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Name_________________________________
Chemistry Semester Exam Review – Due January 12 – No late papers accepted
Chemistry Exam Schedule:
11th period Tuesday, January 17th, 12:35-2:15
8/9 period Wednesday, January 18th 10:10-11:50
Alternate options available – due extenuating circumstances – this must be pre-approved in writing
1st period Tuesday, January 17th 8:10-9:50
5/6th period Wednesday, January 18th 8:10-9:50
The Semester exam will consist of 3 parts, and represent 20% of your grade
Multiple choice – 100 points
Written – 25 points - problems/fill in the blank/short answer/graph
Lab practical – 25 points – given on Thursday, January 12th.
Bring 2 #2 pencils and a calculator to the exam. A periodic table will be provided
If you prepare, you can earn an “A” on this exam. Use the holiday break to complete this
worksheet and complete the seven Review PowerPoints on our website. Do not wait until the
week or weekend before exams.
Exam topics:
Safety
Density Calculations
Scientific Method
Temperature Conversions
Element symbols and names
Metric Conversions
Scientific Notation
Average atomic mass calculations
Significant Figures
Matter – elements, compounds, mixtures, chemical and physical changes
Atomic Structure – atoms, protons, neutrons, electrons, isotopes, ions
Atomic Theory – scientists, electron configuration
This worksheet will be due at the beginning of block on January 12th and returned on January 13th.
You will be completing the lab practical portion of your final exam in class on January 12th. If you
know you will be absent, please make arrangements to complete the lab prior to January 12th. If you
are ill or absent due to another reason and do not complete the lab practical on or before January 12th,
you will receive a written lab practical instead during your regularly scheduled exam.
How to prepare for the semester exam:
Complete this worksheet and Answer all of the questions on the website’s Review PowerPoints.
Remember the website may be found by clicking on Teacher websites on the Beachwood High
School homepage, and the password is: BaldessariScience
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Directions – answer all questions – when provided with a list – check or circle or
fill in the blank
1. Define the following terms:
a . science
b. chemistry
2. Define the following terms:
a . scientific method
b. natural law
c. hypothesis
d. theory
3. Discuss how the scientific method is useful in solving problems outside science.
4. What is a summary of observed behavior?
5. The state of matter for an object that has neither definite shape nor definite volume is
6. The state of matter for an object that has a definite volume but not a definite shape is
7. The state of matter for an object that has both definite volume and definite shape is
8. Anything that has mass and volume is called ______________.
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9. Classify each of the following as a physical (P) or a chemical (C) change
___ baking a cake
___ boiling water
___ burning gasoline
___ lighting a match
___A piece of sulfur is burned.
___an ice cube melting in a drink
___boiling alcohol
___boiling water
___burning paper
___butter melting
___chopping wood
___coffee spilled on a shirt
10. Classify each of the following as a physical (P) or a chemical (C) change
___cooking an egg
___decomposing meat
___decomposing water
___digesting a pizza
___dissolving sugar in water
___driving a car
___evaporating alcohol
___evaporating water
___fermenting fruit juice
11. Classify each of the following as a physical (P) or a chemical (C) change.
___gasoline evaporating
___Potatoes rot
___grinding coffee beans.
___Rocks are ground to sand
___grinding grain
___rusting iron
___ironing a shirt
___sanding a table top
___melting ice
___Silverware tarnishes
___paper burning
12. Which of these is a chemical property?
a. Ice melts at 0°C.
b. Oxygen is a gas.
c. Helium is very nonreactive.
d. Sodium is a soft, shiny metal.
e. Water has a high specific heat.
13. In a chemical change, which is a true statement:
a. a phase change must occur
b. the original material can never be regenerated
c. a phase change never occurs
d. the products are different substances from the starting materials
14. All ______________ changes are ______________ changes.
15. If iodine melts at 114°C and boils at 184°C, what is its physical state at 120°C?
16. If iodine melts at 114°C and boils at 184°C, what is its physical state at 98°C?
17. If iodine melts at 114°C and boils at 184°C, what is its physical state at 250°C?
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18. Which of the following describes a chemical property of gold?
a. Gold is a yellow metal.
d. Gold is a very dense metal.
b. Gold is an inert (nonreactive) metal.
e. Gold is a good conductor of heat and
c. Gold is a soft metal.
electricity.
