EOC Exam Review Name:______
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This semester review was compiled using the NC Standard Course of Study for Chemistry. You need to answer each question. This semester review is due by January 6, 2015. This packet will count as two tests and two labs. This will significantly affect your grade!!! Answers will be provided before school beginning December 1. Use your green/yellow “reference packets” as needed. You will provide me with the work you have completed and I will allow you to check your answers for those problems. You turn in questions in consecutive order (1, 2, 3, 4…) on notebook paper. (If you want to work out of order, begin a new sheet of paper each time you skip ahead.)
Atom and Periodic Table Review
1. Sketch a PT similar to the one to the right and then, label metals, nonmetals and metalloids (or semi-metals).
2. Sketch a PT similar to the one to the right and then, label periods and groups.
3. Sketch a PT similar to the one to the right and then, label s, p, d, and f blocks.
4. List the five major properties of metals.
5. Describe the five major properties of nonmetals
6. What are semi-metals/metalloids?
7. Sketch and complete a table similar to the one below.
Particle / Location / Charge / Relative mass(compared with one another)
8. What does the atomic number and mass number tell us about the atom?
9. What symbol is used for atomic number? Mass number?
10. Draw the Bohr model for the Al atom. Fill in the number of protons, neutrons and electrons. It is an aluminum atom with a mass number of 27.
11. Who discovered the proton?
12. Who discovered the electron?
13. Who discovered the neutron?
14. Convert 125 °C to K.
15. The “plum-pudding” model was created by
16. Who performed the “gold foil” experiments?
17. How many protons are there in zinc?
18. How many neutrons are there in mercury?
19. Air is best classified as a(n)
20. Gold is best described as a(n)
21. Water is best classified as a
22. Give 5 examples of a chemical change.
23. Give 5 examples of a physical change.
24. Give 5 examples of a physical property
25. Give 5 examples of a chemical property.
26. State the rule of thumb to determine if a chemical change has occurred.
27. What is difference between a substance and a mixture?
- Complete the following table.
Name / Nuclear/ Isotopic Symbol / Atomic Number / Mass Number / Average atomic mass / Protons / Electrons / Neutrons / Ion Isotope Neutral / Charge
(if applicable)
11 / 10 / 12
Fluorine -18 / 9
Oxygen - 14 / -2
126C
- Calculate the average atomic mass of the following isotopes (show work):
- 15% 55Fe, 85% 56Fe
- 95% 14N, 3% 15N, 2% 16N
- Using the Bohr model for Hydrogen, determine the energy (wavelength and section of electromagnetic spectrum) that is produced when an electron falls from the 3rd to the 1st energy level?
- Red light would be produced when an electron “drops” between which energy levels according to the Bohr model of the Hydrogen Atom?
- What is a quanta? Photon?
- Describe the current model of the atom.
- List the number of electrons in the following energy levels:
1st à______2nd à______
3rd à______4th à______
35. Construct the longhand, short hand, and orbital e- configurations for the following elements.
a. K
b. U
c. Ar
d. As
36. Given the electron configuration below, identify the element, valence electrons, oxidation number and/or number of electrons gained or lost.
a. 1s22s22p1 element:______
b. 1s22s22p63s2 oxidation number: ______
c. 1s22s22p63s23p5 valence electrons:______
d. 1s22s22p63s23p54s23d104p4 oxidation number: ______why?
37. Name the following families on the Periodic Table and identify as representative/main (A) or transition(B) :
Group Name A or B “elements”
1
18
2
17
3-12
38. Match the property to its proper group. (Use the #’s given for each group when matching.)
[Note: Some choices will be used more than once.]
Alkali Metals à 1 Alkaline-earth Metals à 2
Transition Metals à 3 Halogens à 4
Noble Gases à 5
a. Form “salts” when reacted with metals. ______
b. Least reactive of all elements. ______
c. Very reactive with water. ______
d. Most reactive group of all non-metals ______
e. Contain elements that are free in nature ______
f. Contain the hardest and densest metals ______
g. Have a +2 charge when they become an ion ______
h. Have to be shipped in oil when free ______
i. Considered to be inert ______.
