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Name:______________________________
Chemistry Final Review L1
Into Unit
1. Why is Chemistry often called the central science?
2. What are the different branches of Chemistry?
3. State the Law of Conservation of Matter.
Scientific Method
A. Experiment
E. Hypothesis
B. Variable
F. Theory
C. Control
G. Observation
D. Conclusion
H. Law
4. ______ In an experiment, one ____________ is tested at a time to determine how it
affects result.
5. ______When you don’t do anything different than normal in an experiment, it serves as
a __________ group.
6. ______ Is a possible answer to a question
Math in Chemistry
7. List the SI base units for the following:
Volume __________
Mass _____________
Amount/count _______________
Temperature __________
8. For the following, list the number of significant figures in each:
A. 0.0000095________________
B. 745672345 _________________
C. 0.0346001________________
D. 29480000___________________
9. How many liters in 445 mL?
Name:______________________________
10. How many meters is 651 nm?
11. Sally has to make some temperature measurements. She reads a thermometer to
be 52.2oC, 51.5oC, 52.3oC, and 52.2oC. The actual temperature is 49.2oC
12. Do his measurements exhibit high precision? ______________
13. Do his measurements exhibit high accuracy?______________________
Explain!
14. Measurements are always uncertain because
A. Instruments aren’t designed for measurements
B. All measurements involve some estimation
C. People don’t know how to use instruments
D. None of the above
E. All of the above
15. 614.0 cm – 2.134 cm =
a. 612 cm
c. 611.87 cm
b. 611.9 cm
d. 611.866 cm
16. 428 / 41
a. 10
c. 10.4
b. 10.
d. 10.44
17. Convert the following to scientific notation:
a. 2000
b. 0.0947
c. 23998
d. 6097000.0
18. Convert the following to standard notation:
a. 2.6 x 106
b. 1.2 x 10-4
c. 5.11 x 100
d. 2.300 x 1012
19. How many significant figures do the following numbers have?
a. 2.30
b. 1000
c. 0.20100
d. 3.2 x 103
Name:______________________________
20. A piece of pie has a mass of 200.0g and a volume of 140mL. What is its density?
a. 1.4286 g/mL
b. 1.428 g/mL
c. 1.43 g/mL
d. 1.4 g/mL
21. A toy rocket flew 23.0m when launched. How many yards did it fly? (2.3cm = 1.0 in)
22. Convert 123oC to Kelvins?
Matter
23. An element
a. can be broken down into simpler substances
b. are used to make other elements
c. are used to make compounds
d. are never found in the periodic table of elements
24. Chemical reactions can be used to separate
a. elements
b. pure substances
b. mixtures
d. compounds
25. A change in the force of Earth’s gravity on an object will affect its
a. mass
b. density
c. weight
d. kinetic energy
26. An property that depends on the amount of material that is present.
a. intrinsic
b. extrinsic
27. Classify each of the following as either a physical or chemical change.
_______________________ A. folding paper
_______________________ B. burning paper
_______________________ C. dissolving MIO in water
_______________________ D. cutting your hair
_______________________ E. bleaching your hair
Name:______________________________
28. Identify each as an element, compound, or mixture. For mixtures, identify it as
homogeneous or heterogeneous.
_______________________ A. grape Kool Aid
_______________________ B. Jello with fruit in it
_______________________ C. air
_______________________ D. a piece of glass (SiO2)
_______________________ E. carbon dioxide
_______________________ F. silicon
_______________________ G. water
_______________________ H. copper wire
29. The four states of matter are: __________________________________________
_________________________________________________________________.
The Atom
_____30. Group 1
_____31. Group 2
_____32. Group 9
_____33. Group 18
A.
B.
C.
D.
E.
F.
Transition metals
Alkali metals
Alkaline Earth metals
Noble gases
Inner transition metals
Halogens
34. Write the complete chemical symbol for an atom with 31 protons, 38 neutrons, and
28 electrons.
