Download chemistry final exam - Mr. Carlson`s Chemistry Class

CHEMISTRY FINAL EXAM
1. The following molecule, H2, is: A. Organic B. Inorganic C. A gas D. Both B
and C
2. Matter is anything that has: A. force and weight B. Kinetic energy and Potential
energy C. Volume and Mass D. Electrons and a nucleus
3. The law of conservation and energy states that energy cannot be: A. Created or
changed B. Created or destroyed C. Changed or destroyed D. None of the above
4. The 5 states of matter are solid, liquid, gas, : A. Silly Putty and Jell-O B. Plasma
star and neutron C. Plasma and neutron star D. Ice and heat
5. Express the following calculation in the proper number of significant figures for
this calculation, 3.034 + 5.1 : A. 8.134 B. 8.13 C. 8 D. 8.1
6. Choose the correct number of significant figures for this calculation, 3.034 X 5.1:
A. 15.4 B. 15.47 C. 15 D. 15.5
7. Determine the kinetic energy of Mr. Carlson’s golf ball with a mass of .55 kg as it
rolls down the fairway with a velocity of 9.3 m/s: A. 23.8 J B. 24. J C. 2.6 J D.
2.56 J
8. Calculate the mass of a substance with a volume of 30. mL and a density of 5.00
g/mL : A. 150 g B. 6.0 g C. 1.5 X 102 D. 1.5 X 103
9. The chemical names for these elements, respectively, Li, C, and F are: A.
Lithium, Calcium, Fluorine B. Lithium, Carbon, Fluorine C. Lead, Carbon,
Fluorine D. Carbon, Lithium, Fluorine
10. These elements are in Group 2: A. Barium and Hydrogen B. Lithium and Barium
C. Beryllium and Magnesium D. Sodium and Magnesium
11. These elements are Alkali metals: A. Hydrogen and Lithium B. Beryllium and
Magnesium C. Lithium and Beryllium D. Potassium and Rubidium
12. The chemical symbol for Sodium is: A. S B. So C. Na D. N
13. Which one of these theories was a flaw in Dalton’s model of the atom: A. Atoms
of different elements have different physical and chemical properties B. Atoms of
different elements combine in simple, whole number ratios to form chemical
compounds C. All matter is made of indivisible and indestructible atoms D. None
of these were flaws.
14. The flaw that existed in Thomson’s plum pudding model of the atom was that: A.
Atoms cannot be subdivided or combined B. A ball of positive charge with
electrons in it. C. A ball of negative charge with protons in it D. Too much
pudding, not enough plums.
15. The element Oxygen has how many protons, electrons, and neutrons,
respectively: A. 8,16,8 B. 8,8,8 C. 16,16,8 D. 8,8,16
16. The atomic mass of Boron, using 3 significant figures, is: A. 11 B. 11.0 C. 10.8
D. 10.9
17. The electron configuration for Magnesium is: A . 1s22s22p6 B. 1s22s23s22p6 C.
1s22s22p63s2 D. 1s22s42p6
18. The orbital diagram for Lithium is: A.
B.
C.
D.