39. Define: ATOMIC RADIUS
In the following, number the elements 1 – 4, with 1 being the smallest and 4 being the largest
a. Mn Br Ga K
b. Mg Ar S Cl
c. Bi N P As
Justify your answers
40. Identify the smaller ion of the two listed and justify your answer.
a. N-3 N Justify
b. Be+2 Be Justify
41. Define: Ionization Energy
In the following, number the elements 1 – 4, with 1 being the smallest and 4 being the largest
a. Mn Br Ga K
b. Mg Ar S Cl
c. Bi N P As
Justify your answers
42. Define: Electronegativity / Electron Affinity
In the following, number the elements 1 – 4, with 1 being the smallest and 4 being the largest.
a. Mn Br Ga K
b. Mg Ar S Cl
c. Bi N P As
Justify your answers
Formulas and Atomic Stoichiometry Review
43. Write the chemical formula that would exist between the following elements, then draw the Lewis structure that confirms the formula.
a. Zn & F à ______
b. Al & O à ______
c. Ca & S à ______
d. K & Br à ______
44. Name each of the following compounds.
EOC Exam Review Name:______
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a. AlCl3 à ______
b. CO2 à ______
c. LiNO3 à ______
d. Fe2O3 à ______
e. Na2CO3 à ______
f. P2O5 à ______
g. SO3 à ______
h. Ba(C2H3O2)2 à ______
i. NH4OH à ______
j. ZnS à ______
EOC Exam Review Name:______
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45. Write the chemical formula from the following names:
EOC Exam Review Name:______
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a. Potassium nitrate à ______
b. Carbon monoxide à ______
c. Silver oxide à ______
d. Copper (II) chloride à ______
e. Nitrogen dioxide à ______
f. Aluminum sulfate à ______
EOC Exam Review Name:______
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46. Calculate the GFM of the following compounds:
a. NaBr à ______c. Al2(S2O3)3 à ______
b. Mn3(PO4)2 à ______d. Ag2SO3 à ______
47. Make the following conversions.
a. 3.65 moles H2CO3 = ______g H2CO3
b. 5.10 x 1028 molecules CO2 = ______moles CO2
c. 37.9 g K2S = ______moles K2S
d. 195 g Ca(OH)2 = ______molecules Ca(OH)2
48. What is the % composition of each element in the following compounds:
a. Li2SO4
b. Ca(NO2)2
49. Calculate the empirical formula for the following.
a. 32.38 % Na, 22.65 % S, and 44.99 % O
b. 66% Ca and 34 % P
50. Calculate the molecular formula for:
a. A compound made of 25.3% copper, 12.9% sulfur, 25.6% oxygen, and water, with an molecular mass of 249.7 g/mol.
b. The empirical formula of a compound is CH2. Its molecular mass is 70 g/mol. What is its molecular formula?
c. A compound is found to be 40.0% carbon, 6.7% hydrogen, and 53.5% oxygen. Its molecular mass is 60.0 g/mol. What is its molecular formula?
Reaction Stoichiometry Review
I. Chemical Reactions
51. Balance the following reactions and then classify them.
a. __HCl + ____Al à ____AlCl3 + ____H2 Classification à
b. ____Zn + ____O2 à ____ZnO Classification à
c. ___CH4 + ____O2 à ____CO2 + ____H2O Classification à
d. __Mg(NO3)2 + ____Cu3PO4 à ____Mg3(PO4)2 + ___CuNO3 Classification à
e. ___H2O2 à ____H2O + ____O2 Classification à
52. Predict the products and balance the reaction for the following.
a. ____Al + ____O2 à
b. ____H2O à
c. ____C2H6 + ____O2 à
d. ____Ag2SO4 + ____Ba3N2 à
e. ____FeCl3 + ____F2 à
53. Answer the following questions that involve experimentation.
a. The “pop” test is used to check for ______.
b. If a glowing splint reignites ______was present
c. When a student places a glowing/burning splint into a test tube containing a gas, the splint is immediately extinguished (goes out); therefore ______was present.
d. The process in which an electrical current is passed through an object in order for it to decompose is called
______.
e. What must be present in order for something to burn? ______
54. Use the activities series to decide if the following reactions will occur.
a. Pb2O3 + Li à ???? ______D. Al + HCl à ???? ______
b. ZnF2 + Cu à ???? ______E. Fe + MgSO à ???? ______
c. H2S + Hg à ???? ______F. Cr + AuI3 à ???? ______
- What are three possible categories of products in a double replacement reaction?
