Semester 2 Practice Final. Fill in answers on scantron!
Significant Figures
1. Which of the following represents the greatest amount?
a. 5.3 X 104
b. 5.3001 X 103
c. .000057
d. 53,010
2. The diameter of a carbon atom is 0.000 000 000 154 m. What is this number
expressed in scientific notation?
a. 1.54 x 1012 m
b. 1.54 x 10-12 m
c. 1.54 x 1010 m
d. 1.54 x 10-10 m
3. How many significant figures are there in the measurement 0.0034 kg?
a. two
b. three
c. four
d. five
4. How many significant figures are there in the measurement 811.40 grams?
a. two
b. three
c. four
d. five
5. What is the measurement 111.009 mm rounded off to four significant digits?
a. 111 mm
b. 111.0 mm
c. 111.01 mm
d. 0110 mm
Metrics
6. Which temperature scale has no negative temperatures?
a. celsius
b. fahrenheit
c. kelvin
d. pascal
7. How many centimeters are there in 3 kilometers?
a. 3 x 10-5 cm
b. 3 x 10-3 cm
c. 3 x 103 cm
d. 3 x 105 cm
8. Which of the following ratios is a correct conversion factor for changing
kilometers into meters?
a. 0.001 km
1m
b. 1000 km
1m
c. 1000 m
1 km
d. 0.01 m
1 km
Matter
9. Which state of matter takes both the shape and volume of its container?
a. solid
b. liquid
c. gas
d. both b and c are correct
10. Matter is defined as anything that…
a. has a fixed volume and mass
b. has a definite volume
c. can be weighed on a balance
d. has mass and takes up space
11. Which of the following processes could a chemist use to physically separate a
solid metal product from a solution?
a. decomposition
b. distillation
c. filtration
d. evaporation
Iron combines with oxygen from the air to form rust as follows:
→
4Fe + 3O2
2Fe2O3
12. If the entire nail turned to rust, how would the mass of the rust compare to the
mass of the original nail?
a. The mass of the rust would be less than the nail it came from.
b. The mass of the rust would be the same as the nail that it came from.
c. The mass of the rust would be more than the nail it came from.
d. The mass of the rust would be impossible to predict.
86.2 g of iron nails were dropped into a clear solution of silver nitrate. Over time the solution
remained clear however a silver/black solid “beard” was visible on the nails. When the
researchers shook the solution the beard dispersed and eventually settled to the bottom of the
beaker. Also a slight increase in temperature was measured.
The following equation describes the reaction:
Fe (s) + 3 AgNO3 (aq) → Fe(NO3)3 (aq) + 3 Ag (s)
13. Which of the following indicates a chemical change occurred in the reaction?
a. new solid appears
b. temperature change
c. neither (a) nor (b)
d. both (a) and (b)
14. When you combine table salt (NaCl) with water what type of mixture do you make?
a. colloid
b. suspension
c. heterogeneous
d. homogeneous
Subatomic Particles
15. Neon, Argon and Krypton behave in a similar fashion due to the following:
a. they have the same number of neutrons
b. they have the same number of protons
c. they have the same number of energy levels
d. they have the same number of valence electrons
16. The nucleus of an atom is…
a. Positively charged and has a high density.
b. Positively charged and has a low density.
c. Negatively charged and has a high density.
d. Neutrally charged and has a high density.
17. The following is the correct electron configuration for which element?
1s22s22p63s23p64s1
a.
b.
c.
d.
argon
potassium
sulfur
carbon
18. Which of the following correctly represents an atom with fourteen neutrons?
a.
29
14
b.
14
7
c.
9
5
Si
N
B
d. 27
13 Al
19. Which of the following sets of symbols shows the number of protons, and number
of electrons correctly?
a. In, 49 protons, 49 electrons
b. Zn, 30 protons, 65.4 electrons
c. Cs, 55 protons, 132.9 electrons
d. F, 19 protons, 19 electrons
Nomenclature
20.
Which of the following is the correct name for N2O5
(a) nitrate
(b) nitrogen oxide
(c) dinitrogen pentoxide
21. Which is the correct formula for chromium (III) sulfate
a.
b.
c.
d.
22.