2s
2s
1s
1s
1s
2s
1s
3s
19. The three quantum numbers for Sodium are : A. n=2, l=s, ms= +/- ½ B. n=3, l=s,
ms= +/- ½ C. n=3, l=p, ms= +/- ½ D. n=1, l=s, ms= +/- ½
20. Determine the number of neutrons for 157 N: A. 7 B. 8 C. 9 D. 15
21. The alkaline-earth metals are found in Group: A. 1 B. 2 C. 13 D. 14
22. The main-block elements are Group 1 and 2 and Groups: A. 13-18 B. 14-18 C.
13-17 D. 3-18
23. Which group is stable and unreactive? : A. Halogens B. Alkali metals C. Noble
gases D. Metalloids
24. Which group has a single electron in the highest energy level?: A. Alkali metals
B. Alkaline-earth metals C. Halogens D. Noble gases
25. Which element reacts more readily with chlorine: A. Sodium B. Fluorine C.
Magnesium D. Calcium
26. The group that has the most negative electron affinity is the: A. Halogens B.
Noble gases C. Alkali metals D. Pink Floyd
27. The most electronegative group is the : A. Noble gases B. Halogens C. Alkali
metals D. Hydrogen
28. This element has the highest ionization energy: A. Lithium B. Sodium C.
Potassium D. Cesium
29. What is the mass in grams of 5.20 X 1010 mol of uranium. The molar mass of
uranium is 238 g: A. 2.10 X 108 g B. 1.238 X 1013 g C. 2.184 X 108 g D. 1.24
X 1013 g
30. Calculate the number of atoms in 10.0g of sulfur: A. 5.31 X 10-22 atoms B. 5.91
X 10-22 atoms C. 1.88 X 1023 atoms D. 1.88 X 1023 grams
31. Calculate the number of atoms in 54.0g of Magnesium: A. 1.34 X 1024 atoms B.
5.91 X 1023 atoms C. 2.10 X 10-21 atoms D. 1.45 X 1023 atoms
32. The formula for aluminum fluoride is : A. AlF2 B. AlF C. AlF3 D. Al2F3
33. The formula for ammonium hydroxide is: A. NH3O B. NH3  H2O C. NH4OH
D. NH4HO
34. The formula for copper (II) phosphate is: A. Cu2(PO4)2 B. Cu2P3 C. Cu3(PO4)2
D. Cu3P2
35. The name for this compound is, (NH4)2SO4 : A. Ammonia sulfate B.
Ammonium sulfite C. Ammonia sulfate D. Ammonium sulfate
36. The molar mass of zinc (II) carbonate is: A. 159 g/mol B. 175 g/mol C. 109
g/mol D. 125 g/mol
37. The molar mass of ZnS is 97.5 g/mol. The molar mass of SO2 is 64.1 g/mol. The
percentage of sulfur in SO2 is : A. 25 % B. 50 % C. 75 % D. 33 %
38. Aluminum chlorohydrate is an ingredient used in some antiperspirants. In its
anhydrous form, it has 30.93 % Al, 45.86 % O, 20.32 % Cl, and 2.89 % H. What
is the empirical formula for aluminum chlorohydrate: A. Al3H6ClO2 B. AlHClO3
C. Al2H5ClO5 D. Al5H3Cl2O2
39. The C-H bond in polyethylene is: A. Ionic B. Polar covalent C. Nonpolar
covalent D. Dipole force
40. The oxidation number for oxygen is Fe2O3 is: A. +2 B. –3 C. +3 D. –2
41. The name for the following compound NO, is: A. Nitrogen monoxide B.
Nitrogen dioxide C. Nitrogen oxide D. Nitrous oxide
42. The shape of a compound that has a central carbon atom with double bonds to two
sulfur atoms is: A. Tetrahedral B. Trigonal planar C. Linear D. Bent
43. What is the molecular formula of paradichlorobenzene, an ingredient in moth
balls that has a molar mass of 147.00 g/mol and an empirical formula of C3ClH2?:
A. C3ClH2 B. C9Cl3H6 C. C6Cl2H4 D. C1.5Cl.5H1
44. Put the following word equation into a balanced formula equation:
nitrogen dioxide + water  nitric acid + nitrogen monoxide
A. NO2 + H2O  2HNO3 + NO
B. 2NO2 + H2O  HNO3 + 3NO
C. 3NO2 + H2O  3NO3 + NO
D. 3NO2 + H2O  2HNO3 + NO
45. Balance the following equation: CaH2 (s) + H2 (l)  Ca(OH)2 (aq) + H2 (g)
A. 1:2:1:1
B. 1:1:2:1
C. 1:2:1:2
D. 2:1:2:1
46. Al2O3 + 3H2SO4  Al2(SO4)3 + 3H2O. How many moles of Al2(SO4)3 would
would be produced if 6 mol of H2SO4 reacted with an excess of Al2O3?