II. Stoichiometry
56. How many grams of NH3 are produced when excess N2 reacts with 11.7 g of H2?
N2 + 3H2 à 2NH3
57. When 15.4 grams of Al is added to HCl, how much HCl is needed to react completely with the Al?
2Al + 6HCl à 2AlCl3 + 3H2
58. What mass of Cu could be produced when 4.77 g of K reacts with excess CuSO4?
59. How much O2 is needed to react completely with 31.9 g of C2H6?
60. How much Al2(SO4)3 is produced when 6.55 g of Na2SO4 reacts with excess Al(OH)3?
Energy in reactions
61. A fire is what type of energy reaction? ______
62.
A first aide cold pack is what type of energy reaction? ______
63. What type of energy reaction is the diagram A? ______
64. What type of energy reaction is the diagram B? ______
65. What is the minimum amount of energy required for a reaction to start? ______
The graph below is a potential energy diagram of a compound which is formed from its elements.
66. Which interval represents the heat of reaction? ______
67. Which interval represents the activation energy of the forward reaction? ______
68. What would change if a catalyst was added? What is a catalyst?
69. Where is the activated complex found?
70. Explain the collision theory?
Phases Review
PHASE CHANGES
71. Define the following phase changes and describe the change in kinetic energy.
a. Solid à Liquid è ______KE è ______
b. Solid à Gas è ______KE è ______
c. Gas à Liquid è ______KE è ______
d. Liquid à Solid è ______KE è ______
e. Liquid à Gas è ______KE è ______
f. Gas à Solid è ______KE è ______
72. Label the following chart according to a phase change from ice to steam
E
140 oC D
C
B
10 oC
A
Energy
73. From the above chart, answer the following questions:
a. What is the boiling point of the substance?
b. Which letter represent where vaporization and condensation occur?
c. Which letter(s) show a change in kinetic energy?
d. Which letter shows where crystallization can occur?
e. What is the melting point of the substance?
f. Which letter(s) show a change in potential energy?
74. How much energy is required to raise 16.7 g of ice at –27 oC to steam at 162 oC?
75. How much energy is lost when 14.7grams of liquid water freezes?
76. If you fill a sauce pan with 1000grams of water and heat the water from 21.70C to 98.0oC, how much heat is required?
77. What mass of water was boiled if 340 000J of heat was required?
Phase Diagrams
B
760
I II
III
220 A
55 70 165 190
Temperature (oC)
a. What section represents the gaseous phase? ______
b. What is the substances normal boiling point? ______
c. What is point B called? ______
d. Is the solid more or less dense than the liquid? ______
e. Would an increase of pressure favor melting or freezing? ______
f. What section represents the solid phase? ______
g. What is the substances normal melting point? ______
h. What is the critical temperature? ______
i. What does point A represent? ______
j. What section represents the liquid phase? ______
k. What pressure and temperature would all three states of matter coexist? ______
KMT Review
Gas Laws Review:
78. Which of the following gas laws match up to the following descriptions:
a. relationship between temperature and pressure à ______
b. our atmospheric pressure is a practical example à ______
c. explains how a hot air balloon works à ______
d. relationship between volume and pressure à ______
79. A tire has an air pressure reading of 35.1 psi on a day when it is 30 °C. What would be the air pressure of this tire on a day when it is 0 °C?
80. A hot air balloon can rise only when its air volume is 2560 L. If air inside an air balloon has a volume of
1100 L at 130 °C, what must the temperature become in order for the balloon to be able to fly?
81. NH3 will occupy a volume of 1.45 L under 165 kPa. What must the pressure be if the volume of NH3 rises to 6.01 L?
82. A certain gas occupies a volume of 25.1 cm3 at STP. What would be the volume of this gas if the pressure was 175 torr and the temperature was 147 °C?
83. How many times faster will oxygen gas diffuse compared to argon gas?
84. A gas with a volume of 48.7 L exerts a pressure of 187 mm Hg. The gas is composed of 24.1 L of methane, 11.1 L of carbon monoxide, and 13.5 L of ammonia. What is the pressure of the carbon monoxide?
85. Air will leak out of a punctured tire due to ______.
86. What kind of gas will diffuse the fastest? Answer à ______
Molar Volume and the Ideal Gas Law
87. What is the value of molar volume according to Avogardro’s principle? ______
88. What is the formula for the ideal gas law? ______
89. What value of R corresponds to the following pressures:
a. atm à ______c. mm Hg à ______