material about phase changes and kinetic energy in fluids, you should be able to understand what is going on well enough to answer them.
Open up the worksheet (see link near the bottom of the lesson). Since you can't do the graphing part of the experiment, just answer the first five questions on the worksheet and the last seven questions. If you watch the video carefully and review the material about phase changes and kinetic energy in fluids, you should be able to understand what is going on well enough to answer them.
Unit 3 - Exploring Laws for Gases and Conservation of Mass
2. Gases and Kinetic Molecular Theory
For this lesson you need to understand the two graphs that are shown. The first graph (Energy Distribution in a Gas) is described by this video. You only need to watch the first minute or two. After that the video gets to more advanced topics. The second graph (Phase Diagram) is described here.
For this lesson you need to understand the two graphs that are shown. The first graph (Energy Distribution in a Gas) is described by this video. You only need to watch the first minute or two. After that the video gets to more advanced topics. The second graph (Phase Diagram) is described here.
5. Pressure: Volume Relationships in Gases (Boyle's Law)
http://www.brightstorm.com/science/chemistry/kinetic-molecular-theory/boyles-law
http://www.brightstorm.com/science/chemistry/kinetic-molecular-theory/boyles-law
7. Temperature: Volume Relationships in Gases (Charles' Law)
When using Charles' Law it is important to remember that all your temperature measurements must be in Kelvins. If you have the temperature in Celsius you just add 273 to get the temperature in the Kelvin scale. So if it is 5 degrees Celsius outside right now it is 278 (5 + 273) kelvin, or 278K. The reason we use the Kelvin Scale is that it has no negative temperatures. Zero kelvin is absolute zero, the coldest temperature possible in the universe. Watch this video for an explanation of Charles’ Law, a demonstration, and an example problem.
When using Charles' Law it is important to remember that all your temperature measurements must be in Kelvins. If you have the temperature in Celsius you just add 273 to get the temperature in the Kelvin scale. So if it is 5 degrees Celsius outside right now it is 278 (5 + 273) kelvin, or 278K. The reason we use the Kelvin Scale is that it has no negative temperatures. Zero kelvin is absolute zero, the coldest temperature possible in the universe. Watch this video for an explanation of Charles’ Law, a demonstration, and an example problem.
8 Experiment: Finding Absolute Zero Experimentally (Optional)
What is the coldest weather you have ever been in? What do you think makes cold air cold? In the last lesson you learned that the only difference between cold air and warm air is that on average the air molecules are moving around more quickly in warm air. Because they are bouncing off of things at a higher speed and more often they feel “hotter.” When they move more slowly they impart less energy to the objects around them and they feel “colder.” For the same reason warmer air exerts more pressure on the walls of containers they are in. So a balloon with warm air in it will shrink as the air gets colder.
Since you probably don’t have the materials for this experiment, watch the video in the lesson and use the graph below. This is a graph of the volume of a gas (like the air in a balloon or the air in the Erlenmeyer flask shown in the video) as you change its temperature. Answer the questions for the project using this graph. If you extend the line on the graph until it crosses the horizontal axis (where volume = zero) you can find absolute zero (it is a negative number in the Celsius scale), which is the coldest temperature possible for all substances. Absolute zero is how cold it would be if molecules weren’t moving at all. Brrrrrrr!
What is the coldest weather you have ever been in? What do you think makes cold air cold? In the last lesson you learned that the only difference between cold air and warm air is that on average the air molecules are moving around more quickly in warm air. Because they are bouncing off of things at a higher speed and more often they feel “hotter.” When they move more slowly they impart less energy to the objects around them and they feel “colder.” For the same reason warmer air exerts more pressure on the walls of containers they are in. So a balloon with warm air in it will shrink as the air gets colder.
Since you probably don’t have the materials for this experiment, watch the video in the lesson and use the graph below. This is a graph of the volume of a gas (like the air in a balloon or the air in the Erlenmeyer flask shown in the video) as you change its temperature. Answer the questions for the project using this graph. If you extend the line on the graph until it crosses the horizontal axis (where volume = zero) you can find absolute zero (it is a negative number in the Celsius scale), which is the coldest temperature possible for all substances. Absolute zero is how cold it would be if molecules weren’t moving at all. Brrrrrrr!
