Atom and Periodic Table Review
This semester review was compiled using the NC Standard Course of Study for Chemistry. You need to answer each question. This semester review is due by January 6, 2015. This packet will count as two tests and two labs. This will significantly affect your grade!!! Answers will be provided before school beginning December 1. Use your green/yellow “reference packets” as needed. You will provide me with the work you have completed and I will allow you to check your answers for those problems. You turn in questions in consecutive order (1, 2, 3, 4…) on notebook paper. (If you want to work out of order, begin a new sheet of paper each time you skip ahead.)
Atom and Periodic Table Review
1. Sketch a PT similar to the one to the right and then, label metals, nonmetals and metalloids (or semi-metals).
2. Sketch a PT similar to the one to the right and then, label periods and groups.
3. Sketch a PT similar to the one to the right and then, label s, p, d, and f blocks.
4. List the five major properties of metals.
5. Describe the five major properties of nonmetals
6. What are semi-metals/metalloids?
7. Sketch and complete a table similar to the one below.
|Particle |Location |Charge |Relative mass |
| | | |(compared with one another) |
| | | | |
| | | | |
| | | | |
8. What does the atomic number and mass number tell us about the atom?
9. What symbol is used for atomic number? Mass number?
10. Draw the Bohr model for the Al atom. Fill in the number of protons, neutrons and electrons. It is an aluminum atom with a mass number of 27.
11. Who discovered the proton?
12. Who discovered the electron?
13. Who discovered the neutron?
14. Convert 125 °C to K.
15. The “plum-pudding” model was created by
16. Who performed the “gold foil” experiments?
17. How many protons are there in zinc?
18. How many neutrons are there in mercury?
19. Air is best classified as a(n)
20. Gold is best described as a(n)
21. Water is best classified as a
22. Give 5 examples of a chemical change.
23. Give 5 examples of a physical change.
24. Give 5 examples of a physical property
25. Give 5 examples of a chemical property.
26. State the rule of thumb to determine if a chemical change has occurred.
27. What is difference between a substance and a mixture?
28. Complete the following table.
|Name |Nuclear/ Isotopic |Atomic Number |Mass Number |Average atomic mass |Protons |
| |Symbol | | | | |
|[HCl] decreases | | | | | |
|[NaCl] increases | | | | | |
|Temperature decreases | | | | | |
|[H2O] increases | | | | | |
|[NaOH] increases | | | | | |
|Pressure increases | | | | | |
|Temperature increases | | | | | |
Acid and Base Review
29. For the following compounds, determine if the compound is an acid, base, or salt. Name the compound and then determine its relative strength.
|Compound |Acid / Base / Salt |Name |Relative Strength |
|NH3 | | | |
|H2SO4 | | | |
|K2CO3 | | | |
|LiCl | | | |
|HCl | | | |
|Zn(OH)2 | | | |
|Ca(OH)2 | | | |
|HNO3 | | | |
|NH4C2H3O2 | | | |
|MgCO3 | | | |
|AgOH | | | |
|HClO3 | | | |
|NaOH | | | |
Bronsted – Lowry Acid / Base Theory
30. For each of the following reaction, label each compound as acid, base, conjugate acid, or conjugate base.
a. NH3 + HCl ( NH4+ + Cl-
____ ____ ____ ____
b. BaSO4 + 2HF ( H2SO4 + BaF2
____ ____ ____ ____
c. HC3H3O3 + LiBr ( LiC3H3O3 + HBr
____ ____ ____ ____
d. HSO3- + H2O ( SO3-2 + H3O+
____ ____ ____ ____
pH
31. Answer the following questions.
Acid or Base Color of indicator
a. pOH = 2.89 [H+] = _____________ __________________ blue litmus_____________
b. [NaOH] = 5.99 x 10-8 M pH = ______________ __________________ red litmus _____________
c. [H3O+] = 8.67 x 10-6 M [OH-] = ____________ __________________ universal ______________
d. [H+] = 1.88 x 10-10 M pH = ______________ __________________ blue litmus_____________
e. [HCl] = 8.11 x 10-2 M pOH = ____________ __________________ red litmus _____________
f. [KOH] = 5.33 x 10-7 M [H+] = _____________ __________________ pheonothalein___________
g. pH = 2.08 [H+] = _____________ __________________ universal ______________
h. [OH-] = 3.44 x 10-9 M pOH = ____________ __________________ blue litmus_____________
i. pH = 8. 23 [H+] = _____________ __________________ pheonothalein___________
Dilution
32. How much concentrated 18M sulfuric acid is needed to prepare 250 mL of a 6.0 M solution?
33. To approximately how much water should 50.mL of 12M hydrochloric acid be added to produce a 4.0M solution?
Titrations
34. Describe the graph to the right.
35. Answer the following questions about titrations.
a. The solution of known concentration is called the ____________________________.
b. The solution of known concentration is placed in the _________________ during a titration.
c. 36.7 mL of 6.72 M NaOH is used to neutralize 61.8 mL of H2CO3. What is the molarity of the H2CO3?
d. 206 mL of 3.92 M Mg(OH)2 can be used to neutralize how much 1.77 M HCl?
Precipitation Reactions
36. Balance the following reactions and determine the precipitate.
a. ___K2SO4 + ___Ba(NO3)2 ( ___KNO3 + ___BaSO4
Precipitate ( _________________
b. ___BaCl2 + ___Na2SO3 ( ___BaSO3 + ___NaCl
Precipitate ( _________________
c. ___Zn(NO3)2 + ___(NH4)2S ( ___ZnS + ___NH4NO3
Precipitate ( _________________
d. ___HgCl2 + ___K2S ( ___HgS + ___KCl
Precipitate ( _________________
e. ___Na2CO3 + ___CaCl2 ( ___NaCl + ___CaCO3
Precipitate ( _________________
f. ___CuCl2 + ___(NH4)3PO4 ( ___Cu3(PO4)2 + ___NH4Cl
Precipitate ( __________________
Nuclear Review
37. What are three types of radiation?
38. What are fission and fusion? Give common examples of how they are used or where they are found.
39. For the following statements, determine the type of radiation that best fits the description.
a. most dangerous ( ________________________________
b. no mass ( ______________________________________
c. shielded by aluminum foil ( ________________________
d. mass is equivalent to that of an electron ( _____________
e. largest form of radiation ( _________________________
f. double positive charge ( ___________________________
g. (-1) charge ( ____________________________________
h. most penetrating ( _______________________________
i. shielded by skin ( ________________________________
j. shielded by several inches of lead ( __________________
40. Complete the following nuclear reactions:
23892U ( 42He + _________________ d. 6430Zn + 0-1e ( ______________
3719K + 0+1e ( ___________________ e. 15763Eu ( 11H + ______________
3115P + 42He ( 10n + ______________ f. 23190Th + 10n ( 0-1e + _________
41. _________________________ is the splitting of nuclei and ___________________ is the combining of nuclei.
42. Name three devices used to detect radiation.
43. _____________ occurs in nuclear bombs and in nuclear power plants. ____________________ occurs in the sun.
44. Phosphorous – 32 has a half-life of 14.3 years. How many grams will remain after 57.2 years of a 4.0 g sample of Phosphorous – 32?
45. Sketch the table below, label the areas mentioned in question 37. Then identify the number of valence electrons and oxidation number for each family.
-----------------------
[pic]
[pic]
Potential Energy
D
E
C
B
A
Reaction
A.
B.
C.
D.
E.
Pressure (torr)
................
................
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