Acs General Chemistry Study Guide 2015
Laboratory Chemistry; Preparing for Your ACS Examination in Organic Chemistry: The Official Guide (commonly called the Organic Chemistry Study Guide) This guide includes 164 pages of information in essentially three categories. First, there is a brief explanation of content in organic chemistry.
2015–present Senior Instructor II, University of Oregon. 2013–2015 Morrill Professor, Iowa State University. 1998-2013 Professor of Chemistry, Iowa State University.
2013-2014 Visiting Lecturer, University of Oregon. 2006 Visiting Professor, University of Arizona.
1990-1998 Associate Professor, Iowa State University, 1988-1990 Associate Professor of Chemistry and Director of Freshman Programs, University of Massachusetts – Dartmouth. 1985-1988 Assistant Professor of Chemistry and Director of Freshman Programs, University of Massachusetts – Dartmouth. 1983-1985 Visiting Lecturer and General Chemistry Laboratory Coordinator, Southeastern Massachusetts University.
1978-1983 Director of the Chemistry Lecture Demonstration Laboratory, Purdue University. 2014 American Chemistry Society George C. Gupta, T., Burke, K.A., Mehta, A., Greenbowe, T.J.
Impact of guided-inquiry-based instruction with writing and reflection emphasis on chemistry students’ critical thinking abilities. Journal of Chemical Education, 92(1), 32–38. Augspurger, A.E., Stender, A.S., Marchulk, K., Greenbowe, T.J., Fang, N. Dark field microscopy for analytical laboratory courses.
Journal of Chemical Education, 91(6), 908-910. And Greenbowe, T.
“Reading Guide and Sample AP Chemistry Test Questions for N. Tro’s Chemistry (3 rd Edition).” Pearson Education, Inc.: Upper Saddle River, NJ.
AP® Chemistry Guided Inquiry Activities for the Classroom: Curriculum Module. DeWane & T.J. Greenbowe (Eds.). The College Board: New York, NY.
And Greenbowe, T. “Acid-base neutralization reactions,” In AP® Chemistry Guided Inquiry Activities for the Classroom: Curriculum Module. DeWane & T.J. Greenbowe (Eds.). The College Board: New York, NY. Greenbowe, T.J.; Gelder, John I.; Abraham, M.R.
“Computer Simulations and Animations for Electrolysis”. Pearson Education, Inc.: Upper Saddle River, NJ.
Parham, T., Cervato, C., Gallus, W., Larsen, M., Hobbs, J., and Greenbowe, T. Are movies and popular media driving students’ poor understanding of volcanic processes? Journal of College Science Teaching, 41(1), 14-19. And Greenbowe, T.J. “A Shoebox Polarimeter: An Inexpensive Analytical Tool for Teachers and Students.” J. Educ., 88(8), 1194–1197. Parham, T.L.; Cervato, C.; Gallus, W.A.; Larsen, M.; Hobbs, J.; Stelling, P.; Greenbowe, T.J.; Gupta, T.; Knox, J.A.; Gill, T.E.
“The InVEST Volcanic Concept Survey: Exploring Student Understanding About Volcanoes.” Journal of Geoscience Education, 58 (3), 177-187. Chemists’ Guide to Effective Teaching Volume II. Greenbowe, M. Copper (Eds.). Pearson/Prentice-Hall: Upper Saddle River, NJ. Liu, Han-Chin; Andre, T.; Greenbowe, T.J. “Impact of Learner's Prior Knowledge on Their Use of Chemistry Computer Simulations: a Case Study.” Journal of Science Education and Technology (17), 466-482.
Schroeder, J.D, and Greenbowe, T.J. “Implementing POGIL in the Lecture and the Science Writing Heuristic in the Laboratory: Student Perceptions and Performance in Undergraduate Organic Chemistry.” Chemical Education Research and Practice (9), 149-156. Rudd, II, J.A.; Greenbowe, T.J.; Hand, B.M.
“Using the Science Writing Heuristic to Improve Students’ Understanding of General Equilibrium.” Journal of Chemical Education, 84(12), 2007-2012.
The first thing you need to do is purchase the ACS official study guide. The book is just over 100 pages long and provides example questions along with explanations for the correct answer.
It is separated into the following categories, each containing an impressive set of practice questions similar to the ones you will find on the exam. Atomic Structure. Molecular Structure and Bonding.
Stoichiometry. States of Matter/Solutions. Energetics (also known as thermochemistry or thermodynamics). Dynamics.
Equilibrium. Electrochemistry/Redox. Descriptive Chemistry/Periodicity. Laboratory Chemistry In many Gen Chem I courses, dynamics and equilibrium are not discussed, and they will not be reviewed in this article.
The exam focuses on remembering important constants and trends, and that is where a good memory and steady studying can boost your grade on this exam. Isotopes are varied forms of an element that have different mass numbers. It is almost guaranteed that the exam will contain an isotope question: for example, something like this: How many protons are in the isotope 28Al? It is important to remember that different isotopes of an element will not vary in the number of protons. The amount of protons will always be the atomic number, which in the case of aluminum (Al) is 13. The number of electrons in 28Al, or any isotope of the pure element (aluminum metal), is also 13. The only way the amount of electrons will change is if there is a charge on the atom.