19 . Which are compounds:
a. table salt
b. carbon
c. copper
d. water
20. Which of the following are elements?
a. sodium
d. cotton
chloride
e. carbon
b. water
f. blood
c. glucose
g. salt
e. mercury
h. earth
i. oxygen
j. iron ore
k. wood
l. silver
m. brass
n. iron
p. blood
21. An element is a collection of a single kind of ______________.
22. An example of a mixture is
a. hydrogen fluoride
b. purified water
23. An example of a pure substance is
a. elements
b. compounds
24. Sand on the beach is an example of
a. a homogeneous mixture
b. a heterogeneous mixture
c. gold
d. the air in this room
c. pure water
d. carbon dioxide
c. a compound
d. an element
25. A solution can be a heterogeneous or a homogeneous mixture. T/F ______________
26. Classify each of the following as an element (E), a compound (C), a homogeneous mixture
(Homo), or a heterogeneous mixture (HET).
a. table salt ______________
k. oily water _____________
b. chlorine gas ______________
l. 14K gold _____________ _
c. sand in water ______________
m. pure silver ______________
d. soil (dust)______________
n. aluminum ______________
e. petroleum ______________
o. distilled water ______________
f. sodium chloride _________
p. tap water ______________
g. aluminum ______________
q. brass ______________
h. caffeine ______________
r. tungsten ______________
i. tap water _______________
s. sodium chloride ______________
j. milk _________________
t. air ______________
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27. A solution can be distinguished from a compound by its
a. variable composition
c. heterogeneous nature
b. liquid state
d. lack of color
28. The process of boiling off the water from a salt solution to recapture the salt is a
______________ process.
29. A pure substance made up of more than one kind of atom is called
a. a homogeneous mixture
d. an element
b. a heterogeneous mixture
e. an alloy
c. a compound
30. When salt is mixed in to water, it dissolves to form saltwater. Which is the BEST process to
use if I want to remove the salt from the water?
31. We use distilled water in the lab because:
32. Ice floats in water because:
33. The element that is found in group 3, period 4 is: _________________
34. During the labs done in class, many chemical changes have been observed. What
observation will tell you a chemical change has happened?
35. The elements in the modern periodic chart that we use is arranged by increasing
____________________________
36. Fact 1: Iron is brown. Fact 2: Iron becomes red after it is exposed to oxygen
The first fact describes a ________________________ The second fact describes a
________________________________
37. The Russian chemist who proposed the first periodic chart based on physical and chemical
properties was ____________________
38. What property of elements did Moseley use to order the elements from beginning to end on
his table?__________________________
39. In the atoms of pure stable elements, there are usually the same number of electrons as the
number of__________________________
40. The mass of the atoms of an element is determined by its______________________
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41. An atom with 7 protons in it is definitely a ____________ atom.
42. An atom with an atomic mass of 16 is usually a _______________atom.
43. Carbon atoms typically have ________ neutrons.
44. Elements that behave the same and share similar properties are typically found in a
_________________ on the periodic table
45. If two objects measure differently on a balance, we would say the two objects have different
___________________________
46. If two objects of the same size and shape have different masses, they would also have
different____________________
47. When dissolving salt into water, the salt that is being dissolved is also called
the_______________
48. If I completely dissolve Potassium Nitrate into water, I will see only a clear liquid. This
tells me that I have made a ___________________________
49. Which sub-atomic particle is directly related to the identity of the element? _____________
50. Which sub-atomic particle is involved in bonding? ___________________
51. Which sub-atomic particle accounts for some mass in the nucleus and determines the isotope
of the element? ________________
52. The amount of oxygen entering a Tyrill burner can be adjusted by _____________________
53. A Barium ion has a 2+ charge. How many electrons should it have? _________________
54. An isotope of carbon has a mass of 14. How many neutrons should it have? ____________
55. An isotope of Oxygen has a mass of 17. How many protons should it have? ____________
56. If someone catches on fire in the lab, we should help that person by:
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57) Fill in the missing information on the chart
Chemical
Symbol
Mass #
Atomic #
# Protons
# Neutrons
# Electrons
O
20
6
3
18
7
58. Given the following mass, volume, and density information, calculate the missing quantity.
293.5 g
? mL
2.12 g/mL
59. Determine how many significant figures are in each of these numbers
a) 6.57 g
f) 30.071 g
b) 0.15 kg
g) 0.106 cm
c) 28.00 ml
h) 0.00067 g
d) 250 m
i) 0.02300 cm
e) 0.07000 g
j) 26.5009 cm
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60. For each of the following, make the indicated conversion.
a.
