Chemistry 2016 Fall Review
Name________________________Per___
Safety/Scientific Method/Significant Figures/Lab Equipment
1. The safest way to dilute concentrated sulfuric acid is to add…
a. A series of small volumes of water to the acid while stirring.
b. The acid to water slowly, while stirring constantly.
c. The acid to a small volume of water and then add more water.
d. Dilute sulfuric acid to a small volume of the concentrated acid.
2. The reason for wafting or fanning a small amount of chemical vapors toward the nose as a means to detect odors in
a test tube is to …
a. Avoid experimental error from excessive loss of mass of reactants or products.
b. Avoid splashing chemicals into the face of any person.
c. Protect the respiratory tract against potentially harmful vapors.
d. Determine the relative strength of the odor before smelling directly.
3. You have solid chemicals in excess of what you need. You should:
a. Pour it down the drain in the sink and rinse with lots of water.
b. Pour it back in the jar it came from.
c. Leave it for someone to use it next class.
d. Put in the waste container provided for chemical waste.
4. While working with chemicals in the lab, Joanna found a chipped glass beaker. She should
a. Use it.
b. Put tape over the chip.
c. Put it in the trash.
d. Put it in the container for broken glassware.
5. How many significant figures does this electronic balance show?
a. 0
b. 2
c. 3
d. 4
3.041 g
For questions 1-2 use the situation below.
Bart thinks that if mice are exposed to microwaves, then they will live longer than normal. He takes 50 mice and
microwaves them for 10 seconds. Another 50 mice are set aside and not put in the microwave. He found that the
average life span of the microwaved mice was 16 months; the average life span of the second group was 22 months.
6. What is the dependent in the situation above?
a. Microwave exposure
b. Breed of mouse
c. Average lifespan of mouse
d. Sex of mouse
7. What is the independent variable in the situation above?
a. Microwave exposure
b. Breed of mouse
c. Average lifespan of mouse
d. Sex of mouse
8. How do you write 3.431 x 106 ml in standard notation?
a.
34310 ml
b.
3431 ml
c.
0.000003431 ml
d.
3431000 ml
9. Which of these instruments will give the most precise volume measurement?
a. A
b. B
c. C
d. D
A
B
C
D
Classification of Matter
10. H2O is best classified as a(n):
a. compound
b. element
c. homogeneous mixture
d. heterogeneous mixture
11. A salad is classified as a(n):
a. heterogeneous mixture
b. compound
c. element
d. homogeneous mixture
12. Why is oxygen classified as a pure substance and air is classified as a mixture?
a. Oxygen contains only one substance, but air contains several substances.
b. Oxygen has a higher density than air.
c. Oxygen undergoes phase changes, whereas air is always a gas.
d. Oxygen is more reactive than air.
13. The picture to the right represents a(n) ______.
a. mixture of elements
b. mixture of compounds
c. compound
d. mixture of elements and compounds
14. The picture to the right represents a(n) ______.
a. element
b. mixture of elements and compound
c. mixture of compounds
d. compound
15. Which of the following is an example of a chemical change?
a. burning wood
b. an apple being cut
c. an ice cube melting
d. liquid water evaporating
16. A sugar cube is heated in a test tube over a Bunsen burner. The sugar cube turns black and has less mass than
before it was heated. These changes occur because the sugar has –
a. melted
c. reacted chemically
b. boiled
d. become hydrated
17. Which process is a physical change of water?
a. freezing the water
b. decomposing the water into hydrogen and oxygen
c. reacting water with sulfuric acid
d. adding a hydrogen atom to form hydronium (H3O+)
18. Which state of matter is characterized by high density and no compressibility?
a. gas
b. solid
c. liquid
d. both b and c
19. A copper wire is ductile (it can be stretched into a thin wire). This is an example of a(n):
a. physical & chemical property
b. chemical property
c. physical property
d. element
Periodic Table & Atomic Structure
20. To change Ca to Ca2+, you need to:
a. gain two neutrons
b. lose two protons
c. gain two electrons
d. lose two electrons
21.
22.
16
8𝑂
17
8𝑂
and
a.
b.
c.
d.
17
8𝑂
are examples of oxygen:
neutrons
ions
isotopes
molecules
has how many protons and neutrons?
a. 8 and 17
b. 8 and 9
c. 9 and 17
d. 8 and 25
23. What is the symbol for an ion which has 9 protons and 10 electrons?
a. Fb. O2c. N3d. F1+
24. What do elements in the same family share?
a. similarity in size
b. similarity in symbol
c. similarity in properties
d. similarity in date of discovery
25. According to what you know about the modern periodic table, which of the following elements would have the same
properties as strontium?
a. Ca
b. S
c. Li
d. Cl
26. Which of the following atoms would expect to have largest atomic radius?
a. Li
b. Rb
c. Be
d. Al
27. Which of the following elements is incorrectly paired?
a. chlorine-noble gases
b. fluorine-halogens
c. copper-transition metals
d. magnesium-alkaline earth metals
28. Which of the following groups does Iron (Fe) belong to?
a. alkali metals
b. halogens
c. transition metals
d. lanthanides
29. According to the average atomic mass of isotope A and B, identify the element.
Isotope
% Abundance
% Abundance / 100
Atomic Mass
A
69.2%
62.93
B
30.8%
64.93
Element:
Part of Mass
Average Atomic Mass
a.
b.
c.
d.