An atom with a charge, called an ion, will have the charge written as a superscript. The aluminum ion Al 3+, which has a charge of +3, would have 10 electrons.
A positive charge means electrons are lost when the atom becomes an ion. The number of neutrons is slightly trickier. You must subtract the atomic number from the atomic weight (mass number). In this case, that would be 28-13, which is 15. So 28Al has 15 neutrons.
A good way to remember this is to think of neutrons as the 'black sheep' of the atom. They have no charge, so it requires a little more effort to figure out how many of them there are. This topic gets a little tricky, especially if you are not good at remembering names. Expect to see at least one question on the geometry of an atom. As the exam does not want you to waste unnecessary time on a simple task, it is likely that the structure will already be done for you: now it is just a matter of knowing your stuff.
It is important to remember that lone electrons on the central atom of the structure count as a side of the figure. Many books will use a to figure out the geometry, but this technique is rather involved for this exam and will not be discussed. There is not much to say about this topic, either you know it or you don't. This topic is used frequently in the test and you should have a solid knowledge of these three things: 1. How to find the empirical and molecular formula for a compound 2.
How to find the percent composition of a compound 3. How to determine the mass of a compound yielded using a balanced equation You will also need to know how to use Avogadro's number correctly (6.022 x 10 23). Some questions may ask you to find the amount of atoms or molecules in something, in which case you need to know that there are 6.022 x 10 23 molecules in one mole of something. There are two things that should be stressed regarding this topic. The first is that you know what a phase diagram is and what it represents. It represents phase changes in an element or compound under different temperatures and pressures: the x axis is temperature and the y axis is pressure.
A phase diagram usually has a nice prong shape, with the middle being the liquid phase, the left side being the solid phase, and the bottom is the gas phase. It is also important to know the names of phase changes (sublimation, condensation, etc.). The most importance thing about energetics is knowing your equations and strategies! Remember: q=mcΔT and under constant pressure: -mcΔT=mcΔT Also remember to keep your constants straight! Your value for the specific heat has units, which should match your other variables. Specific heat values will be given to you, of course. You should also know how to calculate ΔH, which is done in several ways: 1.
Hess's Law: If you don't remember, Hess's Law requires manipulation of several equations that are combined (along with respective ΔH) to calculate ΔH for a target reaction. NΣProducts - nΣReactants, where n is the number of moles (given in a balanced equation) and respective ΔH values are given for the formation or decomposition of the compounds in the reaction.
It is also good to know. Though some courses will have covered electrochemistry in detail, others leave out that subject to save time. It will not be discussed here, but for more information.
Redox There will be at least one redox-related question on the exam. Here are a few things to keep fresh in mind. How to determine oxidation numbers (remembering that certain elements, like oxygen, sulfur, hydrogen, and flourine have set oxidation numbers). How to determine reduced and oxidized elements in a reaction (and their agents!).
How to properly balance a reaction performed in either basic or acidic solution (though this is less likely to appear, it is good to know if continuing on with chemistry) And on that note, know the difference between a 'solution' and a 'solvent'! A solvent dissolves in a solute, and creates a solution.
This topic really tests your ability to remember closely related periodic trends, as well as specific traits. Here is a list of what you might see. Questions about physical properties of the transition metals.
For example, transition metals usually turn vibrant colors when ionized. Questions about atomic radii. This is where you NEED to know the trend. The smaller elements are in the upper right corner while the largest are in the bottom left corner. Ions are tricky, this is where you need to compare the amount of protons in the atom and the amount of electrons.
If an atom has more protons than electrons, then the nucleus is more effective at pulling electrons in, making it smaller. Questions about electronegativity. The trend here is, the smaller the atom, the more electronegative it is.
This is also good to know if you get a question about polarity. There needs to be an uneven spread of polar bonds in a molecule in order to be polar. Knowing your equipment. Sure, you know what a beaker is, but how about a mass spectrometer? (it separates atoms by size, by the way). Knowing your significant figures. This is a huge deal in any science.
If you don't know this by now, you better get going! You also need to be fknow how many significant figures common lab equipment can read to.
A buret measures to two decimal places, by the way. Knowing the difference between precision and accuracy.
Let's say your target number is 35.51. If you get 35.81 and 35.80, that is precise, but not accurate.
If you get 35.90 and 35.70, that is accurate, but not precise. You may also be asked to calculate percent error. The equation for this is: absolute value (actual - theoretical) / actual value. For more information on managing or withdrawing consents and how we handle data, visit our Privacy Policy at: Show Details Necessary HubPages Device ID This is used to identify particular browsers or devices when the access the service, and is used for security reasons.
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Acs General Chemistry Study Guide 2017
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Acs General Chemistry Study Guide 2015 Pdf
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