0.00000770 to standard scientific notation
b.
26000000 to standard scientific notation
61. Make the indicated temperature conversion. Show your work
– 21.2 oF to Kelvin
62. Make the following conversions. SHOW ALL OF YOUR WORK!
a. 180 days =
milliseconds
b. 3.1 x 10-3 kL =
mL
63. Complete the following table using the correct number of SIGNIFICANT FIGURES.
RULER #
LENGTH
1
0.5 ft
2
6.0 in
3
15.2 cm
4
15.24 cm
Show your work here:
WIDTH
0.5 ft
6.1 in
15.5 cm
15.49 cm
LENGTH
cm
cm
cm
cm
WIDTH
cm
cm
cm
cm
PERIMETER
cm
cm
cm
cm
AREA
cm2
cm2
cm2
cm2
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64.
CALCULATE THE AVERAGE ATOMIC MASS FOR EACH ELEMENT BELOW. THEN IDENTIFY THE
ELEMENT’S ATOMIC NUMBER,
# OF PROTONS, # OF ELECTRONS AND # OF NEUTRONS.
TO RECEIVE CREDIT, ALL CALCULATIONS MUST BE SHOWN. DON’T FORGET TO
SIGFIGS IN YOUR CALCULATIONS. CIRCLE OR HIGHLIGHT ALL ANSWERS.
Isotope
54
Fe
56
Fe
57
Fe
58
Fe
Mass (amu)
53.9396
55.9349
56.9354
57.9333
IN ORDER
MAINTAIN
% Abundance
5.845%
91.754%
2.119%
0.282%
65. List 5 important safety rules
1)
2)
3)
4)
5)
66. When should you use the eyewash station?
67. How would you separate an un-dissolved solid like sand from a liquid like water?
68. Two atoms with the same number of protons but different numbers of neutrons are known
as________________________
69. What is the most abundant element on the earth (including the crust, oceans, and
atmosphere)?
70. What is the most abundant element found in the human body?
71. How many of the following did Dalton discuss in his atomic theory?
Atoms
ions
neutrons
electrons
isotopes
protons
72. What is the law of constant composition?
73. A substance composed of two or more elements combined chemically in a fixed proportion
by mass is a __________
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74. The fundamental “particle” of a chemical element according to Dalton’s theory is
the____________;
75. In chemistry, a formula is used to represent a __________________.
76. How many of each type of atom is indicated in the formula (NH4)2C8H4O2?
77. The total number of atoms indicated by the formula Ca3(PO4)3 is
78. How many nitrogen atoms are indicated by the formula Al(NO3)3?
79. Who is considered the father of the periodic table? ______________________
80. The first scientist to show that atoms emit tiny negative particles was _________________
81. The scientist whose alpha-particle scattering experiment led him to conclude that the nucleus
of an atom contains a dense center of positive charge is___________________________
82. Which atomic particle determines the chemical behavior of an atom?________________
83. List the three main subatomic particles. Provide their charge and relative size.
84. Which subatomic particle has the smallest mass? ___________________
85. Identify each of the following.
a. The heaviest noble gas
b. The transition metal that has 24 electrons as a +3 ion
c. The halogen in the third period
d. The alkaline earth metal that has 18 electrons as a stable ion
85a. Atoms of the same element having the same atomic number but different mass numbers are
called ___________________________.
86. The mass number of an atom equals ______________________.
87. The number of protons in the nucleus of an atom is called its_______________
88. Classify the following as a metal (M), nonmetal (NM), or metalloid (ML).
a. arsenic ____
f. cesium ____
b. argon____
g. carbón ____
c. calcium ____
h. calcium ____
d. plutonium ____
i. copper ____
e. cerium ____
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89. Which of the following elements are an alkali metal?
