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Study Guide Exam # 2
PreAP Chemistry
Name:
Exam # 2 will be September 26 and 27 and will be over Units 2 and 3.
Collect all of your materials and put them in order. Use the handy check-off sheet below to help you
be organized!
Then, go through the materials and re-work the problems in them. Cover your answers and
actually DO the work again to quiz yourself. Remind yourself what the labs were all about, and
work through them as if you were doing it again. Get an extra copy of the periodic table and
practice labeling it. Have a friend quiz you: “Is Fe a metal or a non-metal? How do you know?” etc.
Use the list of topics to make sure you know everything you should know.
ASK QUESTIONS if you have questions! Ask in class on Thursday and Friday!
Mrs. Cummings’ office hours are Monday mornings at 8 a.m. and Thursday after school.
Mr. Hughes’ office hours are Monday mornings at 8 a.m. and Tuesday after school.
Handouts You Should Have For Unit 2:
1.
2.
3.
4.
I have it
I have worked
through it
again in detail
Packet: Density (3 pages)
A labeled full-page copy of the periodic table
Coloring the Periodic Table Practice
Nomenclature (Naming Non-Metals and Naming Simple
Ionic Compounds)
5. Lab: Properties of Elements: Metals, Nonmetals, and
Metalloids
6. BW and Practice Quiz Density 9.3 9.4
7. BW 9.6 9.7 Elements Lab, Density
8. Class Notes on Atomic Structure (on your own paper in
your own handwriting)
Handouts You Should Have for Unit 3:
1. Packet: Models of the Atom (includes Lessons 11 and 12)
2. BW 9.12 9.13 Algebra, History of the Atom
3. Packet: Class Notes Isotopes and Average Atomic Mass
(includes Lesson 13 and the Average Atomic Mass
worksheet)
4. BW Nuclide Symbols and Isotopes (includes L14: Isotopia
and IP Atomic Models)
5. BW September 16 and 19
6. Packet: Nuclear Fission and Nuclear Fusion
Use the list of topics on the back of this paper to help you make sure you’ve gone over
everything.
Topics on the exam will be:
Unit 2 Atoms and Molecules
1. Density – how to calculate it, how to use it to identify materials, how to measure it in lab,
how cm3 is related to ml, how materials of different densities will stack
2. Given a periodic table, identify whether a certain element will be a metal, a nonmetal, or a
metalloid (G)
3. Describe three differences between metals, nonmetals, and metalloids (G)
(malleability, luster, and conduct electricity)
4. Given a sample of an element, use physical properties to classify the element as a metal,
metalloid, or nonmetal (L)
5. Given a periodic table, label alkali metals, alkaline earth metals, halogens, and noble gases.
Label transition metals. (G).
6. State four parts of Dalton’s Atomic Theory (G)
1. All Elements are composed of small, indivisible particles called atoms.
2. All atoms of the same element have exactly the same properties.
3. Atoms of different elements have different properties.
4. Compounds are formed when atoms are joined together. Since atoms are indivisible,
they can join together only in simple, whole number ratios.
7. Identify whether a compound is ionic or covalent (molecular) by determining if a metal is
present in the name (L)
8. Name covalent compounds (L)
9. Name ionic compounds that contain metals in groups 1A, 2A, and 3A (L)
Unit 3 Atomic Structure
10. Describe how the model of the atom has changed through time, citing the contributions of
Democritus, Plato, Aristotle, Dalton, Thomson, Rutherford, and Bohr. Include simple
sketches of the models and descriptions of what evidence each experiment provided (G, L)
11. Determine the number of protons, neutrons (approximate), and electrons in an atom from
information on the periodic table. [L]
12. State that a nuclide symbol includes the mass number and atomic number, and state the
meaning of each of those numbers. Determine the number of protons, neutrons, and
electrons from the nuclide symbol. (L)
13. Draw simple pictures of atoms (Bohr model) from nuclide symbols (L)
14. Given information about an atom, write the nuclide symbol and name (such as 31P,
Phosphorus-31) (L)
15. Define isotope (G)
16. Calculate average atomic mass of a sample of atoms, from percentages and from simple,
whole numbers of atoms (L)
17. From the average atomic mass, estimate the number of neutrons present in the isotopes
(Rh)
18. Interpret a graph of the isotopes (neutrons vs. protons) (L)
19. Explain why there are more neutrons than protons in the larger elements (protons repel
each other) (L)
20. Compare and contrast fusion and fission (L)
21. Compare and contrast nuclear reactions with chemical reactions (L)