9. Experiment: Charles' Law and a Metal Can
For this experiment you can watch this video of similar a experiment if you don't have the materials to do it at home.
The same thing is happening with this 55 gallon drum - First they heated the air inside the drum so that fewer, faster-moving air molecules could maintain atmospheric pressure. Then they sealed the tank and cooled it down again. Describe what happens next according to Charles' Law. Plain old atmospheric air pressure can crush enormous cans too, like this train storage tank!
12. Combined Gas Law
http://www.brightstorm.com/science/chemistry/kinetic-molecular-theory/combined-gas-law
14. Counting Gas Particles: The Measure of the Mole
http://www.khanacademy.org/video/the-mole-and-avogadro-s-number?playlist=Chemistry
16. Demonstrating Conservation of Mass with Balanced Equations
http://www.khanacademy.org/video/balancing-chemical-equations?playlist=Chemistry
http://www.brightstorm.com/science/chemistry/kinetic-molecular-theory/combined-gas-law
14. Counting Gas Particles: The Measure of the Mole
http://www.khanacademy.org/video/the-mole-and-avogadro-s-number?playlist=Chemistry
16. Demonstrating Conservation of Mass with Balanced Equations
http://www.khanacademy.org/video/balancing-chemical-equations?playlist=Chemistry
Unit 4: The Discovery of the Atom: Nature's Building Blocks
1. The Golden Years of Chemistry
Intro to the atom - SciTechUK
John Dalton – Xtra Normal
J.J. Thomson – SciTechUK
4. Masters of Classic Atomic Theory
Short History of Atomic Theory - Discovery Channel
Ernest Rutherford – SciTechUK
Niels Bohr
Introduction to the Atom - Khan Academy
6. Designing an Organizational Map: The Periodic Table
Who set up the Periodic Table? BBC
These two videos show why it is set up the way it is. - Khan Academy
An understanding of valence electrons will be especially important for this unit and the next one.
8. The Bohr Model Revisited
This lesson is all about electron configuration in the atom. It is a complex concept so it will serve you well to take a little extra time to watch these videos though it may not be necessary to watch them all. You will need to understand the order in which the energy levels are filled and how many electrons fit into each level.
Orbitals and Electron Configuration I - Khan Academy
Orbitals and Electron Configuration II - Khan Academy
Example – Configuration for Iron and Lanthanum - Khan Academy
Example – Configuration for Nickel and Zirconium - Khan Academy
10. Charging Up: Ionization of Atoms
Ionization Energy Trends in the Periodic Table - Khan Academy
This video will be helpful in the next unit as well.
12. A Closer Look Inside: Nuclear Reactions
Types of Decay - Khan Academy
Half Life - Khan Academy
Fission and Fusion - Cassiopeia Project
Intro to the atom - SciTechUK
John Dalton – Xtra Normal
J.J. Thomson – SciTechUK
4. Masters of Classic Atomic Theory
Short History of Atomic Theory - Discovery Channel
Ernest Rutherford – SciTechUK
Niels Bohr
Introduction to the Atom - Khan Academy
6. Designing an Organizational Map: The Periodic Table
Who set up the Periodic Table? BBC
These two videos show why it is set up the way it is. - Khan Academy
An understanding of valence electrons will be especially important for this unit and the next one.
8. The Bohr Model Revisited
This lesson is all about electron configuration in the atom. It is a complex concept so it will serve you well to take a little extra time to watch these videos though it may not be necessary to watch them all. You will need to understand the order in which the energy levels are filled and how many electrons fit into each level.
Orbitals and Electron Configuration I - Khan Academy
Orbitals and Electron Configuration II - Khan Academy
Example – Configuration for Iron and Lanthanum - Khan Academy
Example – Configuration for Nickel and Zirconium - Khan Academy
10. Charging Up: Ionization of Atoms
Ionization Energy Trends in the Periodic Table - Khan Academy
This video will be helpful in the next unit as well.
12. A Closer Look Inside: Nuclear Reactions
Types of Decay - Khan Academy
Half Life - Khan Academy
Fission and Fusion - Cassiopeia Project
Unit 5 - Molecular Structure
1. Chemical Accounting: Stoichiometry
Stoichiometry examples – Khan Academy
This video is optional and takes things a bit deeper.