a. Ca
c. Fe
b. Cu
d. Na
e. Sc
90. Which of the following elements is an alkaline earth metal?
a. Ca
c. Fe
b. Cu
d. Na
e. Sc
91. Which of the following is a noble gas?
a. Ar
c. H2
b. N2
d. O2
e. CO2
92. Provide a list of several elements that are similar. How do you know this?
93. The distance between two successive peaks or troughs in a wave is called _____________
94. The ______________ indicates the number of waves that pass a given point per second.
95. The ______________ indicates how fast a given peak of a wave moves through space.
96. A packet of energy of electromagnetic radiation is called
97. We usually use the term ______________ for all forms of electromagnetic radiation.
98. The form of EMR that has more energy per photon than X-rays is _________________
99. The form of EMR that has less energy per photon than microwaves is ______________
100. Which color of visible light has the most energy per photon? _________________
101. Which color of visible light has the least amount of energy per photon?
_________________
102. The lowest possible energy state of an atom is called its ______________ state.
103. The energy levels of the hydrogen atom (and all atoms) are ______________, meaning that
only certain discrete energy levels are allowed.
104. The ____________________________ is a phenomenon that may be caused by the burning
of fossil fuels, which increases the CO2 content in the earth’s atmosphere.
104. ______________ is a form of oxygen that protects us from high-energy radiation emitted by
the sun.
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105. The probability map for an electron is called an ____________________
106. As the principal energy level increases in an atom’s orbitals, the average distance of an
electron energy level from the nucleus ______________.
107. The shape of an s orbital is ________________
108. The shape of a p orbital is _______________________
109. The shape of a d orbital is ________________________
110. Give the maximum electron capacity of each of the following orbital’s: s,p,d,f
.
111. State the maximum number of electrons allowed in each.
a. third principal energy level ______________
b. any p sublevel ______________
c. a 3d orbital ______________
112. What is the maximum number of electrons that can be put into each of the following
subshells?
a. 4d ______________
c. 5f ______________
b. 4f ______________
d. 2s ______________
113. The number of unpaired electrons in an oxygen atom is ____________
114. Provide the electron configurations for the following elements: (continued on next page)
phosphorus atom is_____________________________
carbon atom is _________________________________
Si __________________________________________
Fe___________________________________________
Co___________________________________________
Mn__________________________________________
Sc___________________________________________
Sb___________________________________________
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Cu___________________________________________
Ni____________________________________________
K_____________________________________________
Br_____________________________________________
Pb_____________________________________________
Ba_____________________________________________
115. The halogens (Group 7) contain how many valence electrons?___________
.
116. The elements chlorine and iodine have similar chemical properties because :
117. The alkali metals have how many valence electrons?____________
118. The noble gases contain how many valence electrons? _______________________
119. When moving down a group (family) in the periodic table, the number of valence electrons
a. remains constant
b. increases
c. doubles with each move
d. decreases regularly
e. changes in an unpredictable manner
.
120. The Group 3 elements through the Group 8 elements form an area of the periodic table
where the electron sublevels being filled are ____________________
121. The number of unpaired electrons in a cobalt atom is _______________
122. Which of the following atoms has the largest atomic radius?
a. Na
c. Si
b. Mg
d. P
e. C
123. Which of the following atoms has the highest ionization energy?
a. Na
c. Si
b. Mg
d. P
e. Cl
124. Which of the following atoms has the smallest atomic radius?
a. As
c. Bi
b. Sb
d. P
e. N
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125. Which of the following has the largest atomic radius?
a. Na
c. P
b. Mg
d. N
126. Which of the following has the highest ionization energy?
a. K
c. C
b. Ca
d. N
.
127. Which of the following has the smallest atomic radius?
a. N
c. Br
b. F
d. Cl
128. Which of the following atoms has the highest ionization energy?
a. Al
c. P
b. Si
d. As
e. O
e. O
e. S
e. Sb
129. Metal atoms tend to ______________ electrons and form ______________ ions.
130. Of the metals in Group 1, which has the highest ionization energy?
131. Order the elements S, Cl, and F in terms of increasing ionization energy.
132. Order the elements S, Cl, and F in terms of increasing atomic radii.
133. Which has the larger atomic radius, S or Si?
134. Which has the higher ionization energy, Rb or Cs?
135. Which has the higher ionization energy, K or Br?
136. Which properties generally increases as we go from the lower left to the
upper right of the periodic table?
137. What are the general trends in ionization energy
138. How does magnesium compare with sodium in terms of the following properties?
a. atomic size
b. number of outer shell electrons
c. ionization energy