35. Element X has two natural isotopes. The isotope with mass 62.9265 amu has a
relative abundance of 69.17%. The isotope with mass 64.9278 amu has a relative
abundance of 30.83%.
What is the average atomic mass of element X?
What is the identity of element X?
Name:______________________________
36. Fill in the sections of the table that are empty.
Element
# of
protons
# of
neutrons
# of
electrons
10
10
Mass #
Charge
(+, −, 0)
-1
226
+1
88
Rn
0
Nomenclature
37. What are the 3 types of bonds?
38. Which type of bond occurs with a transfer of electrons?
39. Which type of bond occurs with a sharing of electrons?
40. Potassium chloride has which type of bond?
41. When are Roman numerals used in naming compounds?
42. Name the following compounds. Both ionic and covalent molecules are here, and
they are mixed!
A. KOH ___________________________
B. LiF _____________________________
C. SO2 _____________________________
D. N2O3 ____________________________
43. Give the correct formula for the following:
A. Zirconium (II) nitratate __________________________
C. Nitrogen gas _______________________
D. Sulfuric Acid ______________________________
G. Phosphorus pentachloride ________________________
H. Barium hydroxide _________________________
Name:______________________________
Reactions and Equations
A. Coefficient
B. Reactant
C. Product
D. Balanced
E. Endothermic
F. Exothermic
G. Subscript
H. Precipitate
I. Diatomic
J. Aqueous
_____ 44. A reaction that releases heat.
_____ 45. A reaction that absorbs heat.
_____ 46. A starting substance in a chemical reaction.
_____ 47. A new substance formed in a chemical reaction.
_____ 48. A solid product.
_____ 49. A solid compound dissolved in water.
Write out a word equation for the following equations.
50. Ag2O
51. Sb
---------------> Ag + O2
+ Cl2 ----------->
SbCl2
52. Why do we balance equations?
Substitute symbols and formulas for names, and then write a balanced equation for each
of the following reactions.
53. Ethane (C2H6) gas burns in air to make carbon dioxide and water.
54. Magnesium reacts with carbon dioxide to form to make magnesium oxide and
carbon.
Name:______________________________
Balance the following reactions.
55. ___ Na + ___ O2→ ___ Na2O
56. __ BaCl2 + ___ NaOH → ____ Ba(OH)2 + ___ NaCl
57. ___ Fe+ ___ CuSO4 → ____ Cu + ___ FeSO4
58. ___ NbI3 + ___ I2 → ___ NbI5
Identify the type of chemical reaction shown below as synthesis (S), decomposition (D),
single replacement (SR), double replacement (DR), or combustion (C).
59.
S + Cl2 → SCl2
60.
Al + H2O → Al2O3 + H2
61.
NaF → Na + F2
62.
C7H14 + O2 → CO2 + H2O
63.
KBr + AgNO3 → AgBr + KNO3
Given the following reactants predict the products. Add if the reactions are classified as AcidBase in addition to the other classifications.
64. CuO (s) à
65. AgNO3 (aq) + HCl (aq) à
66. H2SO4(aq) + Ca(OH) 2(aq) à
67. Mg(s) + TiCl4(aq)
à
68. SF4(s) à
69. What is the activity series, and why is it important when working with single
replacement reactions?
Name:______________________________
For #64-68 (above), give the complete and net ionic equations for 3 of them.
70. complete:
net:
71. complete:
net:
72. complete:
net:
For #64-68 (above) problems provide any redox half reactions that occur (3 of the
problems are redox, 2 are not. It is up to you to decide which is which)
73.
74.
75.
The Mole
76. What is the value of Avogadro’s number?
77. What does it tell you?
78. How many moles are in the following?
a. 2.8 x 1024 atoms of carbon
b. 23 grams of oxygen
79. How many grams are in the following?
a. 31.2 liters of nitrogen at STP
b. 2.61 x 1022 atoms of boron
Name:______________________________
80. A sample of a molecular compound was analyzed and found to contain 25.9g
Nitrogen and 74.1g Oxygen. Determine the empirical formula of the compound.
