Physical Science: Chemistry
Study Guide – Final Exam
Test consists of 90 multiple choice questions.
Introduction Unit– Graphing, measuring, and metric system
1. Where on the graph would I put the independent variable? _________________________
2. Where on the graph would I put the dependent variable? _________________________
3. Time is always considered the _____________________ variable.
4. How should measurements in the metric system be written, as fractions or decimals? _____________________
5. List all the metric prefixes in order from largest to smallest, starting with „kilo-„.
6. List and describe the 5 steps of the scientific method.
7. What is a hypothesis?
8. What are two things that all good hypotheses have to do?
9. What is a variable?
10. What is the control of an experiment?
11. Create a graph of the data listed below using the graph area.
Time (s)
0
2
4
6
8
10
12
Speed (cm/s)
0
4
8
12
16
20
24
Unit 1: States of Matter/Thermal Chemistry
12. What is mass? In what units can it be recorded?
13. What measuring devices are used to determine mass?
14. What is volume? In what units can it be recorded?
15. What measuring devices are used to determine volume?
16. Describe the properties of plasma
17. Complete the following chart, listing the states of matter in order of least energy to most and
stating whether they have a definite volume and/or a definite shape.
18. What is the volume of the object in the picture? ______mL
19. What is the “meniscus” and where do you measure it from?
This is a phase-change diagram for water.
20. Label the phase change diagram as the temperature is increasing and decreasing.
21. Explain what is happening during Leg B and Leg D.
22. What is the difference between vaporization, evaporation, and condensation?
23. Particles move as the states of matter change from low to high temperatures. Illustrate below the motion and
spacing of these particles in a melting ice cube. Describe the attractive forces between the particles in each state.
___________________
___________________
___________________
24. Define the following:
Conduction: _____________________________________________________________________________
Convection: _____________________________________________________________________________
Radiation: _______________________________________________________________________________
25. What is specific heat? _____________________________________________________________________
26. What is the difference between heat and temperature?
27. Heat (thermal energy) flows from objects/areas with a ____________________ temperature to objects/areas
with a ______________________ temperature.
28. Describe the molecular make-up of a material that is generally a good conductor.
29. Give 3 examples of materials that would be good thermal conductors.
30. Give 3 examples of materials that would be good thermal insulators.
31. What is the freezing point/boiling point of water in degrees Celsius and Fahrenheit?
Unit 2: Atomic Theory/Periodic Table
32. The building blocks of matter are________.
33. What are the three subatomic particles, their charges and their locations in an atom?
34. Define strong nuclear force.
35. The atomic number of an element is the same as the ________. The number of neutrons + the number of
protons tells us the ________.
36. Draw an example of a periodic table tile. Be sure to label the element name, chemical symbol, atomic mass,
mass number, and atomic number. Next, draw one to represent Nitrogen.
37. Define isotope and identify how many protons, neutrons, and electrons are in a Hydrogen-3 (Tritium) isotope?
38. What are valence electrons? How can you figure out how many valence electrons an element has? Name the
diagram used to show the valence electrons of an element.
39. Calcium has an atomic number of 20. How many filled energy levels does it have? How many electrons are left
over?
40. Why are Noble Gases considered non-reactive?
41. What do scientists call the place where electrons are found? ___________________________
42. What are the benefits of the following elements?
Chlorine:
Fluorine:
Aluminum:
43. What are the only two elements that are liquid at room temperature? ______________________________
44. Identify where on the periodic table these families are found, their valence electrons and their oxidation
numbers:
Halogens: ______________________________________________________________________________
__________________________________________________________________________________ _____
Alkali metals: ___________________________________________________________________________
_______________________________________________________________________________________
Alkaline Earth Metals: ____________________________________________________________________
_______________________________________________________________________________________
Noble Gases: ________________________________________________________________________
__________________________________________________________________________________________
45. As you move from left to right across the periodic table, what happens to the mass and size of the elements?
46. The ________ ________ of an element is the total number of protons and neutrons in the nucleus.
47. Fill in the following chart.
Atomic Number
Protons
Neutrons
Mass
Electrons
Na
Cl-1
Li+1
48. Elements with similar properties are listed in a single column on the periodic table called ______________.
49. Be able to name the discoveries of the following scientists:
a.
Bohr: _____________________________________________________________________
b. Dalton: _____________________________________________________________________
c.