Cr3SO4
Cr(SO4)3
CrSO4
Cr2(SO4)3
Determine the correct name for S-2
a. sulfur
b. sulfate
c. thiosulfate
d. sulfide
(d) nitro oxygen
23. Which of the following is a nonmetallic group of elements?
a. Li, Na, K, Rb
b. H, He, Li, Be
c. F, Cl, Br, I
d. B, Al, Sc, Y
24. In which of the following sets are the charges given correctly for all ions?
a. Na+, Mg+, Al+
b. K+, Sr2+, O2c. Rb-, Ba2-, P3+
d. H2+, Li+, Ne25. Which of the following is NOT a possible compound of copper?
a. Cu2F
b. CuO
c. copper (II) oxide
d. copper (I) chloride
26. Which of the following pairs of elements would most likely form an ionic
compound?
a. Mg and F
b. N and S
c. O and Cl
d. Na and Al
27. What is the charge of the iron ion in this formula: Fe(NO3)2 ?
a. 0
b. 1+
c. 2+
d. 3+
28. What is the correct formula of copper (II) phosphate?
a. Cu2(PO4)3
b. Cu3(PO4)2
c. 2CuPO4
d. Cu(II)PO4
29. In the name mercury (II) oxide, the roman numeral means that:
a. 2 atoms of mercury combine with oxygen
b. 2 atoms of oxygen combine with mercury
c. mercury has a +2 charge
d. oxygen has a +2 charge
30. Determine the correct formula for potassium chromate
a. KCr
b. KCrO4
c. K2CrO4
d. K2Cr2O7
Reactions
31. Which of the following is true for all chemical reactions?
a. The total mass of the reactants increases.
b. The total mass of the products is greater than the total mass of the reactants
c. Water is released
d. The total mass of the reactants equals the total mass of the products.
32. ____Al + ____HCl  ____AlCl3 + ____H2
If the chemical equation above were correctly balanced the coefficients would be:
a.
b.
c.
d.
1, 3, 2, 3
2, 6, 2, 3
3, 1, 3, 1
1, 2, 1, 1
33. Classify the following reaction:
Au2O3  4 Au + 3 O2
a.
b.
c.
d.
e.
composition
decomposition
combustion
single replacement
double replacement
34. Classify the following reaction:
CH4 + 2 O2  CO2 + 2 H2O
a. composition
b. decomposition
c. combustion
d. single replacement
e. double replacement
35. Determine the correctly written chemical equation
a. 3 KClO3  3 KCl + 9 O2
b. 2 Na3PO4 + 3 ZnSO4  3 Na2SO4 + Zn3(PO4)2
c. C6H14 + 9 O2  6 CO2 + 7 H2O
d. 3 Cl2 + AlBr3  AlCl3 + 3 Br2
36. Which of the following describe an exothermic reaction?
(a) 2 H2 (g) + O2  2 H2O + heat
(b) NH4NO3 (s) + H2O (l) + heat  NH4+1 (aq) + NO3-1 (aq)
(c) ∆H = + KJ/mole
(d) CaCO3 + energy
→ CaO + CO
The following equation describes the reaction:
Fe (s) + 3 AgNO3 (aq) → Fe(NO3)3 (aq) + 3 Ag (s)
37. Determine the type of reaction that the researchers witnessed.
a. composition (synthesis)
b. combustion
c. single replacement
d. double replacement
38. Which of the following explains why the reaction occurs?
(a) Nitrate is more active than silver
(b) Iron is more active than silver
(c) Silver is more active than iron
(d) Iron is more active than nitrate
39. Which of the following is a double replacement reaction?
a.
b.
c.
d.
3K + FeCl3
3KCl + Fe
2KBr
2K + Br2
3H2 + N2
2NH3
NaCl + AgNO3
AgCl + NaNO3
Cu(s) + 2AgNO3(aq)
→
Cu(NO3)2(aq) +
2Ag(s)
40. What type of reaction is above?
a. double replacement
b. single replacement
c. synthesis (combination)
d. combustion
e. decomposition
41. Which of the following indicates that a chemical change occurred in a reaction?
a. formation of a new solid
b. unexpected color change
c. change in temperature
d. all of the above
42. Why does this reaction occur?
a. copper is above silver on the activity series
b. silver is above copper on the activity series
c. nitrate is above silver on the activity series
d. silver is above nitrate on the activity series
43. A reaction takes 20 minutes. In order to speed up this reaction what could
someone do?