81. Calculate the molecular formula of the compound whose molar mass is 147g and
empirical formula is C3H2Cl.
82. What is the concentration of Hydrochloric acid (HCl) if 0.90 grams of the HCl are
dissolved in 250.0 mL? Is this a strong acid?
Stoichiometry
83. Calculate the mass of ammonia (NH3) formed when 5.40g of hydrogen gas reacts
with an excess of nitrogen. Be certain to balance the equation.
84. If 80.0g of Cu reacts with 25.0g S, which is the limiting reactant? How much excess is
left?
2 Cu + S à Cu2S
Name:______________________________
Energy and Thermodynamics
85.Label all parts of the heating curve
86.Label all parts of the phase diagram
_____ 87. The First Law of Thermodynamics states:
a. Matter is neither created nor destroyed
b. Energy is constant within a system
c. The amount of energy in a reaction depends on the size of the molecules
in the reaction
d. The energy of the universe is constant
Name:______________________________
_____ 88. An Exothermic reaction is when:
a. Energy flows out of a system
b. Energy flows into a system
c. The system is at equilibrium
d. A reaction that doesn’t occur
_____ 89. The amount of energy needed to raise the temperature of a substance by one
degree:
a. Heat capacity
b. Specific het capacity
c. Thermal energy
d. Entropy
_____ 90. The amount of disorder in an object or system:
a. Heat capacity
b. Specific heat capacity
c. Thermal energy
d. Entropy
_____ 91. Temperature is defined as:
a. the measure of how hot or cold something is
b. the measure of the flow of energy
c. the measure of heat
d. All the above
92. Iron with a mass of 35 g is heated and then placed in a beaker containing 600 g of
water. The temperature of the water increases from 25˚C to 33˚C. The specific heat of
iron is 0.451 J/g˚C. What was the original temperature of the piece of iron?(*Hint*-this
will be a large answer).
93. How many joules are released when 360.0 grams of water (the amount of liquid in a 12
oz. can) are cooled from 4.00 x 106 oC (the hottest temperature ever achieved by man,
during a thermonuclear explosion) to -272.75 oC (the coldest temperature achieved by
man using refrigeration). Is this an endo- or exothermic process?
Name:______________________________
Gas Laws
____ 94. According to kinetic molecular theory, gas particles
a. are spaced far apart.
b. are constantly moving.
c. have mass.
d. all of the above.
____ 95. Kinetic energy
a. is energy associated with movement.
b. increases with increasing temperature.
c. is given by ½mv2
d. all of the above.
____ 96. The diffusion of a gas is its tendency to
a. move through other gases
b. move away from other gases
c. decompose
d. do nothing
____ 97. According to kinetic molecular theory,
a. the gas molecules themselves have a volume of zero.
b. the gas molecules exert no attractive and repulsive forces on one another
c. when gas molecules collide with one another, energy is conserved.
d. all of the above.
98. A 3.0L tank of O2 gas is a pressure of 2.5 atm. What will the volume of oxygen be if it
is reduced to a pressure of 0.75 atm? Assume constant temperature.
99. A gas in a hot air balloon at 38.0oC has a volume of 2.97L and a pressure of 3.14atm.
The air is heated to 118.0oC and the volume drops to 1.04L. What is the new
pressure (in atm)?
100. What is the volume of 20 moles of a gas under 4 atm of pressure at 14 oC?
R= .0824atm-L/mol-K
R= 8.314 Pa-L/mol-K
Name:______________________________
EMR
101. Label the properties of the wave depicted below.
B
C
A
D
E
_______ Which letter represents the wavelength of the wave?
_______ Which letter represents the amplitude of the wave?
_______ Which letter shows a crest?
_______ Which letter shows a trough?
_______ Can frequency be drawn in? (Yes or No)
102. If energy decreases, frequency ______________, and wavelength
________________.
103. List all of the sections of the electromagnetic spectrum from the shortest to the
longest wavelengths in order.