Democritus: _____________________________________________________________________
d. Rutherford: _____________________________________________________________________
50. Where are nonmetals located on the periodic table? ___________________ Metals? ___________________
51. Ionic bonds form between __________________________________
52. Covalent bonds form between ________________________________
53. In the formation of an ionic bond, the metal ________________ electrons and the nonmetal ____________
electrons.
54. Define diatomic molecule and provide four examples.
55. What is the difference between a monoatomic ion and a polyatomic ion?
56. What is so unique about Carbon?
57. How do you figure out how many valence electrons an atom will have by looking at the periodic table?
58. What does the oxidation number tell us about an element? How do you figure out an element‟s oxidation
number by looking at the periodic table?
59. How many valence electrons does an atom need to be considered stable? _____
60. What are the only 2 elements that don‟t follow this rule? _____________. How many valence electrons do
they need? ____
61. Draw the dot diagram for the following elements:
Tin
Lead
Xenon
Iodine
Cesium
62. How many atoms of each element are in 4H2O. Put a box around the coefficient and circle the subscript.
H= __________________________ O=_____________________________
Unit 3: Nomenclature,Formula Stoichiometry & Bonding
63. Complete the following table by writing the chemical formula of the compound formed by the two ions.
Br-
CO32-
OH-
Ni3+
NH4+
Ba+
Al3+
64. Complete the following table by writing the chemical formula and naming the compound formed.
Chlorine
Magnesium
Lithium
Sodium
Calcium
Unit 4: Equations and Organic Chemistry
Balance the following equations:
65.
__C7H17 + __O2  __CO2 + __H2O
66. __CaCO3 + __H3PO4  __Ca3(PO4)2 + __H2CO3
67. __Ag2S  __Ag + __ S8
68. __KBr + __Fe(OH)3  __KOH + __FeBr3
69. __KNO3 + __H2CO3  __K2CO3 + __HNO3
70. __Pb(OH)4 + __Cu2O  __PbO2 + __CuOH
71. __Cr(NO2)2 + __(NH4)2SO4  __CrSO4 + __NH4NO2
72. __KOH + __ Co3(PO4)2  __K3PO4 + __Co(OH)2
73. __KNO3  __KNO2 + __O2
74. __O2 + __CS2  __CO2 + __SO2
75. __BaF2 + __K3PO4  __Ba3(PO4)2 + __KF
76. __Al + __ H2SO4  __Al2(SO4)3 + __H2
Sulfate
Oxygen
77. List the reactants and products for the following equation: _1_WO3 + _3_H2  _1_W + _3_H2O
78. What is meant by “Atoms are conserved in chemical reactions” (Law of Conservation of Mass)?
79. Predict the products of the following reactions and identify what type of reaction it is.
AgNO3 + Cu
2H2O
_______________ Type of reaction:
_______________ + ______________ Type of reaction:
80. Define physical property: _______________________________________________________________________
81. Define chemical property: _______________________________________________________________________
Classify each of the following as being a physical (P) or chemical (C) property.
82. Blue color ____
83. Density ____
84. Flammability ____ 85. Melting point ____
86. Hardness ____
87. Odor ____
88. Sour taste ____
89. Reacts with acid to form H2 ____
90. Define physical change and give examples.
__________________________________________________________________________________________
91. Define chemical change and give examples.
__________________________________________________________________________________________
92. Is dissolving a physical or a chemical change? Explain why this is.
93. Explain how a chemical change occurs when a piece of paper is burned.
94. What is the result of a chemical change?
95. Compare/contrast endothermic and exothermic reactions in regards to heat energy.
96. Identify the following examples below as “endothermic” or “exothermic”.
_____________________ Instant cold pack
___ __________________Drain cleaner
______________________ Meal, Ready to Eat (MRE)
Unit 5: Acids & Bases
97. Predict the product(s) of the following acid-base neutralization reaction.
HCl + NaOH  _______________ + _______________
What two products form from a neutralization reaction?
98. Predict the products(s) of the following chemical reactions
AgNO3 + Cu
2H2O
_______________ Type of reaction:
_______________ + ______________ Type of reaction:
99. What is the pH scale and what does it measure?
100. List the characteristics of acids and bases.
101. List common tests used to indicate acids and bases.
102. List the formula and name for common acids and bases.
Chapter 22-Nuclear Reactions
Review Questions:
103. Compare/contrast fission and fusion. (Include what happens inside the sun.)
104. Why does nuclear decay occur?
105. What is Carbon-14 used for?
106. Long term exposure to radiation is known to cause _______________.