a. heat the solution
b. use a larger container
c. add more reactant solution
d. add more water to the solution
44. ___ C4H10 + ___ O2 → ___ CO2 + ___ H2O
Determine the coefficients for the preceding reaction
(a) 1,1,4,5
(b) 2,13,8,10
(c) 2,6,4,5
(d) 1,1,1,1
____Al + ____O2 → ____Al2O3
45. If the chemical equation above were correctly balanced the coefficients would be:
a. 1, 1, 1
b. 1, 2, 5
c. 4, 3, 2
d. 2, 3, 2
46. What type of reaction is in the box above (number 45)?
a. synthesis (combination)
b. decomposition
c. single replacement
d. double replacement
47. Explain what happens to atoms during a chemical reaction.
a. atoms are rearranged
b. atoms can be created
c. atoms can be destroyed
d. atoms can be destroyed and turned into new atoms
48. Determine the solvent in an aqueous solution of ammonium nitrate
a. ammonium
b. nitrate
c. benzene
d. water
49. Determine the solute in an aqueous solution of ammonium nitrate
a. ammonium
b. salt
c. ammonium nitrate
d. water
Stoichiometry
50. The independent variable in a research study
a. remains constant throughout the study
b. is changed by the researcher
c. is the variable for which data is collected
d. may confuse the results of the study
51. Consider the following reaction:
2 Mg (s) + O2 (g)
→
2 MgO
If 48 g of magnesium react completely with 32 g of oxygen what mass of magnesium oxide
would you expect to collect?
a. 80 g
b. 16 g
c. 48 g
d. 40 g
52. Determine the correct description of the following reaction:
2 C2H6 + 7 O2 → 4 CO2 + 6 H2O
a. 2 moles of ethane reacts with 7 moles of O2 to form 4 moles of CO2 and 6 moles H2O
b. 2 grams of ethane react with 7 grams of O2 to form 4 grams of CO2 and 6 grams of H2O
c. 2 molecs of ethane react with 14 molecs of O2 to form 4 molecs of CO2 and 6 molecs of H2O
d. 22.4 L of ethane reacts with 44.8 L of oxygen to form 4 L of CO2 and 6 L of H2O.
53. Aluminum reacts with sulfuric acid to produce aluminum sulfate and hydrogen
gas according to the formula:
2Al(s) + 3H2SO4(aq)
Al2(SO4)3(aq) + 3H2(g)
How many grams of aluminum sulfate would be formed if 250 grams of sulfuric
acid completely reacted with aluminum?
a.
b.
c.
d.
2.5 grams
268 grams
291 grams
327 grams
Terry and Lyle dropped 1.5 grams of copper pellets into a solution of silver nitrate. The
solution changed color from colorless to blue. A silverish/black coating formed on the
surface of the copper pellets and eventually fell to the bottom of the test tube. A slight
change in temperature was noted. This is the reaction:
→
Cu(s) + 2AgNO3(aq)
Cu(NO3)2(aq) + 2Ag(s)
54. What is the mass of the silver produced, assuming an excess of silver nitrate?
a. 2.5 grams
b. 5.1 grams
c. 5.5 grams
d. 8.0 grams
55. How many atoms of copper were added to the AgNO3?
a. 6.44 x 1021
b. 1.42 x 1022
c. 2.55 x 1025
d. 5.70 x 1025
86.2 g of iron nails were dropped into a clear solution of silver nitrate. Over time the
solution remained clear however a silver/black solid “beard” was visible on the nails.
When the researchers shook the solution the beard dispersed and eventually settled to
the bottom of the beaker. Also a slight increase in temperature was measured.
The following equation describes the reaction:
Fe (s) + 3 AgNO3 (aq) → Fe(NO3)3 (aq) + 3 Ag (s)
56. Determine the number of moles of Ag expected if you reacted 86.2 g of Fe with an excess of
AgNO3.
a. 1.54 moles
b. 4.63 moles
c. 499 moles
d. 1.94 moles
57. Determine the # of Fe atoms present when 86.2 g Fe react with an excess of AgNO3.
a. 9.29 atoms
b. 9.29 x 1021 atoms
c. 9.29 x 1024 atoms
d. 9.29 x 1023 atoms
Acid/Base
58. A substance that has a sour taste in solution, is a proton donor and changes the
color of blue litmus paper to red is a(n):
a. acidic compound
b. basic compound
c. neutral compound
d. salt compound
59. Which of the following represents the pH of a basic solution?
a. 0
b. 6
c. 7
d. 14
60. Any substance that has a bitter taste, turns bromothymol blue the color blue and is a
proton acceptor is considered a(n)
a. acid
b. base
c. salt
d. transition metal
61. Which of the following represents the pH of an acid?
a. 14
b. 11
c. 5
d. 7
62. Determine the conjugate base of HCO3-1
a. H2CO3
b. CO3-2
c. H3CO3+1
d. CO2
63. You know a substance is an acid if what ion is present when the substance is dissolved?
(a) OH-1
(b) OH+1
(c) H-1
(d) H+1
64.
You know a substance is a base if what ion is present when the substance is dissolved?
(a) OH-1
(b) OH+1
(c) H-1
(d) H+1