104. Suppose your favorite FM radio station broadcasts at 102.1MHz (1.021 X 108Hz). What is
the wavelength of the station?
105. X rays have a wavelength of 1.10 X 10-9m. What is the energy associated with this wave?
106. How much energy is needed for Hydrogen’s electron to jump from n=2 to n=5?
Name:______________________________
Nuclear
107. What is the minimum amount of uranium called?
108. What is the spontaneous emission of nuclear radiation?
109. Where are protons located?
110. What is the charge of a beta particle?
111. What is a positively charged electron?
112. The measure of which a radioactive substance loses half of its radioactivity.
113. Where are the heaviest elements (greater than lead) created?
114. What is the type of decay that releases an electron and turns a neutron into a proton?
115. This equation states that the energy released by the reaction is equal to the mass
multiplied by the speed of light squared.
116. What is the mass of an alpha particle?
117. What is the mass associated with a gamma ray?
118. What type of radiation is most easily blocked?
119. If you start with 8.0 g of C-14, how much is left after 2 half lives?
Complete the following nuclear equations.
120.
______ + 3781Rb → 3681Kr
15
121. 8
O → 157 N + ______
58
122. 28
Ni + −10 e → _______
Name:______________________________
238
123. 92
U → _______ + 24 He
18
124. 9
F → 178 O + _____
Electron Configurations
Use the diagrams to answer the questions or complete the statements
Figure 6-3
_____ 125. What is the charge on the ion that would most readily be formed by
magnesium in Figure 6-3?
a.
1+
c.
1–
b.
2+
d.
2–
_____ 126. In Figure 6-3, what is the charge on the ion that would most readily be formed
by sulfur?
a.
1+
c.
1–
b.
2+
d.
2–
_____ 127. In Figure 6-3, which of the elements shown would be unlikely to form any
compounds?
a.
Al
c.
P
b.
Si
d.
Ar
Name:______________________________
_____ 128. Which of the four orbital diagrams in the figure above is correct for
phosphorus?
a.
a
c.
c
b.
b
d.
d
_____ 129. In Figure 4-4, what is the total number of electrons that can occupy the n = 3
level?
a.
3
c.
9
b.
6
d.
18
Write the electron configuration of the following elements:
130. Na
131. Cu
132. F
133. I
The Periodic Table
Match the person with their contribution to the Periodic Table.
_____134. Mendeleev
_____135. Moseley
_____136. Dobereiner
_____137. Newlands
A. arranged elements by atomic number
B. grouped elements in to sets of three
C. predicted the existence and properties of three
undiscovered elements
D. organized elements into repeating groups of eight, which
he termed octaves
Name:______________________________
For each of the following pairs, circle the atom or ion that has the larger atomic radius.
138. Na or Ca
139. N or N3140. Ca or Ca2+
141. O or F
For each of the following pairs, circle the atom that has the higher ionization energy.
142. Cl or Br
143. Rb or K
144. Mg+ or Mg2+
145. Te or I
For each of the following pairs, circle the atom that has the lower electronegativity.
146. Be or B
147. P or Sb
Acids and Bases
148. For the following reactions, identify the acid, the conjugate acid, the base, and the
conjugate base:
HNO3 + H2O à H3O+ + NO3CO32- + H2O à HCO3- + OH-
149. What is the pH of an HCl solution that has a concentration of 2.34 x 10-5 M?
150. What is the pOH of the solution?
Name:______________________________
151. What is the pH of a solution of KOH with a concentration of 1.26 x 10-3 M?
152. If the pH of a solution of HNO3 is 2.60, what is the concentration of H+ ions?