A. 3 B. 1 C. 6 D. 2
47. The balanced chemical equation for the synthesis of the pollutant nitrogen dioxide
from nitrogen monoxide and oxygen gas is:
A. 6NO2  6NO + 3O2
B. 2NO2 + O2  2NO
C. 3NO  NO2 + O2
D. 2NO + O2  2NO2
48. Mass-Mass If 0.500g of sulfur dioxide from pollutants reacts with excess water
and oxygen found in the air, how many grams of sulfuric acid are produced?
2H2O + O2 + 2SO2  2H2SO4
A. .382 grams B. 1.53 grams C. .765 grams D. .510 grams
49. The two compounds being compared in #48 are: A. O2 and H2SO4 B. SO2 and
H2SO4 C. H2O and H2SO4 D. O2 and SO2
50. The last step in determining how many grams of sulfuric acid are produced is:
A. 2mol H2SO4
B. 2mol SO2
C. 98.09g H2SO4 D. 82.09 g H2SO4
2mol SO2
2mol H2SO4
1mol H2SO4
1mol H2SO4
51. Mole-Mass 2KClO3  2KCl + 3O2
If I have 4.0 moles of KClO3, how many grams of O2 do I have?:
A. 1.62 X 102 g B. 1.9 X 102 g C. 4.7 X 103 g D. 5.7 X 105 g
52. For #51, I have 4.0 moles of KClO3, how many moles of O2 do I have?:
A. 4.0 B. 3.0 C. 8.0 D. 6.0
53. Density 4NH3 + 5O2  4NO + 6H2O ; Ammonia gas= 25.0 mol ; Density
of NO = 1.340 g/L ; How many moles of NO will be produced if I have an
excess of O2?: A. 6 mol B. 6.25 mol C. 25.0 mol D. 100. mol
54. How many grams of NO will be produced if I have an excess of O2?: A. 750.g
B. 180. g C. 25.0 mol D. 100. mol
55. How many liters of NO will be produced?: A. 134. L B. 140. L C. 2.24 X 103 L
C. 600. L
56. Limiting Reactant
O
H
O
OH
+
H3C-OH 
+
H2O
O
Butanoic acid
Methanol
Methyl butanoate
Water
What is the chemical formula for butanoic acid?: A. C3H5O2 B. C3H7O2 C. C4H6O2
D. C4H8O2
57. If 50.0 g of butanoic acid react with 40.0g of methanol, then which compound is
limiting reactant? : A. Methyl butanoate B. Methanol C. Butanoic acid D. Water
58. Refer to #57. How many grams of Methyl butanoate can be produced?:
A. 81.3 g B. 57.9 g C. 103. g D. 21.4 g
59. Percent Yield
MgCl2  Mg + Cl2 ; If I have 50.0g of MgCl2, and I
produce 30.0g of Cl2, what is my percent yield? A. 52% B. 33% C. 60% D. 80%
60. 2C + 2H2O  CH4 + CO2 ; If this reaction has a percent yield of 85.0%, how
much methane can be obtained from 1250g of carbon?: A. 620.g B. 546.g
C. 233.g D. 710.g
EXTRA CREDIT
(Put work and answer on the answer sheet)
+5 E.C. points
61. Plaster of Paris, CaSO4  ½ H2O, has many uses, including castings and dental
cement. It can be obtained by heating gypsum CaSO4  2H2O. How many liters of
water vapor evolve when 5.00L of gypsum are heated at 110C to produce plaster of
Paris? At 110C the density of CaSO4  2H2O is 2.32 g/mL, and the density of water
Vapor is 0.581 g/L.
CaSO4  2H2O  CaSO4  ½ H2O + 3H2O
1.______
2.______
3.______
4.______
5.______
6.______
7.______
8.______
9.______
10._____
11._____
12._____
13._____
14._____
15._____
16._____
17._____
18._____
19._____
20._____
21._____
22._____
23._____
24._____
25._____
26._____
27._____
28._____
29._____
30._____
31._____
32._____
33._____
34._____
35._____
36._____
37._____
38._____
39._____
40._____
41._____
42._____
43._____
44._____
45._____
46._____
47._______
48._______
49._______
50._______
51._______
52._______
53._______
54._______
55._______
56._______
57._______
58._______
59._______
60._______
61. Show Work