Instructions for the Christmas Take-home
This represents a 100 point grade.
Please print out a copy of this assignment.
Answer all questions as you would a regular homework assignment.
HAVE A PARENT SIGN IT, NO MATTER HOW YOU DO IT (TYPED OR HAND-WRITTEN).
The due date is the first class day back (Jan 2, 2008 is Day 6; C & F are due then; Jan 3, 2008 is Day 3; A is due then).
A deduction of 10- (minus 10) will be assessed for each day late; any assignments not handed in by Monday, January 7, 2008, will be given a zero).
NOTE: Friday, Day 7 (Jan 4, 2008) will be a test on STOICHIOMETRY.
THE ASSIGNMENT BEGINS ON THE NEXT PAGE! (SCROLL DOWN!)
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NAME: ______DECEMBER 18, 2007
CHEMISTRY CHRISTMAS TAKE HOME EXAM MR. SCIAME
1. The apparent charge (oxidation number) of oxygen in most molecular compounds is
a. 2+ b. 1+ c. 1- d.2-
2. The only common polyatomic ion having a positive charge is
a. nitrate. b. sulfate. c. ammonium. d. chromium.
3. The naming system that identifies the 2+ charge compound of iron sulfide as iron(II) sulfide is the
a. European System. b. Stock System. c. International System. d. Traditional System.
4. A binary ionic compound made from sodium and chlorine is named
a. sodium chloride. b. sodium chlorate. c. sodium chlorite. d. sodium chlorine.
5. In an ionic compound of aluminum oxide the aluminum atom has a charge of 3+ and the oxygen atom has a charge of 2-. What is the formal unit for aluminum oxide?
a. AlO b. A1606 c. A1203 d. Al302
6. The type of formula that is used for an ionic compound is
a. empirical. b. molecular. c. structural. d. any of the above.
7. In most cases compounds formed from two nonmetals are of a type called
a. periodic. b. ionic. c. semimetallic. d. molecular.
8. The elements with the most nonmetallic properties would be found in which section of the periodic table?
a. upper right b. upper left c. lower right d. lower left
9. The empirical formula of C12H26 is
a. C12H26. b. C6H13. c. CH14. d. CH.
10. The chemical formula in the figure to the right is an example of a(n)
a. mathematical formula. B. empirical formula c. molecular formula d. structural formula
11. The ratio of iron (Fe) atoms to oxygen (0) atoms in the formula, Fe203, is
a. 2:3. b. 3:2. c. 1:2. d. 1:3.
12. All of the following elements form diatomic molecules except
a. iodine. b. hydrogen. c. phosphorous. d. chlorine.
13. A chemical formula is used to represent
a. the composition of a compound. b. the number of atoms in a molecule of an element.
c. both the the above. d. neither of the above.
14. A chemical symbol is used to represent a chemical
a. solution. b. mixture. c. compound. d. element.
15. If a calcium ion has a 2 + charge, the total number of positive charges represented by one formula unit of Ca3(P04)2 is
a. 1. b. 2. c. 3. d. 6.
16. Which of the following properties is not associated with metallic elements?
a. malleable b. brittle c. ductile d. good conductors
17. If the compound PbO is named plumbous oxide, what is the name of Pb02?
a. plumbous oxide b. plumbic oxide c. plumbic peroxide d. plumbous peroxide
18. Charges on the ions of some elements can be determined from the position of the element in the periodic table. For example, the elements in Group 2 have charges of
a. 2+. b. 1+. c. 1- d. 2-
19. In the traditional system, the name of the compound P205 is
a. phosphorous pentate. c. diphosphorous pentoxide.
b. phosphorous oxide. d. phosphorous(II) oxide.
20. The apparent charge (oxidation number) of sulfur in the molecular compound SO2 is
a. 2+. b. 4+. c. 2- d. 4-
For questions 21-28, find the mass of the compound in units (u):
21. Na2S (Na = 23 u; S = 32 u)
a. 55 u b. 64 u c. 78 u d. 87 u
22. Ba(NO3)2 (Ba = 137 u; N = 14 u; O = 16 u)
a. 261u b. 294 u c. 303 u d. 321 u
23. (NH4)3P (N = 14.0 u; H = 1.0 u; P = 31.0 u)
a. 56.0 u b. 85.0 u c. 87.0 u d. 93.0 u
24. CH3Cl (C = 12.0 u; H = 1.0 u; Cl = 35.5 u)
a. 48.5 u b. 50.5 u c. 51.5 u d. 54.5 u
25. SiF4 (Si = 28.1 u; F = 19.0 u)
a. 47.1 u b. 63.4 u c. 92.1 u d. 104.1 u
26. Cu2SO4 (Cu = 63.5 u; S = 32.1 u; O = 16.0 u)
a. 223.1 u b. 233.1 u c. 234.4 u d. 249.1 u
27. NaHCO3 (Na = 23.0 u; H = 1.0 u; C = 12.0 u; O = 16.0 u)
a. 52.0 u b. 76.0 u c. 84.0 u d. 88.0 u
28. H2S03 (H = 1.0 u; S = 32.1 u; 0 = 16.0 u)
a. 50.1 u b. 82.1 u c. 85.1 u d. 87.1 u
Write either the traditional or Stock system name for each of the following compounds.
29. Na2S
30. NH4C1
31. CuF
32. CuF2
33. PbSO4
34. Hg(NO3)2
35. A12O3
36. N2O4
37. H2S (acid name)
38. HC1O3 (acid name)
Write the formula for each of the following compounds.
39. nickel(II) chloride
40. cuprous nitrate
41. ammonium sulfate
42. magnesium nitride
43. mercury(I) sulfide
44. carbon monoxide
45. nitrogen(III) oxide
46. diphosphorus pentoxide
47. sulfurous acid
48. periodic acid
49. sodium chloride
50. tin (IV) iodide