2. Valence Structure
It will probably help if you watch either this video or this video again from Unit 4 lesson 4.
4. Determining Chemical Formulas
This video shows a good way of doing this. – Bryan Moss Chemistry
You can just watch the first 6.5 minutes because this lesson doesn’t deal with polyatomic ions which he talks about after that. Polyatomic ions will be dealt with in Lesson 7.
5. Electron Availability: Prelude to Bonding
You will probably want to review this video on ionization from Unit 4 Lesson 10 – Khan Academy
Then watch this one. – Khan Academy
You can focus on the first half of the video where he talks about ionization energy and especially starting at 3.5 minutes when he talks about electronegativity.
7. Types of Chemical Bonds
You may want to finish the video you started in Lesson 4 where Bryan Moss discusses polyatomic ions.
Then watch Ionic, Covalent, and Metallic Bonds – Khan Academy
Pay attention to this video because seeing how atoms with higher elecronegativity “hog” the electrons will help you understand how some molecules can be polar.
8. Polar Covalent Molecules and Dot Structures
The video you just watched from lesson 7 will help you understand polarity and electron dot symbols.
Stoichiometry examples – Khan Academy
This video is optional and takes things a bit deeper.
2. Valence Structure
It will probably help if you watch either this video or this video again from Unit 4 lesson 4.
4. Determining Chemical Formulas
This video shows a good way of doing this. – Bryan Moss Chemistry
You can just watch the first 6.5 minutes because this lesson doesn’t deal with polyatomic ions which he talks about after that. Polyatomic ions will be dealt with in Lesson 7.
5. Electron Availability: Prelude to Bonding
You will probably want to review this video on ionization from Unit 4 Lesson 10 – Khan Academy
Then watch this one. – Khan Academy
You can focus on the first half of the video where he talks about ionization energy and especially starting at 3.5 minutes when he talks about electronegativity.
7. Types of Chemical Bonds
You may want to finish the video you started in Lesson 4 where Bryan Moss discusses polyatomic ions.
Then watch Ionic, Covalent, and Metallic Bonds – Khan Academy
Pay attention to this video because seeing how atoms with higher elecronegativity “hog” the electrons will help you understand how some molecules can be polar.
8. Polar Covalent Molecules and Dot Structures
The video you just watched from lesson 7 will help you understand polarity and electron dot symbols.
10. Experiment: Demonstrating Polar Properties
You don’t have to perform this experiment yourself. Just watch this video about water (a polar molecule) and answer the questions. Since Carbon Tetrachloride has four identical atoms bonded to one central atom it will be shaped just like a methane molecule which was described in the lesson on Polar Covalent Molecules. Is it polar or not?
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CHEMISTRY B
Unit 1: Chemical Reactions, Rates, and Equilibrium
B 1:15 Activity: Exploring Factors that Affect Equilibrium
N2O4 is colorless, NO2 is reddish-brown. This reversible reaction is heat dependent so it will move more in one direction or the other as temperature changes. That means that as the water is heated N2O4 will be turning into NO2 or NO2 will be turning into N2O4 until equilibrium is reached at the new temperature. Can you tell from the picture which way the reaction is going as temperature is increased? For question 2 the answer should either be that the products or the reactants are favored. For question 3 you are asked which reaction is exothermic. In other words, which direction (from left to right or right to left) would this reaction proceed while releasing heat? You can tell this because if a reaction needs heat to proceed it will be favored by an increase in temperature. The opposite (heat-releasing) reaction would be favored by a decrease in temperature. Let me know if you need help. This can be difficult to understand.
N2O4 is colorless, NO2 is reddish-brown. This reversible reaction is heat dependent so it will move more in one direction or the other as temperature changes. That means that as the water is heated N2O4 will be turning into NO2 or NO2 will be turning into N2O4 until equilibrium is reached at the new temperature. Can you tell from the picture which way the reaction is going as temperature is increased? For question 2 the answer should either be that the products or the reactants are favored. For question 3 you are asked which reaction is exothermic. In other words, which direction (from left to right or right to left) would this reaction proceed while releasing heat? You can tell this because if a reaction needs heat to proceed it will be favored by an increase in temperature. The opposite (heat-releasing) reaction would be favored by a decrease in temperature. Let me know if you need help. This can be difficult to understand.