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Your chemistry final will be on _____________________________ Room # ________. The
final begins at 10:00. You must bring the following with you or you will not be permitted to
take the final:
 2 #2 pencils
 calculator
 text book
The following will be included on the final exam.
The exam consists of
a. 100 multiple choice questions
b. 6 math problems worth a total of 100 points
c.
2 essential questions to answer, worth 10 points each. You have your choice of two out of the 4
questions given. The topics of these questions are:
Question 1
Hydrate lab, calculate percent water of hydrate, and analyze likely sources of error
Question 2
Describeing atomic model changes over time
Question 3
Significance of the mole
Question 4
Significance of the periodic table in determining properties of atoms
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Final Exam Sample Problems Sheet
1. An element has r has two naturally occurring isotopes: X-63 and X-65. The relative
abundance of X-63 is 69.17%; the atomic mass of X-63 is 62.94 amu; the relative
abundance of X-65 is 30.83%; the atomic mass of X-65 is 64.93 amu. (10 points)
a. Determine the average atomic mass for X. You must show all of your work and
include the units.
b.
What element is element “X”
2. You are given 0.551 g of ferric nitrite. (20 points)
1. Calculate the molar mass and percent composition of ferric nitrite. (5)
2. Calculate the number of moles of ferric nitrite in 0.551 g (5)
3. Calculate the number of molecules in 0.551 g of potassium ferricyanide(5)
3. Chemical analysis of citric acid shows that it contains 64.27% C, 7.19% H, and 28.54% O.
a. What is its empirical formula? (10 points)
b. If the molar mass of the molecular formula 168.19, determine the molecular formula of
the compound (10 points)
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4. The following questions refer to the molecule PCl3
a) Draw its Lewis structure (10 points)
b) What is the name of the shape of the molecule (2 points)
c) Is it polar or nonpolar? (2 points)
d) What type of intermolecular force would occur between these molecules? (2 points )
e) Would the boiling point likely be low, medium or high for this compound?(2 points )
f) Name the hybridization that occurs on the central atom of this molecule (2 points)
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5. Aluminum carbonate reacts with magnesium bromide
Write the balanced equation for this reaction
a. If 15.0grams of aluminum carbonate reacts with 46.0 grams of magnesium bromide,
what is the limiting reagent? (10)
b. How many grams of each product will be produced ? (5)
c. What is the excess reagent?
d. How many grams of excess reagent will remain ? (5)
6. (10 points)
a. . What is the electron configuration notation for Zr ________________________
b. What is the shorthand notation for Pb ___________________________________
c. Write the orbital notation for S ________________________________________
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Other types of questions
1. Define matter
2. Distinguish between quantitative and qualitative data
3. Distinguish between intensive and extensive properties
4. Distinguish between a physical and chemical properties
5. Distinguish between endothermic and exothermic changes
6. List the 6 phase changes, determine which are endothermic and which are exothermic
7. Define solid, liquid, and gas
8. Distinguish between pure substances and mixtures
9. How many significant digits are in .005700
10. How many significant digits are in 240,000,100
11. Distinguish between accuracy and precision
12. Round .00980040 to 3 significant digits
13. Write 2.5 x 105 in standard notation
14. Write 450,300 in scientific notation
15. Write .005701 in scientific notation
16. (3.35 x 107) + (2.26 x 106)
17. (2.24 x 104) - (3.1 x 102)
18. (3.2 x 105) x (8.1 x 102)
19. (4.5 x 10-3) / (2.25 x 104)
20. Meaning of kilo?
21. If a substance has a mass of 3.2g and a volume of 8.7 ml. What is its density.
22. How do you convert from celsius to kelvin?
23. Where on the periodic table are the metals? Metalloids? Nonmetals? Nobel gases?
24. What is Dalton's atomic theory?
25. What is an atomic mass unit?
26. What is the law of Conservation of mass?
27. Describe Rutherford’s experiment and his model of the atom
28. What did Bohr find?
29. How are wavelength and frequency related?
30. What is an isotope?
31. How do you find how many grams of an element are in a mole?
32. How many atoms are in a mole?
33. What is an orbital?
34. What are quantum numbers?
35. What is: Hund's Rule, Pauli exclusion principle? Aufbau principle? Heisenberg uncertainty
principle?
36. What happens to the frequency of light as its wavelength increases?
37. How manyelectrons are in the 1st energy level? 2nd energy level? 3rd? 4th?
38. How many orientations or sublevels do the following have: s____ p____ d____ f_____
39. How many electrons can each of the following hold? S___ p____ d____ f____
40. How did Mendeleev and then Mosely arrange the periodic table?
41. What are the alkali metals:
alkaline earth metals
transition metals:
42. What is ionization energy
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43. What happens down a group and across a period for the following trends:
Atomic radius:
GROUP
PERIOD
Ionization energy:
Electron affinity
Shielding effect
Electronegativity
47. Oxidation number of halogens: alkaline earth metals alkali metals
48. How many extra electrons does the slfate polyatomic ion have?
49. What are anions and cations?
50. What is the formula for triphosphorus pentoxide?
51. What is the formula for iron III sulfide?
52. What is a covalent bond?
An ionic bond?
53. Know how to subtract electronegativities to find bond type (ionic, polar and nonpolar
covalent) Ex: What kind of bond is between: H-F _____ O-O _____ Ca-Cl_______
(you will need to look up their electronegativities)
54. What is the octet rule?
55. What is the relationship between bond length and bond energy?
56. Use VSEPR theory to find the shapes of:
O2
CCl4
CS2
PCl3
57. Are the above molecules polar or nonpolar?
58. Name the molecules from #56.
59. State the hybridization around the central atom that is occurring in each molecule in
question 56.
60. Be able to determine if a reaction is SD, DD, COM, SYN, or DEC ( 6 questions)
Forr the next questions, identify what type of reaction it is. Use the abbreviations S, D, SD, DD,
AB, or C.
1. AgNO3 + NaCl  NaNO3 + AgCl
2. F2 + 2 NaCl  2 NaF + Cl2
3. CH4 + 2 O2  CO2 + 2 H2O
4. 2 Mg + O2  2 MgO
5. HCl + NaOH  NaCl H2O
6. H2O  H2 + O2
Special Decompositions:
What do the following decompose into:
7. Metal hydroxides
8. Metal carbonates
9. oxyacids
61. What do these symbols mean? (s)(aq)
(ppt)

62. Be able to predict products if given reactants and balance.
63. What is the ideal gas law?