Hg
Pb
Cu
Pt
30. Which scientist believed that electrons travel in discrete energy levels around the nucleus like planets around the
sun?
a. John Dalton
b. J.J. Thomson
c. Ernest Rutherford
d. Neils Bohr
31. How does the speed of visible light compare with the speed of gamma rays, when both speeds are measured in a
vacuum?
a.
The speed of visible light is greater
b.
The speed of gamma rays is greater
c.
The speeds are the same
d.
The speed depends on the color of light
32. How are frequency and wavelength related?
a.
as wavelength goes up, frequency goes down
b.
as wavelength goes up, frequency goes up
c.
they are not related
d.
they don’t really exist
33. Which of the following best describes the relationship, if any, between wavelength and energy for electromagnetic
radiation?
a.
b.
c.
d.
As wavelength increases, energy increases.
As wavelength increases, energy decreases.
There is no relationship between wavelength and energy.
As wavelength decreases, energy decreases.
34. What is the energy of a photon of green light with a frequency of 5.80 x 1014 Hz?
a. 1.14 x 10-48 J
c. 3.84 x 1019 J
47
b. 8.76 x 10 J
d. 3.84 x 10-19 J
35. What is the energy of a photon whose frequency is 5.20 X 1015 s-1?
a. 3.45 X 10 -18 J
b. 3.65 X 10 18 J
c. 1.34 X 10 -49 J
d. 7.84 X 10 48 J
Naming & Writing Formulas & Bonding
36. What is the correct formula for the compound hexaphosphorus tetrasulfide?
a. 6PS4
b. P4S6
c. P6S4
d. P7S4
37. The chemical formula for magnesium bromide is
a. Mg2Br
b. MgBr
c. MgBr2
d. Mg2Br3
38. What is the correct formula for disulfur nonoxide?
a. S2O9
b. S2O8
c. S9O2
d. 2SO7
39. The correct formula of an ionic compound containing Na +1 and O-2 is______.
a. NaO2
b. NaO
c. NaO3
d. Na2O
40. What is the correct formula for ammonium phosphide?
a. (NH4)3P
b. (NH4)3P4
c. NH4P4_
d. NH3P4
41. What is the correct compound name for N2O7?
a. dinitrogen oxide
b. dinitrogen heptoxide
c.
d.
trinitrogen pentaoxide
trinitrogen quatraoxide
42. The correct formula for tin (III)sulfide is:
a. Sn3S2
b. Sn3S3
c.
d.
Sn2S3
Sn2S2
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43. What is the correct name for Mg(NO3)2
a. magnesium nitride
b. magnesium (II) nitrite
c. magnesium dinitrate
d. magnesium nitrate
44.
45.
Which of the following is the correct Lewis structure for ammonia, NH3?
A
B
C
D
Based on the Lewis dot structure from above, what is the shape of an NH3 molecule?
a. tetrahedral
b. linear
c. bent
d. trigonal pyramidal
45. Metals are good conductors of heat and tend to
a. be brittle
b. lack luster
c. be malleable
d. have poor electrical conductivity
Nuclear Chemistry
47. Look at the graph to the right. How many grams of the substance remain after two half-lives?
a. 50 g
b. 25 g
c. 12.5 g
d. 6.25 g
Match the nuclear equation with the correct name of the reaction:
48. _____ Fission
49. _____ Beta decay
a.
U
51. _____ Fusion
234
90
C  14N 
14
b.
1
50. _____ Alpha decay
Th  24He
238
92
c.
d.
0
1
e
H  2H  4He  01n  
1
0
n
U
235
92
Kr 
91
36
Ba  301 n
142
56
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52.Balance the following nuclear equations
Chemical Reactions
53. Which coefficients correctly balance the formula equation
NH4NO2(s)  N2(g) + H2O(l)?
a. 1, 2, 2
b. 1, 1, 2
c. 2, 1, 1
d. 2, 2, 2
54. When this equation is correctly balanced, the coefficient in front of AlCl 3 will be…
___AlCl3 + ___Ba(OH)2  ___Al(OH)3 + ___BaCl2
a. 1
b. 2
c. 4
d. 6
55. When 127 g of copper reacts with 32 g of oxygen gas to form copper (II) oxide, no copper or oxygen is left over. How
much copper (II) oxide is produced?
a. 32 g
b. 95 g
c. 127 g
d. 159 g
2Cu + O2  2CuO
56. Which of the following reactions is an example of a single-replacement reaction?
a.
b.
c.
d.
2AgNO3 + Cu  Cu(NO3)2 + 2Ag
NaOH + HCl  NaCl + H2O
CO2  C + O2
4Fe(OH)2 + O2  4Fe(OH)3
57. Which of the following reactions is a decomposition reaction?
a.
b.
c.
d.
S8 + 8O2  8SO2
O2 + 2H2O  2H2O2
2KClO3  2KCl + 3O2
2Na + 2AgCl  2NaCl + 2Ag
58. Which is an example of a synthesis reaction?
a.
b.
c.
d.
HCl + KOH  KCl + H2O
Pb(NO3)2 + 2HBr  PbBr2 + 2HNO3
C + O2  CO2
Mg + H2SO4  MgSO4+ H2
59. What are the missing coefficients for the equation below?
___Al2 (SO4)3
+
__ _ KOH

___ Al(OH)3
_ _ _ K2SO4
a. 1, 3, 2, 3
b. 2, 12, 4, 6
c. 4, 6, 2, 3
d. 1,6, 2,3
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